# High Performance Zinc Oxide Nanorod-Doped Ion Imprinted Polypyrrole for the Selective Electrosensing of Mercury II Ions

Zouhair Ait-Touchente, Houssem Eddine El Yamine Sakhraoui, Najla Fourati, Chouki Zerrouki, Naima Maouche, Nourdin Yaakoubi, Rachid Touzani, Mohamed Chehimi

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Zouhair Ait-Touchente, Houssem Eddine El Yamine Sakhraoui, Najla Fourati, Chouki Zerrouki, Naima Maouche, et al. High Performance Zinc Oxide Nanorod-Doped Ion Imprinted Polypyrrole for the Selective Electrosensing of Mercury II Ions. Applied Sciences, 2020, 10 (19), pp.7010. 10.3390/app10197010. [hal-02991833](https://hal-02991833)

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Article

High Performance Zinc Oxide Nanorod-Doped Ion Imprinted Polypyrrole for the Selective Electrosensing of Mercury II Ions

Zouhair Ait-Touchente <fnref n="1" />,*, Houssem Eddine El Yamine Sakhraoui <fnref n="2" /> ID, Najla Fourati <fnref n="3" />,*, CNRS, IN2P3, UMR CNRS 8029, Cnam, 75003 Paris, France; zerrouki@cnam.fr
Chouki Zerrouki <fnref n="3" />, Naima Maouche <fnref n="2" />, Nourdin Yaakoubi <fnref n="4" />, Rachid Touzani <fnref n="1" /> ID and
Mohamed M. Chehimi <fnref n="5" />,*, ID

Received: 3 September 2020; Accepted: 30 September 2020; Published: 8 October 2020

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**Abstract:** A biomimetic, ion-imprinted polymer (IIP) was prepared by electropolymerization of pyrrole at the surface of gold electrodes decorated with vertically grown ZnO nanorods. The vertical growth of the nanorods was achieved via an ultrathin aryl monolayer grafted by reduction of diazonium salt precursor. Pyrrole was polymerized in the presence of L-cysteine as chelating agent and Hg<fnref n="2" />⁺ (template). Hg<fnref n="2" />⁺-imprinted polypyrrole (PPy) was also prepared on a bare gold electrode in order to compare the two methods of sensor design (Au-ZnO-IIP vs. Au-IIP). Non-imprinted PPy was prepared in the same conditions but in the absence of any Hg<fnref n="2" />⁺ template. The strategy combining diazonium salt modification and ZnO nanorod decoration of gold electrodes permitted us to increase considerably the specific surface area and thus improve the sensor performance. The limit of detection (LOD) of the designed sensor was ~1 pM, the lowest value ever reported in the literature for gold electrode sensors. The dissociation constants between PPy and Hg<fnref n="2" />⁺ were estimated at [K<sub>d1</sub> = (7.89 ± 3.63) mM and K<sub>d2</sub> = (38.10 ± 9.22) pM]. The sensitivity of the designed sensor was found to be 0.692 ± 0.034 µA.pM<sup>-1</sup>. The Au-ZnO-IIP was found to be highly selective towards Hg<fnref n="2" />⁺ compared to cadmium, lead and copper ions. This sensor design strategy could open up new horizons in monitoring toxic heavy metal ions in water and therefore contribute to enhancing environmental quality.

**Keywords:** ionic imprinted polypyrrole; zinc oxide nanorods; mercury ions; diazonium salts; electrochemical sensor

1. Introduction

One of the most serious problems affecting water is chemical pollution by organic or inorganic compounds such as pesticides and heavy metals, respectively. Among the inorganic pollutants, mercury (II) presents several health and ecosystem concerns [1–4]. Mercury is released into the environment in large quantities through waste from thermal power plants, cement kilns, chlor-alkali plants, gold mining and trash incinerators (hazardous waste, medical waste, regular garbage, etc.) [5–8]. Exposure to mercury ions, even at low doses, can lead to severe central nervous system problems and vital human organ damage [2,8–11]. The discharge of mercury into the environment is forbidden

<footnote n="1">1 LCAE-FSO, Université Mohammed Premier, Oujda 60000, Morocco; r.touzani@ump.ac.ma</footnote>

<footnote n="2">2 Laboratoire d'Electrochimie et Matériaux, Université Ferhat Abbas, Sétif-1 19000, Algeria; h_sakhraoui@hotmail.com (H.E.E.Y.S.); nmaouche@univ-setif.dz (N.M.)</footnote>

<footnote n="3">3 SATIE, UMR CNRS 8029, Cnam, 75003 Paris, France; zerrouki@cnam.fr</footnote>

<footnote n="4">4 LAUM, UMR CNRS 6613, Le Mans Université, 72085 Le Mans, France; nourdin.yaakoubi@univ-lemans.fr</footnote>

<footnote n="5">5 ICMPE, UMR CNRS 7182, CNRS, 94320 Thiais, France</footnote>

<footnote>* Correspondence: zouhair.aittouchente@gmail.com (Z.A.-T.); fourati@cnam.fr (N.F.); chehimi@icmpe.cnrs.fr (M.M.C.); Tel.: +33-6-63-05-46-08 (M.M.C.)</footnote>
by the United States Environmental Protection Agency (USEPA), European Union (EU) and World Health Organization (WHO). The environmental monitoring of mercury is very much important to avoid any further damage to the ecosystem [12]. The WHO has set a maximum permissible limit of (1 µg·L⁻¹/5 nM) for mercury [13]. Developing reliable, sensitive and selective methods for the determination of mercury concentrations in food and drinking water is thus of particular significance.

Electrochemical sensors [4,14–17] are an excellent alternative combining miniaturization, speed and low cost. Field analysis of metal pollutants (even within a processing plant, for example) will be possible thanks to portable, wireless and ultra-sensitive potentiostats [18].

Ion imprinted polymers (IIPs) constitute a new class of sorbents possessing selectivity and affinity for the separation, pre-concentration or removal of target ions [14,16,19–21]. IIPs are prepared by the formation of specific recognition sites in the framework of organic polymers and usually prepared by the bulk polymerization method [16,22]. Template ions are then removed, leaving cavities or “artificial receptor sites” in the polymer layer that have appropriate shape, size and orientation of the functional groups for ion recognition at the rebinding stage [23–25]. For this reason, imprinted polymers are coined “plastic antibodies” for their ability to mimic antibodies. One of the most common applications of IIPs is solid phase extraction (SPE), which permits the pre-concentration of metal ions traces in environmental samples like natural water or seawater [26–28]. IIPs as electrochemical sensors have shown remarkable selectivity, good thermal stability, low cost and excellent sensitivity [29–34].

The current challenge for most scientific researchers is to improve the performance of electrochemical sensors, including the limit of detection, in order to detect heavy metal ions at trace levels and by using very simple and inexpensive methods. To address this issue, we reasoned to increase the electroactive surface using nanoparticles to form a nanostructured sensing layer [35,36].

Zinc oxide is considered to be a very important functional oxide among many semiconductor metal oxides [37] and, more generally, is one of the most used materials in applied sciences currently. It is a semiconductor; its wurtzite structure has a wide band gap (Eg = 3.37 eV at 300 K) and a large exciton binding energy (60 meV) [38,39]; it has excellent biocompatibility, good chemical/thermal stability, mixed chemical bonds (covalent/ionic) [37], and it excellent properties allow it to be used in many applications as a nanomaterial, including in Gratzël cells [40], varistors [41], optical waveguides [42] and in many optoelectronic devices [38,43]. In addition to these applications, ZnO is widely used in the field of sensors, i.e., gas and heavy metal ion sensors [37,44–50].

ZnO thin films are prepared by many techniques such as chemical vapor deposition [51], spray pyrolysis [52], DC-sputtering [53], pulsed laser deposition [54], radiofrequency (RF) magnetron sputtering [55], pulsed laser deposition [56], electro-deposition [57] and sol–gel-dip-coating [58]. The low temperature chemical method [59–61] investigated herein is one of the most used techniques [47,53,59–61] for the preparation of thin films of ZnO due to its simplicity and operation at low temperatures. This method is carried out in three steps, (i): synthesis of ZnO NPs, (ii): deposition of NPs by spin-coating on gold electrodes, and (iii): growth of ZnO NRs) and rests on the use of ZnO NPs as a seed layer to nucleate the growth process of ZnO NRs. This hydrothermal/chemical method is advantageous due to its low cost and the fact that it facilitates control over the density and overall orientation of nanorod arrays and permits control of the morphology of ZnO by varying the growth conditions such as growth time [61] and temperature [62].

In two recent conference proceedings [63,64], we have proposed to combine the advantage of diazonium surface modification for the vertical growth of ZnO nanorods and sensing properties of polypyrrole. In this follow-up, we provide an in-depth study targeting the ultimate detection limit using ZnO nanorod-embedded ion imprinted polypyrrole. Besides the central role of diazonium modification of the working electrode for the growth of vertically aligned ZnO nanorods, such surface chemistry ensures robust adhesion of the polypyrrole sensing layer [65]. This strategy of gathering the salient features of diazonium salts, ZnO nanorods and ion imprinting of polypyrrole has never been reported before, with the exception of our short proceedings papers [63,64]. We believe it has much to
offer to the surface scientist in the quest of constructing a robust electrochemical sensor to address environmental issues.

Herein, a polypyrrole-based IIP was prepared in the presence of $Hg^{2+}$ as a template and L-cysteine as a chelatant agent deposited on a gold electrode sequentially functionalized with diazonium salts and nanostructured with ZnO nanorods in order to have very high roughness for the selective removal of mercury ions in a sample medium (KCl solution). For comparison, an IIP on a bare gold electrode was prepared. A non-imprinted polymer was also prepared in the same conditions of IIP but in the absence of any $Hg^{2+}$. Electropolymerization time, incubation time and number of cycles of electroreduction of diazonium salts were investigated and optimized. Electrode sensing materials were characterized by atomic force microscopy (AFM) in order to account for the morphological structures of the nanocomposites. Square wave voltammetry (SWV) experiments permitted us to determine the optimal parameters for sensing $Hg^{2+}$, namely linear response range and the limit of detection of the ZnO-IIP sensor. Selectivity and competition between mercury and other ions was investigated by examining the electrochemical responses in the presence of copper, lead and cadmium taken as interfering metal ions.

## 2. Materials and Methods

### 2.1. Reagents

First, 4-Aminobenzoic acid (≈99%), methanol (MeOH), $H_2SO_4$ (95%), $H_2O_2$ (30%), tetrabutylammonium tetrafluoroborate (99%), zinc acetate dihydrate (99.99%), sodium hydroxide (≈97%), hexamethylenetetramine (99%), acetonitrile (99.8%), potassium hexacyanoferrate(III) (≈99%), potassium hexacyanoferrate(II) trihydrate (≈98.5%), potassium chloride, pyrrole (Py) (98%), lead nitrate $Pb(NO_3)_2$, copper(II) nitrate hemi(pentahydrate) (98%) and mercury(II) chloride (≈98%) were purchased from Sigma-Aldrich (Saint-Quentin-Fallavier, France). Pyrrole was purified through an alumina basic column and then stored in dark at 4 °C. Cadmium sulfate 8/3-hydrate (≈99%) was supplied by VWR Prolabo (Fontenay-sous-Bois, France).

Zinc nitrate hexahydrate (≈99%) was obtained from Merck (Fontenay-sous-Bois, France), and isopentyl nitrite (≈97%) was supplied by Alfa Aesar (Heysham, UK). The organic solvents used were of analytical grade and all aqueous solutions were prepared using ultrapure milli-Q water.

### 2.2. Instruments and Characterization

All electrochemical measurements were carried out with a Bio-Logic portable potentiostat (model PG581). Conventional three-electrode cell was used. A silver chloride electrode (SSC, +0.222 V vs. SHE), a platinum grid and a gold substrate were the reference, counter and working electrodes, respectively.

Topographical characterization was performed by atomic force microscopy (AFM, MFP-3 Asylum Research). X-ray photoelectron spectroscopy (XPS) analyses were conducted using a K Alpha apparatus (Thermo Fisher Scientific, East Grinsted, UK) fitted with an Al monochromatic X-ray source (1486.6 eV; spot size = 400 µm). A flood gun was used for charge compensation.

### 2.3. Surface Functionalization with Diazonium Salt

In order to mitigate the impurities likely to be present on the surface of the gold electrode and which can subsequently alter the quality of the surface modification, the gold substrates were cleaned with acetone in 10 min and then in a mixture of piranha (98% $H_2SO_4$/30% $H_2O_2$ 2:1 V/V) for 20 and 10 min in ethanol. We then washed the gold electrodes thoroughly with distilled water and dried them at 60 °C.

The surface modification was carried out by electrografting of 4-carboxybenzene-diazonium-tetrafluoroborate (previously prepared [66] and characterized by FTIR and carbon-13 NMR) on gold electrodes by cyclic voltammetry at scan rate of 100 mV/s between -1.0 and 0.0 V/SSC for 20 cycles, in acetonitrile solution, containing 1 mM of diazonium salt and 0.1 M of tetrabutylammonium
tetrafluoroborate. The modified electrodes were then rinsed with ultrapure water and ethanol and dried. The number of cycles was optimized and controlled using ferrocyanide redox probe.

## 2.4. Synthesis, Deposition and Vertical Growth of ZnO

The ZnO grafting procedure was performed in three steps by the low temperature method (Mekki et al. [47], Pacholski et al. [60]; Chander and Raychaudhuri [61]): (i) synthesis of ZnO nanoparticles from zinc acetate [Zn(CH3COO)2] and sodium hydroxide (NaOH), (ii) deposition of these nanoparticles on the surface and (iii) the vertical growth of the ZnO nanorods.

### 2.4.1. Nanoparticle Synthesis

Zinc acetate [Zn(CH3COO)2]. 2H2O] is among the most widely used precursors in several syntheses, including the synthesis of zinc oxide (ZnO) nanoparticles [62,67]. In this work, 0.1 M [Zn(CH3COO)2]. 2H2O] was reacted with 0.03 M (NaOH) in methanol under stirring and heating at 60 °C. The various synthesis steps carried out are detailed below.

The first step corresponds to the dissolution of [Zn(CH3COO)2]. 2H2O] in methanol (CH3OH). The second step is a chemical reaction between the species present in the solution to form the precipitation of metal hydroxide. The last step is the heat treatment to convert the zinc hydroxide particles to zinc oxide.

$$Zn(CH_3COO)_2 + CH_3-CH_2-OH \rightarrow Zn^{2+} + 2 CH_3COO^-$$

The sodium hydroxide dissolves in the solution to give Na+, which will bind to the acetate; the OH- group will precipitate with the Zn2+ which is in the solution, before obtaining the zinc monoxide, which has a white color.

$$Zn^{2+} + 2 OH^{-} \rightarrow Zn(OH)_2 \downarrow$$

$$Zn(OH)_2 \rightarrow ZnO + H_2O$$

### 2.4.2. Deposition of ZnO Nanoparticles on Aryl-Modified Gold Electrodes

After synthesis, ZnO nanoparticles were deposited on the modified gold electrode (Au-diazo) by spin-coating to serve as a germination layer for the nucleation process during the growth of ZnO nanorods. These electrodes were dried in the oven at 125 °C for one hour before proceeding to the growth step.

### 2.4.3. Vertical Growth of ZnO Nanorods

For the nanorod growth step, the ZnO NP-coated arylated gold substrates were immersed in a beaker containing a 30 mM solution of the zinc nitrate hexahydrate [Zn(NO3)2. 6H2O] and 30 mM hexamethylenetetramine (HMT) dissolved in 200 mL of distilled water; the mixture was kept at 95 °C for 5 h with constant stirring. Since the particles act as a nucleation site, after the five hours of growth, the samples were removed from solution, rinsed with distilled water and dried (for 1 h at 125 °C).

## 2.5. Preparation of Au-IIP, Au-ZnO-IIP and Au-ZnO-NIP

Two different IIPs were prepared. The first one was made on a bare gold electrode and the second one was prepared on a gold electrode modified with diazonium salt and ZnO nanorods. These two configurations were carried out in two steps; for the first, a thin PPy barrier layer was deposited by chronoamperometry for 2 s at an applied potential of 1.05 V (vs Ag/AgCl) in a KCl solution containing 10-2 M of purified pyrrole (monomer) and 10-4 M of L-cysteine; the second step involved 8 s in a KCl solution containing 10-2 M of purified pyrrole, 10-4 M of L-cysteine and 10-3 M of Hg2+ (template). These different steps were carried out by chronoamperometry at an applied potential of
1.05 V (vs. Ag/AgCl). The non-imprinted polymer (Au-ZnO-NIP) was also prepared under the same conditions in the absence of any Hg²⁺ ion template.

## 2.6. *Choice and Role of the Chelating Agent*

The formation of mercury receptor sites in the ZnO-IIP was achieved using L-cysteine, a chelator of mercury. This choice was driven by the thiophilicity of metal ions [68–70] and especially high affinity of L-Cys for Hg²⁺ [71]. L-cysteine is an ideal compound, bearing electron-rich functional groups such as -NH₂, -COOH and -SH, which allow it to have a Hg-cysteine complex [72–74]. The incorporation of L-cysteine/Hg²⁺ into polypyrrole is likely to take place via electrostatic bonds between the carboxylic group of L-cys and the nitrogen of pyrrole (Scheme 1) [74].

<figure><img src="image_4.png" /><figcaption>**Scheme 1.** Schematic representation of Hg²⁺ complexation by L-cysteine in the polypyrrole layer.</figcaption></figure>

## 2.7. *Electrochemical Measurements*

The comparison between the prepared configurations, the Hg²⁺ detection tests, selectivity, competition between Hg²⁺ and other ions was controlled by square wave voltammetry between -0.95 and 0.95 V under the following conditions: E-pulse: 0.01 V, E-step: 0.01 V, frequency: 25 Hz, equilibration time: 2 s. After each use, the IIP was extracted for 20 min in EDTA and then 10 min in ultra-pure water with gentle stirring. Once the IIP was extracted, it could be used another time.

# 3. Results and Discussion

## 3.1. *Surface Functionalization by 4-Carboxybenzenediazonium Tetrafluoroborate and Quasi-Vertical Growth of ZnO*

Scheme 2 displays the general three-step design of IIPs. To do so, we functionalized the surface of the gold electrode with carboxyphenyl groups from the corresponding diazonium salt (Scheme 2A, (1)) and then deposited (by spin-coating) ZnO nanoparticles for the vertical growth of the ZnO nanorods (Scheme 2A, (2)). The second step consisted of the formation of the ion-imprinted polypyrrole by electropolymerization of the pyrrole in the presence of L-cysteine (chelator) and Hg²⁺ template (Scheme 2B).

The different steps followed for the formation of ionic cavities are illustrated in Scheme 2C [75]. Removal of the template by washing, adapted to the nature of the functional monomer–template bond, leaves artificial sites capable of selective rebinding of the template.
<figure><img src="image_5.png" /><figcaption>**Scheme 2.** Schematic illustration of experimental procedures. (A): Design of ZnO nanorods, (B): design of the ion imprinted polymer and (C): principle of formation of an artificial receptor within a polymer matrix for hosting metal ion template at the rebinding step.</figcaption></figure>

The electroreduction of the diazonium salt carried out by cyclic voltammetry in 20 cycles in the range -1.0 to 0.0 V (vs. Ag/AgCl) gave a virtually zero reduction current (Figure 1A) resulting from a passivation of the electrode following the grafting of diazonium groups (formation of gold-diazo covalent bonds). The electroreduction peak is centered at -0.2 V (vs. Ag/AgCl). This step of surface functionalization by the diazonium salt makes it possible to tether ZnO NPs to the surface on the one hand and enables vertical growth of ZnO NRs on the other hand. We have shown in a previous work that the growth of ZnO NRs on a surface not modified by diazonium salts gives an orientation of the NRs in all directions and in a random manner [47].

<figure><img src="image_6.png" /><figcaption>**Figure 1.** Cyclic voltammograms corresponding to the electrografting of 4-carboxybenzenediazonium tetrafluoroborate. (A) Electroreduction, (B) passivation test in H₂O/KCl 0.1 M solution, containing 0.01 M of K₃[Fe(CN)₆] and 0.01 M of K₄[Fe(CN)₆]: (1): as-received gold electrode; (2): cleaned electrode and (3): after electrografting of the diazonium salt. Scan rate: 100 mV/s, 20 cycles for electrografting.</figcaption></figure>
Passivation of the electrode was followed by cyclic voltammetry in the presence of 0.01 M of K₃[Fe(CN)₆] and 0.01 M of K₄[Fe(CN)₆]. Results presented in Figure 1B indicate that the electrode was passivated while keeping its conductive character (Figure 1B, red). The diazonium salt step makes it possible to achieve an almost homogeneous distribution of quasi-vertical growth of ZnO nanorods [47].

## 3.2. Preparation of IIP and NIP-Based Electrodes

Mercury oxidation on gold electrodes yields two peaks: the first peak is attributed to the oxidation reaction of Hg(0) to Hg(I) (in the form Hg₂²⁺) while the second peak is due to the transformation of Hg(I) into Hg²⁺ [68,76,77]:

$$1/2\text{Hg}_2^{2+} \rightarrow \text{Hg}^{2+} + \text{e}^{-} \quad (\text{or } \text{Hg(I)} \rightarrow \text{Hg(II)} + \text{e}^{-})$$

Before preparing the films on gold electrodes, we first characterized the signature of mercury with a gold disk working electrode in a solution containing mercury and KCl 0.1 M. The response obtained by SWV shows that the oxidation of mercury on gold gives two peaks at 0.061 and 0.71 V (vs. Ag/AgCl) (Figure 2). The position of the two peaks depends on the pH of the solution, the nature of the working electrode, the electrolyte and the layer or film deposited on gold. In the following, we will consider the most intense peak located at 0.71 V (vs. Ag/AgCl), which corresponds to Hg²⁺. This dominant peak means that most of the mercury is converted to Hg²⁺.

<figure><img src="image_7.png" /><figcaption>**Figure 2.** Characteristic peaks of mercury oxidation on gold electrode in H₂O/KCl 0.1 M solution. Conditions: E-pulse: 0.01 V, E-step: 0.01 V, frequency: 25 Hz, equilibration time: 2 s.</figcaption></figure>

A thin PPy barrier layer was deposited by chronoamperometry (CA) for 2 s before Au-ZnO-IIP electro-formation to prevent the complexation of mercury by Au-ZnO electrodes (Figure 3A, black curve). Both ZnO-IIP and ZnO-NIP were prepared by the same technique (Figure 3A, red curve) and then compared using SWV (Figure 3B). On the one hand, one can notice the obvious difference between the responses of ZnO-IIP and ZnO-NIP, i.e., mainly for the peak current corresponding to a potential of around 0.62 V (vs. Ag/AgCl) in the case of ZnO-IIP will be considered for quantitative monitoring of mercury. On the other hand, the removal of Hg²⁺ from ZnO-IIP by EDTA leads to a flat SWV response, close to that of ZnO-NIP (Figure 3B). This means that all receptor sites have been released and thus can be reused for rebinding the target ions.
<figure><img src="image_8.png" /><figcaption>**Figure 3.** (A): Electropolymerization of pyrrole by chronoamperometry at a constant potential of 1.05 V/SSC. (black) Barrier layer, (red) Polymerization of pyrrole in the presence of L-cysteine and Hg²⁺ (B): square wave voltammetry (SWV) of IIP and NIP in H₂O/KCl 0.1 M solution.</figcaption></figure>

In order to showcase the central role of ZnO nanorods, we prepared two different IIPs: the first was prepared directly on a bare gold electrode and the second IIP was prepared on Au-ZnO. After extraction of the metal ions from these two IIPs in EDTA solution, they were incubated in 10⁻³ M mercury solution for 20 min for the rebinding test.

From the results displayed in Figure 4, one can notice the important role of ZnO NRs thanks to the spaces between the NRs. ZnO NRs will be considered as a substrate for depositing the polymer matrix instead of depositing it directly on the gold electrode.

<figure><img src="image_9.png" /><figcaption>**Figure 4.** SWV voltammograms in H₂O/KCl 0.1 M solution after incubation of Au/Hg-IIP and Au-ZnO/Hg-IIP in 10⁻³ M Hg²⁺. Conditions: E-pulse: 0.01 V, E-step: 0.01 V, frequency: 25 Hz, equilibration time: 2 s.</figcaption></figure>

Square wave voltammograms presented in Figure 4 show that the current intensity of the IIP prepared on ZnO nanorods is twice as high as that prepared on bare gold electrodes. Given that the surface area used on the bare gold electrode to form Au/Hg-IIP is identical to that used to form Au-ZnO/Hg-IIP, this can be related to the increase in the surface area thanks to ZnO nanorods, which makes it possible to deposit more IIP and thus a large number of artificial sites to capture more Hg²⁺ ions.

### 3.3. *Surface Analysis by XPS*

Figure 5 shows the survey spectra for the bare gold electrode, Au/diazo-COOH, Au-diazo-ZnO nanoparticles, Au-diazo-ZnO nanorods, ZnO-IIP and ZnO-NIP.
<figure><img src="image_10.png" /><figcaption>**Figure 5.** XPS survey scans of Au electrode, Au/diazo-COOH, Au-diazo-ZnO nanoparticles, Au-diazo-ZnO nanorods, ZnO-IIP and ZnO-NIP.</figcaption></figure>

Firstly, comparison of the XPS spectrum of bare gold electrode with Au/diazo-COOH confirms the effective reductive electrografting reaction of the diazonium salt on the gold electrode. Indeed, it is noticed the presence of characteristic signals of the diazo-COOH, namely C1s and N1s peaks centered at 285 eV and 400 eV, respectively (Figure 5). It should be noted that the surface-grafted layer seems to be relatively thin (less than 10 nm); this was also confirmed by the atomic percentages shown in Table 1. The atomic percentage of gold decreased from 41.6% for the bare gold electrode to 35.8% after electrografting of the diazonium salt, with a small increase in the percentage of carbon (grafting of the diazonium salt while keeping the conductive activity of the electrode).

<table><caption>**Table 1.** Surface chemical composition of Au electrode, Au/diazo-COOH, Au-diazo-ZnO nanoparticles, Au-diazo-ZnO nanorods, ZnO-IIP and ZnO-NIP nanocomposites as determined by XPS.</caption><thead><tr><th>Samples</th><th>Au</th><th>C</th><th>O</th><th>N</th><th>Zn</th><th>Hg</th></tr></thead><tbody><tr><td>Bare gold electrode</td><td>41.6</td><td>42.2</td><td>16.2</td><td>-</td><td>-</td><td>-</td></tr><tr><td>Au/diazo-COOH</td><td>35.8</td><td>45.9</td><td>14.3</td><td>3.97</td><td>-</td><td>-</td></tr><tr><td>Au-diazo-ZnO NPs</td><td>-</td><td>60.6</td><td>28.3</td><td>0.43</td><td>10.7</td><td>-</td></tr><tr><td>Au-diazo-ZnO NRs</td><td>0.87</td><td>32.3</td><td>38.5</td><td>0.97</td><td>27.4</td><td>-</td></tr><tr><td>ZnO-IIP</td><td>0.07</td><td>43.0</td><td>33.2</td><td>2.38</td><td>20.7</td><td>0.57</td></tr><tr><td>ZnO-NIP</td><td>1.61</td><td>43.5</td><td>33.3</td><td>2.95</td><td>18.7</td><td>-</td></tr></tbody></table>

After the deposition of ZnO nanoparticles by spin-coating, we have the appearance of a peak at 1022 eV which corresponds to the Zn2p<sub>3/2</sub> of ZnO (Figure 5), with an atomic percentage of 10.7%. After the ZnO growth step, the atomic percentages of zinc and oxygen increase (27.4% and 38.5%, respectively). We can also note a decrease in the peaks corresponding to the Au4f<sub>7/2</sub> and C1s signals (Figure 5), which confirms the success of the ZnO nanorods growth step.

Comparison of the XPS spectra of ZnO-IIP and ZnO-NIP (Figure 5) indicates the grafting of a polypyrrole film on the surface of the electrode. However, mercury is present only in the case of the IIP
material, which indicates that the template has been well trapped in the polymeric matrix. The atomic percentage of Zn for NIP and IIP decreased due to screening ZnO with polypyrrole (Table 1).

As per the thickness of the aryl layer, it was determined using the Beer–Lambert exponential decay of the intensity of bare gold:

$$I = I^{\circ} \exp(-d/\lambda \cos\theta)$$

where I is the peak intensity of Au4f$_{7/2}$ core level signal after coating, I° is the intensity for the bare gold, d is the aryl thickness, λ the mean free path of Au4f$_{7/2}$ in the aryl layer and θ the analysis angle (here, θ = 0, and cosθ = 1). The thickness is estimated to be 0.43 nm by considering λ to be around 4.1 nm, which, for a monolayer of aryl groups given the fact that the size of length of benzoic acid, is around 0.49 nm.

As will be shown below by AFM, ZnO NPs are large compared to the sampling depth (~2–10 nm) in XPS. For this reason, no gold is detected for Au-diazo-ZnO NPs. After growth of the NRs, Au4f doublet is detected again, which signifies that deposition of the NRs probably induces partial leaching of ZnO NPs, hence the escape of Au4f electrons between the NRs and their detection in XPS.

### 3.4. Topographical Characterization

The atomic force microscopy (AFM) measurements have been carried out in order to monitor the topographic changes after each surface functionalization step. The evidence of nanorod growth is not the purpose herein, that being clearly shown in a previous work [47]. Therefore, we can use standard tapping mode AFM probes instead of high aspect ratio ones. The robustness of the former allows comparative investigation of several samples’ surfaces without changing the probe. Two-dimensional AFM images of (5 × 5) µm$^2$ have thus been achieved on the same sample, before (bare gold substrate) and after each functionalization step (diazonium salt, ZnO nanoparticles, ZnO nanorods, then IIP) and finally after extraction of the Hg$^{2+}$ template (Figure 6).

<figure><img src="image_11.png" /><figcaption>**Figure 6.** The generated 5 × 5 µm$^2$ AFM images of (A) bare gold electrode, (B) gold electrode-diazonium salt, (C) Au/Diazo/ZnO nanoparticles, (D) Au/Diazo/ZnO nanorods, (E) Au/Diazo/ZnO NRs-IIP, (F) extracted Au/Diazo/ZnO NRs-IIP.</figcaption></figure>
The AFM images (Figure 6A–F) exhibit a granular-like aspect and seem different enough in both shape and size. The grafting of diazonium salt (Figure 6B) leads to the formation of a layer veiling the granular appearance. The latter is again visible (Figure 6C) after grafting the ZnO nanoparticles, with higher contrast than for the bare gold surface (Figure 6A). Figure 6D, which corresponds to ZnO nanorod growth, exhibits the largest size of surface singularities, which seems reduced by the electropolymerization of IIP (Figure 6E). The extraction of template from the IIP film (Figure 6F) leads to a different aspect that is probably due to the local rearrangement of the IIP.

Despite the usefulness of AFM images, qualitative description remains limited due to the high contrast that may exist in the presence of multiple defects with high amplitudes. Measurements should therefore be considered from a quantitative point of view by considering relevant roughness statistical parameters, such as rms roughness (Sq) and peak-valley height (Sp-Sv). Values of these two parameters are presented in Figure 7.

<figure><img src="image_12.png" /><figcaption>**Figure 7.** Root-mean-square height (Sq) and peak-valley height (Sp-Sv) values after the different functionalization steps, from bare gold substrate to electrosynthesis of IIP and the further extraction of the imprinted Hg<sup>2+</sup> template ions.</figcaption></figure>

As expected, each surface modification leads to a noticeable change in roughness parameters. The most important one occurs after diazonium salt grafting. This first step of functionalization led to an increase in (Sq) and (Sp-Sv) parameter values by a factor of 5.7 and 7.8, respectively. The increase in roughness continued with the grafting of ZnO NPs, but to a lesser extent, by a factor of 1.7 for (Sq), while the (Sp-Sv) value remains relatively stable. The growth of the nanorods generated a variation in the two considered parameters by a factor of 2.9 and 2.4, respectively. The electro-polymerization of IIP produced a coating effect resulting in a significant decrease in the values of the two roughness parameters by a factor of 4.7 for (Sq) and 3.3 for (Sp-Sv). These two parameters decreased by a factor of around 1.5 only, after the analyte extraction step. This slight decrease is probably due to the local rearrangements which occur once the Hg<sup>2+</sup> ions are extracted from the polymer matrix.

The corresponding 2D images of ZnO NPs (Figure 8a) and ZnO NRs (Figure 8b), show the dimensions of the ZnO NPs and NRs. The diameter of the NPs is between 70 and 80 nm, while that of the obtained NRs is in the range of 300–350 nm (the same diameter was obtained in our previous work [47]). Figure 8c,d represents 2D and 3D images for the same analysis area on a surface of (80 × 80 µm<sup>2</sup>). The growth of NRs is generally homogeneous, and the height after growth of NRs reaches 325 nm (Figure 8d).
<figure><img src="image_13.png" /><figcaption>**Figure 8.** Two/three-dimensional images of Au-diazo-ZnO NPs and Au-diazo-ZnO NRs. (a) Au-diazo-ZnO NPs with NPs diameter on (5 × 5 µm²) image, (b) NRs diameter on (5 × 5 µm²) image, (c) (80 × 80 µm²) 2D image of Au-diazo-ZnO NRs and (d) (80 × 80 µm²) 3D image of Au-diazo-ZnO NRs.</figcaption></figure>

### 3.5. Extraction Time in EDTA and Incubation Time in Mercury Solutions

Ethylenedinitrilo tetraacetic acid (EDTA) has been used in this work to extract mercury ions from the ZnO-IIP sensor. EDTA is an acid that is difficult to biodegrade. It is a stable chelator used in several applications, such as the medical field and the nuclear industry, but it is also used to adsorb heavy ions through functional groups, avoiding their precipitation [78–80]. Experiments (results not shown here) indicate that the optimum extraction was obtained by incubating the IIP in EDTA 0.1 M, for 20 min, and by then rinsing the films for 10 min in ultra-pure water.

The film obtained after extraction was incubated in a mercury solution (10⁻⁴ M) for different periods of time. Results presented in Figure 9 indicate that the number of Hg²⁺ ions captured by the sensor increased only slightly between 20 and 40 min, compared to the sharp increase between 5 and 20 min of incubation. For practical reasons, the incubation time was set to 20 min.
<figure><img src="image_14.png" /><figcaption>**Figure 9.** Hg-IIP response after different incubation times in 10⁻⁴ M mercury solution/H₂O/KCl 0.1 M.</figcaption></figure>

### 3.6. Electrochemical Sensing of Mercury

SWV was used to investigate the electrochemical response of the ZnO/Hg²⁺-IIP sensor towards mercury in solution at different concentrations. Sensor response was recorded, via the characteristic peak current, for concentrations between 10⁻¹² and 10⁻³ M (Figure 10).

The sensor limit of detection (LOD) was determined from the lowest concentration that gave a visible signal [81,82], instead of the method based on the signal to noise ratio of 3, as usually done. Here, the obtained LOD of 1 pM is much lower than the WHO maximum permissible limit in drinking water of (1 µg.L⁻¹).

To confirm the performance of the sensor, this Hg²⁺ detection step was conducted on three different ZnO/Hg²⁺-IIP, and the average calibration curve is shown in Figure 11 (variations of output signal of electrochemical IIP-based sensor versus Hg²⁺ concentrations).

<figure><img src="image_15.png" /><figcaption>**Figure 10.** Follow-up of peak current variations (determined from SWV measurements in H₂O/KCl 0.1 M solution) according to the potential. Conditions: E-pulse: 0.01 V, E-step: 0.01 V, frequency: 25 Hz, equilibration time: 2 s.</figcaption></figure>
<figure><img src="image_16.png" /><figcaption>Figure 11. Peak current variation versus Hg²⁺ concentration; electrochemical experimental data were fitted by a combined model (one binding site + Hill model). The inset is added to highlight the goodness of the fit according to the proposed model.</figcaption></figure>

The dissociation constant $K_d$ is an important parameter that determines the degree of affinity between the polymer and the template. Different analytical models were tested to fit the experimental data of the electrochemical measurements. The most appropriate one was a combination of the one site model and Hill model (Figure 11). The choice of this model makes it possible to take into consideration the mechanical restructuring of polymers at the nanometric scale [83].

$$Y(C) = \frac{A_1 \times C}{K_{d1} + C} + \frac{A_2 \times C^{\alpha}}{K_{d2}^{\alpha} + C^{\alpha}}$$

where y (C) is the output sensor's signal response (current) for a given concentration (C) of Hg²⁺. $K_{d1}$ and $K_{d2}$ are the first and second dissociation constants, $A_1$ and $A_2$ are empiric constants, and $\alpha$ is an empiric ponderation exponent. The values obtained for $K_{d1}$ and $K_{d2}$ were in the order of (7.9 ± 3.6) mM and (38.1 ± 9.2) pM, respectively. The value of $K_{d2}$ is consistent with that linked to the binding of Hg²⁺ to the Cys4 site in CP-CCCC peptide, which shows that the IIP can imitate biological entities in terms of affinity for heavy ions [71,83]. The $\alpha$ value of 0.06 ± 0.002, indicates positive cooperative interactions between Hg²⁺ ions and other binding sites [71].

The sensor sensitivity, computed from the slope at the origin of current/concentration curves (i.e., at lower concentrations), was in the order of 0.692 ± 0.034 µA.pM⁻¹. This value shows that this LCys-PPy sensor prepared on Au-ZnO to capture mercury is very sensitive compared to several sensors intended to detect heavy metals [84–86]. In addition to these interesting metrological features, we also tested the selectivity of the sensor by comparing the recognition of the targeted Hg²⁺ to lead, cadmium and copper ions. The rationale for this set of ions is the following: Cd²⁺ has an ionic radius close to that of Hg²⁺; Cu²⁺ has a lower ionic radius than Hg²⁺, whereas Pb²⁺ is a larger ion than the targeted Hg²⁺.

We first incubated the extracted film in a solution containing an ion of the chosen ions with a concentration of 10⁻⁴ M (Figure 12A). The second step was to mix several ions with Hg²⁺ with the same concentration of each ion (Figure 12B, black curve) and conduct another test in a solution containing Pb²⁺ and Hg²⁺ with a concentration of Pb²⁺ greater than 100 times that of Hg²⁺ (Figure 12B, red curve).
<figure><img src="image_17.png" /><figcaption>**Figure 12.** Evaluation of sensor's selectivity. (A): SWV curves in H₂O/KCl 0.1 M solution of ZnO/Hg(II)-IIP electrodes incubated in 10⁻⁴ M solutions of either mercury, cadmium, lead or copper ions for 20 min. (B): Competition tests. Conditions: E-pulse: 0.01 V, E-step: 0.01 V, frequency: 25 Hz, equilibration time: 2 s.</figcaption></figure>

The incubation of the extracted film each time in 10⁻⁴ M solution of a single chosen ion (Figure 12A) shows that ZnO-IIP is specific for Hg²⁺.

The competition tests (Figure 12B) were carried out by incubating the extracted film in a solution containing equal concentrations (10⁻⁴ M) of Cu²⁺, Hg²⁺ and Pb²⁺ ions. The tests have shown that in the presence of Cu²⁺ and/or Pb²⁺, the extracted film detects Hg²⁺ highly selectively. One can note the existence of some competition, since in Figure 12A, the height of the Hg²⁺ peak is 106 µA but slightly decreases to 94 µA in the presence of both Cu²⁺ and Pb²⁺ at the same concentration of 10⁻⁴ M (Figure 12B). If the Hg²⁺ concentration is decreased to 10⁻⁶ M, one can note a decrease in the height of the peak to 77 µA in the presence of 10⁻⁴ M Pb²⁺ (Figure 12B). Quantitatively speaking, there is a clear selectivity of the sensor to Hg²⁺; indeed, competition of other ions to the artificial receptors occurs but remains marginal. This is very important to prove, because in most fundamental studies, selectivity tests are usually conducted in single metal ion solutions and not in mixtures [87].

In a mixture containing 10⁻⁴ M of Pb²⁺ and 10⁻⁶ M of Hg²⁺, we note that despite the low concentration of mercury with the presence of other ions, the sensor remains specific to Hg²⁺, hence the importance of shaping the receptor sites with this template. This also shows that there is no competitive chemisorption of Pb²⁺ which hampers the response of the sensor to the Hg²⁺ ions.

The performance of the IIP sensors designed so far is compared to that of a number of other sensors described in the literature (Table 2). Embedding ZnO nanorods in the IIP film provided a unique LOD, as low as 1 pM.

<table><caption>**Table 2.** Comparison of the analytical performance of Au-ZnO/Hg-IIP to that of other handpicked relevant sensors reported in the literature.</caption><thead><tr><td>Electrode</td><td>Analytical Method</td><td>Electrolyte</td><td>LOD</td><td>Ref</td></tr></thead><tbody><tr><td>Glassy carbon electrode GC/SH/AuNPs</td><td>Square wave anodic stripping voltammetry (SWASV)</td><td>HCl solution</td><td>10 nM</td><td>[13]</td></tr><tr><td>Carbon-paste electrode (CPE)</td><td>Differential pulse voltammetry (DPV)</td><td>HCl solution</td><td>0.52 nM</td><td>[31]</td></tr></tbody></table>
<table><caption>**Table 2. Cont.**</caption><thead><tr><td>Electrode</td><td>Analytical Method</td><td>Electrolyte</td><td>LOD</td><td>Ref</td></tr></thead><tbody><tr><td>Glassy carbon electrode</td><td>Difference pulse voltammetry (DPV)</td><td>PBS (pH 7.0)</td><td>0.42 nM</td><td>[88]</td></tr><tr><td>Carbon-paste electrode (CPE)</td><td>Electrochemical Impedance Spectroscopy (EIS)</td><td>Nitrate solution</td><td>1.95 nM</td><td>[89]</td></tr><tr><td>Commercial screen-printed carbon electrode (SPCE)</td><td>Differential pulse voltammetry (DPV)</td><td>KNO<sub>3</sub>/HNO<sub>3</sub> solution (pH 2.7)</td><td>0.104 nM</td><td>[90]</td></tr><tr><td>Glassy carbon electrode</td><td>Square wave anodic stripping voltammetry (SWASV)</td><td>K<sub>3</sub>[Fe(CN)<sub>6</sub>] solution</td><td>0.1 nM</td><td>[91]</td></tr><tr><td>Carbon paste electrode (CPE)</td><td>Square wave anodic stripping voltammetry (SWASV)</td><td>HCl solution</td><td>18 pM</td><td>[92]</td></tr><tr><td>Glassy carbon electrode (GCE)</td><td>Differential pulse voltammetry (DPV)</td><td>PBS (pH 7.0)</td><td>0.2 µM</td><td>[93]</td></tr><tr><td>Carbon nanomaterials/AuNPs</td><td>Anodic stripping voltammetry (ASV)</td><td>KCl solution</td><td>0.03 µM</td><td>[94]</td></tr><tr><td>Mechanical Pencil Lead-NiS/Reduced Graphene Oxide</td><td>Anodic stripping voltammetry</td><td>PBS 1 mg/mL</td><td>0.8 nM</td><td>[95]</td></tr><tr><td>Platinum/(D) mordenite decorated modified glassy carbon electrode (GCE)</td><td>Cyclic voltammetry (CV)</td><td>KCl solution</td><td>3.4 nM</td><td>[96]</td></tr><tr><td>Gold/polyethylene terephthalate (PET)</td><td>Differential pulse voltammetry</td><td>HNO<sub>3</sub>/KCl</td><td>2.49 nM</td><td>[97]</td></tr><tr><td>Zincophosphite NPs (NTOU4nano)/polyaniline (PANI)</td><td>Differential pulse voltammetry</td><td>PBS (pH 7.0)</td><td>3.49.10<sup>-11</sup> M</td><td>[98]</td></tr><tr><td>Zinc oxide nanorods grafted on a Gold electrode</td><td>Square Wave Voltammetry (SWV)</td><td>KCl solution</td><td>1 pM</td><td>This work</td></tr></tbody></table>

## 4. Conclusions

A new electrochemical sensor based on a biomimetic ion-imprinted polymer for the detection of mercury (II) traces was prepared on a gold electrode with a strategy based on the combination of the surface modification with a diazonium salt and the growth of ZnO nanorods followed by electropolymerization of the pyrrole in the presence of the template (Hg<sup>2+</sup>) and L-cysteine as crosslinker. These two steps (diazonium salt and ZnO nanorods) permitted us to increase the performance of the final sensor (Au-diazo-ZnO/IIP) in terms of selectivity and limit of detection (LOD), which is in the picomolar range. This is proven by investigating the performance of an IIP prepared directly on a bare gold electrode, without any surface modification and in the absence of any ZnO nanorods.

The fit of the electrochemical results obtained by the one site/Hill model allowed us to determine the dissociation constants $[K_d] = (7.89 \pm 3.63)$ mM and $K_d = (38.10 \pm 9.22)$ pM as well as the sensitivity, which was equal to $0.692 \pm 0.034$ µA.pM<sup>-1</sup>.

The competitivity and selectivity tests were undertaken using several ions such as Cu<sup>2+</sup>, Pb<sup>2+</sup> and Cd<sup>2+</sup>, taking into account the ionic radius and their concentration in an aqueous medium. IIP showed excellent ability to distinguish between mercury and different competitive ions even at
low concentrations. Au-diazo-ZnO/IIIP can therefore be used for environmental applications to detect mercury in the laboratory or for field analysis using a portable potentiostat.

**Author Contributions:** Conceptualization of the research work by Z.A.-T., N.F., C.Z.; Methodology by Z.A.-T., N.F., C.Z., M.M.C.; Validation by Z.A.-T., N.F., C.Z., R.T., M.M.C.; Formal Analysis by Z.A.-T., H.E.E.Y.S., N.F., C.Z., N.M., N.Y., M.M.C.; Writing of Original Draft was done by Z.A.-T., N.F., C.Z., M.M.C.; Writing: Review and Editing by Z.A.-T., H.E.E.Y.S., N.F., C.Z., N.M., N.Y., R.T., M.M.C.; Supervision: N.F., C.Z., R.T., M.M.C.; Funding Acquisition: N.F., C.Z., N.M., N.Y., R.T. All authors have read and agreed to the published version of the manuscript.

**Funding:** This research was funded by La Région Pays de Loire, grant No LMAC/MEMSAW (recipient: N.Y.) and by the Algerian Ministry of Higher Education and Scientific Research, grant number PNE 474 (recipient: H.E.E.Y.S.).

**Acknowledgments:** The authors are indebted to SATIE and ICMPE for internal financing to support the project.

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

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