# Sum-Frequency Generation Spectroscopy at Aqueous Electrochemical Interfaces

Ba Lich Pham, Alireza Ranjbari, Abderrahmane Tadjeddine, Laetitia Dalstein, Christophe Humbert

► To cite this version:

Ba Lich Pham, Alireza Ranjbari, Abderrahmane Tadjeddine, Laetitia Dalstein, Christophe Humbert. Sum-Frequency Generation Spectroscopy at Aqueous Electrochemical Interfaces. Symmetry, 2024, 16, pp.1699. 10.3390/sym16121699. hal-04867763

HAL Id: hal-04867763

https://universite-paris-saclay.hal.science/hal-04867763v1

Submitted on 6 Jan 2025

HAL is a multi-disciplinary open access
archive for the deposit and dissemination of sci-
entific research documents, whether they are pub-
lished or not. The documents may come from
teaching and research institutions in France or
abroad, or from public or private research centers.

L'archive ouverte pluridisciplinaire HAL, est
destinée au dépôt et à la diffusion de documents
scientifiques de niveau recherche, publiés ou non,
émanant des établissements d'enseignement et de
recherche français ou étrangers, des laboratoires
publics ou privés.

<figure><img src="image_1.png" /></figure>

Distributed under a Creative Commons Attribution 4.0 International License
<figure><img src="image_2.png" /></figure>

symmetry

IMPACT
FACTOR
2.2

CITESCORE
5.4

Review

# Sum-Frequency Generation Spectroscopy at Aqueous Electrochemical Interfaces

Ba Lich Pham, Alireza Ranjbari, Abderrahmane Tadjeddine, Laetitia Dalstein and Christophe Humbert

Special Issue

Chemistry: Symmetry/Asymmetry—Feature Papers and Reviews

Edited by
Prof. Dr. György Keglevich

<figure><img src="image_3.png" /></figure>

<figure><img src="image_4.png" /></figure>
<figure><img src="image_5.png" /></figure>

Review

# Sum-Frequency Generation Spectroscopy at Aqueous Electrochemical Interfaces

Ba Lich Pham<sup>1,*</sup> and Alireza Ranjbari<sup>1,2</sup>, Abderrahmane Tadjeddine<sup>1</sup>, Laetitia Dalstein<sup>3</sup> and Christophe Humbert<sup>1,*</sup>

**Abstract:** The electrochemical interface (EI) is the determining factor in the yield and mechanism of sustainable energy storage and conversion systems due to its intrinsic functionality as a dynamic junction with the symmetry breaking of the molecular arrangement for complex reaction fields of mass transport and heterogeneous electron transfer. At the EI, the externally applied potential stimulus drives the formation of the electrical double layer (EDL) and governs the adsorption of interfacial adsorbate species in aqueous electrolyte solutions. Water and its aqueous electrolyte systems are integral and quintessential elements in the technological innovation of various fields such as environmental sciences, electrocatalysis, photocatalysis, and biochemistry. Although deciphering the structure and orientation of water molecules at the electrode-electrolyte interface in a quantitative analysis is of utmost importance, assessing chemical phenomena at the buried EI was rather challenging due to the intricacy of selecting interface-specific methodologies. Based on the non-centrosymmetry of the interfaces' electronic properties, sum-frequency generation (SFG) spectroscopy has been manifested to be specifically well suited for probing the EI with detailed and comprehensive characteristics of adsorbates' chemical structures and electrochemical events. In this review, we holistically engage in a methodical and scrupulous assessment of the fundamental EDL models and navigate towards the connection of the renowned Stark effect and potential dependence of SFG spectra at heterogeneous electrode-electrolyte interfaces. We dissect the development, advantages, and available geometrical configurations of *in situ* SFG spectroscopy in harnessing the EI. A broad spectrum of applications in unraveling the water orientations and rationalizing the convoluted mechanism of fuel-generated electrocatalytic reactions with particular encumbrances and potential resolutions is underscored by leveraging SFG spectroscopy.

**Keywords:** surface symmetry breaking; surface and bulk molecular geometry; sum-frequency generation spectroscopy; water interfaces; electrical double layer; spectroelectrochemical cells

<figure><img src="image_6.png" /></figure>

check for
updates

**Citation:** Pham, B.L.; Ranjbari, A.; Tadjeddine, A.; Dalstein, L.; Humbert, C. Sum-Frequency Generation Spectroscopy at Aqueous Electrochemical Interfaces. *Symmetry* **2024**, *16*, 1699. https://doi.org/10.3390/sym16121699

Academic Editor: György Keglevich

Received: 8 November 2024

Revised: 16 December 2024

Accepted: 18 December 2024

Published: 21 December 2024

<figure><img src="image_7.png" /></figure>

**Copyright:** © 2024 by the authors.
Licensee MDPI, Basel, Switzerland.
This article is an open access article
distributed under the terms and
conditions of the Creative Commons
Attribution (CC BY) license (https://
creativecommons.org/licenses/by/
4.0/).

## 1. Introduction

Water molecules are a pivotal instrumental component in aqueous chemical processes due to their ubiquitousness on Earth. In reactions, they can appear in the form of a reactant, a product, or a polar solvent for the solvation process. To exemplify, the two key electrochemical energy conversion processes based on chemical equations of water ($H_2O \rightleftharpoons H_2(g) + \frac{1}{2}O_2(g) - \Delta_f G^{\circ}_{298K} = +237.22 \text{ kJ} \cdot \text{mol}^{-1}$ for $H_2O(l)$, +228.66 kJ·mol⁻<fnref n="1" /> for $H_2O(vap)$) [1,2] in the electrocatalytic water splitting/water-based electrolysers (forward) and fuel cells (backward) contribute to addressing the imminent worldwide vacancies of green energy and water resources (Figure 1). Water is also the pervasive polar solvent for

<footnote n="1">¹ Institut de Chimie Physique, Université Paris-Saclay, Centre National de la Recherche Scientifique (CNRS), UMR8000, 91405 Orsay, France; alireza.ranjbari@universite-paris-saclay.fr (A.R.); abderrahmane.tadjeddine@universite-paris-saclay.fr (A.T.)</footnote>

<footnote n="2">² Département de Chimie, Institut Universitaire de Technologie d'Orsay, 91190 Gif-sur-Yvette, France</footnote>

<footnote n="3">³ Laboratoire Ondes et Matière d'Aquitaine, Université de Bordeaux, Centre National de la Recherche Scientifique (CNRS), UMR5798, 33400 Talence, France; laetitia.dalstein@u-bordeaux.fr</footnote>

<footnote>* Correspondence: lich.pham-ba@universite-paris-saclay.fr (B.L.P.); christophe.humbert@universite-paris-saclay.fr (C.H.)</footnote>
most physical and chemical phenomena owing to its high dielectric constant (κ ≈ 78.49 at 25 °C) [3]. Thus, their indispensable appearances bolster the technological innovation and research development for hygro-sensors, soil and mineral (de)formation, ocean acidification, and pollutants' reduction in environmental chemistry [4,5]; for metabolism of charged biomembranes in living organisms [6,7]; for applications of colloidal nanoparticles in nanotechnology [8]; for hydrogen/oxygen evolution reaction (HER/OER) in oxide-based photocatalysis (artificial photosynthesis) [9]; and for hydrogen oxidation/oxygen reduction reaction (HOR/ORR) in solid oxide fuel cells [10,11], as depicted in Figure 1. During these chemical occurrences, there are two common underlying features: (1) water molecules interact with charged solid surfaces, and (2) the yield of chemical reactions is governed by the interaction of chemical species at the water interfaces. The reason for the first characteristic is that water molecules possess a high net dipole moment (μ = 1.85 D or C·m) so that ions are easily dissolved, and charges on the surface of the material in aqueous solutions are generated responsively for chemical transformations. Then, the station of chemical changes here is considered to be the interface between a solid material (inorganic oxides, semiconductors, metals) and an aqueous solution.

<figure><img src="image_8.png" /><figcaption>**Figure 1.** Schematic representations of electrochemical reactions in the solid oxide (a) fuel cells (SOFCs), (b) electrolytic cells (SOECs), and (c) photocatalytic water splitting regarding the water cycle. Green and red arrows in (a,b) indicate the half-reactions at the anode and cathode of the fuel cell and electrolytic cell, respectively. Two types of conductors (proton and oxygen ions) exist in solid oxide-based cells. SOFC and SOEC are two key components in the energy transition, corresponding to gas to power (G2P) and power to gas (P2G) processes, respectively. In (c), oxide-based photocatalytic water splitting occurs via three mechanistic steps: (1) exciton (electron-hole) excitation through light absorption (photocatalyst + *hν* → *e*⁻ + *h*⁺), (2) charge separation and migration of charge carriers toward the photocatalyst's surface, and (3) surface reactions (HER at the conduction band (CB) and OER at the valence band (VB)). NHE refers to the normal hydrogen electrode.</figcaption></figure>
The formation of charged interfaces in an aqueous solution can be derived from five key origins: (1) electrochemical process when applying an external potential to an electrode (Pt, Au, glassy carbon, etc.) in an electrochemical cell, (2) pH change via (de)protonation of surface groups (proteins or colloidal particles: ≡NH₂ + H⁺ ⇌ ≡NH₃⁺ where ≡ is surface-bound), (3) ion exchange between electrolyte solution and material surface via dissociation of surface groups (SiO₂, TiO₂: ≡ROH ⇌ ≡RO⁻ + H⁺ with pKₐ = -log(([(RO⁻)][H⁺])_{local})/[(ROH)])), (4) ion adsorption from surrounding aqueous solution (Al₂O₃), and (5) surface complexation through chemical complexion reaction [12]. Amongst these five particular ways of a charged surface generation, the charged electrode-electrolyte interface (origin (1)), which is defined as the electrochemical interface or electrified interface (EI), is the centerpiece of sustainable energy conversion and storage systems (batteries, supercapacitors, fuel cells, corrosion, etc.). Electrochemical interfaces are directly related to structural dynamics and heterogeneity, specifically, the charge and ion transfer at the interface boundary of the metal (electron conductor) and the aqueous electrolyte (ion conductor), which is the core of decisively manipulating the efficiency of electrochemical energy conversion [13]. On the one hand, the pursuit of optimizing the matching between the novel electrolyte and modified/functionalized electrode materials, and discovering next-generation electrocatalysts to improve the overall electrochemical performance is mainly inclined to more preference. On the other hand, the knowledge of the dynamic nature of aqueous electrochemical interfaces is still overlooked and insubstantial. Therefore, to understand the mechanism of electrochemical transitions under an aqueous medium, in-depth insight into water interfaces must be addressed and analyzed.

At electrochemical interfaces, the active sites are the key features that drive the electrochemical mechanism in electrocatalysis (specifically HER in Figure 2a,b and OER in Figure 2c). At the microscopic scale, adsorption layers close to the metal surface form a specific configuration for charge transfer and water reactivity. Water molecules and solvated adsorbate ions interplay in close proximity via covalent bonds and three other types of weak intermolecular interactions (van der Waals/ London dispersion interactions, electrostatic forces, and hydrogen bonds) [14,15]. Thus, knowing how to manipulate and control their structure, composition, and density could ameliorate the kinetics and robustness of the metal surface. Regarding the critical factors maneuvering the complexity of electrochemical interfaces, they can be derived from: (1) the chemical nature of the electrode surface structure, (2) the composition of the electrolyte solution (multivalent ions), and (3) the environmental conditions (concentration, pH, ionic strength, temperature) that affect the structure of adsorbed layers [12,16]. Nevertheless, the pattern of adsorbate layers (ad-layers) is primarily contingent upon an external electrical potential between the working electrode surface and a counter electrode. In principle, when applying a negative/positive potential on the working electrode, the energy level of electrons on that electrode increases/decreases (surface charge accumulation), resulting in attracting atoms that bear a partially positive (δ⁺) electric charge or being attracted by atoms that bear a partially negative (δ⁻) electric charge, respectively. These propensities navigate surface charge and absorbates' orientation and reorganization of electrochemical systems. Hence, the potential-dependent behavior of the electrochemical interface displays a kinetic and dynamic delineation of the electrode surface and adsorbed species and water molecules chemistry.

Numerous analytical electrochemical methods (differential-pulse (DPV) and square-wave (SWV) voltammetries, chronoamperometry (CA), linear sweep voltammetry, cyclic voltammetry (CV), anodic/cathodic stripping voltammetry (SV), etc.) purely determine the macroscopical bulk information of electrochemical systems without much detailing about structural changes upon any redox events. Particularly, DPV, SWV, and SV are electroanalytical techniques aiming to eliminate the residual current (comprising non-faradaic charging current from the electrical double layer and faradaic current from the redox reaction of trace interferents or impurities) and to enhance the faradaic current from the
redox reaction of interest [17]. To analyze the know-how of complex electron transfer reactions on a microscopic scale, surface characterization methods such as microscopy, diffraction, or spectroscopy are required to be coupled with analytical methods. Selecting a hyphenated system that combines two classical methods, electrochemistry and microscopic/spectroscopic techniques, relies on both the requirements of high temporal and spatial resolution. Hyphenating the electrochemical interfaces with surface characterization techniques can be conducted through *ex situ* (off-line) or *in situ* (on-line) approaches. *Ex situ* methods refer to performing the surface characterization outside the electrochemical cell in an external device under an ambient or high vacuum environment such as transmission electron and scanning electron microscopy (TEM and SEM), while *in situ* methods involve the characterization measurement of the electrode surface within being immersed in the aqueous solution of the electrochemical cell, often under operating conditions such as potential control [3,18]. Provided that the electrode is removed from the electrochemical environment, leading to the possible variation of the nature and stability of the electrode surface, *ex situ* techniques limit the capability to be well-fitted with electrochemistry coupling. Surface characterization tools are required to study a true atomistic insight into complex electrochemical interfaces on *in situ* (simulated realistic operating conditions) or even *operando* realistic conditions during electrochemical reactions. Hence, *in situ* structural characterization of electrochemical interfaces provides a detailed molecular-level rationale of the electrode-electrolyte surface structure and elementary steps of the interface reactions.

<figure><img src="image_9.png" /><figcaption>**Figure 2.** Schematic illustrations of (a,b) the hydrogen evolution reaction (HER) mechanisms and (c) the more complex oxygen evolution reaction (OER) mechanisms in electrocatalysis or heterogeneous catalysis where M\* symbolizes the active site of the metal M electrocatalyst; M\*-H\*ad is the chemically surface-adsorbed hydrogen ad-atom; M\*-OH, M\*-O, M\*-OOH are the adsorbed metal hydroxide, oxide, hydroperoxide intermediates, respectively. In the HER, a direct coupling mechanism between the adsorbed species and the other non-adsorbed reactant (Eley-Rideal mechanism) is expressed in the Volmer-Heyrovsky pathway, while the Volmer-Tafel mechanism obeys the Langmuir-Hinshelwood type which both reactants first adsorb on the active sites before a coupling reaction occurs. Blue curved arrows denote the reaction steps in an acidic condition while orange ones are in an alkaline or a neutral medium. Dashed lines represent the formation of chemical bonding. This scheme is inspired by references [16,19,20].</figcaption></figure>
In surface chemistry, scanning tunneling microscopy (STM) and atomic force mi-
croscopy (AFM) from the scanning probe microscopy technique are two potential candi-
dates for providing high-resolution surface characterization tools [3]. While AFM over-
comes the restriction to the electronically conductive surface of STM, which is not the
case for metal electrode surfaces, it offers supplementary configuration about surface to-
pography and surface forces. Due to the tip's presence and its possible interaction with
the surface, the electrochemistry-coupled surface techniques can probe and induce local
changes in conductivity, kinetically reaction rates, thermodynamically electrical potentials,
and chemical reactivity with high spatial resolution, such as scanning electrochemical
microscopy (SECM) [21] and electrochemical scanning tunneling microscopy (ECSTM) [22].
Nevertheless, their diffusional broadening effect and the convolution of reactivity and
topography in their electrochemical response are their limitations [23,24]. Interestingly, a re-
cent study has revealed the dynamics of ion transport at the electrode-electrolyte interface
(the EDL) by employing a transient single-particle imaging technique [25].

The introduction of spectroscopy to electrochemistry (spectroelectrochemistry) can extend even more chemical and electronic structure information of molecules at the interface. X-ray photoemission spectroscopy (XPS) [26,27], adsorption, and emission spectroscopies (XAS and XES) [28–30] are considered element-specific surface-sensitive techniques revealing the electronic energies and the nature of redox states of species. Likewise, energy-dispersive X-ray analysis (EDX) or Auger electron spectroscopy (AES) also render the binding energy of the emitted X-rays or Auger electrons for elemental analysis, respectively. However, electron-based spectroscopy methods generally oblige an ultra-high vacuum (UHV) framework, and it is quite challenging to characterize surfaces under liquid environments and/or buried electrodes [31]. In this context, optical spectroscopic methods such as infrared reflection absorption (IRRAS) and Raman [32] spectroscopies can be good assets. Total internal reflection (TIR) configuration for optical spectroscopies (TIR Raman scattering or attenuated total reflection (ATR) IR) is categorized as non-destructive and surface-sensitive probes for thin films and interfaces [33–35]. The principle of TIR-based spectroscopies relies on the generation of an evanescent wave at the interface between two media (e.g., non-metallic glass prism and air or sample solution) and the interaction of this wave with sample surface [34]. However, coupling TIR optical spectroscopies (IR and Raman) with an electrode (metal surface) encounters several issues: (1) strong adsorption of IR radiation by metals with high absorption coefficients, (2) poor penetration at sample surface and loss of evanescent field due to reflection and scattering phenomena, (3) energy diversion of surface plasmon polariton (SPP) effect from the evanescent wave, and (4) the opacity of metal to IR light [33]. As a result, the nature of light interaction at the electrochemical interface in TIR configuration is non-ideal for coupling with a metal surface because it does not support efficient Raman/IR signal generation.

With the influential breakthrough of surface- and tip-enhanced Raman scattering (SERS [36,37] and TERS [38,39]) and surface-enhanced infrared absorption spectroscopy (SEIRAS) [40–46], surface-plasmonic (SP) enhancement-based electrochemical vibrational spectroscopies can recently be able to potently reach down to single atomic scale for buried electrochemical interfaces probing due to their high surface specificity. The limiting factors in these techniques in the breadth of practical applications are the obligation of having (1) a rough surface of noble metal electrodes (e.g., Au, Cu, or Ag) or nanoparticles (nanostructure-based or tip-based mode) and (2) “hot spots” in the gap between the nanoparticles for surface sensitivity. Noticeably, the reproducibility and repeatability of the tips in TERS can be onerous [39]. Thus, the inevitable inhomogeneity on the surfaces yields elusive interfacial information about conformation and orientation at the molecular level. The ultrathin, pinhole-free dielectric shell-isolated nanoparticle-enhanced Raman spectroscopy (SHINERS) was devised to resolve this hurdle for flat electrodes (metal, graphite) [47–50]. Some research has also employed the principles of nuclear magnetic resonance spectroscopy (NMR) or imaging (MRI) methodology to study the phenomena of electrified interfaces [51–54] but NMR spectroscopy requires exclusive cells, and probes in
the setup and still remains challenges to couple due to its nature of the bulk sensitivity and *in situ* MRI is relatively nascent and in its early stages of development.

One of the fundamental limitations of linear optical spectroscopies (UV-Vis and IR) in the external reflection spectroscopic mode (normal mode) is that they are bulk sensitive [55]. The selectivity and sensitivity of interface data acquisition do not yield solely from the electrical double layer (EDL) surface region but also emanate largely from bulk contributions. To address this issue, an even-order non-linear optical spectroscopy is utilized to provide a plausible solution to surface insensitivity. Vibrational sum frequency generation spectroscopy (SFG or VSFG) or sum-frequency vibrational spectroscopy (SFVS) suffices the demand for an *in situ* molecular-specific and inherently surface-sensitive technique for analyzing the chemical vibrational data fingerprint of molecules at electrode-electrolyte interfaces. The innate symmetry breaking at electrochemical interfaces is the hallmark of symmetry rules to achieve SFG signals. One appealing feature SFG offers is the congruence of operation on both well-defined single crystals and rough electrode surfaces. Even though SFG seems to be a potentially applicable probing method, electrochemical interface analysis remains a challenging task by virtue of the intricate nature of the interfaces and the inadequately developed and limited variety of methodologies. Traditional homodyne SFG is not able to allocate the separation of the real and imaginary parts of the interfacial vibrational signal and thereby reveal an equivocal determination of molecular organization [56]. Phase-sensitive/-specific or heterodyne-detected SFG (PS-SFG or HD-SFG) advances the surface sensitivity, reaching sub-monolayer surface coverage as low as a few percent of a monolayer compared to its predecessor (direct or homodyne SFG) [57]. These merits could be decisive elements for probing electrode-electrolyte interfaces by PS-SFG vibrational spectroscopy under *operando* conditions.

It is correct that heterodyne-detected (HD)-SFG offers several significant advantages over conventional SFG in some aspects. Conventional SFG with homodyne detection can only extract the absolute square of the second-order nonlinear susceptibility $|\chi_{S,eff}^{(2)}|^2$ in SFG spectra and the spectral distortion from the interference between resonant and non-resonant contributions and/or between distinctive vibrational resonances [58]. However, HD-SFG has addressed this issue and provided molecular-level insights into the up/down orientation of interfacial molecules from the sign of the imaginary part $(\pm \text{Im}\chi_{S,eff}^{(2)})$. Despite all the advantages of HD-SFG mentioned above, the development of *in situ* HD-SFG for electrochemical systems encounters some barriers: (1) the requirement of complex and expensive setup for HD scheme with respect to the conventional ones, (2) time resolution limitation to couple with fast electrochemical techniques, (3) challenges in application to rough surfaces, and (4) high sensitivity to environmental conditions (temperature, vibrations, light interference, etc.). As a whole, HD-SFG is an advanced SFG spectroscopic technique and remains a valuable tool for studying electrochemical interfaces, particularly in energy and catalysis research. Continued developments in instrumentation and data analysis procedures may resolve the aforementioned limitations and enlarge its applicability.

Astonishingly, terahertz (THz) spectroscopy has lately been adopted in conjunction with studies about the water interfacial layers without [59] and with *in situ* electrochemical conditions [60,61]. Terahertz spectroscopy is a spectroscopic method using submillimeter radiation (between microwave and far-infrared regions in the electromagnetic spectrum) to study a wide variety of materials (1 THz = 33 cm⁻¹ = 1 ps = 0.3 mm). Initial results of hydrogen-bonded water networks at the Au electrode in different aqueous pH environments [40] suggest THz as a potential and exceptional technique for further studying the structures of water at the buried EI.

This review aims to provide a thorough insight into *in situ* SFG-electrochemistry coupling systems to decipher the chemical occurrences and surface organization at aqueous interfacial regions under a potentiostatically controlled electrochemical environment. First and foremost, we will emphasize the classical theories of the electrical double layer in Section 2, which serves as a cornerstone for the fundamental and applied research in electrochemical energy storage and chemical conversions. Some critical limitations of mean-field
theory are succinctly discussed. Furthermore, we herein address the principles of SFG spectroscopy's symmetry selection rules in Section 3 for non-centrosymmetric electrochemical interfaces. Particularly, we also highlight the well-known vibrational Stark effect and the distinct potential-dependent attribute of the SFG signal. Some considerations for experimental configurations with respect to spectroelectrochemical cells are also supplemented. We will then delve into the particular studies (water molecules, charged molecules, and neutral molecules) of SFG at the aqueous electrochemical interfaces in Section 4, leaning towards applications of electrocatalysis, adsorption-desorption phenomena, and electrochemical transformation. Last but not least, we present some perspectives and initiatives for future research considerations to gain a better comprehension of electrochemical interface studies.

## 2. Descriptive Models of the Electrical Double Layer and Its Mean-Field Theory

Despite the aforesaid prominent significance of electrochemical interfaces in many fields in the Introduction, the electrical double layer (EDL) and its models must be concomitantly and indispensably discussed. To interpret structurally the arrangements of contributing species in a charged interface, it necessitates constructing a descriptive model to speculate its properties and examine the rightness and appropriateness of the model to real phenomena [3]. Irrespective of the ways in which a charged interface is formed, an electrostatic attraction to oppositely charged species (counterions) from an aqueous bulk solution originates from this interface. Electrochemically, an electric field exerting an external potential on a charged electrode will draw distant counterions towards the electrode via attractive forces. This migration accumulates counterions near the electrode, and it is contemporaneous with the coions' diminution. This movement is associated with a flow of transient charging current. The region of two opposite charged layers at the electrode-electrolyte interface is conventionally regarded as the electrical double layer (EDL).

The aforementioned definition of the EDL is the earliest and simplest model commencing from Helmholtz's postulate (1853) [62]. The direct binding of counterions to the electrode surface is organized in a way that their total charges are equivalent to the total charges of the electrode surface. This neutralization results in two sheets of charge with opposite polarities, referred to as a parallel-plate capacitor (the Helmholtz layer, or compact layer, or Stern layer later on) (Figure 3a). The potential in the Helmholtz layer reduces linearly, and the differential capacitance of this capacitor-like arrangement is calculated by $C_d = \frac{\varepsilon\varepsilon_0}{d}$ (in farads, F) where $\varepsilon$ is the dielectric constant of the medium or relative permittivity (dimensionless), $\varepsilon_0$ is the vacuum permittivity ($8.85 \times 10^{-14} \text{ F}\cdot\text{cm}^{-1}$), and $d$ is the interplate spacing or thickness of the double layer (cm) [63]. This description is beneficial in elucidating the basic features of charged surfaces, but the shortcoming of the Helmholtz model directly stems from the evaluation of a constant capacitance. Utilizing electrochemical impedance spectroscopy (EIS), the capacitance $C_d$ actually depends on applied potential and electrolyte concentration, so $\varepsilon$ and $d$ become variables. A more sophisticated concept was proposed by Gouy (1910) [64] and Chapman (1913) [65], individually taking thermal fluctuations of the ions into consideration. This thermal motion partly liberates counterions apart from the electrode surface to the bulk, which causes spatially inhomogeneous ion distribution along the surface normal under potential control and establishes the expanse of the EDL rather than a molecular layer. Thus, they introduced a so-called "diffuse layer" from the thermal effect and formulated the equilibrium ions' distribution by Poisson-Boltzmann theory to flat surfaces (Figure 3a).
<figure><img src="image_10.png" /><figcaption>**Figure 3.** (a) Schematic representation of the electrical double layer (EDL) description according to the Gouy-Chapman-Stern model (GCS) and (b) the illustrative potential profile through the Stern layer (a linear drop) and diffuse layer (an exponential decrease) to the bulk. IHP: inner Helmholtz plane or Stern plane, OHP: outer Helmholtz plane, DL: diffuse layer, SP: slipping or shear plane/shear zone or hydrodynamic plane of shear. Due to the negatively charged surface of the working electrode (WE), the electrical potential is negative. For the sake of simplicity, the dipole moments of only some water molecules are presented. It is noteworthy to highlight that, in long-established chemical practice, the dipole moment direction (arrow) points from the atom with a partial positive charge ($δ^+$) to the atom with a partial negative charge ($δ^−$) to indicate the electron density shift, which is contrary to the International Union of Pure and Applied Chemistry (IUPAC) definition or the convention in physics [66,67]. In the context of this review, the arrow of dipole moment obeys the chemistry convention. Depending on the way of elucidating the phenomena, the Stern layer is also considered as the binding interfacial layer (BIL) [68] or inner region according to [69].</figcaption></figure>

In the diffuse layer (DL), the electrical potential ($φ$) obeys an exponential decay with respect to the distance starting from the outer Helmholtz plane (OHP, $z = 0^+$) (Figure 3b):

$$φ(z) = φ_{0+} \times e^{-κz} = φ_{OHP} \times e^{-\frac{z}{κ^{-1}}} \quad (1)$$

where $φ_{OHP}$ or $δ_{Stern}$ is the surface potential (mV) at the OHP (red dashed vertical line), $κ^{-1}$ is Debye length (Å), and $z$ is the distance from the electrochemical interface (Å). The Stern potential ($δ_{Stern}/OHP$) is the boundary potential that distinguishes the potential profile discrepancies between the Stern layer (linear reduction) and the diffuse layer (exponential reduction). It is approximately assumed to be equal to the zeta potential ($ζ$)—electrokinetic potential at the slipping or shear plane (SP) in colloidal dispersions. The SP is the con-
ceptual boundary within the DL of the EDL where the fluid begins to flow independently from the stationary charged surface (green dashed vertical line in Figure 3). There is an infinitesimal disparity between these two values due to the hydration shell formation. It is also noteworthy to mention that the potential/point of zero charge (PZC or particularly potential of zero total charge (PZTC) where the actual surface potential at $z = 0$ equals 0 ($\varphi_0 = 0$)) in electrochemical interfaces and the isoelectric point (IEP) in colloidal sciences are also not unnecessarily tantamount to each other [70]. By definition, the IEP is the concentration of potential-determining ions (counterions) such as $pH_{(IEP)}$ where $\zeta$ potential is at 0 mV, inducing the electrokinetic instability of colloidal systems (e.g., rapid coagulation or flocculation of metal particles) while the surface charge at the PZC is zero (no excess charge prevailing at the electrode) (Figure 3b). The sign of $\zeta$ potential is defined as the difference between the pH at the IEP and the measured pH of the solution. This means that there are still some charged species (specifically adsorbed, partially or non-hydrated ions) at the Stern layer when reaching IEP (non-zero surface charge) so IEP and PZC are not interchangeable. The definitions of PZC and the importance of PZC determination are considered in greater detail in Section 3.4. In summary, surface potential directly refers to the solid-liquid interface, particularly the electrode-electrolyte interface whilst $\zeta$ potential is ascribed to the hydrodynamic interface.

Furthermore, whether or not the surface potential ($\varphi_0$) is determined by the experiment is still debatable and ambiguous. Technically, amongst other types of electrical potentials (internal Galvani potential $\varphi$ and external Volta potential $\psi$), the surface potential $\varphi$ (also known as surface potential jump or surface electrical potential) is estimated when a charged species penetrates into the internal bulk phase of metal M from a distance of approximately 1 µm with respect to the interface (Figure 4a,b). For the treatment of the EDL, the defined surface potential simply covers all regions of the EDL (the Stern and diffuse) and can be related to the potential drop in the Stern layer and the potential from the diffuse layer by $\varphi_0 = \varphi_{\text{Stern}}^{\text{drop}} + \varphi_{\text{OHP}}$ [71]. In other words, the surface potential $\varphi_0$ can be trivially expressed as the electrical potential difference between the electrode surface and the bulk ($\psi_\infty = 0$), and it does not become a paradox with the definition of internal Galvani potential $\varphi$ due to no metal bulk intervention. Nonetheless, the assumption of an infinitely thin or sharp surface (continuum model) and the equivocality of bulk position do not effectuate a clear-cut experimental determination of $\varphi_0$ [12]. Only external potential $\psi$, specifically $\varphi_{\text{OHP}}$ for the EDL, can be experimentally accessible from the measurable potential difference in a common phase condition.

<figure><img src="image_11.png" /><figcaption>**Figure 4.** Schematic illustrations of the discrepancies among (a) surface potential ($\varphi$), outer/external potential ($\psi$), and inner/internal potential ($\varphi$) of metal M, as well as (b) the Volta ($\Delta\psi$) and Galvani ($\Delta\varphi$) potential differences between two metals $M_1$ and $M_2$. This figure is adapted from the reference [72], Copyright © 2022 The Electrochemical Society of Japan.</figcaption></figure>
About a decade later, Debye and Hückel (1923) treated the non-linearized Poisson-Boltzmann equation for calculating the potential and ion distribution around spherical or curvature-like surfaces [73]. From solving the linearized Poisson-Boltzmann equation, the decay length or “Debye length”, which is a critical parameter to characterize the thickness of the diffuse layer, is extracted (Figure 3a,b).

$$ \lambda_D = \kappa^{-1} = \left( \frac{\varepsilon\varepsilon_0 k_B T}{e^2 \sum_i^N C_i^0 \varkappa_i^2} \right)^{1/2} = \left( \frac{\varepsilon\varepsilon_0 k_B T}{2e^2 I} \right)^{1/2} \quad (2) $$

where $\lambda_D = \kappa^{-1}$ is Debye length, $k_B$ is Boltzmann constant, $T$ is the absolute temperature (in Kelvin), $\varepsilon$ is the elementary charge, $C_i^0$ is the bulk concentration of ion $i$ which is with the corresponding charge $\varkappa_i$, $N$ is the total number of charged species, and $I$ is the ionic strength of ionic solution ($I = \frac{1}{2} \sum_i^N C_i^0 \varkappa_i^2$). From (2), it is evident that $\lambda_D$ and $I$ are inversely proportional to each other: the Debye length decreases when ionic strength increases and vice versa. For a dilute aqueous solution ($\varepsilon = \kappa \approx 78.49$) containing only $\varkappa: \varkappa$ electrolyte ($M^{\varkappa} + X^{\varkappa}$) at 25 °C, $\lambda_D = [(3.29 \times 10^7) \varkappa C]^{-1/2}$ (cm) where C is the bulk concentration of electrolyte MX (in M) [3].

The Poisson-Boltzmann theory is a continuum mean-field approach based on three main assumptions in the treatment of the diffuse electrical double layer: (1) all ions are distinct, individual point charges and solely interact with each other through electrostatic forces, (2) solvent, specifically water, is a continuous medium with a constant dielectric constant $\kappa$, and (3) ions in solution possess a continuous charge distribution near a planar solid surface and the interplate spacing $d$ follows a spatial average distance from the electrode surface (Boltzmann distribution) [3,14]. The Gouy-Chapman model described sufficiently and relatively well the ions' distribution in the EDL for many applications, especially in the aqueous system of low monovalent electrolyte concentrations (<0.2M) and low potentials (<50-80 mV) [14]. This could be merely attributed to the prevalence of Coulombic interactions in most systems and the neglect of major local structural considerations. On the other hand, the model is invalid to predict the value of $C_d$ in high electrolyte concentration systems under high potentials compared to the point where charges of surface are neutralized (potential of zero charge, PZC). The rationale for the imperfections could be ascribed from Poisson-Boltzmann theory assumptions per se by disregards of (1) finiteness of ions' size and their non-Coulombic interactions (hydration shell, hydrogen bonding), (2) the encumberment of the electric field on water molecules at the interface and counterions' effect to $\kappa$ value of water, (3) the nature of ions and their heterogeneous surface charges, and (4) the impracticality of an ideal planar surface [14].

To address the limitations of the Gouy-Chapman model, Stern (1924) considered the finite property of counterions' size and hydration effect by combining the ideas of two former models [74]. The Stern model (or Gouy-Chapman-Stern (GCS) model) modified double layers into two distinctive layers: (1) the inner Stern layer, or Helmholtz layer, and (2) the outer Gouy-Chapman layer, or diffuse layer (Figure 3a). The Stern layer is an adsorbed layer of possible water molecules at the interface and immobile hydrated counterions detached from the electrode surface at a defined distance ($d_{Stern}$). The electric field interferes with the static dipole moment of polar water molecules, resulting in a thermodynamically favorable orientation and organization at the interfacial region. The solvation process of ions by surrounding water molecules establishes hydration shells of ions that keep them in a finite proximity to the surface. Thus, $d_{Stern}$ is the “plane of closest approach” estimated by the distance from the electrochemical interface to the core of hydration shells, which is marked as the outer Helmholtz plane (OHP) (red dashed vertical line in Figure 3a). This plane is the border separating the Stern layer from the diffuse layer. On the contrary, solvated ions (counterions and coions) in the diffuse layer are mobile in traveling in a Poisson-Boltzmann solution. This layer is characterized by the above-mentioned Debye length ($\lambda_D$) from OHP to the bulk solution. Furthermore, the combination of the Stern layer and the Gouy-Chapman diffuse layer resembles two
capacitor-like structures in series, so the total differential capacitance ($C_{GCS}$) of the GCS model is calculated as $C_{GCS}^{-1} = C_{OHP}^{-1} + C_{DL}^{-1}$ where $C_{OHP}$, $C_{DL}$ are the capacitances of the Stern and diffuse layers, respectively (Figure 3b). If the electrochemical interface is under the conditions of larger polarizations $\varphi_{applied} \gg \varphi_{PZC}$ and high electrolyte concentration in the aqueous solution, counter ions incline to dwell stably at OHP close to the electrode surface, which is alike to the Helmholtz model.

Later on, Grahame (1947) introduced the adsorption phenomena of specifically adsorbed species and non-specifically adsorbed solvated ions to the GCS model, which was constructed via long-range Coulombic forces and overlooked the chemical identities of counterions [75]. Grahame defined an inner plane in the Stern layer (inner Helmholtz plane, IHP) that some non-hydrated coions, partially hydrated counterions, and neutral molecules act as adsorbates to tightly attach to the electrochemical interface via peculiar short-range interactions (orange dashed vertical line in Figure 3). That determines the two sub-layers in the Stern layer: IHP consists of "specifically adsorbed" species while OHP is the plane of "non-specifically adsorbed" counterions' residence (Figure 3a). The organization of species at IHP was totally dependent upon the applied potentials, electrolyte's nature and concentration, and electrode characteristics. Furthermore, Bockris, Devanathan, and Müller (1963) sharpened the GCS model by designating the variation of water solvent's relative permittivity [76]. To be more specific, the rotation intactness of water's "effective" dipole moment from their collective alignment reduces strongly from IHP to OHP until the diffuse layer (bulk-like water is free to rotate with more or less no alignment) despite retaining the dipole moment of individual water molecules with ca. 1.85 D (Figure 3a). Within IHP, a packed monolayer of water under the influence of a strong electric field leads to its dielectric saturation, while water in hydration shells has a more randomized orientation compared to IHP but is still aligned. The dielectric strength of water, then, decreases when going further into the interface. Figure 3 demonstrates the holistic picture of the electrical double layer model. There are numerous review papers discussing the EDL elsewhere [77,78], which readers can refer to and look into in detail.

All in all, the GCS model prevailingly and widely succeeds in disentangling the EDL in dilute aqueous electrochemistry. It does not, however, suffice to explain the metal/liquid interface of non-aqueous electrolyte (the ionic liquid), and other driving forces, especially strong Coulombic interactions, should be taken into account [79].

### 3. Sum-Frequency Generation Spectroscopy at Electrochemical Interfaces

#### 3.1. Fundamentals of Sum-Frequency Generation Spectroscopy

From the optical spectroscopic point of view, the polarization of materials $P(\omega)$ is defined as:

$$P(\omega) = \varepsilon_0\chi^{(1)}E(\omega) + \varepsilon_0\chi^{(2)}E(\omega)^2 + \varepsilon_0\chi^{(3)}E(\omega)^3 + \dots \quad (3)$$

where $E(\omega)$ is the electric field, $\chi^{(n)}$ is the electric susceptibility of the $n^{th}$ order. In linear first-ordered optical processes such as refraction, IR/Vis absorption and emission, diffusion, and extinction employed in the study of $\chi^{(1)}$ properties of materials, their polarization is the first term ($P(\omega) = \varepsilon_0\chi^{(1)}E(\omega)$). These are one-photon spectroscopies with no frequency (color/energy) conversion. Nonetheless, the polarization of non-linear processes (normally second and third order) also contains latter terms. These multi-photon spectroscopies occur within a spectral range going from the IR to the Vis wavelengths, requiring the use of laser sources for the generation of non-linear optical processes. While third harmonic generation (THG) and Raman processes (four-photon mixing), fluorescence, optical Kerr effect, and sum-frequency generation (SFG) under a static field are third order processes, second harmonic generation (SHG) and sum/difference-frequency generation (SFG/DFG) spectroscopies are three-photon mixed second-order optical processes with a third-rank tensor $\chi^{(2)}$ (Figure 5). To investigate the optical and electronic characteristics of materials at interface and bulk, non-linear optical spectroscopies up to $\chi^{(3)}$ are efficient enough to analyze in practice.
Regarding the prerequisite condition for the occurrence of a second-order non-linear optical process, it requires the non-centrosymmetric materials to exhibit a non-zero susceptibility ($\chi^{(2)} \neq 0$) under the electric dipole approximation. For instance, susceptibility is not null at (1) anisotropic crystals, (2) chiral entities (stereoisomers, enantiomers) [80,81], or (3) at the symmetry-breaking interface of two dielectric media (a centrosymmetric crystal and an electrolyte solution), and (4) from electric-quadrupolar response of bulk materials. It is forbidden for centrosymmetric materials, such as bulk materials, due to the appearance of an inversion center (i) or a center of symmetry. From the principle of group theory, any molecules containing both symmetry elements (a $C_2$ axis through a $(\frac{360}{2} = 180)^0$ rotation angle and a mirror plane at right angles) under the symmetry operation of inversion (i) are described as being centrosymmetric [82,83]. The vanishing of $\chi^{(2)}$ at a centrosymmetry medium yields non-linear processes of even parity (second-order), becoming an ideal surface-sensitive optical technique to probe the molecular responses (electronic and/or vibrational information of materials) at electrochemical interfaces. While SHG is a prominent surface-specific second-order non-linear optical tool to study the electronic properties of molecular structures near surfaces, SFG is considered an *in situ* vibro-electronic spectroscopic probing tool from atomic to complex interfaces [84].

<figure><img src="image_12.png" /><figcaption>**Figure 5.** Molecular energy diagrams for linear (IR) and non-linear optical spectroscopies (Raman, CARS/CSRS, SFG/DFG and SHG). (g: ground state, v: vibrational state, e: virtual electronic states ($e_1$ and $e_2$); IR: infrared, CARS: coherent anti-Stokes Raman scattering, CSRS: coherent Stokes Raman scattering, SFG: sum-frequency generation, DFG: difference-frequency generation, SHG: second-harmonic generation; Vis: visible, NIR: near-infrared, S: Stokes, AS: anti-Stokes. This figure is inspired by reference [85], Copyright © 2019 MDPI.</figcaption></figure>

Sum-frequency generation (SFG) spectroscopy is a second-order nonlinear optical probe describing a conversion of two processes: an absorption of an infrared (IR) photon,
proceeded by an anti-Stokes (AS) Raman scattering of a visible (Vis) photon (or near IR 800 nm which historically was defined as visible in femtosecond SFG setups). Provided that the generated photon acquires $\omega_{AS} = \omega_{Vis} + \omega_{IR}$, incident laser beams, a sum-frequency photon is detected. Therefore, to efficiently generate an SFG photon from combining $10^6$ Vis photons and $10^6$ IR photons, it is a must for two intense laser beams to spatially and temporally overlap at the probed interface so that two conservation laws are met: $\omega_{SFG} = \omega_{Vis} + \omega_{IR}$ (energy) and $k_{SFG} = k_{Vis} + k_{IR}$ (momentum or phase matching condition) [85]. By convention, the energy conservation law is stated in frequency ($\nu$) but expressed in wavenumber ($\omega$ in cm$^{-1}$) in the practical sense. The frequency terms, henceforward, will literally mean the energy marked in cm$^{-1}$ in SFG spectra and other analyses. A detailed comparison between SFG and two individual constituent spectroscopies (IR and Raman) is represented in Table 1.

<table><caption>**Table 1.** Vibrational spectroscopies (IR absorption, Stokes Raman scattering, SFG) in comparison.</caption><thead><tr><th>Criteria</th><th>IR Absorption</th><th>Raman Scattering</th><th>SFG</th></tr></thead><tbody><tr><td>Order of susceptibility</td><td>χ<sup>(1)</sup>(ω<sub>IR</sub>)</td><td>χ<sup>(3)</sup>(ω<sub>Vis</sub>, -ω<sub>Vis</sub>, ω)</td><td>χ<sup>(2)</sup>(ω<sub>IR</sub>, ω<sub>Vis</sub>)</td></tr><tr><td>Selection rule</td><td>(∂μ/∂Q<sub>v</sub>)<sub>0</sub> ≠ 0</td><td>(∂α/∂Q<sub>v</sub>)<sub>0</sub> ≠ 0</td><td>(∂μ/∂Q<sub>v</sub>)<sub>0</sub> ⊗ (∂α/∂Q<sub>v</sub>)<sub>0</sub> ≠ 0</td></tr><tr><td>IR resonance</td><td>ω<sub>IR</sub>-resonant</td><td>non ω<sub>IR</sub>-resonant</td><td>ω<sub>IR</sub>-resonant</td></tr><tr><td>VIS resonance</td><td>non ω<sub>Vis</sub>-resonant</td><td>ω<sub>Vis</sub>-resonant<sup>1</sup></td><td>ω<sub>Vis</sub>-resonant<sup>2</sup></td></tr><tr><td>Coherence</td><td>coherent</td><td>incoherent</td><td>coherent</td></tr><tr><td>Optical configuration</td><td>directional</td><td>diffused</td><td>directional</td></tr><tr><td>Surface selectivity</td><td>non surface-specific</td><td>non surface-specific</td><td>intrinsically high</td></tr><tr><td>Detection sensitivity</td><td>High but not intrinsic</td><td>Low<sup>3</sup></td><td>High</td></tr><tr><td>Reference spectra<br>subtraction</td><td>Yes</td><td>Yes</td><td>No</td></tr></tbody></table>

At the molecular level, an SFG process can be active if and only if the molecular hyperpolarizability $\beta$ (non-linear second-order electric polarizability) is simultaneously Raman and Infrared active (selection rules). In other words, from the macroscopic view of the non-linear second-order susceptibility of a structured surface (a set of molecules at an interface), $\chi_{lmn}^{(2)}$ is always different from zero because of the symmetry breaking of the electronic properties at this specific location, so $\beta_{ijk} \neq 0$ at the microscopic point of view. Thus, there must be a change in both Raman polarizability $\alpha$ and IR dipole moment $\mu$ of the vibrational transitions of structured molecular systems during SFG spectroscopy at interfaces. While Two-Color SFG (2C-SFG) spectroscopy, where both IR and visible beams are tuned, can assess the vibro-electronic spectroscopic information of non-centrosymmetric interfaces, SFG can also operate in the mode of one-color tuning (either $\omega_{Vis}$ or $\omega_{IR}$) [86]. With a fixed visible wavelength ($\omega_{Vis}$ is constant) in the vibrational SFG without electronic specificity, $\chi_{lmn}^{(2)}$ is written as:

$$ \chi_{lmn}^{(2)} = N_s \sum_{ijk} \langle T_{ijk}^{lmn} \rangle \beta_{ijk} \neq 0 \quad (4) $$

where $N_s$ is the surface density of the adsorbed molecules, $T_{ijk}^{lmn}$ indicates the coordinate transformation from molecular framework to structured sample, and

$$ \beta_{ijk} = \sum_{v=1}^{n} \frac{1}{2\hbar\omega_v} \frac{\left(\frac{\partial\alpha_{ij}}{\partial Q_v}\right)_{Q_v=0} \left(\frac{\partial\mu_k}{\partial Q_v}\right)_{Q_v=0}}{\omega_{IR} - \omega_v + i\Gamma_v} \quad (5) $$

where $\alpha_{ij}$ is anti-Stokes Raman polarizability, $\mu_k$ is IR dipole moment, $Q_v$ is $v^{th}$ vibration normal coordinate, $\omega_{IR}$ is the incident IR frequency, $\omega_v$ is the resonant vibration frequency

<footnote n="1">¹ when $\omega_{pump} \equiv \omega_{electronic \ excited \ state}$, ² doubly resonant with respect to IR and Vis beams, ³ high for surface-enhanced Raman spectroscopy (SERS) or shell-isolated nanoparticle-enhanced Raman spectroscopy (SHINERS).</footnote>
of vth mode or the position of the vth peak (in cm⁻¹), and Γv is the damping coefficient of vth vibration mode or half width at half height (HWHH) of the vth peak (in cm⁻¹). When the excitation of IR wavelength or frequency (ωIR) coincides with the eigenfrequency ωv, the resonance of vibrational frequency occurs.

SFG is a versatile technique to study the fundamental characteristics of interfaces: electrochemical interface, nanostructured metal interfaces (plasmonic), and semiconductors (excitons) for the development of biosensors and electrocatalysts [87]. SFG is known as intrinsically surface-sensitive spectroscopy, which is almost the case for species adsorbed at interfaces [88]. In the case of functionalized nanoparticles (Au or functionalized quantum dots, CdTe) grafted with anchoring molecules on a solid substrate (metal, glass, prism...), the SFG signal is derived from grafted or functionalized molecules, substrate, and nanoparticle responses. However, inorganic components (e.g., substrate and nanoparticles) are generally non-resonant to IR vibrational frequencies of the examined range. Taking mercaptopropionic acid ligand-capped CdTe quantum dots (QDs) grafted on the glass substrate through (3-aminopropyl)triethoxysilane (APTES) molecules as an actual instance, it is a combined contribution of the inorganic components of the samples (glass slide and CdTe core) (Ae⁴⁰) and the remaining part from organic components (APTES or functionalized molecules on QDs) (Figure 6). As a result, the effective surface second-order non-linear susceptibility χ interface or χ eff of the interface is expressed as below.

$$ \chi_{\text{interface}}^{(2)} = \chi_{\text{substrate}}^{(2)} + \chi_{\text{adsorbate}}^{(2)} = \chi_{\text{non-resonant}}^{(2)} + \chi_{\text{molecules}}^{(2)} \quad (6) $$

with χ non-resonant = Ae⁴⁰ and χ molecules = Σn v =1 a v e⁴⁰ψ v (the sum of Lorentzian-shape functions), where A is the contribution of amplitude of the background, Φ is the phase of the background, v is the index of peaks (vibrational modes), a v is the amplitude of the vth peak, and ψ v is the phase of the vth peak, which is assumed to be zero for the sake of simplicity. Then, the SFG intensity is calculated as:

$$ I(\omega_{\text{SFG}}) \propto |\chi_{\text{interface}}^{(2)} : E_{(\omega_{\text{IR}})} E_{(\omega_{\text{Vis}})}|^2 \rightarrow I(\omega_{\text{SFG}}) \propto |\mathbf{P}_{(\omega_{\text{SFG}})}|^2 \quad (7) $$

$$ I(\omega_{\text{SFG}}) = \frac{8\pi^3 \omega_{\text{SFG}}^2 \sec^2 \theta_{\text{SFG}}}{c^3 n_{\text{air}}(\omega_{\text{SFG}}) n_{\text{air}}(\omega_{\text{IR}}) n_{\text{air}}(\omega_{\text{Vis}})} |\chi_{\text{interface}}^{(2)}|^2 I_{\text{IR}} I_{\text{Vis}} \quad (8) $$

where

$$ |\chi_{\text{interface}}^{(2)}|^2 = |\chi_{\text{non-resonant}}^{(2)}|^2 + |\chi_{\text{molecules}}^{(2)}|^2 + 2\cos(\arg\chi_{\text{molecules}}^{(2)} - \arg\chi_{\text{non-resonant}}^{(2)}) \quad (9) $$

$$ |\chi_{\text{interface}}^{(2)}|^2 = A^2 + \frac{a_v^2}{(\omega_{\text{IR}} - \omega_v)^2 + \Gamma_v^2} + \frac{2Aa_v}{[ (\omega_{\text{IR}} - \omega_v)^2 + \Gamma_v^2 ]^{1/2}} \underbrace{\cos \left( \psi_v - \Phi - 2\arctan \frac{\Gamma_v}{\omega_{\text{IR}} - \omega_v + [(\omega_{\text{IR}} - \omega_v)^2 + \Gamma_v^2]^{1/2}} \right)}_{B} \quad (10) $$

with IIR and IVis the intensities of the incident IR and visible laser beams, respectively. θSFG is the outgoing angle of incidence of the SFG beam travelling to the monochromator. c is the speed of light in vacuum, nair is the refractive index of the upper medium (ambient air) at frequency ω, and B is the value of the cosine function in Equation (10).
<figure><img src="image_13.png" /><figcaption>**Figure 6.** Sketch of sum-frequency generation (SFG) spectroscopy at a nanostructured interface sample: Glass substrate/grafted APTES + HOOC-functionalized quantum dots CdTe/ambient air. ~~~NH₃⁺ is the protonated form of APTES (EtO)₃Si-(CH₂)₃-NH₂ (3-aminopropyl)triethoxysilane and ~~~COO⁻ represents the carboxylate form of mercaptocarboxylic acids HS-(CH₂)ₙ-COOH (n ≤ 3). ◊ denotes the vibro-electronic dipolar coupling of the exciton (electron-hole pair) of QDs to the vibrational resonances of surrounding ligands. From geometry investigation, the optimized angles for Visible and Infrared photons are 55° and 65°, respectively. The polarization scheme is (S:SP) for the SFG, Vis, and IR beams, where the polarization plane of P(x,0,z) and S(0,y,0) is illustrated. Light can be polarized parallel (P polarization) or perpendicular (S polarization) to the plane of incidence (Oxz plane). This figure is inspired by references [87,89,90].</figcaption></figure>

As can be seen, the square norm of the effective second-order susceptibility of a single vibrational mode has the attendance of the non-resonant background, the IR vibrational resonance, and interference factor (phase shift between the substrate and the adsorbed molecules) contributions pertain to the first, second, and third term, respectively. Depending on whether it is a constructive or destructive resonance, the SFG spectrum shapes as a peak (B = +1), a dip (B = -1), or a Fano resonance (B is between -1 and +1) [84].

## 3.2. The Electric Field-Dependent Vibrational Stark Effect at Electrochemical Interfaces

The vibrational Stark effect is an induced energy-level shifting effect (vibrational frequency shifts) of a particular molecular vibrational mode of a molecule experiencing a perturbation of an external electric field [91–93]. An associated transition dipole moment change between the levels is also induced. However, this slight peak shift of a vibrational mode in vibrational Stark spectroscopy does not yield a spectral line shape change [94]. The vibrational responses under the influence of E (vibrational mode variations) were found to be equal to the sum of a linear vibrational dipole moment change Δμ and a quadratic vibrational polarizability change Δα (Equation (11)). The first term is named the linear Stark effect (first-order component) while the latter is referred to as the quadratic Stark effect (in second order) (Figure 7).

$$ \Delta\omega = \omega - \omega_0 = -\frac{1}{hc} \left( \Delta\mu \cdot E + \frac{1}{2} E \cdot \Delta\alpha \cdot E \right) \quad (11) $$

where h is the Planck's constant (6.626 × 10⁻³⁴ J·s), c is the speed of light in vacuum (~3 × 10⁸ m·s⁻¹), ω (ω₀) is the frequency of a molecular vibrational mode with (without) an external electric field, E is the amplitude of interfacial field strength, and Δμ and Δα are the differences in dipole moment (charge separation or charge transfer) and polar-
izability between the ground and excited vibrational states of a molecular vibrational mode, respectively.

<figure><img src="image_14.png" /><figcaption>**Figure 7.** Depiction of the first-order (linear) and second-order (quadratic) electric field-induced Stark effect. This figure is adapted from reference [94], Copyright © 2024 Springer Nature.</figcaption></figure>

Both of $\Delta\mu$ and $\Delta\alpha$ are entirely affected by the circumambient chemical environment of the molecules. Due to field-induced bond changes, the acquired values of $\Delta\mu$ and $\Delta\alpha$ are not identical to the expected values [95]. Thus, these notations are not precisely accurate in the technical sense but acceptable for simplicity. It is worth mentioning that $\Delta\mu$ is also termed as the Stark tuning rate, which signifies the environmentally induced sensitivity of a vibrational frequency to local fields [96]. The amplitude of the Stark tuning rate can be determined experimentally or computationally. This electric-field-induced Stark effect is an analogous principle to the previously renowned magnetic-field-induced Zeeman effect with the splitting of spectral lines of a sample.

In addition, another highlight that should be noted here is that the local electrostatic fields can spring not only from externally applied electric fields from the electrode surfaces but also from solvation field (the Onsager reaction field model [97]), such as solute-solvent interactions, which is also a factor causing the vibrational shift. Therefore, the local field imposed on the molecule is greater than the average interfacial electric field ($E_{external} = -\frac{\partial\varphi}{\partial s}$ where $\partial\varphi, \partial s$ are potential changes and electrode spacing in that direction, respectively), and the measured shifts deviate from the calculated ones. Thus, an introduction of a local field correction factor ($f_{LF}$)—an empirical scaling factor to Equation (11)—necessitates calibrating the bias, and the effective local electric field is expressed as follows: $E = f_{LF}E_{external}$, then (11) becomes:

$$ \Delta\omega = -\frac{1}{hc} \left( \Delta\mu \cdot f_{LF} E_{external} + \frac{1}{2} f_{LF} E_{external} \cdot \Delta\alpha \cdot f_{LF} E_{external} \right) \quad (12) $$

This denoted $f_{LF}$ correction factor is estimated from the data fitting procedure of experimented vibrational spectra under the umbrella of the Stark effect (normally between 1.1 and 1.3) [95,98]. Meanwhile, there are other polarization effects devoted to the frequency shift $\Delta\omega$ of a particular vibrational mode, such as dipole-dipole coupling, hydrogen bonding, ionic strength effect, etc. As water is a common polar solvent with strong associated hydrogen bonds between moieties containing high-electronegativity atoms (F, O, N...) in solute molecules and hydrogen atoms in water molecules, these interactions are likely to alter the chemical nature and electronic structure of the vibrational mode leading to the shifting of $\omega$. Furthermore, it is known that the internal solvation field is $E_{external}$-driven field ($f_{LF}$ is not constant) when imposing an electric field bias. Within the scope of this review, other contributing parameters to $\Delta\omega$ variation stated above are negligible by keeping
ing them constant, so the primary variable is the influence of the interfacial electric field $E_{\text{external}}$ produced from the electrode surface on the vibrational probe.

It is stated that when the permanent dipole moment of the molecule is nonzero, the second-order Stark effect contribution is negligible and generally not taken into account [99]. To be more specific, the strength of the electric field is relatively weak (smaller than 100 MV·cm⁻¹), the second-order contribution of Δα (quadratic term) is insignificant, and Δω becomes directly proportional to the magnitude of E via a linear relationship (Equation (13)) (Figure 7). This means that the linear Stark shift increases when a higher external electric field impinges on the electrode system.

$$ \Delta\omega \approx -\Delta\mu \cdot E_{\text{external}} \qquad (13) $$

In the electrochemical Stark shift experiments, the interfacial electric field is dependent on two variables, which are applied potential and the ionic strength of the solution $E = f(\varphi, I)$. If I is kept constant, $E_{\text{external}} = E(\varphi)$ without letting any current flow through the system, and it was found that the vibrational frequency of the adsorbate molecule varies (Δω) as a function of electrode potential (φ) via a linear dependence [100,101].

$$ \frac{d\omega}{d\varphi} = -\Delta\mu \times \frac{dE}{d\varphi} \qquad (14) $$

Knowing the values of Δμ and the Stark tuning slope ($\frac{d\omega}{d\varphi}$), the absolute $E(\varphi)$ can be determined through a linear correlation with φ described in Equation (16).

$$ \frac{dE}{d\varphi} = -\frac{1}{\Delta\mu} \frac{d\omega}{d\varphi} \qquad (15) $$

$$ E(\varphi) = -\frac{1}{\Delta\mu} \frac{d\omega}{d\varphi}(\varphi - \varphi_{\text{PZC}}) \qquad (16) $$

where $\varphi_{\text{PZC}}$ is the potential of zero charge.

### 3.3. Potential-Dependent Sum-Frequency Generation (SFG) Spectroscopy

When studying the SFG spectroscopy of an electrochemical interface, a charged solid/liquid interface in general, a quadrupole contribution of bulk centrosymmetric component under the influence of a static electric DC field ($E_{\text{DC}}$) through a surface non-specific $\chi^{(3)}$ process is also recognized in the generation of SFG resonances rather than the symmetry-breaking interface contribution itself. In the early 1990s, Eisenthal et al. proved that the signal of second harmonic generation (SHG) depends on the $\chi^{(3)}$-bulk component with a significant contribution [102,103]. As discussed previously in Section 2 about the EDL models of an electrochemical interface, the interface contribution to $\chi_{\text{S,eff}}^{(2)}$ can be regarded from the Stern layer ($\chi_{\text{Stern}}^{(2)}$) with the interface-specific hydrogen-bonding network of water molecules [68]. On the other hand, the bulk quadrupole contribution is referred to as bulk-like water molecules in the diffuse layer (DL) under the effect of a static electrical field. The effective surface second-order non-linear optical susceptibility $\chi_{\text{S,eff}}^{(2)}$ therefore, is expressed via the relation below:

$$ \chi_{\text{S,eff}}^{(2)} = \chi_{\text{Stern}}^{(2)} + \int_{\text{OHP}}^{\infty} \left[ \chi_{\text{Bulk}}^{(2)} + \chi_{\text{Bulk}}^{(3)}(z) \cdot E_{\text{DC}}(z) \right] e^{i\Delta k_z z} dz \qquad (17) $$

where $\chi_{\text{Bulk}}^{(2)}$ and $\chi_{\text{Bulk}}^{(3)}(z)$ designate the second-order electric-quadrupole bulk non-linear susceptibility and the third-order bulk non-linear susceptibility of the aqueous solution, respectively, $E_{\text{DC}}(z)$ is the z-dependent static electric field, $\infty$ represents the bulk solution and $\Delta k_z = |k_{\text{Vis,z}} + k_{\text{IR,z}} - k_{\text{SFG,z}}| = k_{\text{SFG,z}} + k_{\text{Vis,z}} + k_{\text{IR,z}}$ represents the phase mismatch of reflected SFG light along the surface normal (with Oz direction) (Figure 8).
<figure><img src="image_15.png" /><figcaption>**Figure 8.** Illustration of an SFG reflection experiment at the air/water interface. Arrows $k_{Vis}$, $k_{IR}$, and $k_{SFG}$ refer to the visible, IR, and SFG beams that can interact at various z-planes. $\theta_{Vis}$, $\theta_{IR}$, and $\theta_{SFG}$ are the incoming angles of incidence for the visible and IR light, and the angle of reflection for the SFG signal, respectively. The dashed vertical arrows denote their projection along the z-axis, and the relevant phase difference. Dotted horizontal lines represent the probing depth with the Stern layer (red) and diffuse layer (black). The charged surface can be from a monolayer of charged molecules (surfactants or fatty acids). This figure is adapted with permission from reference [104], Copyright © 2016 American Chemical Society.</figcaption></figure>

It has been estimated that $\chi_{Bulk}^{(2)}$ is insignificant in (S:SP) polarization configuration for SFG of water [68], thus we have the $\chi_{S,eff}^{(2)}$ or $\chi_{interface}^{(2)}$ coefficient as a combination of two surface second-order non-linear susceptibilities [105]:

$$\chi_{S,eff}^{(2)} = \chi_{Stern}^{(2)} + \int_{OHP}^{\infty} \chi_{Bulk}^{(3)}(z) \cdot E_{DC}(z) e^{i\Delta k_z z} dz = \chi_{Stern}^{(2)} + \chi_{DL}^{(2)} \quad (18)$$

by assuming that: (1) $\chi_{Bulk}^{(3)}$ is more predominantly from mean-field-induced reorientation of bulk water molecules rather than field-induced alignment of hydrogen bonds and electron polarizabilities of molecules [68], and (2) $\chi_{Bulk}^{(3)}(z)$ is approximated as the third-order non-linear susceptibility of bulk water ($\chi_{Bulk}^{(3)}(z) = \chi_{Bulk}^{(3)}$) [106]. The second assumption has not been proved yet. Given these approximations, we replace $E_{DC}(z) = -\frac{d\varphi(z)}{dz}$ and $\varphi_{OHP} = \delta_{Stern} = \int_{OHP}^{\infty} E_{DC}(z) dz = \int_{OHP}^{\infty} \frac{-d\varphi(z)}{dz} dz = -\varphi_{\infty} + \varphi_{OHP}$ into Equation (18) (with the assumption of $\varphi_{\infty} = 0$ at a bulk solution), then it turns out $\chi_{DL}^{(2)}$ is calculated as

$$\chi_{DL}^{(2)} = \chi_{Bulk}^{(3)} \int_{OHP}^{\infty} \frac{-d\varphi(z)}{dz} e^{i\Delta k_z z} dz = \chi_{Bulk}^{(3)} \left[ -\varphi(z) e^{i\Delta k_z z} \Big|_{OHP}^{\infty} + \int_{OHP}^{\infty} -\varphi(z) \times i\Delta k_z \times e^{i\Delta k_z z} dz \right] \quad (19)$$

$$\chi_{DL}^{(2)} = \chi_{Bulk}^{(3)} \left[ \varphi_{OHP} + i\Delta k_z \int_{OHP}^{\infty} -\varphi(z) \times e^{i\Delta k_z z} dz \right] \quad (20)$$

Furthermore, as discussed previously in Equation (1), $\varphi(z) = \varphi_{OHP} \times e^{-\kappa z}$ at the diffuse double layer ($\kappa$ is the inverse of the Debye screening length and the potential is decayed to 2% of its maximum value at $z = 4\kappa^{-1} \approx 36$ nm corresponding to $\approx 120$ layers of water [104]), then we have:

$$\chi_{DL}^{(2)} = \chi_{Bulk}^{(3)} \left[ \varphi_{OHP} - \varphi_{OHP} \times i\Delta k_z \int_{OHP}^{\infty} e^{-\kappa z} \times e^{i\Delta k_z z} dz \right] \quad (21)$$

$$\chi_{DL}^{(2)} = \chi_{Bulk}^{(3)} \left[ \varphi_{OHP} - \varphi_{OHP} \times i\Delta k_z \int_{OHP}^{\infty} e^{(-\kappa + i\Delta k_z)z} dz \right] \quad (22)$$

$$\chi_{DL}^{(2)} = \chi_{Bulk}^{(3)} \times \varphi_{OHP} \left[ 1 - \frac{i\Delta k_z}{-\kappa + i\Delta k_z} e^{(-\kappa + i\Delta k_z)z} \Big|_{OHP}^{\infty} \right] = \chi_{Bulk}^{(3)} \times \varphi_{OHP} \left( 1 + \frac{i\Delta k_z}{\kappa - i\Delta k_z} \right) \quad (23)$$
Finally,

$$ \chi_{\text{DL}}^{(2)} = \left( \frac{\kappa}{\kappa - i\Delta k_z} \right) \chi_{\text{Bulk}}^{(3)} \times \varphi_{\text{OHP}} \quad (24) $$

Therefore, the intensity of SFG signal is directly proportional to the square of the surface potential from diffuse layer to the bulk via the equation below.

$$ I(\omega_{\text{SFG}}) \propto |\chi_{\text{S,eff}}^{(2)}|^2 I_{\text{IR}} I_{\text{Vis}} \propto |\chi_{\text{Stern}}^{(2)} + \left(\frac{\kappa}{\kappa - i\Delta k_z}\right) \chi_{\text{Bulk}}^{(3)} \times \varphi_{\text{OHP}}|^2 I_{\text{IR}} I_{\text{Vis}} \quad (25) $$

Applying the Euler formula, $e^{ix} = \cos(x) + i\sin(x)$, to Equation (25), we have:

$$ I(\omega_{\text{SFG}}) \propto \left| \chi_{\text{Stern}}^{(2)} + \frac{\kappa}{\sqrt{\kappa^2 + (\Delta k_z)^2}} e^{i \arctan(\frac{\Delta k_z}{\kappa})} \times \chi_{\text{Bulk}}^{(3)} \times \varphi_{\text{OHP}} \right|^2 \quad (26) $$

Fundamentally, to acquire an optimum reflected SFG signal, the polarization triplet (SFG:Vis IR) (where the configuration is in order of increasing wavelength, Figure 6) must be selected so that it can leverage and maximize the substrate reflectivity [84]. The influence of surface reflectivity is mathematically expressed by the Fresnel coefficients (R) for reflection. R naturally depends on the refractive indices of two media at the interface n and the incident angles θ (Figure 8). Aside from $\chi_{\text{Stern}}^{(2)}$ and $\chi_{\text{Bulk}}^{(3)}$ tensors, the R values should also be considered in calculating $I(\omega_{\text{SFG}})$ in principle (Equation (26)), but they are neglected here at solid/liquid electrochemical interfaces to avoid further complications. Due to the Oz-depth dependence of the real surface electrostatic field (potential) $E_{\text{DC}}(z)$ and complex phase matching factor $e^{i\Delta k_z z}$, the total $\chi^{(3)}$ term is defined as

$$ \left( \frac{\kappa}{\kappa - i\Delta k_z} \right) \chi_{\text{Bulk}}^{(3)} = C_F \times \chi_{\text{Bulk}}^{(3)} = \chi_{\text{real}}^{(3)} + i\chi_{\text{imaginary}}^{(3)} \quad (27) $$

where $\kappa$ and $\Delta k_z$ are denoted as the inverse of the Debye screening length and the coherence length of SFG process, respectively; $C_F \equiv \frac{\kappa}{\kappa - i\Delta k_z}$ has been called as the correction factor, $\chi_{\text{real}}^{(3)} = \frac{\kappa^2}{\kappa^2 + (\Delta k_z)^2} \chi_{\text{Bulk}}^{(3)}$, $\chi_{\text{imaginary}}^{(3)} = \frac{\kappa\Delta k_z}{\kappa^2 + (\Delta k_z)^2} \chi_{\text{Bulk}}^{(3)}$ [107].

Depending on the relative values of $\kappa$ and $\Delta k_z$, one can separate three cases:

(i) If $\kappa \gg \Delta k_z$, meaning that the coherence length (usually between 20 and 50 nm depending on the optical configurations) of the SFG process is much bigger than the effective thickness of the diffuse layer. In other words, the Debye length is much smaller than the coherence length. This is the case for very high electrolyte concentration ($I > 10^{-1}$ M) and $\chi_{\text{real}}^{(3)}$ is predominant ($\chi_{\text{real}}^{(3)} \approx \chi_{\text{Bulk}}^{(3)}$ and $\chi_{\text{imaginary}}^{(3)} \approx \frac{\Delta k_z}{\kappa} \chi_{\text{Bulk}}^{(3)}$). This leads to the exponential phase matching term close to a unity $\int_{\text{OHP}}^{\infty} e^{i\Delta k_z z} dz \approx 1$, then

$$ \chi_{\text{S,eff}}^{(2)} \approx \chi_{\text{Stern}}^{(2)} + \chi_{\text{Bulk}}^{(3)} \int_{\text{OHP}}^{\infty} E_{\text{DC}}(z) dz \approx \chi_{\text{Stern}}^{(2)} + \chi_{\text{Bulk}}^{(3)} \times \varphi_{\text{OHP}} \quad (28) $$

(ii) When $\kappa \ll \Delta k_z$ ($\pi\Delta k_z^{-1} \ll 4\kappa^{-1}$), the Debye length is bigger than the coherence length thick, which corresponds to very low electrolyte concentration ($I < 10^{-4}$ M) and the significant term is thus $\chi_{\text{imaginary}}^{(3)}$ with small value since $\chi_{\text{real}}^{(3)} \approx 0$ and $\chi_{\text{imaginary}}^{(3)} \approx \frac{\kappa}{\Delta k_z} \chi_{\text{Bulk}}^{(3)}$. This complete destructive interference results in the sole dependence of SFG intensity on $\chi_{\text{Stern}}^{(2)}$ contribution [104].

(iii) Otherwise, the coherence length $\Delta k_z^{-1}$ is comparable to the Debye screening length $\kappa^{-1}$ ($4\kappa^{-1} \approx \pi\Delta k_z^{-1}$ when $I \approx 10^{-3}-10^{-4}$ M), so the total $\chi^{(3)}$ term remains as a complex value with both contributions from the real and imaginary terms.
To sum up, the SFG resonances generation in the aqueous solution stems from two particular regions: (1) hydrogen bonding of water molecules and other noncovalent interactions (van der Waals and electrostatic forces) within the electrochemical interface (the Stern layer) and (2) reoriented/aligned and polarized water molecules perturbed by a surface static electric field $E_{DC}$ (diffuse layer).

### 3.4. Some Controversial Issues Using the Definition of Surface Potential in the SFG Measurements

Due to the disunity of the surface/interface potential definition, it leads to the misnomer of $\varphi_0$. As illustrated earlier in reference [102,103], the interface potential is written in the term of $\varphi_0$ which actually refers to the potential at the OHP or the Stern potential (Gouy-Chapman-Stern model) (Figure 3a,b). Therefore, to be more precise, $\varphi_0$ denotes the interfacial or “surface” potential estimated between the diffuse layer and the bulk ($\varphi_{OHP}$). It is visually located at the specific location $0^+$ referred in Figure 3 (red dashed vertical line) and Figure 8 (red dashed horizontal line). This so-called “surface” potential is not synonymous with the defined $\varphi_0$ potential standardized from the electrode surface (Figure 4), and they are actually correlated via this formula:

$$ \varphi_0 = \varphi_{0 \to 0^+} + \varphi_{0^+ \to \infty} = \varphi_{\text{Stern}}^{\text{drop}} + \varphi_{\text{OHP}} = \varphi_{\text{Stern}}^{\text{drop}} + \delta_{\text{Stern}} \quad (29) $$

where $\varphi_{\text{Stern}}^{\text{drop}} = \frac{\sigma}{C_{OHP}} = \frac{\sigma \times d_{\text{Stern}}}{\varepsilon \varepsilon_0}$ ($\sigma$ is the surface charge density). All of the “surface” potential terms or potential with a subscript of 0 appeared in the references [68,104,106–114] refer to $\varphi_{OHP}$. In summary, when undergoing the influence of a static electric field, the bulk contribution to $\chi_{S,eff}^{(2)}$ depends on ($\chi_{\text{Bulk}}^{(3)} \cdot \varphi_{OHP}$) where the surface potential is the Stern potential. The misnomer of using unspecified surface potential has misled some research [115,116] about $\varphi_0$ and brought about the false usage. For instance, Tan et al. [115] investigated the thickness of interfacial water by time-resolved SFG with implementing Equations (26) and (29). However, the “surface potential” term expressed in the Equation (26) in their paper unfortunately corresponds to $\varphi_0$. Using variable-angle surface spectroscopy, Uddin et al. [116] recently reported on the water structure in the Stern layer, encompassing with the correct “Stern potential” in the third-order susceptibility in the diffuse layer (DL). Even so, they employed a silica deprotonation model to determine the surface potential ($\varphi_0$), which should instead have denoted the Stern potential under the theory of the EDL [3]. Even in the review paper [12] mentioning the experimental methods to determine surface potential $\varphi_0$, it would be erroneous to state that SFG can extract the real $\varphi_0$ surface potential under the auspices of the GCS model.

To estimate the value of $\varphi_{OHP}$, there are two approaches to do so: (1) the approximation approach and (2) the absolute approach. Approach (1) is based on the assumption that the Stern potential can be approximately equal to the measurable potential or potential difference. As discussed earlier in Section 2, $\zeta$ potential from the electrokinetic measurement [117,118] is frequently more or less equivalent to $\delta_{\text{Stern}}$ ($\varphi_{OHP} = \delta_{\text{Stern}} \approx \zeta$) so $\varphi_0 \approx \varphi_{\text{Stern}}^{\text{drop}} + \zeta$ (purple and black dashed horizontal line in Figure 3b). In addition, from Equation (16) in the vibrational Stark effect shown in Section 3.2 and Equation (28) in the case of $\kappa \gg \Delta k_z$, it offers another approximation strategy to determine $\varphi_{OHP}$ via the relation below.

$$ \varphi_{\text{OHP}} \approx \int_{\text{OHP}}^{\text{Bulk}} E_{\text{DC}}(z) dz = a(\varphi - \varphi_{\text{PZC}}) \quad (30) $$

where $a$ is a constant, $\varphi$ is the applied potential, $\varphi_{\text{PZC}}$ is the potential at the PZC. In principle, if $\varphi - \varphi_{\text{PZC}} \gg 0$ (high electric fields), a rigid and highly oriented water adlayer disposes at the electrochemical interface, which kinetically hampers the charge transfer. If $\varphi - \varphi_{\text{PZC}} \approx 0$ (close to the PZC, low electric fields), the dipoles of water molecules have an entropically higher degree of freedom. At the PZC ($\varphi - \varphi_{\text{PZC}} = 0$), the disorder of water molecules reaches the highest (quantitatively ascends to the maximum entropy, $S = k_B \times \ln\Omega$, where $\Omega$ is the number of microstates). Some research has employed this formula to access the potential dependence study [119,120].
This estimation is pertained to the equivalence of the interfacial electric field strength as the potential drop across the interface (the difference between the actual applied electrode potential and the PZC) [120,121]. At this point, it is critical to emphasize that the PZC in this formula and henceforth in the following sections of this review paper refers to the potential of zero free charge (PZFC), not to the potential of zero total charge (PZTC). The conceptual disparity between them is the considered range of charge density ($\sigma$), principally in the attendance of specifically adsorbed species ($H_{ad}$ and $OH_{ad}$) at non-ideally polarized electrodes (Pt, Cu, Ag). While the PZFC displays the potential where only the truly free, electronic excess charge density on the electrode surface equals zero ($\sigma_{diffuse} = 0, \sigma_{total} = \sigma_{IHP} + \sigma_{diffuse} \neq 0, \varphi_{OHP} = 0$), the PZTC expresses the potential at which the sum of both surface charge and the charge portion localized in polar adsorption process dissipates ($\sigma_{diffuse} \neq 0, \sigma_{total} = \sigma_{IHP} + \sigma_{diffuse} = 0, \varphi_0 = 0$) [122,123]. This means that the PZFC does not comprise the additional contributions from adsorbed species (ions, dipoles, etc.) or surface phenomena to the total charge balance. Thus, the PZTC is typically larger than the PZFC. They become homogeneous (PZC = PZFC = PZTC) when no specific adsorption exists ($\sigma_{IHP} = 0$). It is discernible that the existence of a specific adlayer with/without charges maneuvers the electrode surface potential, leading to dissimilar values of the PZFC. For instance, the PZFC of absorbate-free Pt(111) surface and OH-covered Pt(111) surface are 0.26 V vs. standard hydrogen electrode (SHE) [124] and 0.84 V vs. reversible hydrogen electrode (RHE) [125], respectively. Hence, $\varphi_{PZC}$ is an essential quantity for gauging the strength of the interfacial electric field (the EDL field), and determining it is not always straightforward. To acquire the PZFC, it can be experimentally determined by applying several methods: (1) classical double-layer capacitance minimum method by electrochemical impedance spectroscopy (EIS) [126], (2) laser-induced temperature jump [127–129], and (3) electric field-induced second-harmonic generation (SHG) [120]. Meanwhile, the PZTC can be obtained using the following approaches: (1) CO charge displacement method [130,131], (2) immersion method [122], and (3) $N_2O$ reduction method [132].

On the other hand, the absolute approach (2) relies on solving the Poisson–Boltzmann equation in the diffuse layer of only a symmetrical electrolyte or $z:z$ electrolyte ($M^{z+}X^{z-}$) with the total bulk concentration of C (M) (Grahame equation).

$$ \varphi_{OHP} = \frac{2k_B T}{\kappa e} \sinh^{-1} \frac{\sigma}{(8k_B T \varepsilon \varepsilon_0 \times C)^{\frac{1}{2}}} \quad (31) $$

For a symmetrical single charge (1:1) electrolyte system where $C = I$, then $\varphi_{OHP} = \frac{2k_B T}{e} \sinh^{-1} \frac{\sigma}{(8k_B T \varepsilon \varepsilon_0 \times I)^{\frac{1}{2}}}$ [3,133,134]. In general, the surface potential $\varphi_{OHP}$ generated from the surface charge is directly proportional to the arcsin of the surface charge density $\sigma$ and inversely proportional to the ionic strength $I$ of the aqueous solution (b and c are two constants, $\sinh^{-1}$ is the inverse hyperbolic sine).

$$ \varphi_{OHP} \propto b \sinh^{-1} \frac{\sigma}{\sqrt{c \times I}} \quad (32) $$

### 3.5. Experimental Considerations on Spectroelectrochemical Cells Adapted to Sum-Frequency Generation Spectroscopy

#### 3.5.1. Sum-Frequency Generation Experimental Setups

In the $\omega_{IR}$-tuned vibrational SFG or 2C-SFG (both tunable IR and Vis sources), a tunable IR beam is generated in two ways: (1) two conversion stages (optical parameter generator/amplifier, OPG/OPA) or (2) a single stage (optical parametric oscillator, OPO). In general, OPG/OPA system is a single-pass pulse of IR beam at a given excitation repetition rate $f_{ex}$ (MHz), which stands out for its simplicity, flexibility, broad tunability, and robustness [135]. Meanwhile, OPO is a versatile device of $\omega$-tunable IR-Vis-UV radiation converting pump laser wave into signal and idler (lower frequency compared to signal)
waves through a cavity for reverberation and intensity amplification of the conversion
process. Despite the merits of OPG/OPA, its broad-linewidth property can lead to a low
signal-to-noise (S/N) ratio for detection due to the high gain of the signal-idler pairs associ-
ated with the process of OPG/OPA for the phase-matching requirement in comparison with
OPO. Furthermore, OPO can generate either a continuous-wave (CW) output or pulses of
nanosecond (10⁻⁹ s), picosecond (10⁻¹² s), and femtosecond (10⁻¹⁵ s) duration [136].

A conventional SFG setup is based on two short delivering laser pulse systems: Q-
switched nanosecond (ns)/locked-mode picosecond (ps) and ultrashort locked-mode fem-
tosecond (fs) produced from a flashlamp-pumped laser, for example, neodymium-doped
yttrium-aluminum garnet (Nd:Y₃Al₅O₁₂ or Nd³⁺:YAG) laser with emitted wavelength
of 1064 nm. The rationale for the two preferential pulsed laser systems is that SFG is a
three-wave-mixing process, so the detected signal is proportional to δt⁻¹ (δt is the laser
pulse width) [137,138]. In the SFG measurement of a ns/ps input pulse, the narrowband
scheme (narrow linewidth) is employed with a spectral resolution of a few cm⁻¹ in terms of
IR bandwidth (typically < 1 cm⁻¹ for ns systems, 1–20 cm⁻¹ for ps systems). To eliminate
efficiently the reflected input beam (normally Vis light from the wavelength of 532 nm,
SHG from Nd:YAG), spatial and spectral filters and a monochromator are utilized during
the scan of IR vibrational resonances of the molecule of interest (Figure 9a). However, the
IR ps-scanning with a single channel and acquisition time of an SFG spectrum recording
is time-consuming in practice. Thus, the design of a broadband scheme (fs-SFG) for IR
laser first proposed by Richter et al. resolved the frequency tuning issue by operating
in a high-power fs pulsed laser system (Ti:Al₂O₃-sapphire) with a high repetition rate
of 1 kHz [139]. This IR broadband scheme covering a wide range of ωIR (multi-channel)
increases the bandwidth to more than 100 cm⁻¹ in an ultrashort pulse duration of 100 fs
without the need of IR scanning. The acquired non-linear SFG signal is self-dispersive in a
spectrograph, then detected by a charge-coupled device (CCD) camera, which is suitable
for sub-monolayer detection (Figure 9b). In general, the conventional schemes are based
on the homodyne detection. Although multiplex broadband SFG (BB-SFG) ameliorates
the single-channel narrowband SFG (NB-SFG) by offering a shorter acquisition time, they
provide only the mod square of second-order non-linear susceptibility, i.e., |χ<sup>(2)</sup><sub>interface</sub>|², not
the complex quantity of χ<sup>(2)</sup><sub>interface</sub>. Developed by Shen and co-workers, phase-sensitive SFG
(PS-SFG) is a technique that enables the extraction of both the real (Re) and imaginary
(Im) parts of the χ<sup>(2)</sup><sub>interface</sub> independently [140]. The SFG radiation is generated through
narrow bandwidth ps pulses of both ωIR and ωVis. Later on, a pioneered design with
the combination of narrowband ps-scheme of ωVis and broadband fs-scheme of ωIR was
extended by several groups [56,57] and named as heterodyne-detected SFG (HD-SFG) by
Tahara and his colleagues [141,142]. In either PS- or HD-SFG system, a local SF oscillator
(LO, reference beam) for field interference with the SFG signal is involved through the
use of non-centrosymmetric crystals working as a phase-known reference sample (e.g.,
Au, crystalline quartz SiO₂, ZnO, KNbO₃) (Figure 9c). One of the outstanding merits of
PS- or HD-SFG is that more information about a vibrational resonance can be inferred
and elucidated from the Imχ<sup>(2)</sup><sub>interface</sub> spectrum, such as the absorptive band shape and the
up/down orientation of interfacial molecules (±Imχ<sup>(2)</sup><sub>interface</sub>) [143]. Another scheme for
SFG investigation is the time-resolved SFG, in which its broadband signal is generated by
fs input pulses and followed by a Fourier transformation of the “free induction decay” into
the resonance spectral domain. The free induction decay occurs when the time resolution
of the input pulse is drastically shorter than the relaxation of the resonance. Hence, this
feature can address the problem of non-resonant response overwhelming by suppressing
the nearly instantaneous SFG signal from the metal electrode and potentially aid to adopt
in the two-dimensional (2D) coherent transient spectroscopy [144]. The details of these
schemes can be found in some seminal textbooks [145] and elsewhere [137,144,146].
<figure><img src="image_16.png" /><figcaption>**Figure 9.** Schemes for sum-frequency generation spectroscopy: (a) ps narrowband SFG, (b) fs broadband SFG, and (c) PS- or HD-SFG. PMT and CCD stand for photomultiplier tube and charge-coupled device, respectively. This figure is adapted from reference [138], Copyright © 2007 Elsevier and [147], Copyright © 2022 World Scientific Publishing.</figcaption></figure>

### 3.5.2. Hyphenated Spectroelectrochemical Cell Configurations

The unprecedented demonstration of the potential-dependent SFG study was investigated by P. Guyot-Sionnest and A. Tadjeddine in a reflected spectroelectrochemical cell [148]. Broadly speaking, to investigate the SFG signal under controlled electrochemical conditions, it is a requisite to design and fabricate a spectrochemical cell that meets the requirement for the overlapping in space (spatially) and time (temporally) of IR and visible beams as well as specifically probing the electrochemical interface. To circumvent any chemical interactions (oxidation or corrosion) with the cell material during the experiment, the base of the cell is necessarily made of an inert material such as Kel-F (polychlorotrifluoroethylene -[CFCl-CF₂]⁻), polytetrafluoroethylene (PTFE), or polypropylene -([CH₂-CH(CH₃)]⁻). The transparent window that must enable both IR and visible pulses to transmit through and reflect the generated SF can be the prism of CaF₂ (close to 7 µm of wavelength) or BaF₂ (up to 9 µm) [149]. Due to the ion's size compatibility of Ca²⁺ with F⁻ more than Ba²⁺ (hard and soft acids and bases theory), the molar solubility of BaF₂ is larger than CaF₂ in the aqueous solution (pKₛₚ of CaF₂ is 10.41 and BaF₂ is 5.82 at 25 °C). For that reason, CaF₂ is more commonly to be selected [66,150,151]. The prismatic windows can be in distinctive shapes: triangular or hemisphere prism. For the *in situ* SFG study of electrochemical reaction with
gaseous products, the cell can be adjusted with two gas paths (inlet and outlet) towards a gas detection instrument. This configuration can also offer a way to deaerate the solution by inert gases (N₂ or Ar) if the presence of O₂ intervenes in the oxygen reduction reactions (O₂/H₂O₂ and H₂O₂/H₂O).

Regarding the optical configurations of an SFG-coupled spectroelectrochemical cell, the reflection geometry is adopted more commonly than other types (Figure 10a,b).

<figure><img src="image_17.png" /><figcaption>**Figure 10.** Schematic depictions of the (a) five different commonly used optical configurations for spectroelectrochemical cells: (1) normal transmission mode, (2) parallel transmission mode, (3) external reflectance mode, (4) internal reflectance mode, and (5) back scattered mode; (b) some other surface- and tip-enhanced spectroscopic modes (nanostructure-based mode, ATR-based mode, Tip-based mode, and fiber-based mode); and two typical spectroelectrochemical cells coupled with SFG: (c) internal reflection and (d) external thin layer reflection. Dashed lines indicate the electrode-electrolyte interface. In (a,b), blue and red arrows simply present incident and detected light, respectively. This figure is adapted with permission from reference [152], Copyright © 2018 Elsevier for Figure 10a, reference [153], Copyright © 2024 Royal Society of Chemistry for Figure 10b, and reference [154], Copyright © 2020 AIP Publishing for Figure 10c,d.</figcaption></figure>

Depending upon the natural properties of the working electrode, it consists of two particular modes: internal and external (frontside) geometric strategies (Figures 10c and 10d, respectively), which were also commonly adopted in *in situ* Fourier transform infrared spectroscopy (FTIR) spectroelectrochemical investigations [155,156]. To exemplify, the external reflection configuration refers to the thin-layer (<50 µm) formation of an electrolyte solution by slightly pressing the working electrode against the optical window (Figure 10d). The optical window and working electrode are separate components, and a very thin electrolyte layer (micron-thick) is sandwiched between them. Thus, the well-suited material of the working electrode should be non-transparent and possess a high reflectivity, such as metal bulk electrodes (Pt, Au...) or monocrystalline electrodes. This thin electrolyte layer (a few µm of thickness) is maneuvered by a Teflon –[CF₂-CF₂]⁻ spacer. The key
advantage of this mode is that it attenuates the strong water adsorption of the IR pulse in the aqueous electrolyte solution, which can cause a severe diminution of the SFG signal. This geometry is quite analogous to the one used in infrared reflection absorption spectroscopy (IRRAS) [138]. Nevertheless, the benefit of implementing a thin layer appears to be the demerits of the electrochemical mechanism by distortion effect (sluggish mass transport and rapid reactant consumption). Thus, an internal reflection mode will tackle the issues encountered in the external one with a thin film deposited working electrode on the optical window surface (window/electrode/electrolyte) (Figure 10c). To do so, being optically transparent in both IR and visible radiations is a must for the working electrode. Because of that, this internal method is practically valid for limited electrode materials, particularly for battery materials (LiCoO₂, single-layer graphene, or ultrathin-film carbon). The limitations of this geometry are (1) poor signal-to-noise because of the unfavorable Fresnel factor and (2) instability of the ultrathin film electrode sustaining with a low current density [157]. Although typical metal electrodes are not favorable to use in this geometry, there are still some studies coating metal or silicon (Si) on the transparent window for potential-dependent SFG experiments [158–160]. The design principle is similar to the commonly used spectroelectrochemical cell conducted in surface-enhanced infrared absorption spectroscopy (SEIRAS) [161]. Figure 11 depicts a scheme of an external thin-layer spectroelectrochemical cell coupled with a broadband SFG system.

<figure><img src="image_18.png" /><figcaption>**Figure 11.** Schematic configuration of a femtosecond broadband sum-frequency generation spectroscopy (SFG) setup (IR: infrared, Vis: visible) coupled with an external thin-layer spectroelectrochemical cell. WE, RE, and CE represent working electrode, reference electrode, and counter electrode, respectively. CCD is charge-coupled device. This figure is adapted with permission from reference [69], Copyright © 2014 Elsevier.</figcaption></figure>

4. SFG at Aqueous Electrochemical Interfaces

In general, the study of SFG at the electrochemical interfaces can be categorized into three specific major subjects pertaining to the applications of (1) fundamental electrical double layer and interfacial water structures, (2) fuel-generated electrocatalysis (HER/HOR in water oxidation, CO₂ reduction, CO conversion, and methanol (MeOH)/ethanol (EtOH) alcohol oxidation/decomposition), and (3) rechargeable batteries (Li-ion or Li-O₂ batteries for instance). One of the indispensable discussions in these fields is to elucidate the reaction mechanism and intermediates’ identification. There are several reviews about vibrational SFG spectroscopy at electrochemical interfaces but they are unspecific towards water solutions [100,146,153,162,163]. In this review, we only pay attention to the electrochemical interfaces in aqueous electrolyte solutions rather than the ionic liquid electrolytes [164–168] or solid–electrolyte interphase (SEI) in the Li battery field, thus we encourage readers to read some previously published reviews and articles [154,169–171]. Also, we will not
elaborate on our discussion with the study of theoretical simulations in regard to these fields. However, there are copious relevant articles about theoretical studies of water structures at the EDL and SFG at aqueous interfaces [172–187] if readers are interested. Hence, we will organize our discussion based on three pillars: (1) interfacial structures of water molecules on the electrode surface, (2) interfacial structures of charged adsorbates and mechanism, and (3) interfacial structures of neutral or uncharged adsorbates and mechanism.

### 4.1. Interfacial Water Molecules on Electrode Surfaces

Water is the reactant in the electrochemical water splitting towards establishing a sustainable society with a net-zero-emission “green” hydrogen economy and directly related to the mechanistic comprehensions of HER ($2H^+(aq) + 2e^- \rightleftharpoons H_2\uparrow$ or $2H_2O(l) + 2e^- \rightleftharpoons H_2\uparrow + 2OH^-(aq)$) and OER ($H_2O(l) \rightleftharpoons \frac{1}{2}O_2\uparrow + 2H^+(aq) + 2e^-$ or $2OH^-(aq) \rightleftharpoons \frac{1}{2}O_2\uparrow + H_2O(l) + 2e^-$) in an acidic or a basic medium, respectively. A holistic knowledge about the orientation, organization, and dynamics of water itself at the electrode/water interface could, therefore, reinforce and enrich the discernment and efficiency of electro-catalytic reactions. At charged interfaces, an exhaustive and profound literatures utilizing SFG in the study of water molecules in the presence of an EDL were exhibited at (1) conductive metal oxide surface $In_2O_3/SnO_2$ (ITO) [188], (2) nonconducting inorganic solid surfaces such as calcium fluoride $CaF_2$ [185,189–194], oxides (silica/quartz $SiO_2$ [195–201], alumina/sapphire $Al_2O_3$ [202,203], $TiO_2$ [204–206]), or even mica mineral [207], and (3) organic surfaces (charged surfactant monolayer [68,142,208,209], nonionic long-chain alcohol monolayer [210], and biomembranes [113,211–215]). A very recent investigation of the photocatalyst strontium titanate (SrTiO$_3$)/water interface has also been demonstrated [109]. Take the $CaF_2$ surface as an example of an ionic inorganic solid surface; the dissolution of $F^-$ or $Ca^{2+}$ is the origin of triggering the surface charge (Scheme 1 which $\equiv$ denotes the solid surface-bound). The mechanism of $F^-$ liberation is thermodynamically more favorable than $Ca^{2+}$ dissolution (hydration enthalpy) [193]. Otherwise, if these water interfaces are not inherently charged surfaces, they are favorable for surface hydrolysis or water dissociative chemisorption to form hydrophilic OH groups on the surface. Varying the pH of the water solution (acid-base reaction) will generate a charged surface (protonation and deprotonation) [216]. This results in a pH-dependent behavior of SFG at these surfaces. For instance, siloxane bridges (Si-O-Si bonds) in $SiO_2$ surface structure experience a hydrolytic reaction leading to orthosilicic acid or its salt release into solution [217,218] (Scheme 2) or $TiO_2$ surface exhibits a formation of the chemisorbed hydroxyl layer (Scheme 3) [70,219–224].

$$ \equiv(CaF_2)\times \rightleftharpoons (CaF_2)_{x-1} + \equiv(CaF)^+ + F^-(aq) $$

$$ \equiv(CaF_2)\times \rightleftharpoons (CaF_2)_{x-1} + \equiv(F)^{2-} + Ca^{2+}(aq) $$

**Scheme 1.** Mechanism of a charged $CaF_2$ surface formation.

$$ \equiv \text{Si-O-Si(OH)}_2\text{OH} + \text{H}_2\text{O(l)} \rightleftharpoons \text{Si-O-OH} + \text{Si(OH)}_4\text{(aq)}, \text{ at pH < IEP} = 2.0, \text{ then} $$

$$ \equiv \text{Si-O-OH} + \text{H}^+(\text{aq}) \rightleftharpoons \text{Si-OH}_{2^+} \qquad K_{a_1}^{-1} = \frac{[\text{SiOH}_2^+]}{[\text{H}^+][\text{SiOH}]} $$

or

$$ \equiv \text{Si-O-Si(OH)}_2\text{O}^- + \text{H}_2\text{O(l)} \rightleftharpoons \text{Si-O-OH} + \text{Si(OH)}_3\text{O}^-(\text{aq}), \text{ at pH > IEP, then} $$

$$ \equiv \text{Si-OH} + \text{OH}^-(\text{aq}) \rightleftharpoons \text{Si-O}^- + \text{H}_2\text{O(l)} \qquad K_{b_2}^{-1} = \frac{[\text{SiO}^-]}{[\text{OH}^-][\text{Si-OH}]} $$

**Scheme 2.** Mechanism of a charged $SiO_2$ surface formation.
<figure><img src="image_19.png" /><figcaption>**Scheme 3.** Mechanism of a charged TiO₂ surface formation.</figcaption></figure>

From SFG vibrational spectra of water interfaces, the peculiarity exists of three dis-
tinctive bands in the O-H stretching region of well-aligned interfacial water molecules
corresponding to: (1) symmetric O-H stretching mode ($v_1$) of tetrahedrally coordinated
“ice-like” water structures (hexamer) in a highly ordered hydrogen-bonding arrangement
(a broad peak centered ≈ 3200 cm⁻¹), (2) asymmetric O-H stretching mode ($v_3$) of three-
coordinated hydrogen-bonded “liquid-like” water molecules in a disordered network (a
strong broad 3400–3500 cm⁻¹ peak), and (3) forbidden antisymmetric O-H stretching mode
of “free” or “dangling” non-hydrogen bonded O-H bonds from water itself or surface
(a sharp ≈ 3700 cm⁻¹ peak) [143,225–228] (Figure 12a,b). While these first two resonant
features were initially denoted by Shen et al. [200], the latter is normally recorded at the
suppressed water– hydrophobic interfaces where the hydrogen atom must protrude from
the surface [201,229–231]. The terminology of the first two hydrogen-bonded peaks (ice-like
and liquid-like) remains controversial due to the existence of an alternate interpretation
by theoretical calculations for ice and water clusters [225]. This causes unalike pictures of
water at the interface to a certain extent and the reconcilement of the controversy, therefore,
awaits further experiment evidence and simulation results. In the scope of this review, we
will still label them as commonly accepted “ice-like” and “liquid-like” terms as appeared in
the original papers. From Figure 12, it is evident that a higher order of hydrogen bonding
network possesses a lower energy of the OH stretching mode. As a result, the ratio of SFG
signals between ice-like and liquid-like water will serve as an indicator for the interfacial
water arrangement. Another characteristic vibrational mode in the water vibrational spec-
trum at a lower frequency ~1600 cm⁻¹ is the H-O-H bending band (scissoring) δ(HOH)
and this intramolecular vibration mode of isolated water molecules is also proved as a key
identifier in the dynamics of the intermolecular hydrogen bonding organization [112,232].
<figure><img src="image_20.png" /></figure>

**Figure 12.** Molecular model of the hydration interface at (a) a neutral oxide surface covered by a carpet of water's OH groups and (b) an electrically or protonated/deprotonated charged surface. For simplicity of the model, the appearance of aqueous electrolytes is neglected to observe how ice-like water and liquid-like water (water-like) differ. The closest monolayer to the oxide/charged surface (IHP) is the chemisorbed layer of water OH bonds. A subsequent layer is a highly structured ice-like water adlayer possessing an intermingled ordered network with four hydrogen atoms surrounding each oxygen atom in tetrahedral geometry (two hydrogen bonds with 177 pm of bond length, two normal covalent bonds of ≈96–99 pm bond length). The specific trait of this physisorbed immobilized layer (OHP) is the strict restriction of water (low dielectric constant) and hydrated ions' mobility toward the bulk solution. The farthest water layers (diffuse layer to the bulk) contain liquid-like water molecules with a disordered organization and high mobility of water/hydrated ions (higher dielectric constant). Thus, some bulk water molecules potentially exhibit dangle OH bonds. Between the ice-like and water-like layer, the so-called "coexistent layer" is a transitional monolayer characterized by a higher dipolar screening of water compared to the ice-like layer, but ions are non-specifically adsorbed and hydrated (low mobility). This figure is inspired by references [233,234].

Due to the dependence of a charged surface on the pH of the solution, most research has focused on the pH-dependent [210], or ion-identity-dependent properties [235] of water at these oxide surfaces. On the other hand, the temperature-dependent singularity of surface behavior at the air/water interface also highlights significant interfacial properties of water and various electrolyte solutions [236]. Intriguingly, a few research groups [68,111,237] have endeavored to distinguish the interfacial information of water molecules between two particular layers of the EDL (the Stern and diffuse) in a charged surface but mainly from pH dependence. Recently, Montenegro et al. demonstrated the spectroelectrochemical study of water interface at graphene electrode via an internal reflection mode of SFG to separate the surface $\chi_{\text{Stern}}^{(2)}$ contribution and bulk $\chi_{\text{Bulk}}^{(3)}$ contribution [110]. Regarding the study of water structure at electrochemical interfaces a few decades ago, Tadjeddine and co-workers reported the water adsorption on hydrogenated monocrystalline (single crystal) Pt electrodes suggesting a water dimer structure chemisorbs on Pt via three hydrogen bonding interactions [238]. Nevertheless, SFG spectra of Pt(hkl) electrodes in the range of OH bonds in $HClO_4$ solutions were stated infinitesimal and the prevailing water signal was attributed to ion-solvating water [239]. $H^+$ cations and $ClO_4^-$ anions are believed to inhibit the co-adsorption of interfacial water and its derivatives ($H_3O^+$ or $OH^-$) [240]. Thus, we will herein mention some practical issues regarding the spectroelectrochemical study of SFG of the interfacial water and elaborate on some adopted strategies by providing some case studies from different research groups.

There are some perturbing hurdles for the water adlayers' investigation at electrochemical interfaces in the traditional SFG setup: (1) the strong absorption of water molecules at the electrode surface and the bulk in the spectral range of mid-IR laser pulse, and (2) the dominance of non-resonant background signal referred as noise (Equations (6) and (10)) from metallic electrode (e.g., Au [241]) or metal oxide (e.g., transparent conductive indium tin oxide, ITO [242]) surfaces over the SFG signal of our interested interfacial water in the EDL. The rationale for the strong non-resonant contribution from the metal surface is the
electronic intraband and interband electronic transitions in the electronic band structure. To tackle the first practical issue, it was a must to design and fabricate a spectroelectrochemical cell with a micron-thin layer of electrolyte between the working electrode and the window of the cell to mitigate the attenuation effect of the IR input. It was suggested that the total internal reflection geometry with a ≈40–60 nm thick Au electrode for *in situ* SFG measurement under potential control could be a promising solution for this IR absorption phenomenon [243]. In addition, Liu and Shen have lately proposed another initiative to eliminate the deficiencies of unwanted and desired reflected SFG signal separation from the interface by modifying the IR beam geometry [158]. They designed the electrochemical SFG experiments in the Kretschmann configuration to exploit the planar surface plasmon (SP) excitation from the backside of flat Au film. To be more accurate, the IR input incident is from the prism side and the visible input and SFG output are on the opposite side, as depicted in Figure 13. The surface plasmon resonance (SPR) boosts the IR field at the electrochemical interface and resolves the need of having a very thin layer of electrolyte in the spectroelectrochemical cell. Liu et al. further developed the *in situ* SFG scheme utilizing plasmonic nanogratings engraved on the Au electrode to study interfacial water molecules [244]. They found that the adsorption of hydroxyl ions (OH⁻) on Au during the anodic scan rather reinforces the interfacial hydrogen-bonding network of water from +0.4 V to +1.2 V (vs. RHE). After +1.2 V, this network is possibly undermined by either the surface roughening of Au-O bonds or flipped water orientation with hydrogen directing towards the oxidized Au.

<figure><img src="image_21.png" /><figcaption>**Figure 13.** Schematic representation of SFG-electrochemical cell arrangement for the study of the electrochemical interface. This figure is reprinted with permission from reference [158], Copyright © 2014 the Proceedings of the National Academy of Sciences (PNAS).</figcaption></figure>

However, employing the ultrathin film of Au as a working electrode virtually lowers the limit of detection (LOD) of the weak resonant signal from the interfacial water, as mentioned in the second difficulty. The 5d-6s inter-band electronic transition (ΔE = 2.3 eV) at around 550 nm is the reason for the case of Au [245,246]. There are a few possible approaches to achieve effective suppression of the non-resonant response by: (1) utilizing a Two-Color SFG (2C-SFG) spectroscopy where visible input light is also tuned to suppress the Au signal and enhance the water molecule's signal, (2) adopting a temporal delay (several hundred of fs) between visible pulse and IR pulse (greater than the introduced IR pulse duration) to let the non-resonant signal decay, (3) selecting a low non-resonant responded electrode such as graphene or platinum (Pt), or (4) conducting the spectroelectrochemical study with time-resolved SFG or phase-sensitive SFG (Section 3.5.1).

The first-ever interfacial water study of the potential-dependent 2C-SFG at the Au electrode/ aqueous $10^{-3}$ M $H_2SO_4$ solution interface estimated by Nihonyanagi et al. applied the first strategy [245]. They employed a 470 nm visible excitation to acquire the highest signal-to-noise ratio of OH stretching bands of Au film/water interfaces. To be more specific, the dominating tendency of SFG signal at around $3500 \text{ cm}^{-1}$ over that of $3250 \text{ cm}^{-1}$ at -0.2 V vs. Ag/AgCl (saturated KCl) manifested the preferable structure of water
molecules in the disordered “liquid-like” form at the negative charged Au electrode with water dipole towards to the bulk and perpendicular to the electrode surface (Figure 14a). At +0.6V which is close to the PZC (~0.3V), it was observed that the SFG intensity reached the lowest, suggesting that water molecules are entropically higher and tend to align parallel to the surface. Furthermore, the unvariation of the relative phase angle (peak-dip transformation) of SFG spectra of the interfacial water molecules in the range of -0.2 V to +1.0 V indicates that they did not flip their dipole when scanning from negative to positive potentials across the PZC. It is ascribed to the adsorption of a sulfate (SO₄²⁻), not bisulfate (HSO₄⁻) adlayer at the Au electrode. This leads the net charge of the SO₄²⁻/Au interface to become negative at a positively applied potential, which draws H₂O molecules to adsorb with SO₄²⁻ through hydrogen bonds (Figure 14c).

<figure><img src="image_22.png" /><figcaption>**Figure 14.** Potential dependent SFG spectra in the OH stretching region and their cartoon illustrations of the interfacial water structure on (a,c) Au thin film surface in 0.01M H₂SO₄ solution and (b,d) Ag(100) surface in 0.1 M NaF solution. Numbers denote associated peak labels. (a,b) are adapted from fitted curves of references [245], Copyright © 2004 Elsevier and [247], Copyright © 2005 American Chemical Society, respectively. (c) is adapted from the reference [245], with adjustments to the water's dipole moment direction (arrow points from the hydrogen atoms (δ⁺) to the oxygen atom (δ⁻)) and (d) is more detailed with layers of the EDL.</figcaption></figure>
Almost a year later, Schultz et al. published the investigation of water orientations at the Ag(100)/water interface in 0.1 M NaF electrolyte solutions, using an external thin-layer reflected SFG under the electrochemical conditions [247]. The SFG spectra over a potential range from 0.0 V to -1.3 V vs. Ag/AgCl (for the purpose of minimizing Ag surface oxidation and HER production) illustrates more OH stretching peaks, including the presence of (1) 3370 cm⁻¹, (2) 3250 cm⁻¹, (3) 2970 cm⁻¹ frequencies, and (4) a 2800 cm⁻¹ peak at the proximate PZC (-0.8 V) (Figure 14b). The first peak is designated to the disorganized "liquid-like" water structure in the diffuse layer of the EDL with a lower level of hydrogen bonding and a weak interaction with the Ag surface. Peak 1 also exhibits a low dependence on the applied potential and presents a higher signal at 0.0 V. While the 3250 cm⁻¹ peak (peak 2) is normally linked to ice-like tetrahedral geometry, but particularly in the hydration shell of counterions with respect to the surface charge at OHP in the EDL, the specifically absorbed water molecules on the Ag surface at IHP are responsible for the attribution to the OH stretching at 2970 cm⁻¹ (peak 3). Across the PZC, these chemisorbed water molecules can basically bond with the Ag metal electrode via (1) Ag-H bonds (H atoms are the surface pointing atoms) at the negative side of the PZC ($\varphi - \varphi_{PZC} < 0$) or (2) lone pair electronic orbitals on O atoms (O atoms are the surface pointing atoms) at the positive side of the PZC ($\varphi - \varphi_{PZC} > 0$) (Figure 14d) [248]. The deciphering for lowering of the OH stretching frequency/energy stems from the electron-withdrawing effect of the electrode surface charge in the water O-H bonds (electron density reduction). For instance, the charge density accumulates on the Ag side of Ag-H bonds and consequently disperses the electron from the O atom side and weakens the O-H bonds in water. It is reasonable to recognize from the potential-dependent behavior that the SFG intensities of both peaks 2 and 3 reveal a minimum value at the PZC and show an increasing pattern towards either positive or negative potentials. Finally, the 2800 cm⁻¹ peak (peak 4) is only tangible when applying a potential at the PZC or a bit lower (-1.0 V). This observation implies that this OH stretching roots from a positively charged ion adsorbed on the negatively charged surface, and therefore it is labeled for hydronium cations (H₃O⁺) (Figure 14d). It seems that PZC here, albeit being defined as electrode potential at zero charge, refers to LZFC in particular (PZFC ≈ IEP). Even though this study evinced more information about four distinctive water structures in the EDL region at electrified Ag electrode, it contains a paucity of quantitative evidence about the molecular net dipole orientation of water as the previous research in Au. This is due to the fact that Ag does not exhibit a strong non-resonant response to extract the phase of the water resonant signal.

Going further to other thin film metal electrodes, Noguchi et al. continued to develop the potential dependence of SFG spectra in internal reflection mode at Pt/water [249] and Au/water [159] interfaces in 0.1 M HClO₄ solution and juxtapose to highlight the unique structures at these interfaces. The minimum of SFG intensity, close to the PZC is determined around 300 mV and 200 mV (vs. Ag/AgCl) at the Au and Pt electrodes, respectively. These PZC values are in the double layer region. At electrified Pt/H₂O interface, broad SFG bands at ca. 3200 cm⁻¹ and ca. 3400 cm⁻¹ express the presence of two structural systems of typical hydrogen-bonding water solvent: four-coordinated ice-like water and three-coordinated liquid-like water, respectively (Figure 15a). However, a solely major peak at 3400 cm⁻¹ in the Au electrode's study indicates interfacial water molecules structurally oriented more ordered at the Pt surface than at the Au electrode (Figure 15b). The higher oriented organization of water at the Pt surface supports a hypothesis of a stronger interaction between Pt-H₂O (well-ordered) than Au-H₂O (amorphous), which is in accordance with the previous findings from STM images [250,251]. Furthermore, the discrepancy between the SFG spectra of the Pt/H₂O interface in this study and from Tadjeddine's group might be due to the configuration of the spectroelectrochemical cell [249].
<figure><img src="image_23.png" /></figure>

**Figure 15.** SFG signal of interfacial water molecules on (a) Pt electrode and (b) Au electrode in HClO₄ solutions with their corresponding cyclic voltammogram acquired with a sweep rate of 50 mV·s⁻¹. This figure is reprinted with permission from references [249], Copyright © 2008 Elsevier for (a) and [159], Copyright © 2009 Royal Society of Chemistry for (b).

In this study, the authors do not focus only on the interfacial water at the EDL or double layer region, but the potential dependence of SFG spectra covers all the regions of electrified electrodes (hydrogen and oxygen regions) (Figure 16). Specifically, at the oxide region, SFG intensities of OH stretching decrease for both Pt and Au electrodes because of the formation of metal oxide species when moving towards more positive potentials. Several reasons for this decrease are proposed: (1) the breach of highly ordered network of interfacial water due to the electrode surface transformation from atomically flat surface to roughened oxides surface, (2) the electric effect derived from the nature of metal oxides (insulating or semiconducting), which causes an additional potential drop at oxygen layer and a smaller electric field within the double layer, and/or (3) the surface charge variation coming from the oxide layer. In addition, an uncharacteristic sharp peak at approximately 3550 cm⁻¹ was distinguished in the Au oxide formation region (from + 1.0 V vs. Ag/AgCl) except for the broad band centered around 3400 cm⁻¹. It is attributed to the OH stretching band of Au(OH)₂ (3565 cm⁻¹) and AuOH (3569 cm⁻¹), rather than the “free OH” peak, which is originally from the ClO₄⁻ anion adsorption potential region. Despite all the useful information discussed above, this study is still lacking the details of the net molecular dipole change of water molecules across the PZC to verify the water orientation movement.

Implementing a Fabry-Pérot etalon for the visible pulse delaying strategy, developed by Dlott and his colleagues [252,253] (second strategy) to suppress the non-resonant signal, Tong et al. unraveled the first experimental indication of free -OH stretching band (3680 cm⁻¹) at thin film Au/H₂O interface [254] (Figure 17a). In theory, the resonant signal could be attenuated by a factor of ≈(1−t₂/t₁) where t₁ is the IR pulse duration, T₂ is the vibrational dephasing time [146]. Their results depicted that the interfacial water molecules orient with one OH group towards Au surface perpendicularly without hydrogen bonding with another moiety of other water molecules (Figure 17b). The interaction of free OH bonds with the Au surface is relatively weak at all biases and vanishes in the oxygen region. This finding suggests that the Au thin film possesses rather the property of a hydrophobic surface at a molecular level.
<figure><img src="image_24.png" /><figcaption>**Figure 16.** Cyclic voltammogram (CV) of a polycrystalline Pt(poly) electrode in 0.5 M H₂SO₄, scan rate: 50 mV·s⁻¹. While there are three distinctive regions in the Pt(poly) electrode, including the hydrogen region (Pt-H with a strong and a weak adsorption/desorption peak), oxygen region (Pt-OHₐ ad/des and Pt-Oad/des), and a sandwiched double layer region (ad and d/des are adsorption and desorption, respectively), it appears without hydrogen adsorption/desorption in the Au electrode (only double layer region and oxide region with the formation/reduction of Au oxide species). This figure is obtained from our own CV measurements.</figcaption></figure>

<figure><img src="image_25.png" /><figcaption>**Figure 17.** (a) SFG spectrum of non-hydrogen bonded water and (b) its potential-dependent water structure representation. Dotted lines indicate hydrogen bonds. This figure is adapted from reference [254], Copyright © 2017 Wiley.</figcaption></figure>
To omit the complexity of the non-resonant signal from metal substrate, the third method adopts the non-metallic, highly conductive substances for being electrode's materials. An inherently atomically thin, chemically inert monolayer of graphene seems to be a promising candidate for the bias-dependent study of interfacial water structures with SFG. Following that idea, Dreier et al. sharpened the detection of interfacial water structure in contact with a chemical vapor deposited (CVD) grown graphene surface [255]. The SFG data of the OH stretching region evince the existence of water intercalation between graphene and CaF₂, which causes complications in the pH- and voltage-dependent SFG interpretation of mere graphene/H₂O interface. Additionally, the presence of free-OD response (where D is the deuterium isotope ²¹H in heavy water) is not recorded due to the centrosymmetric character (SFG inactive) coming from the presence of water molecules on both sides of graphene. Continuing to characterize the graphene/heavy water (D₂O) interface by homodyne-detected SFG, Montenegro et al. unveiled the marked asymmetry of the OD stretching in SFG spectra between negative and positive potentials [110]. At the negatively charged surface (smaller than -1.0 V vs. Ag/AgCl), they denote the narrow characteristic peak (around 2700 cm⁻¹) for the “free-OD” moiety of heavy water possibly pointing towards graphene while SFG spectra exhibit a swift vanishing of this band and follow an appearance of two broad hydrogen-bonded bands (roughly 2350 cm⁻¹ and 2500 cm⁻¹) at neutral or positive potentials [256] (Figure 18a). This asymmetric transformation is rationalized by the reorientation of O-D bonds towards the bulk (away from the graphene surface), favoring the hydrogen-bonding interactions with proximate water molecules when the EDL field increases.

<figure><img src="image_26.png" /><figcaption>**Figure 18.** The bias-dependent SFG spectra of interfacial water species in the (a) OD stretch spectral region at the graphene/D₂O interface and (b) OH stretch region at the graphene/H₂O interface. This figure is adapted from fitted curves of reference [110], Copyright © 2021 Springer Nature for (a) and [257], Copyright © 2023 Springer Nature for (b).</figcaption></figure>

Lately, the designation of the 2700 cm⁻¹ peak to interfacial D₂O (corresponding to around 3640 cm⁻¹ for the OH stretch) has galvanized Wang et al. into a dispute with Montenegro et al. They conducted the same measurements in the interfacial H₂O but used heterodyne-detected SFG (HD-SFG) [257]. From the negative sign of Imχ² interface spectra, it infers the down orientation of the OH group at 3630 cm⁻¹ (heading to the bulk water), in contrast to the positive Lorentzian fitted Imχ² interface spectra of Montenegro et al. [110]. Thus, they ascribe this negative peak to the OH group of the Ca-OH species at the CaF₂/H₂O interface rather than free-OD at the CaF₂-supported graphene/D₂O interface (Figure 18b). The hydroxylation of the CaF₂ surface, which is a positively charged surface at neutral pH 5.6, can be deciphered via the equation below (Equation (33)), and the proton transfer is supposed to take place between two interfaces (≡ is surface-bound) [258]. The disagreement
and ambiguity of the OH stretch assignment suggest that further demonstrations of the interfacial water behaviors at the graphene/water interface are needed.

$$ \equiv \mathrm{Ca}^{+}\mathrm{F} \cdots \mathrm{H}_{2}\mathrm{O} \rightleftharpoons \mathrm{Ca}(\mathrm{OH})\mathrm{F} + \mathrm{H}^{+}(\mathrm{aq})(\mathrm{CaF}_{2}/\mathrm{graphene}) \quad (33) $$

$$ \mathrm{H}^{+}(\mathrm{aq})(\mathrm{CaF}_{2}/\mathrm{graphene}) \rightleftharpoons \mathrm{H}^{+}(\mathrm{aq})(\mathrm{graphene/water}) \quad (34) $$

Overall, it can be seen in all examined studies that the applied potential (surface charge of electrode) is the driving force of interfacial water structuring. Although there are some technical impediments and shortcomings in the electrochemical SFG coupling (spectroelectrochemical cell or SFG configuration) to study the water structures at interfaces, potential-dependent SFG spectroscopy is still resourceful and a prime tool to deepen our fundamental knowledge of electrochemical phenomena at an electrified electrode/water interface. In addition, the segregation of interfacial information between the Stern and diffuse layer in the EDL in the potential dependent SFG is still deficient and cumbersome. Thus, these initial findings serve as preparation steps to unbolt a direction in probing and investigating the water splitting reactions (HER and OER) and their mechanisms on numerous electrocatalysts under more realistic conditions (operando).

## 4.2. Interfacial Charged Adsorbates on Electrode Surfaces (Electrolytes)

Historically, the electrochemical SFG spectroscopy was delved into experimenting with straightforward, small prototypical species such as CO, CN⁻, and SCN⁻ first, followed up with larger molecules (alcohols), complex structures (aromatic molecules), and ionic compounds. In this section, we emphasize the pivotal significance of the chemisorption of ions in aqueous solutions as a model for electrochemical interface events. Firstly, cyanide (CN⁻) was originally and later thoroughly studied on a polycrystalline Pt electrode by Tadjeddine's group [148,259]. They found two distinct bands of chemisorbed CN⁻ ions, an asymmetrical broad band around 2070–2100 cm⁻¹ where N-adsorbed CN bound to Pt atoms Pt-NC⁻ and another sharp band around 2150 cm⁻¹ corresponding to C-adsorbed CN stretch Pt-CN⁻. Daum et al. argued about the assignment of the second band in a higher frequency of CN⁻ adsorption on Pt(111) and Pt(110) from the disappearance of vibration at negative potentials and likely gravitated towards the idea of microscopic disorder of Pt surface after repeated oxidation-reduction cyclic voltammetric (CV) scans [260]. This disordered, microscopically rough surface favors the formation of surface cyano complexes [Pt(CN)₂]²⁻. In addition, Tadjeddine et al. also strived for CN⁻/Ag interface in ClO₄⁻ solutions, and they could extract the PZC of systems (−1.20 V with CN⁻ and −0.95 V without CN⁻ where the applied potential (E) vs. saturated calomel electrode (SCE)) from the parabolic shaped potential dependence of the non-resonant and the resonant components of $\chi_{S,eff}^{(2)}$ [261]. It is plausible to see the negative shift of PZC values induced by CN⁻ chemisorption.

Simultaneously, thiocyanate SCN⁻ was also well-probed in the spectroelectrochemical study of CN⁻ due to its simple structure and strong adsorption on the electrode surface. In the same study, Tadjeddine et al. indicated that the first band at ca. 2070 cm⁻¹ with a large potential tuning rate at −1.0 V vs. SCE belongs to N-bound adsorbed SCN⁻, while a smaller tuning rate band localized around 2140 cm⁻¹ is attributed to S-bound adsorbed SCN⁻ [259]. The chemisorption varied from N-bound to S-bound configurations as potential elevated. These are two terminal configurations of complexes deduced from the mesomeric (resonance) effect. Broadly speaking, SCN⁻ can possibly be able to complex with metal via bridging arrangements of S- or N-bonding [262]. Wang et al. further examined the adsorption and oxidation of SCN⁻ in HClO₄ acidic electrolyte on polycrystalline Au surface [263]. It was suggested that the adsorption of SCN⁻ on the Au surface is through the S-bound framework in the double layer region (−0.2 V to 0.5 V vs. SCE) and undergoes a phase change of around 0.3 V in both cathodic and anodic sweeps. At a higher potential of 0.7 V, the speculated oxidation of SCN⁻ on Au and product's adsorption occurs in the anodic scan: $\mathrm{SCN}^{-}(\mathrm{aq}) \rightarrow \mathrm{CN}^{-}(\mathrm{aq}) + \mathrm{SO}_{4}^{2-}(\mathrm{aq})$ ((1); this equation only serves as
a depiction for main products but is not balanced), then Au + CN⁻(aq) ⇌ AuCNad (2) and AuCNad + CN⁻(aq) ⇌ [Au(CN)₂]⁻ad (3). In the cathodic scan, the desorption of AuCNad (reverse (2)) and [Au(CN)₂]⁻ad (reverse (3)) or the dissolution of [Au(CN)₂]⁻ad ([Au(CN)₂]⁻ad ⇌ [Au(CN)₂]⁻(aq) (4)) free the Au surface. The electrochemical Stark shift is drastically different in the anodic scan and in the cathodic scan.

Another anion chemisorption that can be of paramount importance in varying reaction pathways and electrochemical yield of rechargeable batteries (lead–acid) or even in the Nafion-based ethanol fuel cell technology [264,265] is (bi)sulfate species (HSO₄⁻ and SO₄²⁻) adsorption. As previously discussed in water structures at the Au surface in H₂SO₄ solution [245], sulfate plays a role as an adlayer in regulating the interfacial water structure under potential control. It is remarked in the ethanol fuel cell study that the co-adsorption of (bi)sulfate species simultaneously fortifies the adsorption of acetate anions CH₃COOad and constrains them within a more well-defined rigid structure. The particular case of lead–acid batteries, commonly known as lead batteries, consists of two electrodes submersed in aqueous sulfuric acid H₂SO₄ solution with an overall reaction as the battery discharges as follows: PbO₂(s) + Pb(s) + 2HSO₄⁻(aq) + 2H⁺(aq) ⇌ 2PbSO₄(s) + 2H₂O(l) with Kₛₓ = 10²(E°PbO₂/PbSO₄)²⁻E°PbSO₄/Pb = 10²(1.62+0.29)² = 10⁶⁴.⁵³ where E°(Pb²⁺/Pb) = -0.126 V, E°(PbO₂/Pb²⁺) = 1.455 V, pKₛₚ(PbSO₄) = 7.66 and the cell diagram is (-) Pb | PbSO₄, H⁺, HSO₄⁻ | PbO₂ (Pb) (+). Bisulfate and sulfate ions are chemically unleashed from the dissociation equilibrium of sulfuric acid: H₂SO₄(aq) → H⁺(aq) + HSO₄⁻(aq) with Ka₁ >> 1, then HSO₄⁻(aq) ⇌ H⁺(aq) + SO₄²⁻(aq) with pKa₂ = 1.99 at 25 °C. Due to the prominence of H₂SO₄ in electrochemical processes, Braunschweig et al. presented the first broadband SFG spectra of (bi)sulfate adlayers on Pt(111) surfaces and marked a dominating vibrational band of symmetric S–O stretching of absorbed (bi)sulfate around 1245–1290 cm⁻¹ only when E > 0.2 V vs. Ag/AgCl [266]. Apart from three specific regions stated in Figure 16, a broad feature centered at 0.16 V in the cyclic voltammogram (CV) is leaned towards the near-saturation coverages of the (bi)sulfate adlayer on Pt(111) (Figure 19a). These ions adsorb on Pt via bidentate or didentate binding geometry and possess a subtle µ dipole moment perpendicular to the Pt surface, which is SFG inactive by virtue of the selection rule. At positively stronger polarization ca. 0.21 V, it experienced an abrupt transition from two-fold into a three-fold coordinated configuration (Pt₃≡O₃SO⁻) of (bi)sulfate anions where the intense band is detected (Figure 19a–c). A second dramatic augment in SFG intensity is observed at E > 0.5 V (Figure 19a–c) and ascribed to the surface hydroxyl (Pt-OH) formation from co-absorbed water molecules via: 2H₂O(l) + Pt → Pt-OHad + e⁻ + H₃O⁺(aq). This weaker hydrogen-bonding of Pt-OH in relation to the hydrogen network of co-adsorbed H₂O with sulfate absorbate (at the PtOₓ formation region in Figure 16) and the released hydronium cations incorporated in the double layer cause the decrease of interfacial electric field and a blue-shift of the vibrational band (reduction of the electrical Stark shift) (Figure 19b–d). One of the intriguing angles in terms of the potential-dependent shift in (bi)sulfate center frequency and intensity that Zwaschka et al. pursued to comprehend experimentally and theoretically is the dipole–dipole interaction. They emphasized the alterations of macroscopic external bias, which linearly change the local field sensed by individual adsorbates dipole–dipole coupling (molecular polarizability), could induce the nonlinearity of the SFG frequency and intensity [267].
<figure><img src="image_27.png" /><figcaption>**Figure 19.** (a) Consecutive series of broadband SFG spectra of (bi)sulfate adsorption on Pt(111) in 0.1 M H₂SO₄. Electrode potentials *E* (V) are indicated on the right-hand side. (b,c) Stark tuning for anodic and cathodic scans of the band in (a), respectively. (d) Bandwidth of the (bi)sulfate band in (a). SFG spectra were recorded with 5s acquisition time and during a scan rate of 5 mV·s⁻¹. This figure is reprinted with permission from reference [266], Copyright © 2010 American Chemical Society.</figcaption></figure>

### 4.3. Interfacial Uncharged Adsorbates and Fuel-Generated Oxidation on Electrode Surfaces (Molecules)

Fuel cells have been researched omnipresently to a greater extent in the substitution of the rapidly exhausted fossil fuels. The electricity is generated from the hydrogen-containing fuel oxidation (hydrogen H₂, *E*°cell,298K = 1.229 V; methanol MeOH, *E*°cell,298K = 1.213 V; ethanol EtOH, *E*°cell,298K = 1.145 V; methane CH₄, *E*°cell,298K = 1.06 V; or even carbon monoxide CO, *E*°cell,1073K = 0.9846 V) by ambient air O₂ [268]. Some of the advantages of fuel cells in comparison with Galvanic cells are the high efficiency of electricity manufacture and environmentally friendly products (H₂O) [269]. Due to the import of hydrogen deposition close to the HER on Pt electrodes in H₂-O₂/Pt fuel cells, Peremans and Tadjeddine conducted bias-evolved SFG experiments on different Pt electrodes (polycrystalline and monocrystalline of (111), (100), and (110) orientation) in H₂SO₄ aqueous solution at underpotential (E > E HER ) and overpotential (E < E HER ) [238,270]. There are a few common features observed for all electrodes: (1) an increase of SFG signals from 1800 to 2100 cm⁻¹ in the cathodic scan from the EDL to the HER onset (≈0.5 V vs. normal hydrogen electrode (NHE)), and (2) the advent of extra 1770 cm⁻¹ resonance peak at overpotential, suggesting its role as an intermediate in the HER. This additional orientation-independent H-Pt SFG resonance frequency is assigned to the bond in dihydride complexes (H₂Pt-Ln where H-Pt vibration at 1735 cm⁻¹) due to the off-range spectral values of onefold or multifold coordinated bound (Figure 20). At underpotential, double resonance peaks exhibit the adsorption of a water dimer at the EDL as reviewed in Section 4.1 while only polycrystalline Pt (Pt(poly)) and Pt(110) electrodes manifest the highest vibration at 2050 cm⁻¹, which is inferred from the corrugations of surfaces.

<figure><img src="image_28.png" /><figcaption>**Figure 20.** The Pt-H configuration at different electrodepositions (underpotential and overpotential of the HER). At the underpotential of the HER, the dimer of water from the EDL binds with three Pt-H bonds via hydrogen bonding while the dihydride Pt complex acting as a HER intermediate is present at the overpotential. This figure is adapted from reference [238,270], Copyright © 1995 AIP Publishing and [271,272], Copyright © 2011 Elsevier.</figcaption></figure>
CO electrochemistry has been immensely researched at Pt electrodes [273–275] and served as a model for surface adsorption phenomena [276] and electro-oxidation reaction (CO oxidation to CO₂ or an intermediate in fuel cells [264,277], which will be discussed later). Lu et al. reported a ~28 cm⁻¹·V⁻¹ Stark tuning rate of CO vibrational peak until the proximity of the CO oxidation onset potential [278]. Later, Noguchi et al. further observed the oxidation mechanism of adsorbed CO on Pt(111) electrode in both 0.1 M HClO₄ acid solution and 0.1 M NaOH alkaline solution [279]. A peak in the SFG spectra is assigned to the stretch of CO adsorbed on-top site of Pt (around 2000–2100 cm⁻¹) in both media. They concluded that anodic CO oxidation in the HClO₄ environment obeys the Langmuir–Hinshelwood (L-H) mechanism with Pt*-OHad being an intermediate: H₂O(l) + Pt ⇌ Pt-OHad + H⁺(aq) + e⁻, then Pt-COad + Pt-OHad ⇌ CO₂↑ + H⁺(aq) + e⁻ + 2Pt* where Pt* is the free Pt sites. On the contrary, COad is oxidized in a random Eley–Rideal (E-R) mechanism with OH⁻ ions in the pre-peak region as follows: Pt-COad + 2OH⁻(aq) ⇌ CO₂↑ + H₂O(l) + 2e⁻ + Pt*, which is consistent with the previous investigation [280]. These two L-H and E-R mechanisms are similar to those presented in Figure 2c.

Amongst several genres of fuel cells, direct methanol/ethanol fuel cells (DMFC/DEFC) garner huge interest because CH₃OH and C₂H₅OH are hydrogen-abundant bio-liquids and they can operate at room temperature (298 K). In DMFC, the electro-oxidation of MeOH occurs at anodic wave as follows: CH₃OH(l) + H₂O(l) ⇌ CO₂↑ + 6H⁺(aq) + 6e⁻. The challenging hindrance during this reaction is the incomplete oxidation of MeOH forming adsorbed CO species on the surface of the Pt electrode: CH₃OH(l) ⇌ COad + 4H⁺(aq) + 4e⁻. Two-fold consequences of the COad layer deserve attention: (1) the reaction of CH₃OH is kinetically slower around 1.5 times, and (2) COad species block active sites of Pt for further reactions (CO poisoning). Using Pt-Ru alloy as electrode material or applying really high overpotentials to galvanize the CO oxidation to CO₂ enables us to resolve the CO poisoning [276]. Preliminary studies pointed out the existence of Pt-CO bound types of bonding during the oxidation of MeOH in acidic solutions (HClO₄ and H₂SO₄) [261,270,281]. COad can not only bond with a single atom of Pt via a linear single bond (terminal Pt-C=O), but also with bridge bonds with two Pt atoms (Pt₂-C=O) at a lower vibrational frequency, higher steric hindrance. The dominance of particular COad bounded species relies on the concentration of MeOH: both terminal bonding mode (linearly bonded) and µ₂-bridging mode (multi-bonded where µ denotes the bridging ligand in coordination chemistry and a subscript of 2 means that the number of Pt metals bound to carbonyl ligand CO is 2) of carbonyl group at high concentration (≥0.1 M) and solely µ₂-bridging mode at lower concentration (4 × 10⁻³ M).

Acting as a model in the fuel cell’s anode compartment, Pt/CH₃OH interface in acidic media was examined by Vidal et al. [282]. Vidal et al. proved that another critical factor rather than bias voltage in the dissociative chemisorption of MeOH and CO oxidation on Pt(110) surfaces is the structural surface quality of electrodes [282]. The MeOH dissociative chemisorption majorly takes place at low potentials on defect sites (steps) and shows a tight packing of COad on the terrace sites when the concentration of MeOH is around 0.1 M. At higher potentials (vs. Ag/AgCl), the signal of CO adsorbed diminishes more acutely on terraces than on defects, suggesting that the CO oxidation occurred at less-densely-populated steps/defects and there is a diffusion process of COad hopping from terraces to defects to sustain CO density at defect sites. Furthermore, Humbert et al. proposed a novel procedure to assess the steady-state stability of CO adlayer on Pt(110) electrode regarding the poisoning in alcohol-based fuel cells [119] as sketched in Figure 21. The potential dependence of the CO layer deposited from CO/HClO₄ solution on Pt(110) is estimated in the range from –800 mV until 1.0 V (vs. Ag/AgCl, 3M KCl). While Pt is polarized negatively, highly concentrated adsorbed CO species block and then quench the HER, the CO oxidation is inhibited by a “frozen” dense layer in positive potentials. In a CO-diluted solution, a dominant spectroscopic feature at around 2060–2080 cm⁻¹ in the range from –500 mV to 600mV is well-known for C-O stretch, signifying the chemisorption of CO on the atop sites of Pt terraces. The weakening of CO bond during the chemical ab-
sorption of CO on Pt is explained by the synergistic effect of σ-donation and π-acceptance (backbonding or backdonation) of carbonyl ligand (ω of free CO is 2143 cm⁻¹) and consequently characterizes CO bonds in a metal-carbonyl complex more like a “partial” double bond (bond order close to 2), rather than a pure triple bond in free CO [151]. The gradual red shifting merely underwent in two regions of potential range except the HER and CO oxidation (from −500 to −50mV with a usual Stark shift Δω₁ ≈ 31 cm⁻¹ and between −50mV and 600mV with a peculiar Δω₂ ≈ 15 cm⁻¹). This occurrence is ascribed to the dipole-dipole coupling inside the CO layer: more dense packing results in a stronger coupling and induces a higher resonance frequency shift. The region of densely packed COad species encumbers ions accessing the electrode surface. As a result, it broadens the OHP (thicker EDL) and lessens the effective electric field. On top of that, an additional shoulder detected at 1955 cm⁻¹ around −200 mV is assigned to Pt-H stretching mode (gray arrow in Figure 21). The co-adsorption of H and CO on Pt is only stable from −250 mV to −50 mV before desorption of hydrogen at higher potentials. The weak intensity of this peak assists the quenching effect of dense CO coverage to the HER. A PZC value of +650 mV is determined, which is also a threshold potential before CO is oxidized.

<figure><img src="image_29.png" /><figcaption>**Figure 21.** SFG spectra of the CO layer deposited from diluted CO solution in HClO₄ on Pt(110) electrode for applied potential (vs. Ag/AgCl, 3M KCl) ranging from (a) −800 mV to −50 mV and (b) −50 mV to 1.0 V. Lines are fitting curves of the data. The same SFG intensity scale is for all spectra. This figure is reprinted with permission from reference [119], Copyright © 2016 American Chemical Society.</figcaption></figure>

Due to the high toxicity of MeOH, DEFC can be an appealing alternative to MeOH-O₂ fuel cells. In addition, it yields more electrons, and more electricity (12e from a complete oxidation of one EtOH molecule). Exemplarily, the cell notation of a DEFC is

$$ \begin{array}{l} (-) \text{Pt-Ru alloy} | \text{C}_2\text{H}_5\text{OH(l)}, \text{OH}^- / \text{H}^+(\text{aq}) | \text{AEM/PEM} | \text{OH}^- / \text{H}^+(\text{aq}), \text{O}_2(\text{g}) | \text{Pt-Ru alloy (+)} \\ \text{Anode} \\ (-): \qquad \text{C}_2\text{H}_5\text{OH(l)} + 3\text{H}_2\text{O(l)} \rightleftharpoons 2\text{CO}_2(\text{g}) + 12\text{H}^+(\text{aq}) + 12\text{e}^- \text{ in PEM} \\ \qquad \text{C}_2\text{H}_5\text{OH(l)} + 12\text{OH}^- (\text{aq}) \rightleftharpoons 2\text{CO}_2(\text{g}) + 9\text{H}_2\text{O(l)} + 12\text{e}^- \text{ in AEM} \\ \text{Cathode} \\ (+): \qquad 3\text{O}_2(\text{g}) + 12\text{H}^+(\text{aq}) + 12\text{e}^- \rightleftharpoons 6\text{H}_2\text{O(l)} \text{ in PEM} \\ \qquad 3\text{O}_2(\text{g}) + 6\text{H}_2\text{O(l)} + 12\text{e}^- \rightleftharpoons 12\text{OH}^- (\text{aq}) \text{ in AEM} \end{array} $$

where PEM is the proton exchange membrane, and AEM is the anion exchange membrane [283]. From the composition of this fuel cell, the metallic electrode is in contact with
an aqueous electrolyte solution, and the efficiency of EtOH oxidation counts upon the electrochemical interaction with a Pt or Pt-based catalyst layer at high overpotentials [284]. Plenty of works endeavoring to analyze the EtOH oxidation mechanism are reviewed substantially elsewhere [285], but Kutz et al. [277] and later Gomes et al. [264] attempted to dig deep into the reaction intermediates identification by potential-dependence SFG spectroscopy. These groundbreaking innovations have unveiled a better deciphering of this EtOH oxidation. Owing to its greater complexity than MeOH oxidation, they identified the vibrational mode of adsorbed intermediates of isotope-labeled EtOH during the reaction steps by applying different potentials on the Pt electrode in an acidic condition. Their investigations support the conclusion that acetaldehyde (AcH or MeCHO) and acetyl (Ac- or MeCO-) are two predominant intermediate species. All in all, Kutz et al. claimed that ethanol may undergo a catalytic oxidation by dehydrogenation to form MeCHO (acetate pathway), or these EtOH and newly formed MeCHO can simultaneously adsorb and quickly decompose into surface adsorbed fragments of -CHₓ or short lifetime -CHₓO (CO pathway). Following the dehydrogenation in the pathway (1) (Figure 22), MeCHO is oxidized further and produces adsorbed acetate, which can only diffuse from the surface by CH₃COOH conversion. On the other hand, adsorbed CO species are formed after the C-C breaking (pathway (1')) and further oxidized to generate the final desired CO₂ molecules. Gomes et al. unraveled various new adsorbed intermediates, shown in red colors in Figure 22. At higher potentials of 0.9 V vs. RHE, the EtOH adsorption and C-C breaking are blocked by the formation of hydroxyl or oxide species of Pt in the oxygen region (anodic scan from 0.5 to 1.0 V vs. Ag/AgCl in Figure 16). Aside from the breakthrough of the new intermediate's assignment, this work also shows the presence of HCHO or HCOOH as the final product of the reaction. By combining density functional theory (DFT) calculations, they indicate for the first time that the mechanism of EtOH under electro-oxidation conditions on the Pt electrode is much more sophisticated than believed so far. The application of SFG in decoding the electrochemical reaction mechanism in aqueous solutions can also be applicable to other organic acids such as formic acid HCOOH [286] or acetic acid CH₃COOH [287].

<figure><img src="image_30.png" /><figcaption>**Figure 22.** Proposed mechanism of EtOH oxidation and its intermediates on a Pt(poly) electrode in an acidic medium based on potential-dependent SFG analysis. The stereochemical configuration of adsorbed intermediates is not considered in this scheme. η^k refers to hapticity, the coordinated number of a ligand to a metal center through "k" contiguous multiple" atoms in coordination complexes. Newly detected adsorbed intermediates are highlighted in red, and the original C-C bond in the EtOH molecule in C₂ intermediates is marked in blue. The remaining are C₁ intermediates. This figure is based on references [264,277].</figcaption></figure>
Beyond addressing the cutting-edge fuel cell technology, anthropogenic global warming and climate change related to greenhouse gas (CO₂) emission is another pressing and exigent issue and huge efforts have been devoted to boosting CO₂ electrolysis. In principle, the overall mechanism of CO₂ electrolysis resembles the electrochemical water splitting (water electrolysis) with the occurrence of the reduction reaction of carbon dioxide (CO₂RR) at the cathode to transform into valid-added C₁, C₂, or long-chain products such as CO, hydrocarbons (CH₄, C₂H₄...), short-chain alcohols (MeOH, EtOH), or even organic acids (HCOOH, (COOH)₂...), via multiple electron transfers coupled with proton transfer steps in aqueous HCO₃⁻ electrolyte solution [288–290]. The major challenges for the CO₂RR under ambient environments are that (1) O=C=O is a linear molecule (D∞h point group) and chemically inert, so electrocatalysts are needed to overcome the high activation energy barrier (Eₐ) of bent-structured CO₂·⁻ radical intermediate formation (C₂ᵥ point group, represented in Equation (1), Table 2), and (2) low faradaic efficiency and poor product selectivity due to the metal electrocatalyst-dependent property of the reaction yield [291]. To be particular, Cu electrochemically reduces CO₂ to hydrocarbons, and post-transition metals such as In and Pb favor forming formate HCOO⁻ while Au and Ag can selectively convert CO₂ into CO [51,292–294]. This CO product can further fuel the Fischer–Tropsch synthesis with H₂ (syngas mixture) to produce mainly higher-chain hydrocarbons. In CO₂ chemistry, the reduction potentials of CO₂RR are pH dependent, and the acid–base equilibria of CO₂ in aqueous solutions include the appearance of bicarbonate HCO₃⁻ and carbonate CO₃²⁻ as follows: (where k<sub>H</sub> or H<sub>C</sub> is the concentration-based Henry solubility constant).

$$CO_2(g) \rightleftharpoons CO_2(aq) \qquad [CO_2]_{aq} = k_H \times P_{CO_2} \qquad (35)$$

$$CO_2(aq) + H_2O(l) \rightleftharpoons HCO_3^-(aq) + H^+(aq) \qquad pKa_1 = 6.35 \qquad (36)$$

$$HCO_3^-(aq) \rightleftharpoons CO_3^{2-}(aq) + H^+(aq) \qquad pKa_2 = 10.33 \qquad (37)$$

<table><caption>**Table 2.** The relevant standard (vs. RHE) and “effective” reduction potentials of CO₂RR (vs. SHE) at pH 7.0, 25 °C [295–297]. RHE: reversible hydrogen electrode, SHE: standard hydrogen electrode.</caption><thead><tr><th>No.</th><th>Half-Electrochemical Thermodynamic Reactions</th><th>E° (V), pH = 0</th><th>E°' (V), pH = 7</th></tr></thead><tbody><tr><td>(1)</td><td>CO₂(g) + e⁻ ⇌ CO₂·⁻</td><td>-1.500</td><td>-1.900</td></tr><tr><td>(2)</td><td>CO₂(g) + 2H⁺(aq) + 2e⁻ ⇌ HCOOH(aq)</td><td>-0.198</td><td>-0.613</td></tr><tr><td>(3)</td><td>CO₂(g) + 2H⁺(aq) + 2e⁻ ⇌ CO(g) + H₂O(l)</td><td>-0.110</td><td>-0.520</td></tr><tr><td>(4)</td><td>CO₂(g) + 4H⁺(aq) + 4e⁻ ⇌ HCHO(aq) + H₂O(l)</td><td>-0.070</td><td>-0.485</td></tr><tr><td>(5)</td><td>2H⁺(aq) + 2e⁻ ⇌ H₂(g)</td><td>0.000</td><td>-0.414</td></tr><tr><td>(6)</td><td>CO₂(g) + 6H⁺(aq) + 6e⁻ ⇌ MeOH(aq) + H₂O(l)</td><td>0.030</td><td>-0.384</td></tr><tr><td>(7)</td><td>2CO₂(g) + 12H⁺(aq) + 12e⁻ ⇌ H₂C=CH₂(g) + 4H₂O(l)</td><td>0.064</td><td>-0.350</td></tr><tr><td>(8)</td><td>2CO₂(g) + 12H⁺(aq) + 12e⁻ ⇌ EtOH(aq) + 3H₂O(l)</td><td>0.084</td><td>-0.330</td></tr></tbody></table>

The pH of the electrolyte solution can shift the equilibrium of (36) and (37), and thus it is a vital parameter for optimizing CO₂RR. While CO₂(aq) completely transforms into its associated (bi)carbonate ions at high pH values (>pKa₂), carbonic acid (H₂CO₃) and HCO₃⁻ are the predominant proton donors to favor the HER at low pH values (<pKa₁). Hence, the pH of the electrolyte for CO₂RR is favorable in the intermediate range from 7 to 9 to ensure the prevalence of HCO₃⁻(aq) species and reach the solubility threshold of CO₂ in water ([CO₂]ₐq ≈ 0.034 M at 25 °C and 1 atm) [51]. However, the competitiveness in limiting the faradaic current of CO₂ conversion between the HER and CO₂RR in aqueous electrolyte solutions is still widely recognized due to the adjacency of the equilibrium potentials of CO₂RR and the HER (Table 2). For 2H⁺/H₂ couple, the reductive potential at pH 7, 25 °C or the “formal” or “effective” reduction potential E°' follows the Nernst equation below.

$$E_{2H^+/H_2} = E^\circ = E^\circ + \frac{0.0592}{2} \log \frac{[H^+]^2}{P_{H_2}} = -0.0592 \text{pH} = -0.0592 \times 7 = -0.414 \text{ (V)} \qquad (38)$$
For other CO₂-based couples, E°(pH 7) = E°' = E° + 0.0592/n log PCO₂/K [H⁺]ⁿ = E° + E⁰'/(2H⁺/H₂) = E° - 0.0592pH = E° - 0.414 (V) where P(CO₂) is a unity (1 atm), and K is the pressure or concentration of the associated product at standard condition (P = 1 atm, C is a unity). There are insignificant differences between values based on the theoretical calculation and measured values.

To promote proton-assisted CO₂RR's selectivity and reactivity, (a) specific catalysts and (b) varying electrolyte and environmental conditions are required to concurrently (1) stabilize the one-electron reduced radical (CO₂·⁻) and (2) suppress the HER by increasing its Eₐ. Considering the recent developments of in situ potential-dependent SFG experiments on CO₂RR, Huang-fu et al. analyzed the reaction intermediates on Cu(poly) and Au electrodes in 0.1 M CO₂-saturated NaHCO₃ solution [292] and found that surface-adsorbed *CO species (around 2100 cm⁻¹ corresponding to the linearly bonded CO) are the key intermediate in CO₂ electrochemical reduction processes only on Au while the ethoxy intermediate (Cu-OEt) with the presence of two asymmetric C-H stretching bands (2936 cm⁻¹ for methylene group and 2996 cm⁻¹ for methyl group) is detected only on Cu. Later, Wallentine et al. also demonstrated in the same system of Au/H₂O interfaces under CO₂RR conditions but evinced the atop-surface-bound adsorbed *CO spectra (from 2088 to 2116 cm⁻¹) with zero non-resonant contribution [298]. It is interestingly reasonable because they adopted a temporal delay strategy (as mentioned in Section 4.1) between 800 nm pulse and the infrared pulse to suppress the non-resonant signal of Au. Additionally, they also introduced a backside geometry of the SFG-electrochemical system to generate the surface plasmon resonance (SPR) coupling to SFG and enhance the sensitivity with a significant signal-to-noise (S/N) improvement [157]. It is noticed that detection limits (LOD) of less than 1% of a surface monolayer can be achievable during CO₂ reduction on Au by utilizing plasmon-enhanced SFG. This technique was first employed by Liu and Shen [158] (also mentioned in Section 4.1). Electrochemically, this report considered the CO₂RR on Au to the CO end-product via the following elementary reaction steps (* is a surface-bound species): CO₂(g) + e⁻ ⇌ *CO₂·⁻ (1), *CO₂·⁻ + H⁺(aq) ⇌ *COOH (2), *COOH + H⁺(aq) + e⁻ ⇌ *CO + H₂O(l) (3), and *CO ⇌ CO(g) (4). It counts on the assumptions that (2) and (3) limit the overall CO₂RR, and (1) is the rate-determining step (RDS). To directly probe the interfacial water species and further distinguish the proton origin between water and (bi)carbonate species during competing HER/CO₂RR, Deng et al. recently attempted to utilize plasmon-enhanced SFG at Au/H₂O interfaces in different aqueous solutions: 0.05 M Na₂SO₄ with Ar and CO₂ purging and Ar-purged 0.1 M NaHCO₃ [299]. To be particular in measuring the interfacial water spectra, one sharp peak observed at 3730 cm⁻¹ is appointed to the “free” non-hydrogen bonded OH band in both Ar-purged and CO₂-purged Na₂SO₄ solution (Figure 23a,b). This finding is in harmony with the previous result of Tong et al. [254]. Another sharp peak (ca. 3650 cm⁻¹) appears when reaching near the onset of HER (−0.8 V vs. Ag/AgCl) in only Ar-purged sulfate solution (Figure 23a). This special feature is assigned to the “free” OH stretch of surface-bound hydroxide (OH⁻) produced during HER for the first time. In the CO₂-purged Na₂SO₄ solution, instead of the OH⁻ origin, a broad 3630 cm⁻¹ peak is believed to come from a weakly H-bonded or singly H-bonded water (Figure 23b). Interestingly, an additional peak is seen around 3400 cm⁻¹ when lowering negative potentials, suggesting the attribution to the interfacial water in the hydrated CO₃²⁻ ions in the Stern layer of the EDL (Figure 23b,c).

In addition, it is concluded that CO₂ purging appreciably improves the kinetics of active HER via two possible CO₂-purged hydrogen production mechanisms: interfacial pH buffering (1) and direct (bi)carbonate reduction (2) with water and (bi)carbonate species serving as proton donor sources, respectively. In mechanism (1), the OH⁻ anions produced from the direct reduction of H₂O (Equation (39) or presented in Figure 2a,b in a basic medium) are assumed to diffuse out of the Stern layer and react with CO₂(aq) and HCO₃⁻(aq) species (Equations (40) and (41)). These acid-role species will neutralize the accumulation of OH⁻ at the EI and buffer the pH of the interfacial region. Based on Le Chatelier's principle, the pH buffering of CO₂(aq) and HCO₃⁻(aq) favors a shift of
Equation (39) in the direction that produces more H₂. Otherwise, H₂CO₃/HCO₃⁻ are directly reduced to produce H₂ (Equations (42) and (43)) without the assistance of pH buffering in mechanism (2), then OH⁻ can be indirectly liberated from the aqueous equilibrium of base-role species: HCO₃⁻ (K₃b₂) and CO₃²⁻ (K₃b₁) with water (the reverse reactions of Equations (40) and (41)). These two mechanisms are summarized in Table 3.

<figure><img src="image_31.png" /><figcaption>**Figure 23.** (a) Potential-dependent SFG spectra of 0.05 M Na₂SO₄ solution purged with Ar, (b) potential-dependent SFG spectra of 0.05 M Na₂SO₄ solution purged with CO₂(g), and (c) pH-dependent SFG spectra of 50 mM Na₂CO₃ solutions. All applied potentials are compared to Ag/AgCl reference electrode. This figure is reprinted with permission from reference [299], Copyright © 2023 Royal Society of Chemistry.</figcaption></figure>

<table><caption>**Table 3.** Two possible mechanisms of HER enhancement by CO₂ purging.</caption><tbody><tr><td colspan="3">(1) Interfacial pH buffering (water as the primary proton donor)</td></tr><tr><td>2H<sub>2</sub>O(l) + 2e<sup>-</sup> ⇌ H<sub>2</sub>(g) + 2OH<sup>-</sup>(aq) K' = 10<sup>2E<sup>0</sup> H<sub>2</sub>O/H<sub>2</sub> 0.0592</sup> = 10<sup>2E<sup>0</sup> 2H<sup>+</sup>/H<sub>2</sub> 0.0592</sup> K<sub>W</sub><sup>2</sup></td><td>(39)</td></tr><tr><td>CO<sub>2</sub>(aq) + OH<sup>-</sup>(aq) ⇌ HCO<sub>3</sub><sup>-</sup>(aq) K<sub>b2</sub><sup>-1</sup> = K<sub>a1</sub> K<sub>W</sub><sup>-1</sup> = 10<sup>7.65</sup></td><td>(40)</td></tr><tr><td>HCO<sub>3</sub><sup>-</sup>(aq) + OH<sup>-</sup>(aq) ⇌ H<sub>2</sub>O(l) + CO<sub>3</sub><sup>2-</sup>(aq) K<sub>b1</sub><sup>-1</sup> = K<sub>a2</sub> K<sub>W</sub><sup>-1</sup> = 10<sup>3.67</sup></td><td>(41)</td></tr><tr><td colspan="3">(2) Direct H<sub>2</sub>CO<sub>3</sub>/HCO<sub>3</sub><sup>-</sup> reduction (H<sub>2</sub>CO<sub>3</sub>/HCO<sub>3</sub><sup>-</sup> as the primary proton donor)</td></tr><tr><td>2CO<sub>2</sub>(aq) + 2H<sub>2</sub>O(l) + 2e<sup>-</sup> ⇌ H<sub>2</sub>(g) + 2HCO<sub>3</sub><sup>-</sup>(aq) K'' = K'K<sub>b2</sub><sup>-2</sup></td><td>(42)</td></tr><tr><td>2HCO<sub>3</sub><sup>-</sup>(aq) + 2e<sup>-</sup> ⇌ H<sub>2</sub>(g) + 2CO<sub>3</sub><sup>2-</sup>(aq) K''' = K'K<sub>b1</sub><sup>-2</sup></td><td>(43)</td></tr></tbody></table>

Based on all observations, the results suggest that the kinetics of active HER in CO₂-saturated Na₂SO₄ solution follows mechanism (2), with a transition from mechanism (2), specifically Equation (43), between -0.8 V to -1.0 V (vs. Ag/AgCl) to the mechanism (1) at lower potentials (from -1.0 to -1.2 V) in 0.1 M NaHCO₃ electrolyte solution. After -1.2 V, the dominant mechanism is the direct water reduction with the support of interfacial pH buffering. These findings indicate the competition of possible proton donors in relation to their acidity and their potential-dependent interfacial concentrations. Although pure water (C = 55 M) is much more concentrated than HCO₃⁻ (C = 0.1 M) in 0.1 M NaHCO₃ electrolyte, HCO₃⁻ (pKa₂ = 10.33) is more acidic than water (pK<sub>W</sub> = 14) and consequently HCO₃⁻ ions is the predominant proton donor at low overpotential. At higher overpotentials (more negative), water claims the leading role in donating protons, and HCO₃⁻ anions are repelled from the interface due to Coulombic repulsion forces. Therefore, it is necessary to decrease the concentration of interfacial water to suppress HER below -1.2 V for electrocatalytically high overpotential CO₂RR.
Another essential development of electrochemical SFG spectroscopy is the adsorption and molecular orientation analyses of adsorbed organic molecules in an aqueous electrolyte solution. It consists of copious investigations of CN-containing class from small to big molecules, such as cyanoacetylene HC≡C-C≡N [300], acetonitrile CH₃-CN [301], 4-cyanopyridine NC-C₅H₄N [302], or even aromatic diisocyanides [101] on Pt or Au electrodes. In detail, the electrode potential dependence of the HCCCN/Au(111) interface in 5 × 10⁻⁴ M NaClO₄ was scrutinized from +0.1 V to +0.5 V vs. NHE and reversely to -1.0 V applied voltage vs. NHE by Humbert et al. [300], as depicted in Figure 24(1). The major signature of the stretching mode of CN moiety is seen at 2225 cm⁻¹ in the shape of a dip. Triple C≡C bond is impalpable due to the very low IR cross-section nature (low dipole moment change). The dip-shaped characteristic attests to the solution-headed -CN orientation and the dominant SFG contribution of the Au surface. From SFG spectra, the -CN vibrational frequencies blue shifted slightly from initial voltage 0.1 V to 0.5 V, and the Stark effect is attributed to this shift (Δω ≈ 20 cm⁻¹), which were in agreement with the value from the previous report on CN⁻/Au(hkl) interface [303]. It is surmised that the Au surface is saturated and passivated by adsorbed HCCCN molecules at threshold polarization (+0.5 V) until reaching the manifestation of HER. At highly negative potentials beyond -0.5 V, disappearance of the CN vibrational signal is elucidated by the desorption of those molecules. With a more complex organic structure with a pyridine ring (C₂v point group), Pluchery and Tadjeddine had already long before published an investigation on the same electrode in 0.1 M NaClO₄. The SFG spectra are acquired from -1.0 until 0.7 V vs. Ag/AgCl in the range of pyridine ring (830–1250 cm⁻¹, nine resonances) and CN (2050–2250 cm⁻¹) stretching modes [302]. From the pyridine region, the “in plane” vibrational modes are predominant at potentially positive and negative polarizations whilst the “out of plane” ones are destructed there and reach the maximum at transitional potentials. These observations are interpreted with the molecular reorganization of 4-cyanopyridine (C₂v symmetry axis) with respect to the surface of Au. They adsorb (a) perpendicularly on positively and negatively charged Au surfaces (upright orientation) and (b) parallel on roughly neutrally charged surfaces (horizontal orientation). As the spectral lineshapes of the CN stretching region switch from a dip (at -0.4 V) to a peak (at +0.4 V) as observed in Figure 24(2,3), it demonstrates that the -CN group flipped their N ending atom from heading towards the solution at negative voltages [300,303] to adsorbing closely to the positive charged surface. Furthermore, the weak SFG activity of the CN signal is possibly credited to the hydrolysis of a small amount of absorbed species. Not long ago, Ge et al. studied the bias-dependent SFG spectroscopy of isocyanide (-NC) groups rather complex systems with benzene ring(s), including 1,4-phenylene diisocyanide (PDI), 4,4'-biphenyl diisocyanide (BPDI), and 4,4''-p-terphenyl diisocyanide (TPDI) [101]. It is known that these aromatic para-substituted diisocyanide molecules bind covalently with Au flat surface to form highly ordered self-assembled monolayers (SAMs) [304,305]. They reported that there is a linearly increasing pattern in frequencies of surface-bound NC stretching from -0.7 to +0.1 V (vs. Ag/AgCl) under the electrochemical Stark effect. Strikingly, they relate the potential dependent behavior to the structure of the electrical double layer by extracting the Stern layer thickness (dStern). It is indicated that dStern of PDI SAM is in the ballpark of the molecular length of PDI, deducing to the electrolyte's non-intrusiveness of the close-packed structure of SAM. This observation is in line with the statement from the previous study on CO poisoning [119]. On the other hand, the values of dStern in BPDI and TPDI cases are smaller than their absorbed monolayer, inferring the infiltration of 0.1 M NaClO₄ electrolyte into the SAM.

Likewise, in the case of 4-cyanopyridine, Schultz and Gewirth also disclosed the phenomena of molecular inversion of an adsorbed zwitterionic species, p-aminobenzoic acid p-H₂N-C₆H₅-COOH (PABA) under the external potential stimuli at PABA/Ag(111) interface in 0.1 M KF solution [306] as sketched in Figure 25. From potentiodynamic SFG spectra, there are some detected vibrational modes: a symmetric mode of COO⁻ at 1405 cm⁻¹ and a bending mode of NH₃⁺ at around 1609 cm⁻¹ in the region from 1350 to
1675 cm⁻¹, and an aromatic CH stretching mode between 2900 and 3450 cm⁻¹. Nonetheless, the latter is vague by the IR adsorption attenuation of water (OH bending mode), so the analysis counts on the COO⁻ and CH peaks. The transition from a peak at a positive surface to a dip at a negative surface depicts the molecular flipping of this zwitterion. At negative scanning to the PZC, PABA orients with its COO⁻ group pointing away from the surface. Around PZC, it is more relaxed and has a more random orientation. Remarkably, the experience of a blue shift in COO⁻ stretching at more positive potentials is preferable to be elucidated by a more condensed phase system (higher packing density but still less than the solid-state) rather than a Stark shift or coordination variation. Thus, this supports the conclusion that PABA forms a dense film with COO⁻ adsorbed on the Ag surface at highly positive potentials.

<figure><img src="image_32.png" /><figcaption>**Figure 24.** (1) SFG spectra of the HC≡C-CN/Au(111) interface at several applied electrode potentials vs. NHE: (a) Vᵢ = +0.10 V, without HCCCN in the electrolyte, (b) Vᵢ = +0.10 V, (c) + 0.16 V, (d) +0.22 V, (e) +0.30 V, (f) +0.38 V, (g) +0.46 V, (h) Vᵣ = +0.50 V, (i) +0.10 V, (j) 0 V, (k) −0.20 V, (l) −0.50 V, (m) −1.0 V; (2) SFG spectra of the 4-cyanopyridine/Au(111) interface at three different potentials vs. Ag/AgCl. Continuous lines are the fitted curves; (3) sketch of molecular orientation of 4-cyanopyridine on Au(111) electrode at different potentials. Figure 24(1,2) are reproduced with permission from reference [300], Copyright © 2008 Elsevier for (1) and [302], Copyright © 2001 Elsevier for (2). Figure 24(3) is adapted from reference [138], Copyright © 2007 Elsevier.</figcaption></figure>

<figure><img src="image_33.png" /><figcaption>**Figure 25.** Graphical representation of the potential-induced orientation of p-aminobenzoic acid on Ag(111) electrode in 0.1 M KF solution. This figure is adapted from reference [306], Copyright © 2005 American Chemical Society.</figcaption></figure>
## 5. Conclusions and Future Perspectives

From the perspective of group theory, electrochemical interfaces (electrode-electrolyte interfaces) break the symmetry elements of a centrosymmetric structure. Sum-frequency generation (SFG) is a non-invasive optical probe providing interface-specific vibrational spectra with sub-monolayer sensitivity, so *in situ* hyphenation of SFG spectroscopy with electrochemical systems will not only assist in unveiling the adsorption of interfacial species at the EDL, but also sharpen the mechanistic understanding of electrocatalytic and photocatalytic reactions via chemical intermediates identification. Whilst water is the sine qua non for driving environmentally sustainable and green-energy-oriented electrochemical processes, probing of the fundamental water structures at electrochemical interfaces by SFG is hardly experimentally demonstrated due to several hurdles: (1) the strong IR adsorption of water molecules and (2) the overwhelming of non-resonant contribution with respect to the resonance of interested species, and (3) the challenges to differentiate the structural orientation of water molecules between two distinctive layers of the EDL (the Stern and diffuse layer) under electrochemical control. The development of SFG with groundbreaking and advanced configurations can offer unprecedented opportunities for potentially addressing these challenges. The complexity of electrocatalytic reactions has been evidenced by SFG spectroscopy. A novel and promising methodology of using THz spectroscopy coupled with the electrochemical-SFG system could also polarize the water molecules rather than applying an external bias on the electrode. Thus, it could offer innovative results in decoding the water structuring at the regime of the electrical double layer.

**Author Contributions:** Writing—original draft preparation, writing—review and editing, figures drawing, visualization, conceptualization, B.L.P.; writing—review and editing, co-supervision, A.R.; writing—review and editing, A.T.; writing—review and editing, co-supervision, funding acquisition, L.D.; writing—review and editing, supervision, funding acquisition, C.H. All authors have read and agreed to the published version of the manuscript.

**Funding:** This research was financially supported by the "Mission pour les Initiatives Transverses et Interdisciplinaires" (MITI-CNRS), grant number "80PRIME2023" through the research project "EMOSEINE". L.D. thanks the French State in the framework of the Investments for the Future programme IdEx University of Bordeaux for its financial support.

**Data Availability Statement:** Not applicable.

**Conflicts of Interest:** The authors declare no conflicts of interest.

## Abbreviations

### Physical Constants, Symbols

<table><tr><td>Universal gas constant</td><td>R = 8.314 J·mol<sup>-1</sup>·K<sup>-1</sup> = 0.08314 L·bar·mol<sup>-1</sup>·K<sup>-1</sup> = 0.08205 atm·L·K<sup>-1</sup>·mol<sup>-1</sup></td></tr><tr><td>Faraday's constant</td><td>F = 96,500 C·mol<sup>-1</sup></td></tr><tr><td>Avogadro's constant</td><td>N<sub>A</sub> = 6.0221 × 10<sup>23</sup> mol<sup>-1</sup></td></tr><tr><td>The elementary charge</td><td>e = 1.6021 × 10<sup>-19</sup> C</td></tr><tr><td>Speed of light</td><td>c = 2.998 × 10<sup>8</sup> m·s<sup>-1</sup></td></tr><tr><td>Planck's constant</td><td>h = 6.626 × 10<sup>-34</sup> J·s</td></tr><tr><td>Boltzmann constant</td><td>k<sub>B</sub> = 1.3807 × 10<sup>-23</sup> J·K<sup>-1</sup></td></tr><tr><td>Zero of the Celsius scale</td><td>0 °C = 273.15 K</td></tr><tr><td>Standard pressure</td><td>p° = 1 bar = 10<sup>5</sup> Pa</td></tr><tr><td>Atmospheric pressure</td><td>1 atm = 1.013 bar = 1.013 × 10<sup>5</sup> Pa = 760 mm Hg = 760 Torr</td></tr><tr><td>Electron-volt</td><td>1 eV = 1.6022·10<sup>-19</sup> J</td></tr><tr><td>Euler's number</td><td>e = 2.7183</td></tr><tr><td>Conversion</td><td>1 pm = 10<sup>-12</sup> m; 1 Å = 10<sup>-10</sup> m; 1 nm = 10<sup>-9</sup> m</td></tr></table>
Equations

Planck–Einstein relation

Relation between standard Gibbs
(free) energy, equilibrium constant,
and standard cell potential
(electromotive force)

Relation between Gibbs energy and
reaction quotient for a reaction

Nernst equation

Henderson–Hasselbalch equation

$$
E = \frac{hc}{\lambda} = h\nu = hc\omega \text{ where } \lambda \text{ [nm], } \nu \text{ [Hz or s}^{-1}\text{], } \omega \text{ [cm}^{-1}\text{]}
$$

$$
\Delta G^{\circ} = -RT\ln K = -nE^{\circ}F \\
\text{or } K = e^{-\frac{\Delta G^{\circ}}{RT}} = e^{\frac{nFE^{\circ}}{RT}} = 10^{\frac{nE^{\circ}}{0.0592}}
$$

$$
\text{where } \frac{2.303RT}{F} = 0.0592 \text{ (V) at } 25^{\circ}\text{C} \\
\text{and } \ln(x) = 2.303\log(x)
$$

$$
aA(aq) + bB(aq) \rightleftharpoons cC(aq) + dD(aq)
$$

$$
\Delta G = \Delta G^{\circ} + RT\ln Q \text{ where } Q = \frac{a\epsilon a_{1}^{d}}{a_{A}^{a} a_{B}^{b}} = \frac{[C]^{c} [D]^{d}}{[A]^{a} [B]^{b}}
$$

$$
\text{when } a_M = [M] \text{ (a is the activity of species M),}
$$
$$
E_{\text{ox/red}} =
$$

$$
E^{\circ}_{\text{ox/red}} + \frac{2.303RT}{mF}\log\frac{[\text{Ox}]^{a}}{[\text{Red}]^{b}} = E^{\circ}_{\text{ox/red}} + \frac{0.0592}{m}\log\frac{[\text{Ox}]^{a}}{[\text{Red}]^{b}}
$$

$$
(\text{when the activity coefficient } \gamma_M \text{ of species M is 1}),
$$
$$
E = E^{\circ} + \frac{2.303RT}{nF}\log Q^{-1} = E^{\circ} + \frac{0.0592}{n}\log Q^{-1} \text{ at } 25^{\circ}\text{C}
$$

$$
\text{pH} = pK_a + \log \frac{[A^-]}{[HA]} \text{ when } K_a \cdot C_{HA}^0, K_b \cdot C_{A-}^0 \gg
$$

$$
K_w \text{ and } [H^+], [OH^-] \ll C_{HA}^0, C_{A-}^0 \text{ (when } \gamma_M = 1)
$$

$$
\text{where } pK_a = -\log K_a; pK_{sp} = -\log K_{sp}; pK_w = -\log K_w = 14 \\
\text{at } 25^{\circ}\text{C.}
$$

References

1. Stamenkovic, V.R.; Strmcnik, D.; Lopes, P.P.; Markovic, N.M. Energy and fuels from electrochemical interfaces. *Nat. Mater.* **2017**, *16*, 57–69. [CrossRef] [PubMed]

2. Millet, P. Fundamentals of Water Electrolysis. In *Hydrogen Production*; Wiley: Hoboken, NJ, USA, 2015; pp. 33–62.

3. Bard, A.J.; Faulkner, L.R. *Electrochemical Methods: Fundamentals and Applications*, 2nd ed.; Wiley: Hoboken, NJ, USA, 2000.

4. Crittenden, J.C.; Trussell, R.R.; Hand, D.W.; Howe, K.J.; Tchobanoglous, G. Physical and Chemical Quality of Water. In *MWH's Water Treatment: Principles and Design*, 3rd ed.; John Wiley & Sons: Hoboken, NJ, USA, 2012; pp. 17–71.

5. Ruiz-Lopez, M.F.; Francisco, J.S.; Martins-Costa, M.T.C.; Anglada, J.M. Molecular reactions at aqueous interfaces. *Nat. Rev. Chem.* **2020**, *4*, 459–475. [CrossRef]

6. Lang, X.; Shi, L.; Zhao, Z.; Min, W. Probing the structure of water in individual living cells. *Nat. Commun.* **2024**, *15*, 5271. [CrossRef]

7. Tarun, O.B.; Okur, H.I.; Rangamani, P.; Roke, S. Transient domains of ordered water induced by divalent ions lead to lipid membrane curvature fluctuations. *Commun. Chem.* **2020**, *3*, 17. [CrossRef] [PubMed]

8. Shi, G.; Wang, H.; Zhang, Y.; Cheng, C.; Zhai, T.; Chen, B.; Liu, X.; Jono, R.; Mao, X.; Liu, Y.; et al. The effect of water on colloidal quantum dot solar cells. *Nat. Commun.* **2021**, *12*, 4381. [CrossRef]

9. Chen, S.; Takata, T.; Domen, K. Particulate photocatalysts for overall water splitting. *Nat. Rev. Mater.* **2017**, *2*, 17050. [CrossRef]

10. Duan, C.; Kee, R.; Zhu, H.; Sullivan, N.; Zhu, L.; Bian, L.; Jennings, D.; O'Hayre, R. Highly efficient reversible protonic ceramic electrochemical cells for power generation and fuel production. *Nat. Energy* **2019**, *4*, 230–240. [CrossRef]

11. Yousaf, M.; Lu, Y.; Akbar, M.; Lei, L.; Jing, S.; Tao, Y. Advances in solid oxide fuel cell technologies: Lowering the operating temperatures through material innovations. *Mater. Today Energy* **2024**, *44*, 101633. [CrossRef]

12. Gonella, G.; Backus, E.H.G.; Nagata, Y.; Bonthuis, D.J.; Loche, P.; Schlaich, A.; Netz, R.R.; Kühnle, A.; McCrum, I.T.; Koper, M.T.M.; et al. Water at charged interfaces. *Nat. Rev. Chem.* **2021**, *5*, 466–485. [CrossRef]

13. Shin, S.-J.; Kim, D.H.; Bae, G.; Ringe, S.; Choi, H.; Lim, H.-K.; Choi, C.H.; Kim, H. On the importance of the electric double layer structure in aqueous electrocatalysis. *Nat. Commun.* **2022**, *13*, 174. [CrossRef]

14. Butt, H.-J.; Graf, K.; Kappl, M. The Electric Double Layer. In *Physics and Chemistry of Interfaces*; John Wiley & Sons: Hoboken, NJ, USA, 2003; pp. 42–56.

15. Harris, D.C. Chapter 16. Electroanalytical techniques. In *Quantitative Chemical Analysis*, 8th ed.; W.H. Freeman: New York, NY, USA, 2010.

16. Chatenet, M.; Pollet, B.G.; Dekel, D.R.; Dionigi, F.; Deseure, J.; Millet, P.; Braatz, R.D.; Bazant, M.Z.; Eikerling, M.; Staffell, I.; et al. Water electrolysis: From textbook knowledge to the latest scientific strategies and industrial developments. *Chem. Soc. Rev.* **2022**, *51*, 4583–4762. [CrossRef]

17. Harvey, D. Chapter 11. Electrochemical Methods. In *Modern Analytical Chemistry*; McGraw-Hill Companies: New York, NY, USA, 2016; Volume 2.1, p. 1122.

18. Pastor, E.; Lian, Z.; Xia, L.; Ecija, D.; Galán-Mascarós, J.R.; Barja, S.; Giménez, S.; Arbiol, J.; López, N.; García de Arquer, F.P. Complementary probes for the electrochemical interface. *Nat. Rev. Chem.* **2024**, *8*, 159–178. [CrossRef] [PubMed]

19. Zhang, L.; Kuang, P.; Yu, J. Introductory chapter: Fundamentals of photocatalysis and electrocatalysis. In *Graphene Oxide-Metal Oxide and Other Graphene Oxide-Based Composites in Photocatalysis and Electrocatalysis*; Elsevier: Amsterdam, The Netherlands, 2022; pp. 1–30.
20. Millet, P. Chapter 2—Fundamentals of water electrolysis. In *Electrochemical Power Sources: Fundamentals, Systems, and Applications*; Elsevier: Amsterdam, The Netherlands, 2022; pp. 37–62.

21. Santana Santos, C.; Jaato, B.N.; Sanjuán, I.; Schuhmann, W.; Andronescu, C. Operando Scanning Electrochemical Probe Microscopy during Electrocatalysis. *Chem. Rev.* **2023**, *123*, 4972–5019. [CrossRef]

22. Bard, A.J.; Abruna, H.D.; Chidsey, C.E.; Faulkner, L.R.; Feldberg, S.W.; Itaya, K.; Majda, M.; Melroy, O.; Murray, R.W. The electrode/electrolyte interface—A status report. *J. Phys. Chem.* **1993**, *97*, 7147–7173. [CrossRef]

23. Wang, Y.; Skaanvik, S.A.; Xiong, X.; Wang, S.; Dong, M. Scanning probe microscopy for electrocatalysis. *Matter* **2021**, *4*, 3483–3514. [CrossRef]

24. Liu, R.-Z.; Shen, Z.-Z.; Wen, R.; Wan, L.-J. Recent advances in the application of scanning probe microscopy in interfacial electroanalytical chemistry. *J. Electroanal. Chem.* **2023**, *938*, 117443. [CrossRef]

25. Wang, L.-X.; Sun, C.; Huang, S.-L.; Kang, B.; Chen, H.-Y.; Xu, J.-J. Single-Particle Imaging Reveals the Electrical Double-Layer Modulated Ion Dynamics at Crowded Interface. *Nano Lett.* **2024**, *24*, 9743–9749. [CrossRef] [PubMed]

26. Favaro, M.; Jeong, B.; Ross, P.N.; Yano, J.; Hussain, Z.; Liu, Z.; Crumlin, E.J. Unravelling the electrochemical double layer by direct probing of the solid/liquid interface. *Nat. Commun.* **2016**, *7*, 12695. [CrossRef]

27. Velasco-Velez, J.J.; Pfeifer, V.; Hävecker, M.; Weatherup, R.S.; Arrigo, R.; Chuang, C.-H.; Stotz, E.; Weinberg, G.; Salmeron, M.; Schlögl, R.; et al. Photoelectron Spectroscopy at the Graphene–Liquid Interface Reveals the Electronic Structure of an Electrodeposited Cobalt/Graphene Electrocatalyst. *Angew. Chem. Int. Ed.* **2015**, *54*, 14554–14558. [CrossRef] [PubMed]

28. Favaro, M.; Drisdell, W.S.; Marcus, M.A.; Gregoire, J.M.; Crumlin, E.J.; Haber, J.A.; Yano, J. An Operando Investigation of (Ni–Fe–Co–Ce)Oₓ System as Highly Efficient Electrocatalyst for Oxygen Evolution Reaction. *ACS Catal.* **2017**, *7*, 1248–1258. [CrossRef]

29. Velasco-Velez, J.-J.; Wu, C.H.; Pascal, T.A.; Wan, L.F.; Guo, J.; Prendergast, D.; Salmeron, M. The structure of interfacial water on gold electrodes studied by X-Ray absorption spectroscopy. *Science* **2014**, *346*, 831–834. [CrossRef] [PubMed]

30. Grespi, A.; Larsson, A.; Abbondanza, G.; Eidhagen, J.; Gajdek, D.; Manidi, J.; Tayal, A.; Pan, J.; Merte, L.R.; Lundgren, E. Probing the electrode-liquid interface using operando total-reflection X-ray absorption spectroscopy. *Surf. Sci.* **2024**, *748*, 122538. [CrossRef]

31. Shimizu, T.K.; Maier, S.; Verdaguer, A.; Velasco-Velez, J.-J.; Salmeron, M. Water at surfaces and interfaces: From molecules to ice and bulk liquid. *Prog. Surf. Sci.* **2018**, *93*, 87–107. [CrossRef]

32. Fleischmann, M.; Hendra, P.J.; Hill, I.R.; Pemble, M.E. Enhanced Raman spectra from species formed by the coadsorption of halide ions and water molecules on silver electrodes. *J. Electroanal. Chem. Interfacial Electrochem.* **1981**, *117*, 243–255. [CrossRef]

33. Nyamekye, C.K.A.; Bobbitt, J.M.; Zhu, Q.; Smith, E.A. The evolution of total internal reflection Raman spectroscopy for the chemical characterization of thin films and interfaces. *Anal. Bioanal. Chem.* **2020**, *412*, 6009–6022. [CrossRef] [PubMed]

34. Woods, D.A.; Bain, C.D. Total internal reflection Raman spectroscopy. *Analyst* **2012**, *137*, 35–48. [CrossRef]

35. Weiling, M.; Pfeiffer, F.; Baghernejad, M. Vibrational Spectroscopy Insight into the Electrode | electrolyte Interface/Interphase in Lithium Batteries. *Adv. Energy Mater.* **2022**, *12*, 2202504. [CrossRef]

36. Shen, A.; Pemberton, J.E. Investigation of trace interfacial water at silver electrodes in a series of normal alcohols using surface enhanced Raman scattering. *Phys. Chem. Chem. Phys.* **1999**, *1*, 5677–5684. [CrossRef]

37. Cui, L.; Liu, Z.; Duan, S.; Wu, D.-Y.; Ren, B.; Tian, Z.-Q.; Zou, S.-Z. Orientation Change of Adsorbed Pyrazine on Roughened Rhodium Electrodes as Probed by Surface-Enhanced Raman Spectroscopy. *J. Phys. Chem. B* **2005**, *109*, 17597–17602. [CrossRef]

38. Martín Sabanés, N.; Ohto, T.; Andrienko, D.; Nagata, Y.; Domke, K.F. Electrochemical TERS Elucidates Potential-Induced Molecular Reorientation of Adenine/Au(111). *Angew. Chem. Int. Ed.* **2017**, *56*, 9796–9801. [CrossRef]

39. Verma, P. Tip-Enhanced Raman Spectroscopy: Technique and Recent Advances. *Chem. Rev.* **2017**, *117*, 6447–6466. [CrossRef] [PubMed]

40. Ataka, K.-I.; Yotsuyanagi, T.; Osawa, M. Potential-Dependent Reorientation of Water Molecules at an Electrode/Electrolyte Interface Studied by Surface-Enhanced Infrared Absorption Spectroscopy. *J. Phys. Chem.* **1996**, *100*, 10664–10672. [CrossRef]

41. Wandlowski, T.; Ataka, K.; Pronkin, S.; Diesing, D. Surface enhanced infrared spectroscopy—Au(111-20nm)/sulphuric acid—New aspects and challenges. *Electrochim. Acta* **2004**, *49*, 1233–1247. [CrossRef]

42. Cuesta, A. ATR-SEIRAS for time-resolved studies of electrode–electrolyte interfaces. *Curr. Opin. Electrochem.* **2022**, *35*, 101041. [CrossRef]

43. Nakamura, M.; Kato, H.; Hoshi, N. Infrared Spectroscopy of Water Adsorbed on M(111) (M = Pt, Pd, Rh, Au, Cu) Electrodes in Sulfuric Acid Solution. *J. Phys. Chem. C* **2008**, *112*, 9458–9463. [CrossRef]

44. Osawa, M.; Tsushima, M.; Mogami, H.; Samjeské, G.; Yamakata, A. Structure of Water at the Electrified Platinum–Water Interface: A Study by Surface-Enhanced Infrared Absorption Spectroscopy. *J. Phys. Chem. C* **2008**, *112*, 4248–4256. [CrossRef]

45. Hou, J.; Xu, B.; Lu, Q. Influence of electric double layer rigidity on CO adsorption and electroreduction rate. *Nat. Commun.* **2024**, *15*, 1926. [CrossRef] [PubMed]

46. Tian, Y.; Huang, B.; Song, Y.; Zhang, Y.; Guan, D.; Hong, J.; Cao, D.; Wang, E.; Xu, L.; Shao-Horn, Y.; et al. Effect of ion-specific water structures at metal surfaces on hydrogen production. *Nat. Commun.* **2024**, *15*, 7834. [CrossRef]

47. Li, J.F.; Huang, Y.F.; Ding, Y.; Yang, Z.L.; Li, S.B.; Zhou, X.S.; Fan, F.R.; Zhang, W.; Zhou, Z.Y.; Wu, D.Y.; et al. Shell-isolated nanoparticle-enhanced Raman spectroscopy. *Nature* **2010**, *464*, 392–395. [CrossRef]

48. Li, C.-Y.; Le, J.-B.; Wang, Y.-H.; Chen, S.; Yang, Z.-L.; Li, J.-F.; Cheng, J.; Tian, Z.-Q. In situ probing electrified interfacial water structures at atomically flat surfaces. *Nat. Mater.* **2019**, *18*, 697–701. [CrossRef]
49. Li, C.-Y.; Chen, M.; Liu, S.; Lu, X.; Meng, J.; Yan, J.; Abruña, H.D.; Feng, G.; Lian, T. Unconventional interfacial water structure of highly concentrated aqueous electrolytes at negative electrode polarizations. *Nat. Commun.* **2022**, *13*, 5330. [CrossRef]

50. Wang, Y.-H.; Zheng, S.; Yang, W.-M.; Zhou, R.-Y.; He, Q.-F.; Radjenovic, P.; Dong, J.-C.; Li, S.; Zheng, J.; Yang, Z.-L.; et al. In situ Raman spectroscopy reveals the structure and dissociation of interfacial water. *Nature* **2021**, *600*, 81–85. [CrossRef] [PubMed]

51. Jovanovic, S.; Jakes, P.; Merz, S.; Daniel, D.T.; Eichel, R.-A.; Granwehr, J. In operando NMR investigations of the aqueous electrolyte chemistry during electrolytic CO₂ reduction. *Commun. Chem.* **2023**, *6*, 268. [CrossRef] [PubMed]

52. Mohammadi, M.; Jerschow, A. In situ and operando magnetic resonance imaging of electrochemical cells: A perspective. *J. Magn. Reson.* **2019**, *308*, 106600. [CrossRef]

53. Griffin, J.M.; Forse, A.C.; Tsai, W.-Y.; Taberna, P.-L.; Simon, P.; Grey, C.P. In situ NMR and electrochemical quartz crystal microbalance techniques reveal the structure of the electrical double layer in supercapacitors. *Nat. Mater.* **2015**, *14*, 812–819. [CrossRef] [PubMed]

54. Wang, Y.; Malveau, C.; Rochefort, D. Solid-state NMR and electrochemical dilatometry study of charge storage in supercapacitor with redox ionic liquid electrolyte. *Energy Storage Mater.* **2019**, *20*, 80–88. [CrossRef]

55. Bols, M.L.; Ma, J.; Rammal, F.; Plessers, D.; Wu, X.; Navarro-Jaén, S.; Heyer, A.J.; Sels, B.F.; Solomon, E.I.; Schoonheydt, R.A. In Situ UV–Vis–NIR Absorption Spectroscopy and Catalysis. *Chem. Rev.* **2024**, *124*, 2352–2418. [CrossRef] [PubMed]

56. Pool, R.E.; Versluis, J.; Backus, E.H.G.; Bonn, M. Comparative Study of Direct and Phase-Specific Vibrational Sum-Frequency Generation Spectroscopy: Advantages and Limitations. *J. Phys. Chem. B* **2011**, *115*, 15362–15369. [CrossRef] [PubMed]

57. Stiopkin, I.V.; Jayathilake, H.D.; Bordenyuk, A.N.; Benderskii, A.V. Heterodyne-Detected Vibrational Sum Frequency Generation Spectroscopy. *J. Am. Chem. Soc.* **2008**, *130*, 2271–2275. [CrossRef]

58. Sayama, A.; Nihonyanagi, S.; Ohshima, Y.; Tahara, T. *In situ* observation of the potential-dependent structure of an electrolyte/electrode interface by heterodyne-detected vibrational sum frequency generation. *Phys. Chem. Chem. Phys.* **2020**, *22*, 2580–2589. [CrossRef]

59. Singh, A.K.; Doan, L.C.; Lou, D.; Wen, C.; Vinh, N.Q. Interfacial layers between ion and water detected by terahertz spectroscopy. *J. Chem. Phys.* **2022**, *157*, 054501. [CrossRef] [PubMed]

60. Nemes, C.T.; Swierk, J.R.; Schmuttenmaer, C.A. A Terahertz-Transparent Electrochemical Cell for In Situ Terahertz Spectroelectrochemistry. *Anal. Chem.* **2018**, *90*, 4389–4396. [CrossRef] [PubMed]

61. Isogai, T.; Uranagase, M.; Motobayashi, K.; Ogata, S.; Ikeda, K. Probing collective terahertz vibrations of a hydrogen-bonded water network at buried electrochemical interfaces. *Chem. Sci.* **2023**, *14*, 6531–6537. [CrossRef] [PubMed]

62. Helmholtz, H. Über einige Gesetze der Vertheilung elektrischer Strome in korperlichen Leitem mit Anwendung auf die thierisch-elektrischen Versuche. *Ann. Phys. Chem.* **1853**, *89*, 211–233. [CrossRef]

63. Helmholtz, H. Studien über electrische Grenzschichten. *Ann. Phys. Chem.* **1879**, *243*, 337–382. [CrossRef]

64. Gouy, M. Sur la constitution de la charge électrique à la surface d'un électrolyte. *J. Phys. Theor. Appl.* **1910**, *9*, 457–468. [CrossRef]

65. Chapman, D.L. A contribution to the theory of electrocapillarity. *Lond. Edinb. Dublin Philos. Mag. J. Sci.* **1913**, *25*, 475–481. [CrossRef]

66. Housecroft, C.E.; Sharpe, A.G. *Inorganic Chemistry*, 5th ed.; Pearson Prentice Hall: Harlow, England, 2018; p. 1137.

67. Mills, I.; Cvitas, T.; Homann, K.; Kallay, N.; Kuchitsu, K. Electric dipole moment. In *Quantities, Units and Symbols in Physical Chemistry*, 2nd ed.; International Union of Pure and Applied Chemistry (IUPAC): Zürich, Switzerland, 1993.

68. Wen, Y.-C.; Zha, S.; Liu, X.; Yang, S.; Guo, P.; Shi, G.; Fang, H.; Shen, Y.R.; Tian, C. Unveiling Microscopic Structures of Charged Water Interfaces by Surface-Specific Vibrational Spectroscopy. *Phys. Rev. Lett.* **2016**, *116*, 016101. [CrossRef]

69. Rey, N.G.; Dlott, D.D. Studies of electrochemical interfaces by broadband sum frequency generation. *J. Electroanal. Chem.* **2017**, *800*, 114–125. [CrossRef]

70. Beranek, R. (Photo)electrochemical Methods for the Determination of the Band Edge Positions of TiO₂-Based Nanomaterials. *Adv. Phys. Chem.* **2011**, *2011*, 786759. [CrossRef]

71. Brown, M.A.; Abbas, Z.; Kleibert, A.; Green, R.G.; Goel, A.; May, S.; Squires, T.M. Determination of Surface Potential and Electrical Double-Layer Structure at the Aqueous Electrolyte-Nanoparticle Interface. *Phys. Rev. X* **2016**, *6*, 011007. [CrossRef]

72. Matsumoto, K.; Miyazaki, K.; Hwang, J.; Yamamoto, T.; Sakuda, A. Electrode Potentials Part 1: Fundamentals and Aqueous Systems. *Electrochemistry* **2022**, *90*, 102001. [CrossRef]

73. Debye, P.H.E.; Zur Theorie der Elektrolyte, I. Gefrierpunktserniedrigung und verwandte Erscheinungen. *Phys. Z.* **1923**, *24*, 185–206.

74. Stern, O. Zur theorie der elektrolytischen doppelschicht. *Z. Für Elektrochem. Und Angew. Phys. Chem.* **1924**, *30*, 508–516. [CrossRef]

75. Grahame, D.C. The Electrical Double Layer and the Theory of Electrocapillarity. *Chem. Rev.* **1947**, *41*, 441–501. [CrossRef]

76. Bockris, J.O.; Devanathan, M.A.V.; Müller, K. On the structure of charged interfaces. *Proc. R. Soc. Lond. A Math. Phys. Sci.* **1963**, *274*, 55–79.

77. Limaye, A.; Suvlu, D.; Willard, A.P. Water molecules mute the dependence of the double-layer potential profile on ionic strength. *Faraday Discuss.* **2024**, *249*, 267–288. [CrossRef]

78. Kornyshev, A.A.; Spohr, E.; Vorotyntsev, M.A. Electrochemical Interfaces: At the Border Line. In *Encyclopedia of Electrochemistry*; Wiley: Hoboken, NJ, USA, 2007.

79. Baldelli, S. Probing Electric Fields at the Ionic Liquid–Electrode Interface Using Sum Frequency Generation Spectroscopy and Electrochemistry. *J. Phys. Chem. B* **2005**, *109*, 13049–13051. [CrossRef]
80. Nafie, L.A. Vibrational optical activity: From discovery and development to future challenges. *Chirality* **2020**, *32*, 667-692.
[CrossRef]

81. Ishibashi, T.-a.; Okuno, M. Chapter 9—Heterodyne-detected chiral vibrational sum frequency generation spectroscopy of bulk and interfacial samples. In *Molecular and Laser Spectroscopy*; Gupta, V.P., Ozaki, Y., Eds.; Elsevier: Amsterdam, The Netherlands, 2020; pp. 315–348.

82. Molloy, K.C. *Group Theory for Chemists: Fundamental Theory and Applications*, 2nd ed.; Horwood: Chichester, UK, 2004.

83. McQuarrie, D.A.; Simon, J.D. *Physical Chemistry: A Molecular Approach*; University Science Books: Sausalito, CA, USA, 1997.

84. Humbert, C.; Noblet, T. A Unified Mathematical Formalism for First to Third Order Dielectric Response of Matter: Application to Surface-Specific Two-Colour Vibrational Optical Spectroscopy. *Symmetry* **2021**, *13*, 153. [CrossRef]

85. Humbert, C.; Noblet, T.; Dalstein, L.; Busson, B.; Barbillon, G. Sum-Frequency Generation Spectroscopy of Plasmonic Nanomaterials: A Review. *Materials* **2019**, *12*, 836. [CrossRef] [PubMed]

86. Humbert, C.; Pluchery, O.; Lacaze, E.; Busson, B.; Tadjeddine, A. Two-Colour Sum-Frequency Generation Spectroscopy Coupled to Plasmonics with the CLIO Free Electron Laser. *Photonics* **2022**, *9*, 55. [CrossRef]

87. Noblet, T.; Dreesen, L.; Boujday, S.; Méthivier, C.; Busson, B.; Tadjeddine, A.; Humbert, C. Semiconductor quantum dots reveal dipolar coupling from exciton to ligand vibration. *Commun. Chem.* **2018**, *1*, 76. [CrossRef]

88. Lambert, A.G.; Davies, P.B.; Neivandt, D.J. Implementing the Theory of Sum Frequency Generation Vibrational Spectroscopy: A Tutorial Review. *Appl. Spectrosc. Rev.* **2005**, *40*, 103–145. [CrossRef]

89. Noblet, T.; Boujday, S.; Méthivier, C.; Erard, M.; Hottechamps, J.; Busson, B.; Humbert, C. Two-Dimensional Layers of Colloidal CdTe Quantum Dots: Assembly, Optical Properties, and Vibroelectronic Coupling. *J. Phys. Chem. C* **2020**, *124*, 25873–25883.
[CrossRef]

90. Pham, B.L.; Piard, A.; Erard, M.; Gayral, A.; Noblet, T.; Dreesen, L.; Humbert, C. Quantum efficiency of excitonic enhancement in nanosensors by rainbow nonlinear optical spectroscopy. In Proceedings of the French, Swiss and German Conference on Photochemistry, Photophysics and Photosciences CP2P'23, Mulhouse, France, 15–17 May 2023.

91. Takashima, K.; Furukawa, Y. Vibrational Stark effect (VSE) on the infrared spectrum of a poly(methyl methacrylate) thin film. *Vib. Spectrosc.* **2015**, *78*, 54–59. [CrossRef]

92. Andrews, S.S.; Boxer, S.G. Vibrational Stark Effects of Nitriles, I. Methods and Experimental Results. *J. Phys. Chem. A* **2000**, *104*, 11853–11863. [CrossRef]

93. Lambert, D.K. Vibrational Stark effect of adsorbates at electrochemical interfaces. *Electrochim. Acta* **1996**, *41*, 623–630. [CrossRef]

94. Kang, B.J.; Rohwer, E.J.; Rohrbach, D.; Zyaee, E.; Akbarimoosavi, M.; Ollmann, Z.; Sorohhov, G.; Borgoo, A.; Cascella, M.; Cannizzo, A.; et al. Time-resolved THz Stark spectroscopy of molecules in solution. *Nat. Commun.* **2024**, *15*, 4212. [CrossRef] [PubMed]

95. Hush, N.S.; Reimers, J.R. Vibrational Stark Spectroscopy. 1. Basic Theory and Application to the CO Stretch. *J. Phys. Chem.* **1995**, *99*, 15798–15805. [CrossRef]

96. Fica-Contreras, S.M.; Charnay, A.P.; Pan, J.; Fayer, M.D. Rethinking Vibrational Stark Spectroscopy: Peak Shifts, Line Widths, and the Role of Non-Stark Solvent Coupling. *J. Phys. Chem. B* **2023**, *127*, 717–731. [CrossRef] [PubMed]

97. Sorenson, S.A.; Patrow, J.G.; Dawlaty, J.M. Solvation Reaction Field at the Interface Measured by Vibrational Sum Frequency Generation Spectroscopy. *J. Am. Chem. Soc.* **2017**, *139*, 2369–2378. [CrossRef]

98. García Rey, N.; Dlott, D.D. Effects of water on low-overpotential CO₂ reduction in ionic liquid studied by sum-frequency generation spectroscopy. *Phys. Chem. Chem. Phys.* **2017**, *19*, 10491–10501. [CrossRef] [PubMed]

99. Verma, N.; Tao, Y.; Zou, W.; Chen, X.; Chen, X.; Freindorf, M.; Kraka, E. A Critical Evaluation of Vibrational Stark Effect (VSE) Probes with the Local Vibrational Mode Theory. *Sensors* **2020**, *20*, 2358. [CrossRef]

100. Bhattacharyya, D.; Videla, P.E.; Cattaneo, M.; Batista, V.S.; Lian, T.; Kubiak, C.P. Vibrational Stark shift spectroscopy of catalysts under the influence of electric fields at electrode–solution interfaces. *Chem. Sci.* **2021**, *12*, 10131–10149. [CrossRef] [PubMed]

101. Ge, A.; Videla, P.E.; Lee, G.L.; Rudshteyn, B.; Song, J.; Kubiak, C.P.; Batista, V.S.; Lian, T. Interfacial Structure and Electric Field Probed by in Situ Electrochemical Vibrational Stark Effect Spectroscopy and Computational Modeling. *J. Phys. Chem. C* **2017**, *121*, 18674–18682. [CrossRef]

102. Ong, S.; Zhao, X.; Eisenthal, K.B. Polarization of water molecules at a charged interface: Second harmonic studies of the silica/water interface. *Chem. Phys. Lett.* **1992**, *191*, 327–335. [CrossRef]

103. Zhao, X.; Ong, S.; Eisenthal, K.B. Polarization of water molecules at a charged interface. Second harmonic studies of charged monolayers at the air/water interface. *Chem. Phys. Lett.* **1993**, *202*, 513–520. [CrossRef]

104. Gonella, G.; Lütgebaucks, C.; de Beer, A.G.F.; Roke, S. Second Harmonic and Sum-Frequency Generation from Aqueous Interfaces Is Modulated by Interference. *J. Phys. Chem. C* **2016**, *120*, 9165–9173. [CrossRef]

105. Nagata, Y.; Mukamel, S. Electrical Double Layer Probed by Surface-Specific Vibrational Technique. *Chem* **2018**, *4*, 1484–1485.
[CrossRef]

106. Dalstein, L.; Chiang, K.-Y.; Wen, Y.-C. Surface Potential at Electrolyte/Air Interfaces: A Quantitative Analysis via Sum-Frequency Vibrational Spectroscopy. *J. Phys. Chem. B* **2023**, *127*, 4915–4921. [CrossRef]

107. Ohno, P.E.; Wang, H.-f.; Geiger, F.M. Second-order spectral lineshapes from charged interfaces. *Nat. Commun.* **2017**, *8*, 1032.
[CrossRef]
108. Wang, H.-F. Sum frequency generation vibrational spectroscopy (SFG-VS) for complex molecular surfaces and interfaces: Spectral lineshape measurement and analysis plus some controversial issues. *Prog. Surf. Sci.* **2016**, *91*, 155–182. [CrossRef]

109. Buessler, M.; Maruyama, S.; Zelenka, M.; Onishi, H.; Backus, E.H.G. Unravelling the interfacial water structure at the photocatalyst strontium titanate by sum frequency generation spectroscopy. *Phys. Chem. Chem. Phys.* **2023**, *25*, 31471–31480. [CrossRef] [PubMed]

110. Montenegro, A.; Dutta, C.; Mammetkuliev, M.; Shi, H.; Hou, B.; Bhattacharyya, D.; Zhao, B.; Cronin, S.B.; Benderskii, A.V. Asymmetric response of interfacial water to applied electric fields. *Nature* **2021**, *594*, 62–65. [CrossRef] [PubMed]

111. Darlington, A.M.; Jarisz, T.A.; DeWalt-Kerian, E.L.; Roy, S.; Kim, S.; Azam, M.S.; Hore, D.K.; Gibbs, J.M. Separating the pH-Dependent Behavior of Water in the Stern and Diffuse Layers with Varying Salt Concentration. *J. Phys. Chem. C* **2017**, *121*, 20229–20241. [CrossRef]

112. Seki, T.; Chiang, K.-Y.; Yu, C.-C.; Yu, X.; Okuno, M.; Hunger, J.; Nagata, Y.; Bonn, M. The Bending Mode of Water: A Powerful Probe for Hydrogen Bond Structure of Aqueous Systems. *J. Phys. Chem. Lett.* **2020**, *11*, 8459–8469. [CrossRef]

113. Seki, T.; Sun, S.; Zhong, K.; Yu, C.-C.; Machel, K.; Dreier, L.B.; Backus, E.H.G.; Bonn, M.; Nagata, Y. Unveiling Heterogeneity of Interfacial Water through the Water Bending Mode. *J. Phys. Chem. Lett.* **2019**, *10*, 6936–6941. [CrossRef]

114. Ohno, P.E.; Saslow, S.A.; Wang, H.-F.; Geiger, F.M.; Eisenthal, K.B. Phase-referenced nonlinear spectroscopy of the α-quartz/water interface. *Nat. Commun.* **2016**, *7*, 13587. [CrossRef] [PubMed]

115. Tan, J.; Wang, M.; Zhang, J.; Ye, S. Determination of the Thickness of Interfacial Water by Time-Resolved Sum-Frequency Generation Vibrational Spectroscopy. *Langmuir* **2023**, *39*, 18573–18580. [CrossRef]

116. Uddin, M.M.; Azam, M.S.; Hore, D.K. Variable-Angle Surface Spectroscopy Reveals the Water Structure in the Stern Layer at Charged Aqueous Interfaces. *J. Am. Chem. Soc.* **2024**, *146*, 11756–11763. [CrossRef]

117. Brown, M.A.; Goel, A.; Abbas, Z. Effect of Electrolyte Concentration on the Stern Layer Thickness at a Charged Interface. *Angew. Chem. Int. Ed.* **2016**, *55*, 3790–3794. [CrossRef]

118. Rehl, B.; Ma, E.; Parshotam, S.; DeWalt-Kerian, E.L.; Liu, T.; Geiger, F.M.; Gibbs, J.M. Water Structure in the Electrical Double Layer and the Contributions to the Total Interfacial Potential at Different Surface Charge Densities. *J. Am. Chem. Soc.* **2022**, *144*, 16338–16349. [CrossRef] [PubMed]

119. Humbert, C.; Busson, B.; Tadjeddine, A. Enhanced Stability of a Carbon Monoxide Monolayer Adsorbed on Platinum under Electrochemical Control Probed by Sum-Frequency Generation Spectroscopy. *J. Phys. Chem. C* **2016**, *120*, 16211–16220. [CrossRef]

120. Xu, P.; von Rueden, A.D.; Schimmenti, R.; Mavrikakis, M.; Suntivich, J. Optical method for quantifying the potential of zero charge at the platinum-water electrochemical interface. *Nat. Mater.* **2023**, *22*, 503–510. [CrossRef] [PubMed]

121. Auer, A.; Ding, X.; Bandarenka, A.S.; Kunze-Liebhäuser, J. The Potential of Zero Charge and the Electrochemical Interface Structure of Cu(111) in Alkaline Solutions. *J. Phys. Chem. C* **2021**, *125*, 5020–5028. [CrossRef] [PubMed]

122. Mohandas, N.; Bawari, S.; Shibuya, J.J.T.; Ghosh, S.; Mondal, J.; Narayanan, T.N.; Cuesta, A. Understanding electrochemical interfaces through comparing experimental and computational charge density-potential curves. *Chem. Sci.* **2024**, *15*, 6643–6660. [CrossRef]

123. Chen, Q.-S.; Solla-Gullón, J.; Sun, S.-G.; Feliu, J.M. The potential of zero total charge of Pt nanoparticles and polycrystalline electrodes with different surface structure: The role of anion adsorption in fundamental electrocatalysis. *Electrochim. Acta* **2010**, *55*, 7982–7994. [CrossRef]

124. Cuesta, A. Measurement of the surface charge density of CO-saturated Pt(111) electrodes as a function of potential: The potential of zero charge of Pt(111). *Surf. Sci.* **2004**, *572*, 11–22. [CrossRef]

125. Huang, J.; Malek, A.; Zhang, J.; Eikerling, M.H. Non-monotonic Surface Charging Behavior of Platinum: A Paradigm Change. *J. Phys. Chem. C* **2016**, *120*, 13587–13595. [CrossRef]

126. Xu, P.; Huang, A.; Suntivich, J. Phase-Sensitive Second-Harmonic Generation of Electrochemical Interfaces. *J. Phys. Chem. Lett.* **2020**, *11*, 8216–8221. [CrossRef] [PubMed]

127. Sebastián-Pascual, P.; Sarabia, F.J.; Climent, V.; Feliu, J.M.; Escudero-Escribano, M. Elucidating the Structure of the Cu-Alkaline Electrochemical Interface with the Laser-Induced Temperature Jump Method. *J. Phys. Chem. C* **2020**, *124*, 23253–23259. [CrossRef]

128. Ding, X.; Sarpey, T.K.; Hou, S.; Garlyyev, B.; Li, W.; Fischer, R.A.; Bandarenka, A.S. Prospects of Using the Laser-Induced Temperature Jump Techniques for Characterisation of Electrochemical Systems. *ChemElectroChem* **2022**, *9*, e202101175. [CrossRef]

129. Ledezma-Yanez, I.; Wallace, W.D.Z.; Sebastián-Pascual, P.; Climent, V.; Feliu, J.M.; Koper, M.T.M. Interfacial water reorganization as a pH-dependent descriptor of the hydrogen evolution rate on platinum electrodes. *Nat. Energy* **2017**, *2*, 17031. [CrossRef]

130. Ganassin, A.; Sebastián, P.; Climent, V.; Schuhmann, W.; Bandarenka, A.S.; Feliu, J. On the pH Dependence of the Potential of Maximum Entropy of Ir(111) Electrodes. *Sci. Rep.* **2017**, *7*, 1246. [CrossRef]

131. Rebollar, L.; Intikhab, S.; Zhang, S.; Deng, H.; Zeng, Z.; Snyder, J.D.; Tang, M.H. On the relationship between potential of zero charge and solvent dynamics in the reversible hydrogen electrode. *J. Catal.* **2021**, *398*, 161–170. [CrossRef]

132. Attard, G.A.; Ahmadi, A. Anion—Surface interactions Part 3. N₂O reduction as a chemical probe of the local potential of zero total charge. *J. Electroanal. Chem.* **1995**, *389*, 175–190. [CrossRef]

133. Zhao, X.; Ong, S.; Wang, H.; Eisenthal, K.B. New method for determination of surface pKa using second harmonic generation. *Chem. Phys. Lett.* **1993**, *214*, 203–207. [CrossRef]

134. Gragson, D.E.; McCarty, B.M.; Richmond, G.L. Ordering of Interfacial Water Molecules at the Charged Air/Water Interface Observed by Vibrational Sum Frequency Generation. *J. Am. Chem. Soc.* **1997**, *119*, 6144–6152. [CrossRef]