# High-Field Growth of Semiconducting Anodic Oxide Films on Metal Surfaces for Photocatalytic Application

Authors: Ronald Vargas; David Carvajal; Brunella Galavis; Alberto Maimone; Lorean Madriz; Benjamín R. Scharifker
Journal: International Journal of Photoenergy
 (2019)

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## Abstract

This work summarizes progresses achieved in the physical chemistry aspects of the growth of anodic oxides under high-field conditions for the synthesis of semiconducting thin solid films and their implementation as photocatalytic materials. We discuss the scope and mechanisms for anodic oxide growth, describing the development of kinetic models and the correlations between theory and kinetic data, leading to fundamental information to characterize the primary processes occurring during the anodization of valve metals under high fields. The main features related to the widely used self-assembly of nanostructures by valve metal anodization are highlighted and briefly discussed. This is followed by general considerations of heterogeneous photocatalysis on these functional materials, considering the kinetics of the heterogeneous catalytic processes involved and the overall photoelectrochemical performance. High control of the characteristics of the materials obtained with the method described, combined with the possibility of electrochemically assisting photocatalysis, allows application of this technology to the treatment of wastewaters, energy conversion, and related fields.


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## Body

## 1. Introduction

Numerous investigations in recent years have focused on the development of heterogeneous photocatalysts activated by sunlight and their applications to the environmental purification of wastewater, conversion of solar energy, and production of H2 [1–22]. Electrochemically assisted photocatalysis shows superior performance in terms of purification of water from organic matter [12], polarization between two electrodes during the photocatalytic process assisting in separating the charge carriers and catalyzing the redox reactions, thus enhancing the efficiency of mineralization of the pollutants [12, 15, 16, 23]. Moreover, efforts have been directed to developing nanostructured photocatalysts of different nature [24–27]. Most applications involve colloidal semiconductors [8, 24, 28], but the use of large area nanostructured thin solid films has been rapidly growing in the past few years [12, 16], and methods to obtain films made of stable materials and/or composites under controlled conditions, with the possibility of modulating the morphology of the nanostructured films, are needed. High-field anodic growth of metal oxide and its alloys offers these possibilities, but to achieve these goals, fundamental understanding of the dynamics of the electrochemical processes in the solid state during metal anodization must be obtained, leading to the rational design of suitable synthetic methods for functional nanostructured films of interest. On the other hand, application of these materials to photocatalytic systems needs the estimation of the kinetic parameters of the heterogeneous reactions and the kinetics of the photochemical processes. Furthermore, optimization of the solar to chemical energy conversion during the photocatalytic process requires the design of efficient photochemical reactors, with appropriate comparison of their performance in relation to different photocatalytic systems.The aim of this work is to summarize the salient physicochemical concepts involved in the growth of anodic oxide films on metal surfaces under high fields, to rationalize the precise control of the structural and morphological characteristics of the semiconductor materials obtained, that this synthetic method allows. We also discuss the heterogeneous photocatalysis based on these functional materials, considering their photoelectrochemical performance as well as the kinetics of the heterogeneous catalytic processes involved, in relation to their use in the environmental problem of treating wastewaters.


## 2. Anodic Oxide Growth on Metal Surfaces

The passivation of iron-based materials was described in 1836 by Schönbein and Faraday, who identified the phenomenon as a chemical process involving the formation of an oxide thin layer on the metal surface [29].In this case, it is usually observed that metals become passive by formation of dense oxide thin films exhibiting low ionic conductivity, thus inhibiting the active dissolution,M→Mz++ze−, or corrosion of the underlying metal, with the oxides representing barriers to the flow of ions and electrons [30, 31]. This leads to valve-like behavior, with current rectification upon reversal of the electrical potential and film thickness proportional to the electric field. The passive thin film is then formed by the anodic reaction depicted by [30, 31].
(1)M+z2H2O→MOz/2+zH++ze−The anodization reaction (1) leads to the synthesis of highly reproducible thin solid films of valve metal oxides. The anodization process may also occur from lower oxides
(2)MOy/2+z−y2H2O→MOz/2+z−yH++z−ye−and an oxide film may also be formed by electrocrystallization of ions from solution
(3)My++zH2O→MOz/2+zH++z−ye−Anodic potentials enhance passivation according to equations (1)-(3) but transpassivity and anodic breakdown cause the opposite effect [31]. The opposite process implies reduction reactions that destabilize the passive films leading to cathodic breakdown.Figure1 shows a simple scheme of the several ion- and electron-transfer reactions (ITRs and ETRs, respectively) that may occur during anodization processes; these chemical process may stabilize or dissolve the passive film [30, 31].Figure 1
Scheme of the several ion-transfer reactions (ITRs) and electron-transfer reactions (ETRs) during the anodization processes.The most important processes are summarized as follows [30, 31]:
(1)
Electron-transfer reactions (iredox), e.g., oxygen evolution
(2)
Growth of the thin oxide film (iox) by the transfer of oxygen ions from the electrolyte into the oxide
(3)
Transfer of metal ions from the oxide to solution and oxidation of water (iox)
(4)
Reduction by the reverse reactions (ired)
(5)
Corrosion, with charge transfer by metal ions compensated by that of oxygen ions (iox+ired=0)
(6)
Capacitive charging of the interface (iC) upon potential changesThe total current flowing through the interface is then described by(4)i=iredox+iox+ired+iC.Following Young [32], a classification based on the experimental observations indicates that the chemical elements with a complete valve effect are Al, Bi, Sb, Ta, Ti, and Nb and those with an incomplete valve effect are Ag, Cd, Fe, Mg, Si, Sn, W, Zn, and Zr, the behavior depending on the composition of the solution used during the anodization process [32].Figure2 shows a typical experimental setup to obtain thin solid films by the anodization process. The preparation of passive films is affected by the experimental conditions [30, 31]. The following aspects are usually important: (i) effects due to the presence of a native passive film and pretreatment of the metal surface; (ii) potential-time program for anodization; (iii) chemistry of the solution: pH, possibility of corrosion, nature of supporting electrolyte, presence of ions as possible doping agents, and additives for the promotion of nanostructures; (iv) hydrodynamics (bubble control in the presence of parallel gas evolution reactions, possibility of erosion of the formed passive film, and enhanced mass transport of ions in the case of synthesis of doped thin films); and (v) posttreatment of the metal oxide film as drying, modification, or thermal treatment.Figure 2
Scheme of experimental setup for obtained thin solid films by the anodization.


## 3. High-Field Anodization

Oxide films of valve metals can be formed after anodic polarization under high fields higher than1×106 V/cm. Under such conditions, oxide growth occurs by ion hopping between regular sites or interstitial positions in the lattice. The hopping mechanism requires an activation energy W which increases exponentially with the jump distance a; thus, it is only possible between neighboring sites [30], and the process is catalyzed by imposing increasingly positive potentials.In general, application of an appropriate anodic polarization implies the formation of an oxide layer involving oxidation of the metal at the metal–oxide interface by reaction with the flux of oxygen ions migrating from the solution across the oxide film, assisted by the electric field. The final result is metal consumption, with the oxide layer growing in the solid state. A representation of this process is shown in Figure3.Figure 3
Scheme of ion transport during high-field anodization.The electrochemical potential of ions and the energies of electrons in the electron bands depend on the local Galvani potential, which is a function of the electronic and ionic conductivities of the metal oxide, the thickness of the film, and the pH of the solution [30, 31]. The excess charges at the interface generate a space charge region within the oxide; therefore, local potential changes result in a linear field that controls the migration of charge carriers, i.e., ions and electrons. Metal oxides usually show semiconducting behavior, thus implying capacitive charge accumulation in the solid state. A potential drop occurs across the film but charge accumulation at the solid–electrolyte interface is only possible for very thin oxide films, in which case the capacitance of the oxide film becomes comparable to the inner Helmholtz plane capacitance at the interface [31]. If the potential drop occurs within the film, then migration of charge carriers within the film controls the anodic growth.Due to several reasons, films may suffer local enhancement of the conductivity during the anodization process. The oxide lattice may not withstand the large ion or electron fluxes arising at very high fields, or else, high reaction rates of corrosion due to the presence of aggressive chemical species (like chloride or fluoride ions) may locally increase the conductivity, leading to breakdown of the passive film. This may be indicated by several effects such as irregular current peaks, visible sparks, potential fluctuations, increasing electrical noise or even audible noise, depending on the oxide bandgap, and the nature and concentration of ions in solution [30–48].


## 4. Kinetic Model

In order to represent the high-field anodization phenomenon, Figure4 shows two lattice planes corresponding to stable sites at the positions “x” and “x+a,” then the ion flux dn/dt at the metal–oxide interface can be obtained from the reaction rate in terms of the mole balance for the transference [30].
(5)dndt=dn→dt−dn←dt=nxp→−nx+ap←,where n→ and n← stand for the ion movements in either direction across the film and p→ and p← are the probabilities of the atomic hopping processes, equivalent to kinetic constants for the microscopic balance. Their values can be estimated with an Arrhenius type relationship.
(6)p=ϑexp−WRT,where ϑ is the attempt frequency for the hopping ions and W is the activation energy of this process. In Figure 4, the ions are centered in stable positions in the lattice; these stable positions imply minima in the potential energy of the crystal.Figure 4
Effect of the electric potential on the activation barrier for the hopping mechanism between two adjacent planes in the oxide lattice.In the absence of an electric field, the activation energy and the hopping probabilities are equal for both hopping directions. An electric field contributes to the potential energy and catalyzes the hopping mechanism due to the asymmetry generated in the energy–position coordinate profile (see Figure4), the potential providing free energy to decrease the effective energy barrier.Considering the fundamental chemical kinetics theory for electrochemical processes by Butler and Volmer (see details and other considerations in, e.g., [30, 33]), the activation energy can be rewritten as
(7)W→=W−αazFEfand
(8)W←=W−1−αazFEf,where α is the transfer coefficient that describes the symmetry of the activation barrier, α defines the distance between positions of minimal energy, z is the charge number of the electroactive species, F is the Faraday constant, Ef is the field strength, and Ef=E−E°/d, where E is the applied potential, E° is the equilibrium potential of the oxide electrode, and d is the thickness of the film.Then, the reaction rate can be expressed in terms of the current flux at the interface after the consideration of the Faraday second lawi=zFdn/dt and substitution of (6), (7), and (8) in (5) yields
(9)i=aϑρCexp−WRTexpαazFEfRT−exp1−αazFEfRT,where ρC=n/azF is the concentration of mobile charges.Furthermore, the presence of a high electric field implies ion movement in the growth direction; the opposite movement is improbable thus the high-field reaction rate becomes(10)i=aϑρCexp−WRTexpαazFEfRT.After recognizing that the exchange current isi0=aϑρCexp−W/RT and the Tafel slope is β=αazF/RT and substituting Ef=E−E0/d, (10) simplifies into (11) as follows:
(11)i=i0expβE−E0d.This is a simple relation that indicates the exponential dependence of the reaction rate with the applied potential. The correspondence of the current–time experimental data obtained at constant potential with (11) thus indicates that the rate-determining step for the oxide growth is the movement of the ions within the oxide. Additionally, if the potential drop occurs only within the film, with 100% Faradic efficiency for film growth, i.e., no oxide dissolution, no oxygen evolution nor capacitive charging, then the film thickness can be estimated as [34]
(12)d=d0+MzFAρox∫0titdt,where d0 is the oxide film thickness initially present, ρox the oxide density, A is the electrode surface area, M the oxide molecular weight, and ∫0titdt is the charge transferred for oxide growth.This result indicates the possibility of describing the oxide thickness during valve metal oxide growth as a linear function of the charge passed during anodic polarization, and it is an important feature for controlling the synthesis of thin films of metal oxide semiconductors. Another significant feature of this methodology is that the potential determines the kinetics of the phenomena that occur at the interface.


## 5. Metal Oxide Nanotubes Synthesized by High-Field Anodization

In 1999, Zwilling and coworkers reported a simple methodology for the synthesis of self-organized metal oxide nanotubes based on the high-field electrochemical anodization technique in HF electrolytes [49]. TiO2 nanotubes were the first nanostructures obtained, but the approach was extended to other valve metals as tungsten, zirconium, hafnium, thallium, titanium alloys, and diverse valve metals alloys [22, 27, 50]. In general, highly ordered arrays of vertically aligned nanotubes or nanopores result from this electrochemical synthesis, in a closely packed structure and with a wide range of characteristics for functional applications, such as
(i)
high photocatalytic activity
(ii)
high resistance to the photocorrosion process
(iii)
good biocompatibility for drug release systems
(iv)
good electrode materials for diverse sensing applications
(v)
electrodes suitable for Li ion batteries and fuel cells
(vi)
good materials for solar energy conversion in solar cells
(vii)
self-cleaning materials
(viii)
materials for new optical devicesAs discussed below, whether oxidation leads to the anodic growth of a compact oxide on the metal surface or the formation of an array of nanotubes is determined by the competition of two chemical processes: the anodic oxide formation at high fields defined by (1) on the one hand and the chemical dissolution of the oxide through the formation of fluoride complexes
(13)MOz/2+z+2F−+zH+→MFz+22−+z2H2Oon the other. The formation of complexes may occur also by direct reaction of fluoride with the metal cation transported by the high field at the oxide-electrolyte interface:
(14)Mz++z+2F−→MFz+22−Figure5(a) shows a simple scheme to visualize the microscopic transport phenomena that occur during the high-field anodization of titanium in aqueous electrolyte. In the presence of fluoride ions, Figure 5(b), the situation changes dramatically by dissolution of TiO2 at the electrode–electrolyte interface. At least two new phenomena need to be considered, (i) the ability to form water-soluble TiF62- complexes and (ii) the incorporation of fluoride into the growing film due to its small ionic radius, implying the field-assisted transport of this ion through the oxide film and thus competing with the transport of oxygen ions O2- in the solid state. The initial nanopores formed at the surface develop in a nanotubular array due to the competition of the high-field electrochemical formation of TiO2 and the formation of Ti-F complexes by the chemical attack of fluoride to the formed TiO2 [22, 50].Figure 5
Anodization process representation in (a) absence of fluoride electrolyte and (b) presence of fluoride electrolyte.Figure6(a) depicts the current-time curve registered from high-field anodization with formation of a nanotube array film. In this case, the electrolyte is an aqueous solution containing fluoride ions. Three stages are observed: in phase I, an initial exponential decay of the current, then the current increases during phase II after a time delay dependent on the fluoride concentration, with shorter delays at higher fluoride concentrations. In phase III, the current reaches a steady state at a value directly proportional to the fluoride concentration in solution. Figure 6(b) depicts the steps involved in the formation of the nanotube array film. A barrier oxide is formed during phase I leading to the decay of the current; during phase II, the surface is locally activated with pores which start to grow randomly, increasing the active area and originating the rising current. In phase III, the pores interfere with each other as the chemical process of film formation and dissolution far from equilibrium is maintained, leading to a steady-state dissipative structure with minimal entropy production [51]; in this stage, the current flow is equally shared by the available pores, and self-ordering conditions are established. A rigorous treatment of self-ordering in the formation of nanotubes is still lacking; theoretical and experimental studies are needed to elucidate it and contribute to the rational optimization of the synthesis of nanotubes. Notwithstanding, the evidence available makes it clear that according to the scheme presented in Figure 6, self-ordered nanotubular films of valve metals can be formed by high-field anodization in fluoride-rich electrolytes. Figure 6(c) shows the ideal nanotubular array film, correlating its formation to the competing rates of the two major phenomena, the electrochemical growth of the metal oxide and its chemical dissolution by formation of the metal-fluoride complex [22, 50].Figure 6
Key steps during the self-organized nanotube layer formation based on anodization process in fluoride electrolyte.According to the discussion above, the factors to consider for the synthesis of nanostructured films are (i) a high-field anodization protocol with a valve metal or an alloy of these metals, (ii) a potential-time program for anodization, (iii) an electrolyte containing fluorides, and (iv) the effects of a native passive film and pretreatment of the metal surface. Currently, self-assembled nanotube films of several semiconductors such as TiO2, WO3, ZrO2, HfO2, Ta2O5, Nb2O5, doped materials, binary alloys such as TiAl, TiNb, TiW, and TiZr, and biomedical alloys such as Ti6Al7Nb and Ti29Nb13Ta4.6Zr have been reported [22, 50].According to the literature [22], nanotube arrays with the following characteristics have been synthesized:
(1)
Directly attached to the metal
(2)
Annealed to an appropriate crystal phase
(3)
Typical dimensions (TiO2 nanotubes):
(a)
Length: 100 nm to 100μm (related to the anodization time)
(b)
Diameter: 10 nm to 500 nm (related to the voltage)
(c)
Wall thickness: 2 to 80 nmThe shape of the nanostructures can be controlled with the anodization voltage and the fluoride content or the nature of the fluoride chemical compound used in the electrolyte. Figure7 shows examples of shapes obtained in the case of TiO2 nanotubes.Figure 7
Experimental TiO2 nanotubes obtained after the anodization of Ti foil synthetized according to the methodology reported in [52].
(a)
(b)


## 6. Photocatalysis Based on Metal Oxides Synthesized under High Fields

### 6.1. General Considerations

The metal oxides synthesized by anodization methods typically result in a thin film with the semiconductor material attached to the metal substrate. This may represent an advantage for the collection of electrons generated during the light activation resulting in good efficiencies. Additionally, these films present good mechanical properties, such as high resistance to erosion and corrosion.The crystallinity of the semiconductor films may be improved after synthesis subjecting them to thermal treatments to promote phase transitions. The crystal phase determines the possibility of using the semiconductor material in some applications, the transformation depending on the temperature and pressure employed in a muffle reactor, and the use of an inert or an oxygen-rich atmosphere promoting stoichiometric or nonstoichiometric growth of the new phases. In certain occasions, mixed phases are of interest and in order to synthesize these materials, an initial phase is at first formed, with new conditions imposed later in accordance to the phase diagram of the material, with the kinetics of the phase transition determining the rate of synthesis of the new material.Doping the thin films formed by anodization is possible, either by incorporation of foreign ionic chemical species in a second anodization bath, by surface modification during a thermal treatment with a vapor compound, or by equilibrium adsorption of organic or inorganic compounds from aqueous solution [16].In general, characterization of the anodic thin films is needed, and diverse experimental techniques have been developed for these purposes: optical, electronic and/or atomic microscopy [50], electrochemical measures controlling voltage, current densities or charges [30–48], electrochemical impedance spectroscopy [53, 54], gravimetric measurements with the electrochemical quartz microbalance [55, 56], infrared absorption, Raman, laser, UV-vis, UV–vis reflectance, luminescence, acoustic, X-rays, resonance, ellipsometry, and neutron-based spectroscopies [15, 44–47, 50, 57–62], and dynamic characterization based on photoelectrochemical methods [23, 63, 64].


### 6.2. Photocatalytic Considerations

Under conditions of MOx/solar light photocatalysis, an electron from the valence band is promoted to the conduction band [65]:
(15)MOx+hν→MOxe−+h+generating a hole h+ in the valence band (VB) and an electron e− in the conduction band (CB). The holes can react with organic compounds to generate free radicals.
(16)h++R→R•++e‐They can also be trapped by water to form hydroxyl radicals on the surface of the photocatalyst:(17)h++H2O→HO•+H++e‐Charge balance is preserved by reaction of electrons in the CB with acceptor species dissolved in the aqueous solution. Thermodynamically, the reduction potential of this chemical species must be equal or more positive than the potential corresponding to the edge of the CB of the semiconductor; another necessary condition for reactivity is that the electron density of the redox couple in the electrolyte must overlap with the density of states of the CB. Frequently, overall charge balance is completed by the oxygen reduction reaction under solar light irradiation(18)e‐+O2→O2•‐or by reduction of an oxidized species Ox in solution capable of being reduced by an electron from the conduction band
(19)e‐+Ox→RedAdditionally, reduction can be electrochemically assisted, this implies separating the anodic and cathodic reactions, and after polarization, the electron at the CB can be extracted to the external circuit, enhancing charge separation, as shown in Figure8. Consequently, electron–hole recombination diminishes and general improvement of the light-induced redox reactions obtain.Figure 8
Scheme of electrochemical assisted photocatalysis.


### 6.3. Reaction Kinetics of the Photocatalytic Process

There are several parameters that influence the photocatalytic process [65, 66], for instance, the intensity of the radiation that reaches the surface of the photocatalyst. This variable is particularly important when the process is carried out on a pilot scale with an irradiance affected by the weather. When a photocatalytic reaction is carried out in a pilot-plant reactor, the reaction time needs normalization with respect to the intensity of incident radiation; otherwise, when considering time as an independent variable, its variation throughout the process by cloud cover and the distribution of the radiant flux in the reactor should be taken into account [67]. This problem has been addressed introducing a standardized lighting time tIpW,n accounting for the average radiation intensity
(20)tIpW,n=tIpW,n−1+ΔtnIexptnIpViVT,Δtn=tn−tn−1,where Ipexptn is the average of solar irradiation intensity measured during an experimental time interval Δtn and Vi and VT represent the irradiate volume in contact with the photocatalyst and the total volume of the reactor, respectively. For photocatalysts that absorb UV light, as TiO2, the typical UV power Ip=30 mW/cm2 of a perfectly sunny day is usually used. In the case of using photocatalysts that absorb visible radiation, (20) can be used considering the average solar radiation of the spectrum of a sunny day, Ip=1000-1500 W/m2 or some value that can be determined, or considered representative for the experimental setup. Advanced considerations for the design and operation of photocatalytic reactors have been reviewed [68].In the case of photocatalysis based on thin solid films obtained by the high-field anodization method, the nature of the film material, the disposition of the film with respect to the illumination, and the possibility of the electrochemical assisted photocatalysis influence the photocatalytic process [12, 15]. The morphology, crystal phase, and composition of the nanocatalyst affect the performance [12, 69]. Also, in photocatalytic reactions, the pH of the solution determines the charge of the catalyst surface. For example, changes in the pH can result in an improvement of the efficiency in the photocatalytic removal of pollutants in the presence of TiO2, due to the impact of the adsorbed states on the reaction rate on the photocatalyst [70–73].Another significant factor in the study of the chemical kinetics of photocatalysis is the nature and concentration of the substrate [28, 74]. Studies of concentration effects at otherwise constant conditions allow estimating the kinetic constants that characterize the reaction. The concentration of the organic substrate influences the saturation of active sites on the catalyst surface, deactivating them at high concentrations [75]. At typical radiation intensities at the surface of the Earth, photocatalytic reactions for the decomposition of organic compounds dissolved in water can be described according to the kinetic model of Langmuir and Hinshelwood. Basically, it involves fast establishment of adsorption-desorption equilibrium of the organic compound on the surface of the photocatalyst, with subsequent surface reaction of the adsorbed species with photogenerated hydroxyl radicals. The rate law describing such behavior is expressed by
(21)r=kKc1+Kc,where r is the reaction rate, c the concentration of the organic compound, k is the rate constant of the surface reaction between hydroxyl radicals and organic compound, and K is the equilibrium constant of adsorption-desorption of the organic compound on the surface of the photocatalyst [5, 65]. From this model, it can be seen that the kinetics of the reaction changes from first order to zero order as the concentration of the substrate increases, since with Kc<<1 the reaction rate becomes proportional to the concentration and with Kc>>1 the kinetics is independent of the concentration. Thus, the observed reaction constant turns out to be inversely proportional to the concentration of the organic compound, kobs=kK/1+Kc. This is difficult to detect from ln c vs. t plots [76]. However, upon plotting the inverse of the initial reaction rate as a function of the inverse of the initial concentration, a linear response is obtained and the kinetic constants characterizing the reaction on the specific photocatalyst can be determined as k=1/intercept and K=intercept/slope [5, 28, 65, 77]. When considering a multicomponent system or when reaction intermediaries accumulate significantly, the Langmuir-Hinshelwood model takes the following form:
(22)r=kKc1+Kc+ΣKici,where ∑Kici represents the contribution of the i-th components of the system; thus, the photocatalytic reaction involves a thermodynamic contribution, the adsorption of the adsorbate on the catalyst surface characterized by K, and a kinetic contribution due to the reaction of the adsorbate with the oxidant agents formed by electron transfer to the hole at the VB of the semiconductor, characterized by k.


## 6.1. General Considerations

The metal oxides synthesized by anodization methods typically result in a thin film with the semiconductor material attached to the metal substrate. This may represent an advantage for the collection of electrons generated during the light activation resulting in good efficiencies. Additionally, these films present good mechanical properties, such as high resistance to erosion and corrosion.The crystallinity of the semiconductor films may be improved after synthesis subjecting them to thermal treatments to promote phase transitions. The crystal phase determines the possibility of using the semiconductor material in some applications, the transformation depending on the temperature and pressure employed in a muffle reactor, and the use of an inert or an oxygen-rich atmosphere promoting stoichiometric or nonstoichiometric growth of the new phases. In certain occasions, mixed phases are of interest and in order to synthesize these materials, an initial phase is at first formed, with new conditions imposed later in accordance to the phase diagram of the material, with the kinetics of the phase transition determining the rate of synthesis of the new material.Doping the thin films formed by anodization is possible, either by incorporation of foreign ionic chemical species in a second anodization bath, by surface modification during a thermal treatment with a vapor compound, or by equilibrium adsorption of organic or inorganic compounds from aqueous solution [16].In general, characterization of the anodic thin films is needed, and diverse experimental techniques have been developed for these purposes: optical, electronic and/or atomic microscopy [50], electrochemical measures controlling voltage, current densities or charges [30–48], electrochemical impedance spectroscopy [53, 54], gravimetric measurements with the electrochemical quartz microbalance [55, 56], infrared absorption, Raman, laser, UV-vis, UV–vis reflectance, luminescence, acoustic, X-rays, resonance, ellipsometry, and neutron-based spectroscopies [15, 44–47, 50, 57–62], and dynamic characterization based on photoelectrochemical methods [23, 63, 64].


## 6.2. Photocatalytic Considerations

Under conditions of MOx/solar light photocatalysis, an electron from the valence band is promoted to the conduction band [65]:
(15)MOx+hν→MOxe−+h+generating a hole h+ in the valence band (VB) and an electron e− in the conduction band (CB). The holes can react with organic compounds to generate free radicals.
(16)h++R→R•++e‐They can also be trapped by water to form hydroxyl radicals on the surface of the photocatalyst:(17)h++H2O→HO•+H++e‐Charge balance is preserved by reaction of electrons in the CB with acceptor species dissolved in the aqueous solution. Thermodynamically, the reduction potential of this chemical species must be equal or more positive than the potential corresponding to the edge of the CB of the semiconductor; another necessary condition for reactivity is that the electron density of the redox couple in the electrolyte must overlap with the density of states of the CB. Frequently, overall charge balance is completed by the oxygen reduction reaction under solar light irradiation(18)e‐+O2→O2•‐or by reduction of an oxidized species Ox in solution capable of being reduced by an electron from the conduction band
(19)e‐+Ox→RedAdditionally, reduction can be electrochemically assisted, this implies separating the anodic and cathodic reactions, and after polarization, the electron at the CB can be extracted to the external circuit, enhancing charge separation, as shown in Figure8. Consequently, electron–hole recombination diminishes and general improvement of the light-induced redox reactions obtain.Figure 8
Scheme of electrochemical assisted photocatalysis.


## 6.3. Reaction Kinetics of the Photocatalytic Process

There are several parameters that influence the photocatalytic process [65, 66], for instance, the intensity of the radiation that reaches the surface of the photocatalyst. This variable is particularly important when the process is carried out on a pilot scale with an irradiance affected by the weather. When a photocatalytic reaction is carried out in a pilot-plant reactor, the reaction time needs normalization with respect to the intensity of incident radiation; otherwise, when considering time as an independent variable, its variation throughout the process by cloud cover and the distribution of the radiant flux in the reactor should be taken into account [67]. This problem has been addressed introducing a standardized lighting time tIpW,n accounting for the average radiation intensity
(20)tIpW,n=tIpW,n−1+ΔtnIexptnIpViVT,Δtn=tn−tn−1,where Ipexptn is the average of solar irradiation intensity measured during an experimental time interval Δtn and Vi and VT represent the irradiate volume in contact with the photocatalyst and the total volume of the reactor, respectively. For photocatalysts that absorb UV light, as TiO2, the typical UV power Ip=30 mW/cm2 of a perfectly sunny day is usually used. In the case of using photocatalysts that absorb visible radiation, (20) can be used considering the average solar radiation of the spectrum of a sunny day, Ip=1000-1500 W/m2 or some value that can be determined, or considered representative for the experimental setup. Advanced considerations for the design and operation of photocatalytic reactors have been reviewed [68].In the case of photocatalysis based on thin solid films obtained by the high-field anodization method, the nature of the film material, the disposition of the film with respect to the illumination, and the possibility of the electrochemical assisted photocatalysis influence the photocatalytic process [12, 15]. The morphology, crystal phase, and composition of the nanocatalyst affect the performance [12, 69]. Also, in photocatalytic reactions, the pH of the solution determines the charge of the catalyst surface. For example, changes in the pH can result in an improvement of the efficiency in the photocatalytic removal of pollutants in the presence of TiO2, due to the impact of the adsorbed states on the reaction rate on the photocatalyst [70–73].Another significant factor in the study of the chemical kinetics of photocatalysis is the nature and concentration of the substrate [28, 74]. Studies of concentration effects at otherwise constant conditions allow estimating the kinetic constants that characterize the reaction. The concentration of the organic substrate influences the saturation of active sites on the catalyst surface, deactivating them at high concentrations [75]. At typical radiation intensities at the surface of the Earth, photocatalytic reactions for the decomposition of organic compounds dissolved in water can be described according to the kinetic model of Langmuir and Hinshelwood. Basically, it involves fast establishment of adsorption-desorption equilibrium of the organic compound on the surface of the photocatalyst, with subsequent surface reaction of the adsorbed species with photogenerated hydroxyl radicals. The rate law describing such behavior is expressed by
(21)r=kKc1+Kc,where r is the reaction rate, c the concentration of the organic compound, k is the rate constant of the surface reaction between hydroxyl radicals and organic compound, and K is the equilibrium constant of adsorption-desorption of the organic compound on the surface of the photocatalyst [5, 65]. From this model, it can be seen that the kinetics of the reaction changes from first order to zero order as the concentration of the substrate increases, since with Kc<<1 the reaction rate becomes proportional to the concentration and with Kc>>1 the kinetics is independent of the concentration. Thus, the observed reaction constant turns out to be inversely proportional to the concentration of the organic compound, kobs=kK/1+Kc. This is difficult to detect from ln c vs. t plots [76]. However, upon plotting the inverse of the initial reaction rate as a function of the inverse of the initial concentration, a linear response is obtained and the kinetic constants characterizing the reaction on the specific photocatalyst can be determined as k=1/intercept and K=intercept/slope [5, 28, 65, 77]. When considering a multicomponent system or when reaction intermediaries accumulate significantly, the Langmuir-Hinshelwood model takes the following form:
(22)r=kKc1+Kc+ΣKici,where ∑Kici represents the contribution of the i-th components of the system; thus, the photocatalytic reaction involves a thermodynamic contribution, the adsorption of the adsorbate on the catalyst surface characterized by K, and a kinetic contribution due to the reaction of the adsorbate with the oxidant agents formed by electron transfer to the hole at the VB of the semiconductor, characterized by k.


## 7. Application of High-Field-Grown Semiconducting Anodic Oxide Films to Photocatalytic Processes

### 7.1. Photo(electro)catalysis

Photocatalysts obtained by high-field anodization have been reported [22, 78, 79, 82–86] with growing interest on self-assembled nanostructures, such as nanotubes of TiO2 and other materials [16, 22, 26, 27, 50]. Additionally, mineralization has been observed with electrochemically assisted photocatalysis [12, 22] and photocatalytic oxidations without polarization have been also reported [9, 50], but, in general, these reports have not been supported by kinetic studies to determine oxidation parameters, hindering identification of conditions for efficient mineralization. The simplest kinetic model to interpret heterogeneous photocatalysis, as discussed above, is that of Langmuir and Hinshelwood, and some reports explore the degradation of pollutants on semiconductor materials synthesized by anodization in terms of this kinetic model [9, 28, 75, 79–81]. Better understanding of the chemical kinetic principles of photocatalytic processes with application of bias potentials is also of interest [75, 82, 83].In recent years, efforts have been oriented in the structural modification of nanometric materials obtained by high-field anodization. The nonmetallic doping by thermal treatments in controlled atmosphere is a common strategy to obtain nanotubes of TiO2 with high oxygen vacancy density and Ti3+ in the structure. This results in new energy levels below the conduction band, increasing the density of charge carriers, improving the separation of charges by capture of electrons, and extending absorption towards the visible range [84, 85]. In addition, nanotube materials have been modified by decoration with metallic nanoparticles or semiconductors improving the generation and separation of charges [86, 87]. These electrodes are chemically stable and are presented as good candidates for the treatment of wastewater both by their high capacity to generate hydroxyl radicals [88] as well as photoanodes in photoelectrochemical cells for the production of H2 through the water-splitting reaction [88–90].The properties of the photocatalyst may be tuned changing the synthesis conditions. For example, mixed oxide nanotube layers of TiNb, TiMo, and TiW have been tested, and it has been found that under visible light-induced photocatalysis, the TiW oxide tubes show very high efficiency for methyl orange degradation [91–95]. A common approach has been to decorate the film with nanoparticles of Ag, Au, and alloys, other oxide materials, or by adsorption of dye sensitizers, with application of external bias. With these, increased photocatalytic activities have been invariably researched [78, 96, 97]. The many reports on the degradation of aliphatic alcohols [98–100], aliphatic carboxyl acids [98–101], aromatic alcohols [99, 102, 103], aromatic carboxyl acids [99, 100, 104], chloroaromatic compounds [99, 105], aromatic nitro compounds [106, 107], amino acids and derivates [99, 108], aromatic amines [109], surfactants [110], herbicides [111], and dyes [112–114] indicate that the materials obtained by the high-field anodization method are able to solve, with high efficiency, the environmental problem of wastewaters.


### 7.2. Analytical Chemistry and Sensing

Taking advantage of the good photocatalytic and structural characteristics of materials synthetized under high-field anodization, various applications as active elements for chemical sensors have been developed.TiO2 nanostructures have been used as photoelectrodes for the determination of chemical oxygen demand (COD) [115, 116]. The results demonstrated the possibility to achieve total oxidation of organic matter composed of diverse organic compounds. The COD study covered the range between 0 and 850 mg O2/L with good results in the presence of chlorides between 0 and 2000 ppm and pH between 4 and 10. In addition, the time of the determination was reduced to intervals between 1 and 5 min. As an added value of these investigations, the design, construction, and commercialization of the COD detection equipment were obtained. The technology based on TiO2 nanostructures formed by high-field anodization results in the principal component of the commercial analyzer COD PeCOD™ from ManTech Inc. The equipment is robust and requires the use of a source of ultraviolet radiation to activate the electrode; the time of average sampling is around 15 min. Recent reports improve reaction conditions for the use of modified TiO2 nanotubes [117].An additional widely documented application is the detection of H2 [15, 22, 118, 119]. The interaction of a gas with a metal oxide semiconductor is primarily a surface phenomenon. Therefore, nanoporous metal oxides offer the advantage of providing large sensing surface areas. It is known that the electrical resistance of materials such as TiO2 nanotubes is sensitive to H2, and the detection process is reversible. In general, the H2 sensor based on nanotubes demonstrated good sensitivity for the wide-range detection of dilute hydrogen atmospheres and high concentrations. For example, typical measurements ranging from 50 ppm to 2% H2 were reported. Another interesting feature is the possibility of performing the detection in a wide temperature range from 20°C to 300°C [15, 118, 119].


### 7.3. Self-Cleaning Surfaces

Anodization by high fields can be used to obtain self-cleaning surfaces [120], with adjustable and/or switchable water adhesion [121] and superhydrophobic properties for the corrosion resistance of the base material [122, 123], and with antimicrobial properties based on the photocatalysis principle too [124].Liu et al. [121] reported the use of two polymers responding to different physicochemical stimuli, (i) poly (N-isopropylacrylamide) and (ii) poly (dimethylamino) ethyl methacrylate. These compounds were used to modify the surface of previously anodized alumina substrates. The final composite material changes the adhesion of water droplets as a function of response conditions such as pH, temperature, and electrolyte composition. This type of surfaces will find applications in microfluids, generation of microdroplets, smart coatings, and self-cleaning surfaces.Similarly, Li and coworkers [120] have commented on the synthesis of alumina surfaces with macro/nanohierarchical structures made on aluminum substrates by an easy and fast anodization method. By means of a modification based on stearic acid, a superhydrophobic surface with a contact angle of 158° and an ultralow slip angle of about 0° was achieved. In addition, the superhydrophobic surface showed self-cleaning properties and corrosion resistance.Also, the antimicrobial properties of the TiO2 nanotubes prepared by the breakdown anodization process were studied. As a main result, the TiO2 nanotubes showed excellent bacterial inhibition percentages of 97.53% for E. coli and 99.94% for S. aureus, after 24 h of UV irradiation. Moreover, the authors demonstrated in the same study that the commercial and control samples did not show any antimicrobial property under the same conditions [124]. Other studies [122, 123] also showed good self-cleaning performance of the anodization process performed on valve metals and, by appropriate chemical modification in a second step, high resistance to corrosion with interesting wettability and anti-icing properties were obtained. In general, these surfaces show promising applications, including outdoor sports equipment, transportation facilities, and industrial machinery.


### 7.4. Photocatalytic Fuel Cell

The photocatalysis process is the light-induced combustion reaction of organic matter; therefore, if carried out in a separated compartment, it allows oxidation or organic compounds yielding the corresponding electron flux as an added value. To achieve this, the oxygen reduction reaction must be coupled in a cell using an appropriate electrocatalytic material, and determining factors are the control of electric losses during operation of the cell as well as selection of appropriate electrodes [125, 126].Liu et al. [127, 128] reported a TiO2-nanotube-array-based photocatalytic fuel cell system using visible light. First, a narrow bandgap semiconductor such as Cu2O and CdS was combined with TiO2 nanotubes. Second, the generation of electrical currents from the photocatalytic oxidation of various refractory organic compounds with oxygen reduction at the secondary electrode was evaluated. The studied model compounds included aromatics, azo dyes, pharmaceutical and personal care products, and endocrine-disrupting compounds. The approach demonstrated the possibility of obtaining energy from various refractory organic compounds with simultaneous water cleaning.Recently, Ye and coworkers [129] evaluated the application of a membrane-free photocatalytic fuel cell composed of a TiO2 nanotube array photoanode and a Cu cathode for micropollutant removal from water. They reported the most important operation conditions to obtain high performance, including pH, pollutant concentration, the oxygen reactive species that were formed, the presence of chemical substances as inorganic ions in the electrolyte, and the hydrodynamic conditions. Also, significantly enhanced removal of a commonly present aqueous micropollutant, 4-chloro-2 methylphenoxyacetic acid, was obtained.In general, it was found that the cell performance depended critically on the good conductivity of the high-field anode, as well as on the efficient photocatalytic degradation of the organic compounds. However, the use of appropriate materials, the quantum efficiency, and the design of reactors are aspects that still need to be improved by modern research [125, 126].


### 7.5. H2 Production

Thermodynamically, H2 production during the photocatalytic process is possible when the photoanode has a more negative conduction band potential than the redox potential required to form H2 from water. In general, the reaction rates of photocatalytic processes on numerous semiconducting materials are limited by the kinetics of the charge transfer process to a suitable redox species. Therefore, modifications of the electrodes with cocatalysts, such as Pt, Rh, Ru, Ag, Au, and its alloys, have been used to promote H2 evolution [22]. Photoanodes based on TiO2 nanotube layers have been reported to be more promising than nanoparticle layers, due to their well-defined geometry on the one hand, but especially because it is more feasible to incorporate cocatalysts, for example, by electrocrystallization and/or simple chemical reduction. Additionally, after the generation of charge carriers by sunlight, the electrons go to the back contact of the photoanode, then, electron lifetime and conductivity become determinant factors for the overall efficiency [17, 22, 26, 130].Spanu et al. [17] investigated a well-defined charge separation platform for photocatalytic H2 evolution based on a Pt-WO3-TiO2 “stacked” structure constructed on anodically grown TiO2 nanotube arrays. These structures show strongly improved photocatalytic H2 evolution, compared to any other single cocatalyst system such as Pt-TiO2, WO3-TiO2, and pristine TiO2 nanotubes. The photocatalytic activity is ascribed to the enhanced charge carrier separation mechanism enabled by the well-defined TiO2-WO3-Pt architecture that provides swift electron transfer through WO3 and towards Pt for H2 evolution.Additionally, Spanu et al. [130] remarked that the photocatalytic H2 evolution reaction on pristine TiO2 occurred with low efficiencies due to (i) trapping and recombination of charge carriers and (ii) sluggish electron transfer kinetics. Recently, this group introduced an approach to fabricate an efficient noble metal-free photocatalytic platform for H2 evolution. By dewetting NiCu bilayers into alloyed NiCu cocatalytic nanoparticles at the surface of TiO2 nanotube arrays, they found improvements in H2 production, especially when the metals were in equimolar proportion. The alloyed NiCu cocatalyst on TiO2 nanotubes allowed them to reach H2 generation rates comparable to those delivered by conventional decoration of TiO2 with noble metals such as platinum.Finally, we have considered the advantages of using anodic oxide thin films and the possibility of precisely controlling the characteristics of the final semiconductor materials by growing them under high fields. By enhancing charge separation through external application of electric potentials, their performance can be improved to facilitate the technological implementation of industrial photocatalysis. This advantage has been employed in several reactors of different design [12, 16, 22, 26, 80], but the industrial production of thin oxide films and photocatalytic reactors based on them is yet to be developed [12, 26].


## 7.1. Photo(electro)catalysis

Photocatalysts obtained by high-field anodization have been reported [22, 78, 79, 82–86] with growing interest on self-assembled nanostructures, such as nanotubes of TiO2 and other materials [16, 22, 26, 27, 50]. Additionally, mineralization has been observed with electrochemically assisted photocatalysis [12, 22] and photocatalytic oxidations without polarization have been also reported [9, 50], but, in general, these reports have not been supported by kinetic studies to determine oxidation parameters, hindering identification of conditions for efficient mineralization. The simplest kinetic model to interpret heterogeneous photocatalysis, as discussed above, is that of Langmuir and Hinshelwood, and some reports explore the degradation of pollutants on semiconductor materials synthesized by anodization in terms of this kinetic model [9, 28, 75, 79–81]. Better understanding of the chemical kinetic principles of photocatalytic processes with application of bias potentials is also of interest [75, 82, 83].In recent years, efforts have been oriented in the structural modification of nanometric materials obtained by high-field anodization. The nonmetallic doping by thermal treatments in controlled atmosphere is a common strategy to obtain nanotubes of TiO2 with high oxygen vacancy density and Ti3+ in the structure. This results in new energy levels below the conduction band, increasing the density of charge carriers, improving the separation of charges by capture of electrons, and extending absorption towards the visible range [84, 85]. In addition, nanotube materials have been modified by decoration with metallic nanoparticles or semiconductors improving the generation and separation of charges [86, 87]. These electrodes are chemically stable and are presented as good candidates for the treatment of wastewater both by their high capacity to generate hydroxyl radicals [88] as well as photoanodes in photoelectrochemical cells for the production of H2 through the water-splitting reaction [88–90].The properties of the photocatalyst may be tuned changing the synthesis conditions. For example, mixed oxide nanotube layers of TiNb, TiMo, and TiW have been tested, and it has been found that under visible light-induced photocatalysis, the TiW oxide tubes show very high efficiency for methyl orange degradation [91–95]. A common approach has been to decorate the film with nanoparticles of Ag, Au, and alloys, other oxide materials, or by adsorption of dye sensitizers, with application of external bias. With these, increased photocatalytic activities have been invariably researched [78, 96, 97]. The many reports on the degradation of aliphatic alcohols [98–100], aliphatic carboxyl acids [98–101], aromatic alcohols [99, 102, 103], aromatic carboxyl acids [99, 100, 104], chloroaromatic compounds [99, 105], aromatic nitro compounds [106, 107], amino acids and derivates [99, 108], aromatic amines [109], surfactants [110], herbicides [111], and dyes [112–114] indicate that the materials obtained by the high-field anodization method are able to solve, with high efficiency, the environmental problem of wastewaters.


## 7.2. Analytical Chemistry and Sensing

Taking advantage of the good photocatalytic and structural characteristics of materials synthetized under high-field anodization, various applications as active elements for chemical sensors have been developed.TiO2 nanostructures have been used as photoelectrodes for the determination of chemical oxygen demand (COD) [115, 116]. The results demonstrated the possibility to achieve total oxidation of organic matter composed of diverse organic compounds. The COD study covered the range between 0 and 850 mg O2/L with good results in the presence of chlorides between 0 and 2000 ppm and pH between 4 and 10. In addition, the time of the determination was reduced to intervals between 1 and 5 min. As an added value of these investigations, the design, construction, and commercialization of the COD detection equipment were obtained. The technology based on TiO2 nanostructures formed by high-field anodization results in the principal component of the commercial analyzer COD PeCOD™ from ManTech Inc. The equipment is robust and requires the use of a source of ultraviolet radiation to activate the electrode; the time of average sampling is around 15 min. Recent reports improve reaction conditions for the use of modified TiO2 nanotubes [117].An additional widely documented application is the detection of H2 [15, 22, 118, 119]. The interaction of a gas with a metal oxide semiconductor is primarily a surface phenomenon. Therefore, nanoporous metal oxides offer the advantage of providing large sensing surface areas. It is known that the electrical resistance of materials such as TiO2 nanotubes is sensitive to H2, and the detection process is reversible. In general, the H2 sensor based on nanotubes demonstrated good sensitivity for the wide-range detection of dilute hydrogen atmospheres and high concentrations. For example, typical measurements ranging from 50 ppm to 2% H2 were reported. Another interesting feature is the possibility of performing the detection in a wide temperature range from 20°C to 300°C [15, 118, 119].


## 7.3. Self-Cleaning Surfaces

Anodization by high fields can be used to obtain self-cleaning surfaces [120], with adjustable and/or switchable water adhesion [121] and superhydrophobic properties for the corrosion resistance of the base material [122, 123], and with antimicrobial properties based on the photocatalysis principle too [124].Liu et al. [121] reported the use of two polymers responding to different physicochemical stimuli, (i) poly (N-isopropylacrylamide) and (ii) poly (dimethylamino) ethyl methacrylate. These compounds were used to modify the surface of previously anodized alumina substrates. The final composite material changes the adhesion of water droplets as a function of response conditions such as pH, temperature, and electrolyte composition. This type of surfaces will find applications in microfluids, generation of microdroplets, smart coatings, and self-cleaning surfaces.Similarly, Li and coworkers [120] have commented on the synthesis of alumina surfaces with macro/nanohierarchical structures made on aluminum substrates by an easy and fast anodization method. By means of a modification based on stearic acid, a superhydrophobic surface with a contact angle of 158° and an ultralow slip angle of about 0° was achieved. In addition, the superhydrophobic surface showed self-cleaning properties and corrosion resistance.Also, the antimicrobial properties of the TiO2 nanotubes prepared by the breakdown anodization process were studied. As a main result, the TiO2 nanotubes showed excellent bacterial inhibition percentages of 97.53% for E. coli and 99.94% for S. aureus, after 24 h of UV irradiation. Moreover, the authors demonstrated in the same study that the commercial and control samples did not show any antimicrobial property under the same conditions [124]. Other studies [122, 123] also showed good self-cleaning performance of the anodization process performed on valve metals and, by appropriate chemical modification in a second step, high resistance to corrosion with interesting wettability and anti-icing properties were obtained. In general, these surfaces show promising applications, including outdoor sports equipment, transportation facilities, and industrial machinery.


## 7.4. Photocatalytic Fuel Cell

The photocatalysis process is the light-induced combustion reaction of organic matter; therefore, if carried out in a separated compartment, it allows oxidation or organic compounds yielding the corresponding electron flux as an added value. To achieve this, the oxygen reduction reaction must be coupled in a cell using an appropriate electrocatalytic material, and determining factors are the control of electric losses during operation of the cell as well as selection of appropriate electrodes [125, 126].Liu et al. [127, 128] reported a TiO2-nanotube-array-based photocatalytic fuel cell system using visible light. First, a narrow bandgap semiconductor such as Cu2O and CdS was combined with TiO2 nanotubes. Second, the generation of electrical currents from the photocatalytic oxidation of various refractory organic compounds with oxygen reduction at the secondary electrode was evaluated. The studied model compounds included aromatics, azo dyes, pharmaceutical and personal care products, and endocrine-disrupting compounds. The approach demonstrated the possibility of obtaining energy from various refractory organic compounds with simultaneous water cleaning.Recently, Ye and coworkers [129] evaluated the application of a membrane-free photocatalytic fuel cell composed of a TiO2 nanotube array photoanode and a Cu cathode for micropollutant removal from water. They reported the most important operation conditions to obtain high performance, including pH, pollutant concentration, the oxygen reactive species that were formed, the presence of chemical substances as inorganic ions in the electrolyte, and the hydrodynamic conditions. Also, significantly enhanced removal of a commonly present aqueous micropollutant, 4-chloro-2 methylphenoxyacetic acid, was obtained.In general, it was found that the cell performance depended critically on the good conductivity of the high-field anode, as well as on the efficient photocatalytic degradation of the organic compounds. However, the use of appropriate materials, the quantum efficiency, and the design of reactors are aspects that still need to be improved by modern research [125, 126].


## 7.5. H2 Production

Thermodynamically, H2 production during the photocatalytic process is possible when the photoanode has a more negative conduction band potential than the redox potential required to form H2 from water. In general, the reaction rates of photocatalytic processes on numerous semiconducting materials are limited by the kinetics of the charge transfer process to a suitable redox species. Therefore, modifications of the electrodes with cocatalysts, such as Pt, Rh, Ru, Ag, Au, and its alloys, have been used to promote H2 evolution [22]. Photoanodes based on TiO2 nanotube layers have been reported to be more promising than nanoparticle layers, due to their well-defined geometry on the one hand, but especially because it is more feasible to incorporate cocatalysts, for example, by electrocrystallization and/or simple chemical reduction. Additionally, after the generation of charge carriers by sunlight, the electrons go to the back contact of the photoanode, then, electron lifetime and conductivity become determinant factors for the overall efficiency [17, 22, 26, 130].Spanu et al. [17] investigated a well-defined charge separation platform for photocatalytic H2 evolution based on a Pt-WO3-TiO2 “stacked” structure constructed on anodically grown TiO2 nanotube arrays. These structures show strongly improved photocatalytic H2 evolution, compared to any other single cocatalyst system such as Pt-TiO2, WO3-TiO2, and pristine TiO2 nanotubes. The photocatalytic activity is ascribed to the enhanced charge carrier separation mechanism enabled by the well-defined TiO2-WO3-Pt architecture that provides swift electron transfer through WO3 and towards Pt for H2 evolution.Additionally, Spanu et al. [130] remarked that the photocatalytic H2 evolution reaction on pristine TiO2 occurred with low efficiencies due to (i) trapping and recombination of charge carriers and (ii) sluggish electron transfer kinetics. Recently, this group introduced an approach to fabricate an efficient noble metal-free photocatalytic platform for H2 evolution. By dewetting NiCu bilayers into alloyed NiCu cocatalytic nanoparticles at the surface of TiO2 nanotube arrays, they found improvements in H2 production, especially when the metals were in equimolar proportion. The alloyed NiCu cocatalyst on TiO2 nanotubes allowed them to reach H2 generation rates comparable to those delivered by conventional decoration of TiO2 with noble metals such as platinum.Finally, we have considered the advantages of using anodic oxide thin films and the possibility of precisely controlling the characteristics of the final semiconductor materials by growing them under high fields. By enhancing charge separation through external application of electric potentials, their performance can be improved to facilitate the technological implementation of industrial photocatalysis. This advantage has been employed in several reactors of different design [12, 16, 22, 26, 80], but the industrial production of thin oxide films and photocatalytic reactors based on them is yet to be developed [12, 26].


## 8. Conclusions

After reviewing the high-field growth of anodic oxide films for photocatalytic application, three important conclusions can be highlighted: (i) the synthesis of nanostructured metal oxides through high-field anodization allows to control the characteristics of the obtained materials; (ii) the electrochemical assistance of the photocatalytic processes on these materials yields efficient wastewater treatment; and (iii) the measure of reaction rates is important to determine and compare the physicochemical parameters, describing the chemical interactions during photoelectrolysis, and to apply this understanding to the design, operation, and control of reactive systems.



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*Source: 2571906-2019-02-25.xml*