# Phenolic Azobenzene as Ligand for Cation Complexation-Syntheses and Applications

Jan Hočevar, Jernej Iskra, Estelle Léonard

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Jan Hočevar, Jernej Iskra, Estelle Léonard. Phenolic Azobenzene as Ligand for Cation Complexation-Syntheses and Applications. Molecules, 2025, 30 (12), pp.2499. 10.3390/molecules30122499. hal-05104727

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Review

# Phenolic Azobenzene as Ligand for Cation Complexation—Syntheses and Applications

Jan Hočevar <fnref n="1" />, Jernej Iskra <fnref n="1" />* and Estelle Leonard <fnref n="2" />,<fnref n="2" />*

**Abstract:** Phenolic azobenzenes have garnered significant attention as functional materials due to their ability to undergo reversible photoisomerization and their potential for cation complexation. This review aims to provide a comprehensive overview of the recent developments in the synthesis, properties, and applications of phenolic azobenzene derivatives in cation binding and complexation. This article explores various synthetic strategies for the preparation of phenolic azobenzenes. Additionally, the mechanisms of cation complexation, including the role of the phenolic hydroxyl group and the azobenzene scaffold, are discussed, along with insights into the coordination chemistry involved. This review further examines the diverse applications of phenolic azobenzene complexes in fields such as ion sensing, catalysis, and biological and DSSC applications.

**Keywords:** phenol; azobenzene; photoisomerization; colorimetric sensors; DSSC dyes; cation complexes

## 1. Introduction

### 1.1. General Presentation of Azobenzenes and Phenolic Compounds

#### 1.1.1. Azobenzene Properties

Azobenzenes are organic molecules containing an azo (-N=N-) functional group linked to two benzene rings [1]. Their unique chemistry arises from their conjugated π-electron system, which affects their optical, electronic, and structural behaviour. One key chemical property of azobenzenes includes the fact that they exist in two isomeric forms, *trans* (E) and *cis* (Z), as shown in Figure 1.

<figure><img src="image_2.png" /><figcaption>**Figure 1.** Two isomeric forms of azobenzenes.</figcaption></figure>

The *trans* form is thermodynamically more stable, whereas the *cis* form has a higher energy and can revert to *trans* under thermal conditions [2]. The isomerization kinetics depend on substituents and solvent polarity. For example, electron-donating groups (-OH, -OCH₃) lower the *cis-to-trans* activation barrier [3]. They also affect the electronic distribution. Indeed, electron-donating groups (EDGs) (e.g., -OH, -NH₂) push electron

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

check for
updates

Academic Editor: Kiril B. Gavazov

Received: 7 May 2025

Revised: 23 May 2025

Accepted: 30 May 2025

Published: 6 June 2025

**Citation:** Hočevar, J.; Iskra, J.; Leonard, E. Phenolic Azobenzene as Ligand for Cation Complexation—Syntheses and Applications. *Molecules* **2025**, *30*, 2499. https://doi.org/10.3390/molecules30122499

**Copyright:** © 2025 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/).

<footnote n="1">¹ University of Ljublana, Faculty of Chemistry and Chemical Technology, Večna pot 113, 1000 Ljubljana, Slovenia; jernej.iskra@fkkt.uni-lj.si (J.I.)</footnote>

<footnote n="2">² Université de Technologie de Compiègne, ESCOM, TIMR, F-60200 Compiègne, France</footnote>

<footnote>* Correspondence: e.leonard@escom.fr</footnote>
density towards the azo bond, stabilizing the *trans* form and shifting absorption maxima to longer wavelengths (bathochromic shift). However, electron-withdrawing groups (EWGs) (e.g., *-NO*₂, *-CF*₃) pull electron density away, destabilizing the *π*-system and affecting light absorption properties [4]. Azobenzenes can undergo redox reactions [5], particularly one-electron reduction, forming radical intermediates. This reduction typically converts the azo (*-N=N-*) bond into a hydrazo (*-NH-NH-*) linkage [6–9] under acidic or catalytic conditions. Azobenzenes act as ligands in metal complexes, coordinating with transition metals such as Fe, Ru, and Pd. Their ability to form charge transfer complexes makes them valuable in organometallic catalysis [10]. For example (Figure 2), in 2016, cyclometallated azobenzene palladium(II) complexes where synthesized, characterized using electronic absorption spectroscopy and electrochemical studies [11]. In 2008, dicyclopalladated complexes were synthesized using azobenzene derivatives, where the palladium centres form five-membered chelate rings through orthometallation. These complexes were characterized by X-ray crystallography and computational methods, providing insights into their structural and electronic properties [12]. A series of arene ruthenium complexes containing *o*-sulfonamide azobenzene ligands was also synthesized. These complexes exhibited uncommon coordination patterns with an exocyclic *N=N* bond. Upon irradiation, they underwent *trans* → *cis* photoisomerization reversibly by thermal isomerization, with rates dependent on solvent, arene group, sulfonamide moiety, and azobenzene substitution [13].

<figure><img src="image_4.png" /><figcaption>**Figure 2.** Examples of azobenzene metal complexes from (a) [11], (b) [12], and (c) [13].</figcaption></figure>

### 1.1.2. Phenolic Properties

Phenolic compounds are aromatic molecules featuring one or more hydroxyl (*-OH*) groups attached to a benzene ring. Their chemical reactivity is largely determined by the electron-donating effects of the hydroxyl group and its ability to participate in various chemical transformations. Phenols are weak acids (pKa~9–11) and can donate protons to form phenoxide anions in basic solutions. The phenoxide ion (*-O*⁻) is more reactive than its neutral form. Phenols can be easily oxidized to quinones [14,15] (e.g., hydroquinone to benzoquinone), and such transformations are crucial in redox reactions, dye chemistry, and electron transport mechanisms. The oxidation rate depends on substituents and environmental pH. The hydroxyl group in phenols participates in hydrogen bonding [16], influencing solubility and physical data (melting and boiling points, for example). Strong hydrogen bonds make phenols more soluble in polar solvents. Phenolic *-OH* groups can coordinate with metal ions (*Fe*³⁺, *Cu*²⁺) [17], forming coloured metal complexes. For
example, Dalal Alhashmialameer and colleagues synthesized a series of iron(III) complexes supported by tetradentate amino-bis(phenolate) ligands. These complexes exhibit square pyramidal geometries, as confirmed by X-ray crystallography. They have been studied as catalysts for the formation of organic carbonates from CO₂ and epoxides. The Fe–O(phenolate) bond lengths range from approximately 1.8690(12) to 1.8805(12) Å, indicating strong iron–oxygen interactions [18]. Another example is detailed by Christopher M. Kozak and co-workers, who synthesized six new iron(III) diamine-bis(phenolate) complexes. These structures were elucidated through single-crystal X-ray diffraction (Figure 3) [19].

<figure><img src="image_5.png" /><figcaption>**Figure 3.** Phenolate metal coordinates from (a) ref [18] and (b) ref [19].</figcaption></figure>

Finally, the main properties are summarized in (Table 1).

<table><caption>**Table 1.** Main properties of two parts of hydroxyazobenzenes.</caption><thead><tr><td>Property</td><td>Azobenzenes</td><td>Phenolic Compounds</td></tr></thead><tbody><tr><td>Acid or Base Behaviour</td><td>Stable but protonated under strong acid conditions</td><td>Weak acids, form phenoxide anions in base conditions</td></tr><tr><td>Electronic Effects</td><td>Azo (-N=N-) bond conjugation influences absorption</td><td>-OH is electron-donating, affects reactivity</td></tr><tr><td>Photoisomerization</td><td>UV-visible light-induced trans-cis switching</td><td>No isomerization, but light can degrade phenols</td></tr><tr><td>Redox Chemistry</td><td>Reduced to hydrazo (-NH-NH-) under mild conditions</td><td>Oxidized to quinones in oxidative media</td></tr><tr><td>Electrophilic Substitution</td><td>Substituent-dependent reactivity</td><td>Highly activated towards substitution reactions</td></tr><tr><td>Metal Coordination</td><td>Forms transition metal complexes</td><td>Coordinates metal ions (e.g., Fe³⁺, Cu²⁺)</td></tr></tbody></table>

## 1.2. Objectives and Scope of This Review

This review focuses on phenolic azobenzenes, highlighting their reversible photoisomerization behaviour and utility in cation complexation. It aims to present a comprehensive summary of recent advancements in their synthesis, structural features, and functional
properties. This review explores diverse synthetic methodologies, emphasizing the role of the phenolic hydroxyl group and azobenzene scaffold in coordinating cations. Mechanical insights into complexation processes are examined alongside their relevance to coordination chemistry. Furthermore, this review outlines the key applications of phenolic azobenzene-cation complexes, particularly in ion sensing, catalysis, biological systems, and dye-sensitized solar cells (DSSCs), thereby defining their significance as multifunctional materials.

## 2. Chemistry of Phenolic Azobenzenes

### 2.1. *Structure and General Properties of Hydroxyazobenzenes*

Hydroxyl-azobenzenes are organic compounds featuring both hydroxyl (-OH) and azo (-N=N-) functional groups attached to benzene rings. The position of the hydroxyl group significantly influences their properties. In *para*-hydroxyazobenzene, for example, ground-state keto/enol tautomerism is observed, affecting its photochemical behaviour [20]. Upon excitation, the *trans*-keto form can isomerize to the *cis* configuration, with the tautomeric equilibrium and isomerization dynamics being solvent-dependent. In aqueous solutions, *para*-hydroxyazobenzene exhibits considerable keto/enol tautomerism in the ground state, leading to specific excited-state behaviours. Indeed, the excited-state intramolecular proton transfer (ESIPT) in *para*-hydroxyazobenzene involves a photoinduced tautomerization between azophenol and quinone-hydrazone forms. Upon UV excitation, the molecule can undergo an ultrarapid intramolecular proton transfer. In the ground state, p-HAB predominantly exists in the enol form, stabilized by intramolecular hydrogen bonding. Upon excitation, the proton transfer to the azo nitrogen occurs, forming the keto tautomer in the excited state [21]. The ESIPT process in p-HAB is influenced by solvent polarity and pH. Polar solvents and acidic conditions can stabilize the keto form, enhancing the ESIPT process. Conversely, in nonpolar solvents or under basic conditions, the enol form is favoured, and ESIPT is less prominent [22].

These characteristics make hydroxyazobenzenes valuable in applications such as light-driven optical switching and photoactive monomers in elastomers for light-sensitive actuators [23]. The infrared (IR) spectra of hydroxyazobenzene compounds [24] exhibit characteristic absorption bands corresponding to different functional groups, including hydroxyl (-OH), azo (-N=N-), and aromatic (-C=C-) vibrations. The characteristic (N=N) IR absorption bands for hydroxyazobenzene are typically observed around 1400–1450 cm⁻¹, but these bands can shift depending on substituents and conjugation with the benzene rings. Other bands (OH, aromatic CH, and CO) are usually observed. However, the exact peak positions and intensities may vary depending on the substituents present on the benzene rings and whether the hydroxyl group participates in intramolecular hydrogen bonding (e.g., with the azo group). Moreover, in the case of *o*-hydroxyazobenzene, it has been established by polarized IR spectra in the region of 4000–400 cm⁻¹ that the molecule of 4-chloro-2'-hydroxy-4'-pentyloxyazobenzene undergoes a spontaneous ordering in thin layers of 10–20 µm [25]. The broad absorption in this region can be attributed to plane-to-plane intermolecular interactions, driven by resonance-assisted hydrogen bonding (RAHB) involving intramolecular O–H···N hydrogen bonds [26].

The UV-visible spectroscopy of hydroxyazobenzenes is a crucial technique for studying their electronic properties and photochemical behaviour. These compounds typically exhibit strong absorption in the visible region due to the electronic π-π* transition of the conjugated azo (-N=N-) system, often accompanied by a weaker n-π* transition. The presence of a hydroxyl (-OH) group at the *ortho* or *para* position to the azo group significantly influences the absorption spectra due to mesomeric effects and intramolecular interactions, particularly hydrogen bonding. In acidic or basic media, these compounds can undergo
bathochromic or hypsochromic shifts due to changes in electron density and tautomeric equilibrium (equilibrium between the azo and hydrazone forms). These properties make hydroxyazobenzenes particularly interesting for applications as dyes, pH indicators, or photochromic materials. For example, (E)-3,4,6-trichloro-2-(p-diazenil)-phenol (t-DZH) can be deprotonated in t-DZ (Figure 4), and this transformation has a strong impact on *trans* → *cis* isomerization [27]. Moreover, these hydroxyazobenzenes can also reversibly photogenerate tuneable pH drops in water up to one pH unit amplitude upon illumination at 365 nm (Figure 4, grey arrows, [28]).

<figure><img src="image_6.png" /><figcaption>**Figure 4.** Molecular structures of t-DZH, c-DZH, t-DZ, and c-DZ with classical *trans* → *cis* isomerization (black arrows, [27]) or light-driven ionization (grey arrows, [28]).</figcaption></figure>

## 2.2. Solvatochromism and Complexation Effects of Azo-Schiff Bases and Hydroxyl-Azobenzenes

Phenolic azo-Schiff bases are a specialized class of ligands that incorporate phenolic, azo, and imine (-C=N-) functional groups, offering multiple coordination sites for metal cation complexation [29]. The phenolic OH group, in particular, plays a crucial role by donating electron density to metal centres, often enhancing complex stability through hydrogen bonding or deprotonation to form phenolate ions [30]. This multi-dentate coordination capability allows phenolic azo-Schiff bases to form stable chelate complexes with a wide range of transition metal ions [31]. While azo dyes exist in azo or hydrazone tautomeric forms, 2-hydroxy Schiff bases exist in phenol-imine, hydrazo-imine, or ketamine tautomers in solid state and solution. When complexation occurs with metal ions, tautomerization favours the phenol-imine isomer (Figure 5) [32].
<figure><img src="image_7.png" /><figcaption>Figure 5. Proposed tautomerism and binding interaction of azo–Schiff base [32].</figcaption></figure>

**3. General Synthetic Methods for Azobenzenes and Hydroxyazobenzenes**

Various synthetic strategies have been developed for the preparation of phenolic azobenzenes, each with specific advantages in terms of selectivity, efficiency, and compatibility with functional groups [33]. These methods usually involve either the coupling of phenolic compounds with azobenzene derivatives or the direct formation of the azo bond between anilines and phenols under controlled conditions [34]. The most commonly used methods for the synthesis of azobenzenes include the azo coupling reaction, the Mills reaction, the Wallach reaction, the oxidation of anilines, and the reduction of nitroaromatic compounds (Figure 6) [35]. While synthetic methods for symmetrically substituted azobenzene derivatives are well established, the development of efficient strategies for their asymmetrical counterparts remains an ongoing challenge [36].

<figure><img src="image_8.png" /><figcaption>Figure 6. General synthetic methods for synthesis of azobenzenes.</figcaption></figure>
### 3.1. Azo Coupling Reaction

Azo coupling reactions are among the most commonly used methods for the synthesis of azobenzenes, involving an electrophilic aromatic substitution (S<sub>E</sub>Ar) reaction of a diazonium salt and an electron-rich arene [37]. The methodology usually begins with the diazotization of an aromatic primary amine using an in situ prepared nitrosonium ion, which is carried out under mild conditions at low temperature (0 °C to 5 °C) to form the diazonium salt (Figure 7) [38]. The electrophilicity of diazonium ions is relatively weak because their positive charge is delocalized. Therefore, phenols as electron-rich arenes are suitable substrates for the coupling reaction with aryl diazonium salts to form the azo compound.

<figure><img src="image_9.png" /><figcaption>b Synthesis of diazonium salt</figcaption></figure>

<figure><img src="image_10.png" /><figcaption>c Azo coupling reaction</figcaption></figure>

<figure><img src="image_11.png" /><figcaption>**Figure 7.** Mechanism of azo coupling reaction.</figcaption></figure>

The substitution usually takes place at the para position, unless this is already occupied, in which case the ortho position is preferred. The reaction often requires short reaction times and generally leads to products of high purity (Figure 8) [39]. This process is extremely versatile and allows for the selective functionalization of both the amine and the nucleophilic component, making it suitable for a wide range of substrates (Figure 8) [40].

As can be seen from the diagram in Figure 8, the yield of azobenzene formation does not depend on the electronic properties of the substituents, and high yields of azobenzene products of 85% to 95% were obtained, irrespective of whether the substituent on the aniline is electron-withdrawing or electron-donating. However, this method requires careful temperature and pH control to ensure the stability of the diazonium salt and to avoid side reactions [41]. The side reactions related to azo coupling are mainly the decomposition of diazonium salt to phenols, chlorobenzene (if hydrochloric acid was used to form this salt), or to any functionalized benzene depending on the presence of nucleophilic moieties [42]. Moreover, the use of sodium nitrite can lead to the formation of nitrobenzene from the corresponding aniline [43]. This is why the acid and temperature used in diazotization not only adjust the pH of the reaction medium to slightly acidic or neutral conditions but also play a crucial role in determining the stability of the resulting diazonium salt. Diazonium
chloride salts, traditionally prepared from aniline, sodium nitrite, and hydrochloric acid, are unstable at room temperature and are normally prepared and used at 0–5 °C. However, diazonium compounds can be isolated as tetrafluoroborate or tosylate salts, which form stable solids at room temperature [44].

a

<figure><img src="image_12.png" /></figure>

b

<figure><img src="image_13.png" /><figcaption>**Figure 8.** Yield of azobenzenes in coupling reaction of phenol with substituted anilines. (a) General pathway and (b) yields depending on R.</figcaption></figure>

In the case of not performing the in situ conversion of aniline to azobenzene, it is also possible to isolate the diazonium salt, which can be further converted to the phenolic azobenzene via a reaction with a sodium acetate (NaOAc) base in aqueous medium (Table 2) [45].

<table><caption>**Table 2.** Synthesis of phenolic azobenzenes using diazonium salt and NaOAc as base.</caption><thead><tr><th>Solvent</th><th>Yield [%]</th></tr></thead><tbody><tr><td>Methanol</td><td>46</td></tr><tr><td>Ethanol</td><td>42</td></tr><tr><td>Acetonitrile</td><td>40</td></tr><tr><td>Acetone</td><td>41</td></tr><tr><td>Dichloromethane</td><td>0</td></tr><tr><td>Methanol–H<sub>2</sub>O = 1:1</td><td>80</td></tr><tr><td>Methanol–H<sub>2</sub>O = 3:1</td><td>89</td></tr><tr><td>Methanol–H<sub>2</sub>O = 9:1</td><td>63</td></tr></tbody></table>
As can be seen in Table 2, the use of a polar solvent is key to achieving higher conversion efficiencies. In fact, when a higher proportion of water is used, the efficiency ranges between 80% and 90% [45].

## 3.2. Baeyer–Mills Reaction

The Baeyer–Mills reaction is one of the most commonly used methods for accessing non-symmetric azobenzenes and is based on the condensation of nitrosobenzene derivatives with anilines [46]. This reactivity can be explained by the proposed mechanism, which involves the nucleophilic attack of the aniline on the nitrosobenzene derivatives in acidic or basic media (Figure 9) [47,48]. The Baeyer–Mills reaction consists of several steps. In the first step (Figure 9a), aniline is oxidized to a nitroso compound, whereby N-phenylhydroxylamine is formed as an intermediate. In the next step (Figure 9b), a reaction takes place between the nitroso compound and aniline, producing azobenzene. The use of suitable reagents and appropriate catalysts is crucial for this reaction, as otherwise, symmetrical azobenzenes are formed in situ (Figure 9c) or overoxidation takes place, leading to the formation of nitroaromatics (Figure 9d) [49].

### a Synthesis of nitroso compound

<figure><img src="image_14.png" /></figure>

### b Synthesis of azobenzene

<figure><img src="image_15.png" /></figure>

### c Example of side reaction : In situ preparation of homoazobenzenes

<figure><img src="image_16.png" /></figure>

### d Example of side-reaction : Formation of nitroaromatics

<figure><img src="image_17.png" /><figcaption>**Figure 9.** Mechanism of Baeyer–Mills reaction.</figcaption></figure>

The reaction exhibits good selectivity, with control over the electronic properties of the reactants, allowing for the fine-tuning of the final product [46]. The presence of electron-
donating groups, such as hydroxyl groups, on the aniline ring can further influence the reactivity and regioselectivity of the process, making this method highly adaptable for the synthesis of functionalized phenolic azobenzenes (Table 3) [50]. Table 3 shows that electron-rich anilines perform poorly in Baeyer–Mills reactions because they have a high propensity to reduce nitrosoarene, which translates into higher yields of the azoxybenzene side products. Anilines with moderately electron-withdrawing and electron-donating substituents give excellent yields of the desired azobenzenes with a minimal formation of azoxybenzene. The yield of azobenzene decreases sharply when arylamines with strongly electron-withdrawing substituents are used, which is probably due to the lower nucleophilicity of the anilines [20]. The position of the functional group in relation to the amine group also affects the yield of azobenzene synthesis. The data presented in Table 3 show that the conversion of aniline (regardless of the nature of the substituent) in the Baeyer–Mills reaction is quite high, with the exception of the 2,6-difluoro and nitro functional groups, where the conversion rate is between 10% and 25%.

<table><caption>**Table 3.** The effects of the substituent on aniline on the formation of azobenzene.</caption><thead><tr><th>R</th><th>Azobenzene yield [%]</th><th>Azoxybenzene yield [%]</th></tr></thead><tbody><tr><td>p-NMe<sub>2</sub></td><td>34</td><td>45</td></tr><tr><td>p-NH<sub>2</sub></td><td>28</td><td>43</td></tr><tr><td>o-NH<sub>2</sub></td><td>8</td><td>91</td></tr><tr><td>p-OMe</td><td>≥95</td><td>5</td></tr><tr><td>2,6-dimethoxy</td><td>46</td><td>35</td></tr><tr><td>p-NHCO<sub>2</sub><sup>t</sup>Bu</td><td>87</td><td>6</td></tr><tr><td>p-OH</td><td>34</td><td>69</td></tr><tr><td>o-OMe</td><td>82</td><td>13</td></tr><tr><td>p-Me</td><td>95</td><td>≤5</td></tr><tr><td>o-NHCO<sub>2</sub><sup>t</sup>Bu</td><td>85</td><td>12</td></tr><tr><td>o-Et</td><td>77</td><td>20</td></tr><tr><td>p-I</td><td>≥95</td><td>≤5</td></tr><tr><td>H</td><td>≥95</td><td>≤5</td></tr><tr><td>o-Br</td><td>49</td><td>8</td></tr><tr><td>p-CO<sub>2</sub>Me</td><td>82</td><td>6</td></tr><tr><td>2,6-difluoro</td><td>12</td><td>≤5</td></tr><tr><td>p-CN</td><td>64</td><td>7</td></tr><tr><td>p-CF<sub>3</sub></td><td>≥95</td><td>≤5</td></tr><tr><td>o-NO<sub>2</sub></td><td>≤5</td><td>≤5</td></tr><tr><td>p-NO<sub>2</sub></td><td>19</td><td>≤5</td></tr></tbody></table>

In cases where azoxybenzene is formed as the main product of the Baeyer–Mills reaction, the subsequent reduction of azoxybenzenes to azobenzenes occurs, and this is discussed in the following sections of this paper.
As can be seen from the above figures and the table, the key to the Baeyer–Mills reaction lies in the production of the nitroso compound. Generally, this is produced by the oxidation of aniline, but it should be noted that not all oxidation conditions allow for the production of a nitroso compound (Figure 10). The nitroso compound can be formed either with Oxone, which is also the most common process, or with another oxidizing agent such as hydrogen peroxide in the presence of a suitable catalyst [51]. Although H₂O₂ presents major problems in transport and handling, it is a green oxidizing agent, due to the formation of non-toxic and environmentally benign byproducts, besides presenting an excellent atom efficiency. In principle, Oxone provides better selectivity for the formation of nitroso compounds, since in the case of the use of H₂O₂/catalyst (using classical catalysts such as SeO₂, Na₂WO₄, MTO), azoxybenzene is often formed directly. On the other hand, new catalytic systems have been developed which, in combination with H₂O₂, allow for the highly selective conversion of aniline to nitroso compounds. One such catalyst is Na-ββ-Ln₄ (Figure 10a), a dimeric POM (polyoxometalate) composed of lanthanide-containing dilacunary Keggin subunits of the β-type that act as Lewis acids, enabling the full conversion of the substrate and total selectivity towards nitrosobenzene. The exact nature of the lanthanide centres affects not only catalytic activity but also the solubility of the catalyst during the reaction. Reaction rates decrease as the atomic number of lanthanide increases, but at the same time, less of the catalyst is transferred to the solution.

<figure><img src="image_18.png" /><figcaption>**Figure 10.** (a) Aniline-to-nitrosobenzene selective oxidation process and molecular structure of Na-ββ-Ln₄ catalysts and (b) aniline conversion at room temperature throughout nine consecutive runs. Reprinted with permission from Ref. [51]. Copyright 2015, Elsevier Inc.</figcaption></figure>

Moreover, the catalyst has excellent recyclability properties. The selectivity of the catalyst towards nitrosobenzene remains constant (100%) even after nine consecutive reaction runs. Interestingly, the time required to obtain 100% conversion decreases in the successive reactions (Figure 10b) [51].

When a combination of KMnO₄ and FeSO₄ is used as an oxidizing agent (Figure 11), this reaction does not lead to the oxidation of aniline to nitrosobenzene. Instead, symmetrical azobenzene is formed directly [52,53].

With certain oxidizing agents, asymmetric azobenzenes can be formed directly and not via the synthesis of a nitroso intermediate [54].

In cases where nitroso compounds are not involved as intermediates in the reaction mechanism, the process can no longer be classified as a Baeyer–Mills reaction but rather as the oxidative coupling of anilines, leading to the formation of azobenzenes, as discussed in the following section of this review article.
<figure><img src="image_19.png" /><figcaption>**Figure 11.** Oxidation of aniline to nitroso derivative or symmetrical azobenzenes using suitable oxidants.</figcaption></figure>

### 3.3. Oxidation of Anilines

The essential difference between the Baeyer–Mills reaction mentioned above and the in situ formation of azobenzene by the oxidation of anilines is that in the latter case, the intermediate oxidized form of aniline is not isolated. It is precisely for this reason that symmetrical azobenzenes are formed in this type of synthesis.

The formation of azobenzenes by the oxidation of aniline is a fairly old process, originally based on electrolytic oxidation [53]. In general, these processes were characterized by synthesizing azobenzenes in lower yields than those of other processes. An example of electrolytic oxidation is the synthesis of azobenzene from trichloroaniline, which was carried out with a platinum (Pt) electrode in dimethylformamide and in the presence of pyridine [55].

It has been reported that various oxidizing agents can generate azo compounds from aromatic amines. When H₂O₂/Na₂WO₄ is used, the initial oxidation of aniline to the azodioxide and its subsequent reduction with Si₂Cl₆ take place. Azobenzene is obtained in very good yield [56].

A variety of metallic and non-metallic reagents, such as Ag₂O, AgO [57], AgMnO₄ [58], MnO₂ [59], KO₂ [60], NaBO₃ [61], Pb(OAc)₄ [62], BaMnO₄ [63], Ce(OH)₃O₂H [64], NiO₂, peroxides (such as hydrogen peroxide or *tert*-butyl hydroperoxide [65]), and even chemicals from electrochemical oxidation [66], were used either stoichiometrically or in excess to synthesize azobenzenes from aromatic amines. This literature review showed that the choice of oxidation reagent has a really big impact on the final yield of azobenzene synthesis. It turns out that the yields in the case of the use of specialties such as BaMnO₄, MnO₂, and AgMnO₄ are high and range between 70% and 90%, in contrast to, for example, NaBO₃, Ce(OH)₃O₂H, NiO₂, and AgO, where the yields are mostly lower than 60%. Furthermore, it is also interesting to note that the yield is also affected by which manganese speciation is used as the oxidation reagent. For example, oxidation with barium manganate gives reproducible results without requiring further activation, while an oxidation reaction with manganese dioxide is not reproducible in many aspects. In addition to the above, BaMnO₄ allows for higher selectivity in oxidation reactions, while at the same time, they are faster and have higher reaction yields [63].

Gold nanoparticles on titanium dioxide (TiO₂) have also been shown to be a very efficient system for the conversion of aniline to azobenzenes, allowing for a very selective conversion to azobenzene (up to 98 %) [67].

Nowadays, the use of green oxidizing agents such as oxygen/air or hydrogen peroxide (H₂O₂) in particular is being researched for this type of oxidation [68], due to the formation
of non-toxic and environmentally benign byproducts. In this case, oxidation reactions are carried out using suitable catalysts such as Zr(OH)₄, and the azobenzene formation efficiencies are between 70% and 90%. However, when oxygen is used as the oxidation reagent, the yields increase above 90%, as a more selective formation of azobenzene occurs with a relatively low proportion of nitrosobenzene (around 2%) and is not significantly dependent on the functional groups present on the aniline [65].

Although the oxidation process is often efficient, it must be carefully controlled to avoid overoxidation, which leads to undesirable byproducts. For example, excessive oxidation can lead to the formation of azoxy or nitro compounds, which are usually more stable and may not be suitable for subsequent reactions or applications. Therefore, the optimization of reaction conditions, including the amount of oxidant and reaction time, is critical to achieve high yields of the desired phenolic azobenzene products. For example, in the case of NaBO₃, the temperature of the reaction mixture proves to be very important. It turns out that the yield of the reaction increases with increasing temperature. In addition to the above, the pH of the reaction mixture also has a major influence, i.e., the yield of the azobenzene formation reaction decreases with an increasing pH of the reaction mixture. In the case of metal peroxides, it turns out that the reaction times in the case of nickel(II) peroxide are much longer than those in the case of ceric trihydroxy hydroperoxide. In the case of the use of O₂ or peroxide as the oxidation reagent in combination with a catalyst, it turns out that reaction conditions such as reaction time and the concentration of the oxidation reagent do not significantly affect the yield of the azobenzene synthesis reaction itself. On the other hand, the choice of peroxide and solvent is very influential. It was found that only the reaction in acetic acid and in the presence of the oxidizing agent tert-butyl hydroperoxide is selective as far as the synthesis of azobenzenes is concerned. In the other cases (using H₂O₂ in combination with H₂O, methanol, and mesitylene as solvents), a nitroso compound or an azoxybenzene is formed. If azoxybenzene is formed in the reaction, it can also be converted to azobenzene with a suitable reducing agent (e.g., Si₂Cl₆). In the case of using oxygen as an oxidizing agent, mesitylene proves to be a significantly better solvent than water in terms of the selectivity of azobenzene formation. On the other hand, the reaction time and solvent do not significantly affect the yield of the azobenzene formation reaction in the case of AgO.

In contrast to the above oxidation processes, the synthesis of asymmetric azobenzene can be achieved in combination with air or oxygen at standard pressure (1 atm) and the use of a copper catalyst (e.g., CuBr or CuCl) (Figure 12 [54]). A similar reaction pathway can be observed in the case of manganese oxide using chlorobenzene as solvent, when in the presence of oxygen and heated to 160 °C [69].

<figure><img src="image_20.png" /><figcaption>**Figure 12.** Oxidation of anilines to form asymmetrical azobenzene.</figcaption></figure>

The above method of the oxidation of anilines and the formation of azobenzenes also allows for the synthesis of symmetrical azobenzenes in yields ranging from 60% to 100% depending on the functional groups on the aniline. In the case of symmetrical azobenzene synthesis, the reaction yields are lower, ranging between 40% and 70% depending on the functional groups on the aniline.
### 3.4. Reduction Reaction of Azoxybenzenes

As shown in the previous sections, overoxidation produces azoxybenzenes containing a N=N bond with an additional oxygen functionality (-N=N(O)-), which can be removed by controlled reduction to give the corresponding azo compounds, leaving the conjugated π-system intact.

The first way to reduce azoxybenzenes is to use various reducing reagents, including hydrogenation catalysts (e.g., palladium or platinum on carbon), metal-based reducing agents (such as zinc, iron, or tin in acidic media), and organic reducing agents such as hydrazine or sodium dithionite [70–72]. In addition, the reduction of azoxybenzenes to azobenzenes can also take place via photochemical conversion [73]. Upon direct irradiation, azoxybenzenes may undergo rearrangement to 2-hydroxyazobenzene and cis-trans isomerization. In contrast, being irradiated in the presence of a photosensitizer (such as acetophenone, benzophenone, thioxanthone, flavone, fluorenone, etc.) with suitable triplet excitation energy leads to a reduction to azobenzene. In the absence of sensitizers, only a change in the geometric configuration of azoxybenzene occurs, and 2-hydroxyazobenzene is formed. As the concentration of the sensitizer increases, the proportion of azobenzene formed also increases. If oxygen is also present in the reaction, it causes a decrease in the proportion of azobenzene formed. The following ketones were efficient photosensitizers to be used to reduce azoxybenzenes to azobenzene: acetophenone (triplet excitation energy $E_{T1} = 74$ kcal/mol), benzaldehyde (72 kcal/mol), benzophenone (69 kcal/mol), thioxanthone (65 kcal/mol), phenylglyoxal (63 kcal/mol), and anthraquinone (62 kcal/mol). On the other hand, the following ketones were not efficient: flavone (62 kcal/mol), Michler's ketone (61 kcal/mol), 2-acetonaphthone (59 kcal/mol), biacetyl (55 kcal/mol), benzil (54 kcal/mol), and fluorenone (53 kcal/mol). Based on these results, the triplet state energy of the azoxybenzene intermediate is estimated to be approximately 62 kcal/mol. It is proposed that 2-hydroxyazobenzene and cis-azoxybenzene originate from the excited singlet state of azoxybenzene, whereas azobenzene forms via the triplet excited state [73].

The reduction of azoxybenzene is usually stepwise, with the oxygen atom being removed to form the azo product. The choice of reducing agent and reaction conditions has a significant impact on the efficiency, selectivity, and functional group tolerance of the process [74]. A process in which azoxyarenes are treated with hydrazine hydrate in the presence of aluminum in methanol under reflux or microwave irradiation is commonly used for such reactions (Figure 13). In general, the yields are quite high in the conversion of azoxybenzenes to azobenzenes (between 85% and 100%), and they are independent of the type of heating of the reaction mixture. On the other hand, the kinetics of the reaction depend mainly on the type of heating. In the case of microwaves, the reaction time is only 2 min, whereas in the case of reflux, it is about five times longer [71].

Another option for introducing a hydroxyl functional group into azobenzene is the Wallach rearrangement. In this reaction, the conversion of azoxybenzene to azobenzene occurs by the rearrangement of the hydroxy group to an azoxy functional group on the aromatic ring. Although the Wallach reaction is used less frequently than other synthesis methods, it is particularly suitable for the regioselective formation of phenolic azobenzenes [75]. Wallach rearrangement only takes place in strongly acidic solutions. It combines the loss of the oxygen bound to the azo group with the formation of a hydroxyl group in the para position to the azo bond in the benzene ring. In contrast to conventional azo coupling reactions based on diazonium salts or nitroso condensation, the Wallach reaction offers an alternative route to azobenzenes, especially in cases where the direct oxidation of aniline derivatives is difficult [76]. As shown in Figure 13, the main product of the Wallach rearrangement is the phenolic azobenzene, which has an -OH functional group at the para site. This rearrangement also produces byproducts such as *ortho*-hydroxyazobenzene,
azobenzene, and some polymeric materials from aniline and sulfonic acids in very small amounts [77]. The reaction of unsubstituted azoxybenzene at room conditions yields 72% *p*-hydroxyazobenzene and 28% azobenzene. In the Wallach rearrangement, sulphuric acid is generally used in concentrations of over 80% after heating to T ≥ 50 °C. With increasing acidity, a slight increase in the amounts of azobenzene and polymeric substances is observed. When azoxyazobenzene is heated to higher temperatures (245–250 °C), azobenzene is formed as the main product with small amounts of *para*- and *ortho*-hydroxyazoxybenzene (Figure 13). In the case of Wallach rearrangement, the formation of a hydroxyl functional group can also promote the dehydration process, leading to the subsequent formation of the polymeric form of azobenzene [78]. In the case of unsubstituted azoxybenzene, 32% *p*-hydroxyazobenzene and 68% azobenzene are obtained. If the para position is occupied, a hydroxyl group forms in the ortho position (Figure 14) [79].

<figure><img src="image_21.png" /><figcaption>**Figure 13.** Reduction reaction of azoxybenzenes and Wallach rearrangement.</figcaption></figure>

<figure><img src="image_22.png" /><figcaption>**Figure 14.** Wallach rearrangement in *para*-disubstituted azoxybenzene.</figcaption></figure>
### 3.5. Reductive Coupling of Aromatic Nitro Derivatives

This reaction involves the selective reduction of nitroarenes to nitroso derivatives, which are starting substrates for the formation of azobenzene(-N=N-). The reaction leads to the production of symmetrically substituted azo derivatives [80]. Commonly used reducing agents include metal-based reagents such as zinc, iron, or tin in acidic or neutral media and catalytic hydrogenation with transition metal catalysts such as palladium, platinum, or ruthenium [81,82]. Nitroaromatics can also be reduced in the absence of a metal-based catalytic system using an alkaline medium or a combination of sodium hydroxide and ethanol [83]. In addition, glucose is often used as a reducing agent in alkaline media [84].

The reaction proceeds via the stepwise reduction of the nitro group, producing reactive intermediates such as nitroso and hydroxylamine species. These intermediates are then coupled, leading to the formation of the azo bond (Figure 15). The reduction process is very sensitive to the choice of reducing agent, catalyst, and reaction conditions, which significantly influence the selectivity of the reaction [85]. Controlling these parameters is important to prevent over-reduction to aniline derivatives [86]. The choice of metal has a major influence on the yield of the reaction in the synthesis of symmetrical azobenzene. Lithium or zinc is most commonly used as a reducing agent in conjunction with an active metal such as Mg, Zn, Al, In, Ti, or Nb. It can be seen that when the metals W, Mo, and Zr as activated metal are used, the reaction to form azobenzene from nitroaromatics does not take place at all [87]. The functional groups present on the nitroaromatic compound also have a major influence on the yield of the reaction. It turns out that they are the most likely to lower the yield of the azobenzene synthesis reaction. One of the main advantages of this method is its versatility, as it is suitable for a wide range of nitroaromatic compounds, including those with electron-donating or electron-withdrawing substituents. The use of metal-based reducing agents provides an efficient route for the selective generation of azo compounds, while catalytic hydrogenation offers a mild alternative with excellent scalability. In addition, the process can be adjusted to control the regioselectivity and functional group compatibility of the resulting azobenzene products.

<figure><img src="image_23.png" /><figcaption>**Figure 15.** Reductive coupling of aromatic nitro derivatives.</figcaption></figure>

In addition, azobenzenes can be prepared via the photochemically excited reduction of nitrobenzenes (Figure 16) [88].
<figure><img src="image_24.png" /><figcaption>**Figure 16.** Photochemical process for reduction of nitrobenzenes to azobenzenes (a) and energy diagram of this conversion (b). Figure (b) reprinted with permission from Ref. [88] under Creative Commons CCBY license.</figcaption></figure>

In the reaction shown above, the inexpensive graphitic $C_3N_4$ represents an efficient photocatalyst for the selective syntheses of a series of azo- and azoxy-aromatic compounds from their corresponding nitroaromatics when exposed to either purple (410 nm) or blue light (450 nm) excitation (Figure 16a). As can be seen in Figure 16b, the photoexcited $e^-$ in the conduction band (CB) of $g-C_3N_4$ possesses sufficient energy to initiate the nitrobenzene reduction. Concurrently, isopropanol (IP) acts as a sacrificial electron donor, undergoing oxidation to acetone (AC), which generates two protons and releases two electrons that recombine with the holes ($h^+$) in the valence band (VB).

The high efficiency and high selectivity towards azo- and azoxy-aromatic compounds can be attributed to the weakly bound photogenerated surface-adsorbed H-atoms and a favourable N-N coupling reaction. The selectivity in this type of reaction is shown by the low proportion of amine formed during the azobenzene synthesis reaction (up to 10%), irrespective of the functional groups present on the nitrobenzene. In addition, using 410 nm light, selective conversion to azobenzene and, at 450 nm, selective conversion to azoxybenzenes occur. The yields of the reactions are very high (between 90% and 100%) and do not significantly depend on the functional group on the nitrobenzene [88].

## 4. Complexation and Crystal Structures

In 1969, Baer et al. studied metal complexes of azo dyes [89]. Particularly, they added cupric chloride or nickel chloride in an aqueous solution of ethylenediamine to o-halide-o'-hydroxyazo compounds, and they obtained several compounds (Figure 17) analyzed by their melting point, their empirical formula, and also their $\lambda_{max}$ value (nm). Their magnetic susceptibility was also determined. For example, the nickel complex was found to be diamagnetic, indicating that the complex has a square planar geometry around the nickel atom. But the copper complexes examined had a magnetic moment equal to or greater than the spin-only value of 1.73, suggesting that no significant interactions occur between copper atoms. The authors indicated that X-ray would have been required to establish the stereochemistry with certainty.

<figure><img src="image_25.png" /><figcaption>**Figure 17.** Example of complexes obtained in ref [89].</figcaption></figure>
With this in mind, a relevant example is the complex chlorido[(E)-3-hydroxy-2-methyl-6-(quinolin-8-yldiazenyl)phenolato]copper(II) monohydrate [90]. In this compound, the hydroxyazobenzene ligand is deprotonated at the ortho position and coordinated to the Cu(II) centre, forming a pseudo-square planar geometry. The crystal structure was determined by X-ray diffraction, revealing the following characteristic bond lengths:

* Cu–O: 1.917 Å.

* Cu–N: (quinoline): 2.008 Å.

* Cu–N: (azo): 1.945 Å.

* Cu–Cl: 2.280 Å.

The complex also shows a weak axial coordination between copper and a chlorine atom from a neighbouring molecule, with a Cu–Cl distance of 2.739 Å, suggesting an intermolecular interaction (Figure 18).

<figure><img src="image_26.png" /><figcaption>**Figure 18.** Copper complex and X-ray structure of chlorido[(E)-3-hydroxy-2-methyl-6-(quinolin-8-yldiazenyl)phenolato]copper(II) monohydrate. Reprinted with permission from Ref. [90]. Copyright 2022, IUCr Journals.</figcaption></figure>

Sometimes, complexation occurs within a synthetic pathway to obtain, after demetal-
lization, ortho-OH azoaryl dyes. This was the case in 2017 where a dinuclear copper (II)
complex was synthesized from copper diacetate and a hydrazone molecule by a Fenton
reaction using H₂O₂ [91]. The crystal structure of this intermediate was determined in
DMF by X-ray diffraction, revealing the following characteristic bond lengths (Figure 19):

* Cu1–O1: 1.944 Å.

* Cu1–O1A: 2.061 Å.

* Cu1–O4: 1.920 Å.

* Cu1–O6: 2.140 Å.

* Cu1–N2: 1.925 Å.
<figure><img src="image_27.png" /><figcaption>**Figure 19.** Copper complex and X-ray structure of intermediate. Reprinted with permission from Ref. [91]. Copyright 2017, Elsevier.</figcaption></figure>

Schiff bases and especially (chiral) salen metal complexes can been employed in (asymmetric) catalysis because of their advantages in stereochemical tuning (with respect to chirality) and redox properties with proper metal ions [92]. These molecules (Figure 20) were synthesized and gave the following crystal structure:

Example for R₁ = OCH₃, R₂ = H:

* Cu1–O2: 1.854 Å.

* Cu1–O3: 1.885 Å.

* Cu1–N1: 1.957 Å.

* Cu1–N3: 1.913 Å.

Concerning photoisomerization capability, the change in UV-vis spectra due to the *trans*-to-*cis* photoisomerization of the azobenzene moiety (R₁ = OCH₃; R₂ = H) showed a shift in π-π* bands to a shorter wavelength. The stable *trans* form was converted to the *cis* form by a metal-to-ligand charge transfer (MLCT) transition, where electrons move to the ligand, as well as other transitions. Moreover, the reversible *cis*-*trans* photoisomerization, which converts the *cis* to the *trans* form by visible light irradiation, was observed for all complexes (Figure 20).

Bi-metallic compounds can also be obtained by the reaction of an ethyynylazobenzene and [RuCl₂(dppe)₂]. This intermediate can react with anilines to obtain Schiff bases, and by the reaction of zinc salts in the presence of phenanthroline or bipyridine, complexes are formed (Figure 21) [93]. It is noticeable that luminescence is observed for all complexes as a result of the intra-ligand π→π* transition and chelation enhanced fluorescence (CHEF) by the coordination of the imine group to Zn(II) in the complexes. The presence of azo chromophore with extended π-conjugation enhances the emission properties of the complexes and varies considerably with donor–acceptor substituents and the π-acidic character of the co-ligands.
a

<figure><img src="image_28.png" /></figure>

b

<figure><img src="image_29.png" /><figcaption>UV-vis spectra (DMSO solution) of 1 after UV light irradiation to yield cis form (Blue: 0 min; Red: 10 min; and Green: 20 min)</figcaption></figure>

<figure><img src="image_30.png" /><figcaption>**Figure 21.** Azo bi-metallic complex.</figcaption></figure>
# 5. Applications of Phenolic Azobenzene Complexes

## 5.1. Colorimetric Sensors

Hydroxyazobenzene compounds are a class of azo dyes known for their vivid colouration. The hydroxyl group plays a key role in metal ion binding through coordination chemistry, especially when the azo-OH moiety is in the *ortho* position of a Schiff base (Figure 22) [94]. When these molecules interact with metal cations, they form stable chelate complexes. These complexes alter the molecule's electron distribution, leading to a visible colour change. This property is exploited in colorimetric detection methods for various cations. UV-Vis spectrophotometry can quantify these changes based on absorbance shifts. Each metal ion produces a characteristic spectral change, enabling selective detection. Commonly detected cations include Cu²⁺ and Cr³⁺ [95], Cd²⁺ and Hg²⁺ [96], Co²⁺, and Al³⁺ [97,98]. Detection is often pH-dependent as protonation affects the ligand binding sites. The simplicity of visual detection makes them suitable for rapid, low-cost analysis [94].

<figure><img src="image_31.png" /><figcaption>**Figure 22.** General structure of azo-Schiff bases.</figcaption></figure>

In the domain of pollutant removal, it is also important to be able to perform selective cation detection [99–101]. With this in mind, azo-phenol-based receptors with an azo core linked to naphthol and variously substituted benzothiazole units were synthesized and investigated for their optical properties. Among them, the nitro-substituted derivative showed enhanced fluorescence upon interaction with Hg²⁺ ions, which enabled detection with the “naked eye” [102]. Spectroscopic analyses—including UV-Vis absorption, fluorescence emission, FT-IR, and ¹H NMR—revealed that the Hg²⁺ ion coordinates favourably with the phenolic oxygen, the azo nitrogen adjacent to the naphthol ring, and the thiazole nitrogen of the benzothiazole unit. This interaction occurs in a terdentate fashion (Figure 23). In addition, photoinduced and Hg²⁺-induced proton transfer reactions supported the presence of *cis-trans* isomerism and azo-hydrazone tautomerism in these systems.

<figure><img src="image_32.png" /><figcaption>**Figure 23.** Azo phenol-based probe for (a) Hg²⁺ detection [102] and (b) Cu²⁺ detection [103].</figcaption></figure>

Only recently (2025) was a naked-eye chemosensor developed that makes it possible to quickly and selectively detect copper cations in solution (Figure 24) [104].
<figure><img src="image_33.png" /><figcaption>**Figure 24.** Selective chemosensing of copper cations. Reprinted with permission from Ref. [103]. Copyright 2025, Elsevier.</figcaption></figure>

## 5.2. *Smart Materials and DSSCs*

Hydroxyazobenzene compounds exhibit promising potential as dyes for dye-sensitized solar cells (DSSCs) due to their ability to form a complex with metal cations. The hydroxyl groups, mainly supported by the Schiff base in their structure, facilitate coordination with metal ions such as $Ti^{4+}$, $Cu^{2+}$ [103,105], $Fe^{2+}$ [106], or $Zn^{2+}$ [106], which enhances electronic communication with semiconductor surfaces.

This complexation often results in improved light-harvesting capabilities by extending the absorption range into the visible spectrum (Figure 25, Table 4). The resulting metal-dye complexes can also promote efficient charge separation and electron injection into the conduction band of $TiO_2$. Moreover, hydroxyazobenzene dyes are synthetically tuneable, allowing for the optimization of photophysical and electrochemical properties. Indeed, their structural versatility supports the fine-tuning of absorption maxima and redox potentials as azo dyes can be synthesized with various functional groups with different absorption spectra, dipole moments, and conjugation lengths [107].

Additionally, these complexes can exhibit strong anchoring to $TiO_2$ surfaces [106]. As the hydroxyl group is complexed with a metal cation, it does not interfere with the other anchoring groups, as carboxylate, sulfonate, or pyridyl anchors, knowing that amongst these groups, OH yields the worst performance, with its inferior UV/vis absorption intensity on the $TiO_2$ substrate and the lowest DSSC performance conversion efficiency [108].

<table><caption>**Table 4.** Spectral and electrochemical properties of compounds 1–9.</caption><thead><tr><th></th><th>E<sub>HOMO</sub> (eV)</th><th>E<sub>LUMO</sub> (eV)</th><th>ΔE (eV)</th><th>Absorption Range/λ<sub>max</sub> (nm)</th><th>Reference</th></tr></thead><tbody><tr><td>1</td><td>-5.85</td><td>-3.13</td><td>2.72</td><td>387-679</td><td>[103]</td></tr><tr><td>2</td><td>-5.74</td><td>-3.11</td><td>2.73</td><td>440-727</td><td>[103]</td></tr><tr><td>3</td><td>-5.92</td><td>-3.18</td><td>2.74</td><td>472-752</td><td>[103]</td></tr><tr><td>4</td><td>-6.64</td><td>-4.02</td><td>2.62</td><td>511-790</td><td>[103]</td></tr><tr><td>5</td><td>-5.483</td><td>-3.429</td><td>2.234</td><td>368</td><td>[106]</td></tr><tr><td>6</td><td>-5.312</td><td>-3.785</td><td>1.527</td><td>387</td><td>[106]</td></tr><tr><td>7</td><td>-5.579</td><td>-3.279</td><td>2.282</td><td>352</td><td>[106]</td></tr><tr><td>8</td><td>-4.36</td><td>-3.73</td><td>0.63</td><td>450</td><td>[105]</td></tr><tr><td>9</td><td>-4.36</td><td>-3.83</td><td>0.53</td><td>402</td><td>[105]</td></tr></tbody></table>

Dye-sensitized solar cells (DSSCs) were constructed to evaluate the performance of hydroxyazobenzene molecules that complex cations under controlled laboratory conditions. These cells served as a testing platform to investigate the photoelectrochemical properties and potential of azobenzene-based dyes as light-harvesting materials. By producing DSSCs
with these compounds, the aim was to gain insight into their efficiency, stability, and suitability for solar energy conversion applications.

For example, two types of materials were tested (Figure 26). The first one was a polychelate [109], whereas the second one was a metal complex [110].

<figure><img src="image_34.png" /><figcaption>**Figure 25.** Molecules involved in DSSC applications (a) from ref. [103]; (b) from ref. [106]; (c) from ref. [106].</figcaption></figure>

<figure><img src="image_35.png" /><figcaption>**Figure 26.** Complexes from (a) ref. [109] and (b) ref. [110].</figcaption></figure>

The photovoltaic parameters of these devices were determined (Table 5). Open-circuit voltage (V<sub>OC</sub>) is the maximum voltage a solar cell can provide to an external circuit, which
is derived from the splitting of hole and electron quasi-Fermi levels. In organic materials (OSC), disorder induces gap tail states. The relaxation of carriers into these tail states brings the electron quasi-Fermi level down and the hole quasi-Fermi level up and hence reduces $V_{OC}$ [111]. In this context, compared to the reference N3 dye ([Ru(dcbpy)₂(NCS)₂]) [112], organometallic compounds 10 and 11 seem to have lower efficiency, but the results can vary a lot depending on the device used (full commercial device, light power, etc.).

<table><caption>**Table 5.** Photovoltaic parameters with Voc: open-circuit voltage; FF: Fill factor; η: overall energy conversion yield.</caption><thead><tr><th>Compound</th><th>V<sub>OC</sub>, mV</th><th>FF</th><th>η, %</th><th></th></tr></thead><tbody><tr><td>I<sub>3</sub><sup>-</sup>/I<sup>-</sup></td><td>724</td><td>0.70</td><td>8.0</td><td>[113]</td></tr><tr><td>N<sub>3</sub></td><td>678</td><td>0.607</td><td>7.3</td><td>[112]</td></tr><tr><td>10</td><td></td><td></td><td></td><td>[109]</td></tr><tr><td>Cu<sub>2+</sub></td><td>400</td><td>0.54</td><td>2.05</td><td></td></tr><tr><td>11</td><td></td><td></td><td></td><td>[110]</td></tr><tr><td>Co<sub>2+</sub></td><td>515</td><td>0.585</td><td>0.742</td><td></td></tr><tr><td>Ni<sub>2+</sub></td><td>495</td><td>0.689</td><td>0.328</td><td></td></tr><tr><td>Pd<sub>2+</sub></td><td>495</td><td>0.654</td><td>0.856</td><td></td></tr></tbody></table>

### 5.3. Catalysis and Coordination Chemistry

The catalytic activity of Cu(II), Co(II), and Ni(II) azo-Schiff base complexes (Figure 27) was tested for the oxidation of various alkenes (cyclooctene, cyclohexene, styrene, α-methylstyrene, and norbornene). It was found that under the optimized reaction conditions, the copper(II) complex displayed 94% conversion for the oxidation of cyclooctene, and the cobalt(II) and nickel(II) complexes exhibited 90 and 85% conversions for the oxidation of α-methyl styrene, respectively. The authors demonstrated that back electron transfer from the complexes to TBHP (tert-butyl hydroperoxide, the oxidant used) breaks the O-O bond and forms tert-butoxyl radicals [114].

<figure><img src="image_36.png" /><figcaption>**Figure 27.** Azo-Schiff base catalyst and proposed mechanism of oxidant activation [114].</figcaption></figure>

Very recently, the Suzuki-Miyaura coupling reactions of phenylboronic acid with aryl bromides were also investigated using Pd(II) complexes (Figure 28) [115].

Various aryl bromides were tested with these complexes, giving very high yields (Table 6), and in the case where 4-bromoacetophenone was used, the highest yield of 99% was obtained with catalysts 12–14, while the lowest efficiency was obtained when catalyst 17 was used (94%). But in the presence of 4-bromobenzaldehyde, the highest yields were
obtained with catalyst 15, while the lowest yield was observed when catalyst 14 was used with 86% efficiency. When an electron-donating group is present, catalysts 13 and 14 seem to work the best. So, there is not really any structure-activity relationship.

<figure><img src="image_37.png" /></figure>

<figure><img src="image_38.png" /><figcaption>**Figure 28.** Some of the complexes used for Suzuki coupling [115].</figcaption></figure>

<table><caption>**Table 6.** Results of Suzuki–Miyaura coupling reactions [115].</caption><thead><tr><th>R</th><th>Catalyst</th><th>Yield (%)</th></tr></thead><tbody><tr><td rowspan="6">CH<sub>3</sub></td><td>12</td><td>95</td></tr><tr><td>13</td><td>88</td></tr><tr><td>14</td><td>97</td></tr><tr><td>15</td><td>91</td></tr><tr><td>16</td><td>95</td></tr><tr><td>17</td><td>90</td></tr><tr><td rowspan="6">OMe</td><td>12</td><td>96</td></tr><tr><td>13</td><td>98</td></tr><tr><td>14</td><td>98</td></tr><tr><td>15</td><td>96</td></tr><tr><td>16</td><td>93</td></tr><tr><td>17</td><td>97</td></tr><tr><td rowspan="6">C(O)CH<sub>3</sub></td><td>12</td><td>99</td></tr><tr><td>13</td><td>99</td></tr><tr><td>14</td><td>99</td></tr><tr><td>15</td><td>97</td></tr><tr><td>16</td><td>98</td></tr><tr><td>17</td><td>94</td></tr><tr><td rowspan="6">CHO</td><td>12</td><td>94</td></tr><tr><td>13</td><td>92</td></tr><tr><td>14</td><td>86</td></tr><tr><td>15</td><td>95</td></tr><tr><td>16</td><td>94</td></tr><tr><td>17</td><td>94</td></tr></tbody></table>

For the N-alkylation reaction via hydrogen borrowing, nickel catalysis using hydrox-yazobenzene as a ligand was performed and gave access to the N-alkylation of a variety
of anilines with alcohols, with moderate to good yields. What is interesting is that the
hydrogen atom transfer (HAT, Figure 29) to the reduced azo backbone for alcohol oxidation
occurred, as opposed to a conventional mechanism [116].

<figure><img src="image_39.png" /><figcaption>**Figure 29.** Proposed mechanism [116].</figcaption></figure>

Bis(phenoxy-azo)titanium(IV) complexes were also used for the polymerization of styrene. It is interesting to note in this article that due to its poor σ-donating character, the N atom of the azo group forms long Ti–N bonds, which in turn lead to a more open coordination sphere around the Ti centre. Unfortunately, the bis(phenoxy-azo)titanium complexes do not undergo photoinduced E → Z isomerization in their chelating azobenzene ligand frameworks. We attribute this behaviour to the relatively strong Ti–N and Ti–O bonds, which cannot be broken in the course of the photoisomerization reaction [117].

When the diazo moieties are part of a porous organic polymer (POP), it can not only permit the complexation of metals such as zinc but also, with a high surface area, allow for the conversion of carbon dioxide. This is the case of Zn/HAzo-POP, which was able to catalyze the reaction between propylene oxide and CO₂ [118].

5.4. *Biomedical and Environmental Applications*

The MCF-7 cell line is a widely used human breast cancer model, originally isolated from a metastatic breast cancer patient in 1970. These cells are estrogen receptor-positive (ER+) and progesterone receptor-positive (PR+), making them an ideal system for studying hormone-dependent breast cancer [119]. MCF-7 cells exhibit an epithelial-like morphology and grow in response to estrogen, allowing researchers to investigate the mechanisms of cancer proliferation, hormone signalling, and drug sensitivity [120]. HeLa cells are the first immortal human cell line, derived in 1951 from the cervical cancer tumour of Henrietta Lacks [121]. These cells are remarkable for their ability to proliferate indefinitely under suitable laboratory conditions,
making them a cornerstone of biomedical research. HeLa cells have been used in countless scientific breakthroughs, including the development of the polio vaccine, cancer research, and studies on viruses and cell biology. However, they are highly genetically unstable, which can affect experimental outcomes. Despite ethical concerns about their origin, HeLa cells remain one of the most important tools in medical and biological research [122].

In this context, it is urgently needed to find anticancer agents and especially cancer-selective ones. Very recently, the cytotoxicity of functionalized hydroxyazobenzene copper(II) complexes (Figure 30) was investigated in the human breast cancer cell line MCF-7 and the human cervical cancer cell line HeLa, demonstrating selective cytotoxicity against cancer cells with a GI₅₀ < 10 µg/mL [123].

Another application, in which hydroxyazobenzene is coupled to rhodamine, is the fluorescence imaging of HeLa cells incubated with Cu²⁺. This experiment confirms that this type of sensor has good cell permeability and can be useful and specific for Cu(II) sensing in living cells [124].

<figure><img src="image_40.png" /><figcaption>**Figure 30.** Structures of ligands (a) in ref. [123], (b) in ref. [124], and (c) in ref. [125] and ellipsoid representation of copper complex from (a) [123]. Reprinted with permission from Ref. [123]. Copyright (Elsevier) 2025.</figcaption></figure>
In 2024, o-aminoazotoluene, which is capable of photoisomerization, and o-vanillin, a potent comutagen, were used to synthesize a new ligand which, upon complexation with copper(II), results in a new copper(II) complex—Cu(L)₂ [125]. This complex had excellent results against MCF-7 cell lines with an IC50 of 4.2 ± 0.53 µM (Figure 30).

In the field of antimicrobial agents, and especially against *Staphyllococcus aureus* or *Pseudomonas aeruginosa*, it was shown that the stronger effect of complexes against the ligand alone could be due to the chelation of ligands with metal ions, facilitating the permeability of the drug to the cell's environment. For example, Schiff base azobenzenes complexed with cobalt, nickel, or copper ions (Figure 31) decrease the minimal inhibitory concentration (MIC) from approximately 350 mg/L for the ligand alone to less than 50 mg/L [126]. Zinc complexes can also have excellent MIC values against Gram-positive and Gram-negative bacteria, compared to chloramphenicol (Table 7, Figure 31) [127]. Copper and nickel complexes of the same ligands were also compared for their ZOI (zone of inhibition) against several bacteria, and the results show that depending on the ligand or the metal, the structure-activity relationship is quite impossible to obtain [128].

<figure><img src="image_41.png" /><figcaption>**Figure 31.** Structure of azo-Schiff base copper complex 18 [126], zinc complex 19 [127], copper and nickel complexes 20 [128], cobalt and nickel complexes 21 [129], and copper and iron 22 [130].</figcaption></figure>

When the examined organisms were *Salmonella typhimurium* and *Staphylococcus aureus*, the results obtained showed that Ni(II) complex 21b (Table 7, Figure 31) displayed good activity towards S. aureus, within the 11.97 mm inhibition zone, whereas Co(II) complex 21a showed high efficiency contra S. Typhimurium within the 11.13 mm inhibition zone [129]. It is interesting to note that azo-azomethine complexes 22a and 22b exhibited
moderate antimicrobial activity against bacterial strains, but this activity was insignificant against fungi, revealing a good selectivity against pathogens [130].

<table><caption>**Table 7.** Compiled antimicrobial effects against bacteria from complexes **19–22**.</caption><thead><tr><th>Micro-Organisms</th><th>ZOI</th><th>MIC</th><th>Ref</th></tr></thead><tbody><tr><td rowspan="4">Salmonella typhimurium</td><td>19a</td><td>-</td><td>125 µM/mL</td><td>[127]</td></tr><tr><td>19b</td><td>-</td><td>250 µM/mL</td><td>[127]</td></tr><tr><td>19c</td><td>-</td><td>125 µM/mL</td><td>[127]</td></tr><tr><td>21a</td><td>11.13 mm</td><td>-</td><td>[129]</td></tr><tr><td rowspan="10">Staphylococcus aureus</td><td>19a</td><td>-</td><td>7.81 µM/mL</td><td>[127]</td></tr><tr><td>19b</td><td>-</td><td>15.63 µM/mL</td><td>[127]</td></tr><tr><td>19c</td><td>-</td><td>3.90 µM/mL</td><td>[127]</td></tr><tr><td>20a</td><td>15 mm(Cu), 12 mm (Ni)</td><td>-</td><td>[128]</td></tr><tr><td>20b</td><td>17 mm (Cu), 13 mm (Ni)</td><td>-</td><td>[128]</td></tr><tr><td>20c</td><td>17 mm (Cu), 12 mm (Ni)</td><td>-</td><td>[128]</td></tr><tr><td>20d</td><td>16 mm (Cu), 14 mm (Ni)</td><td>-</td><td>[128]</td></tr><tr><td>21b</td><td>11.97 mm</td><td>-</td><td>[129]</td></tr><tr><td>22a</td><td>13 mm</td><td>128 µg/mL</td><td>[130]</td></tr><tr><td>22b</td><td>11 mm</td><td>256 µg/mL</td><td>[130]</td></tr><tr><td rowspan="10">Escherichia coli</td><td>19a</td><td>-</td><td>62.5 µM/mL</td><td>[127]</td></tr><tr><td>19b</td><td>-</td><td>250 µM/mL</td><td>[127]</td></tr><tr><td>19c</td><td>-</td><td>62.5 µM/mL</td><td>[127]</td></tr><tr><td>20a</td><td>15 mm (Cu), 20 mm (Ni)</td><td>-</td><td>[128]</td></tr><tr><td>20b</td><td>19 mm (Cu), 14 mm (Ni)</td><td>-</td><td>[128]</td></tr><tr><td>20c</td><td>20 (Cu)</td><td>-</td><td>[128]</td></tr><tr><td>20d</td><td>12 mm (Cu), 14 mm (Ni)</td><td>-</td><td>[128]</td></tr><tr><td>22a</td><td>15 mm</td><td>64 µg/mL</td><td>[130]</td></tr><tr><td>22b</td><td>17 mm</td><td>256 µg/mL</td><td>[130]</td></tr><tr><td rowspan="3">Bacillus subtilis</td><td>19a</td><td>-</td><td>7.81 µM/mL</td><td>[127]</td></tr><tr><td>19b</td><td>-</td><td>31.25 µM/mL</td><td>[127]</td></tr><tr><td>19c</td><td>-</td><td>7.81 µM/mL</td><td>[127]</td></tr><tr><td rowspan="4">Enterococcus faecalis</td><td>20a</td><td>12 mm (Cu), 14 mm (Ni)</td><td>-</td><td>[128]</td></tr><tr><td>20b</td><td>18 mm (Cu), 15 mm (Ni)</td><td>-</td><td>[128]</td></tr><tr><td>20c</td><td>14 mm (Cu)</td><td>-</td><td>[128]</td></tr><tr><td>20d</td><td>17 mm (Cu), 17 mm (Ni)</td><td>-</td><td>[128]</td></tr><tr><td rowspan="4">Enterobacter cloacae</td><td>20a</td><td>12 mm (Cu), 22 mm (Ni)</td><td>-</td><td>[128]</td></tr><tr><td>20b</td><td>15 mm (Cu), 15 mm (Ni)</td><td>-</td><td>[128]</td></tr><tr><td>20c</td><td>17 mm (Cu), 12 mm (Ni)</td><td>-</td><td>[128]</td></tr><tr><td>20d</td><td>13 mm (Cu), 16 mm (Ni)</td><td>-</td><td>[128]</td></tr><tr><td rowspan="4">Micrococcus luteus</td><td>20a</td><td>13 mm (Cu), 14 mm (Ni)</td><td>-</td><td>[128]</td></tr><tr><td>20b</td><td>21 mm (Cu), 17 mm (Ni)</td><td>-</td><td>[128]</td></tr><tr><td>20c</td><td>19 mm (Cu), 14 mm (Ni)</td><td>-</td><td>[128]</td></tr><tr><td>20d</td><td>18 mm (Cu), 16 mm (Ni)</td><td>-</td><td>[128]</td></tr></tbody></table>

## 6. Conclusions

Phenolic azobenzene derivatives represent a uniquely versatile class of compounds at the intersection of photochemistry, coordination chemistry, and materials science. Their dual functional nature—combining the reversible photoisomerization capability of the azobenzene core with the metal-binding propensity of the phenolic group—enables a wide range of applications, from colorimetric sensing and smart materials to catalysis, solar energy conversion, and biomedical fields. The diversity in synthetic strategies, including azo coupling, Baeyer–Mills reactions, and oxidation–reduction pathways, allows for fine structural tuning and functionalization, further broadening their applicability.

Particularly notable is their effectiveness as ligands in the formation of stable metal complexes, which exhibit enhanced photophysical, catalytic, and bioactive properties. These complexes have shown promise not only in environmental and industrial contexts but also in the development of anticancer and antimicrobial agents. As demonstrated in dye-sensitized solar cells (DSSCs), phenolic azobenzene–metal complexes contribute to improved light-harvesting and electron transfer efficiencies.

Future developments in this field could focus on expanding the functional diversity of these ligands, improving synthetic efficiencies, and deepening the understanding of
structure-activity relationships to design next-generation materials with tailored properties. Overall, phenolic azobenzenes stand out as highly adaptable and functional scaffolds for advancing molecular design across multiple scientific domains.

**Author Contributions:** J.H. writing, J.I. writing and correcting, E.L. writing and correcting and templating. All authors have read and agreed to the published version of the manuscript.

**Funding:** This research was funded by TIMR Laboratory, UTC/ESCOM, and Slovenian Research and Innovation Agency (grant P1-0134).

**Acknowledgments:** The authors would like to acknowledge the Erasmus grant which allowed for the travelling of researchers and Students in Slovenia and France.

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

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