Partial Oxidation-Engineered Dendritic α-Fe₂O₃@Fe Photoanode: Enhanced Photoelectrochemical Water-Splitting Performance and Pt-Modified Stability

Abstract

As a renewable energy source, solar energy holds significant potential for addressing future energy and environmental challenges. Concurrently, hydrogen (H₂), as a clean and renewable energy carrier, has garnered substantial attention. Photoelectrocatalytic water splitting to produce H₂ represents an emerging green technology for converting solar energy into hydrogen energy, which has been highly valued by researchers. The key to advancing this technology lies in identifying photoelectrode materials with high catalytic activity and stability. In this study, dendritic α-Fe was synthesized via electrodeposition at the optimal potential of −1.4 V vs. Ag/AgCl for 300 s, and the photoelectrocatalytic performance of α-Fe₂O₃@Fe was enhanced through partial oxidation annealing at 300 °C for 6 h. This approach effectively addressed the issue of the short carrier transport distance in α-Fe₂O₃. The resulting partially oxidized α-Fe₂O₃@Fe(300 °C, 6 h) exhibited a photocurrent density of 281.1 μA/cm² at +0.55 V vs. Ag/AgCl, which was 2.23 times higher than that of the fully oxidized dendritic α-Fe₂O₃(500 °C, 2 h) (125.8 μA/cm²). The influence of deposition potential on photoelectrocatalytic performance was systematically explored, and the optimal deposition potential was identified. Additionally, surface modification with 0.15 wt% Pt (ultra-low loading) was employed to further improve the photocatalytic stability of α-Fe₂O₃(500 °C, 2 h). After continuous operation for 2 h, the photocurrent of the surface-modified sample decreased by only 6.5%, indicating a substantial enhancement in stability.

1. Introduction

Worldwide energy consumption is still dominated by fossil fuels, which emit significant volumes of carbon dioxide, thereby contributing to global warming and climate change. The rise in the international economy is increasing energy consumption. Therefore, the quest for clean and renewable energy is an important concern for human beings nowadays, which is of enormous relevance for the sustainable development of civilization [1]. Hydrogen (H₂) energy is one of the most promising alternatives to fossil fuels, which not only decreases a country’s dependency on fossil fuels but also considerably reduces pollution of the environment. Solar energy, being a clean and sustainable form of energy, offers significant promise for alleviating future energy challenges and environmental difficulties. The effective development of solar energy can provide sufficient energy for mankind to meet the growing global energy demand [2]. In recent years, how to efficiently convert and utilize solar energy has attracted much attention and high priority. Among the various ways of solar energy conversion, water splitting by the solar energy-driven photoelectrochemical (PEC) reaction is an effective approach to produce clean and sustainable H₂ energy. Therefore, PEC technology is a potential technology to fulfill the world’s energy demand and minimize greenhouse gas emissions [3,4].

In 1972, Fujishima and Honda first reported the application of titanium dioxide (TiO₂) as a photoanode in PEC water splitting under UV light illumination [5]. However, TiO₂ possesses a large band gap of 3.0 eV, which restricts its utilization of solar energy to only 4% of the UV light component. Consequently, it is unable to efficiently harness solar energy for water splitting. Since then, there have been continuous efforts to develop suitable materials for fabricating photoelectrodes with both excellent and stable performance. Among the most extensively studied semiconductor photocatalysts are α-Fe₂O₃ [6,7], ZnO [8], WO₃ [9,10,11], BiVO₄ [12], and metal–organic frameworks [13,14]. The synergistic combinations of these materials have been thoroughly investigated to enhance the efficiency of PEC water splitting. Despite these efforts, no single efficient and cost-effective semiconductor material has yet been identified that can fulfill all the necessary criteria for PEC-driven water splitting. An ideal semiconductor photoelectrode must meet several key requirements: efficient light absorption, an appropriate band gap energy, effective charge transfer, low overpotential, and superior stability.

α-Fe₂O₃, with a suitable band gap of 1.9–2.2 eV, can absorb up to 40% of incident sunlight, and its theoretical solar energy conversion efficiency during PEC water splitting is approximately 15.6% [6]. This suggests significant potential for converting water into hydrogen and oxygen. Moreover, α-Fe₂O₃ exhibits several advantageous properties, including stability in alkaline solutions, low cost, ease of availability, and environmental benignity, making it a promising candidate for PEC anode materials. However, α-Fe₂O₃ also has notable limitations [15,16,17]: (i) relatively low absorption coefficients, necessitating a light absorption depth of 400–500 nm to completely achieve light absorption; (ii) rapid recombination of photogenerated holes within approximately 10⁻¹² s, with a short hole diffusion length of only 2–4 nm; and (iii) poor electron mobility in α-Fe₂O₃ (about 10⁻² cm² V⁻¹ s⁻¹). These drawbacks collectively result in a higher rate of charge carrier recombination in α-Fe₂O₃, which hampers the charge transfer process and ultimately leads to inferior PEC water-splitting performance. Currently, significant efforts are being devoted to enhancing the performance of α-Fe₂O₃ photoanodes through various strategies, including morphology modulation, doping, heterojunction construction, and surface modification. For instance, Zhu et al. [18] synthesized MoO_x/Fe₂O₃ composite photoanodes using a solvent-thermal method, with MoO_x serving as a surface passivation layer. This composite achieved a photocurrent density of 3.3 mA/cm². Wu et al. [19] designed a novel photoanode by loading single Co atoms onto g-C₃N₄ and forming a heterostructure with α-Fe₂O₃, resulting in a photocurrent density of 1.93 mA cm⁻², which was 3.22 times higher than that of pristine α-Fe₂O₃. Zhang et al. [20] deposited FeOOH, a co-catalyst, on the surface of α-Fe₂O₃ to reduce the hole transport distance, thereby increasing the photoanode’s photocurrent density by 86% compared to the undeposited surface. Xia et al. [21] prepared Zn/P co-doped α-Fe₂O₃ microconical thin film photoanodes via chemical vapor deposition. Zn/P co-doping enhanced the charge carrier concentration in α-Fe₂O₃, promoting the transfer of bulk and surface carriers and subsequently improving the photocurrent density.

The photocurrent values of bare α-Fe₂O₃ particle films, particularly those with large dimensions such as dendritic films [16,17], are typically very low. This is attributed to the significant resistance encountered during the transfer of charge carriers within these films. Therefore, enhancing the electrical conductivity of α-Fe₂O₃ can be a promising strategy to improve its PEC performance. In this study, the photoelectrochemical water-splitting performance of dendritic α-Fe₂O₃ was significantly enhanced through partial oxidation. Specifically, the photocurrent density of dendritic α-Fe₂O₃@Fe, obtained via partial oxidation, was 2.23 times higher than that of dendritic α-Fe₂O₃ obtained through complete oxidation, as measured at +0.55 V vs. Ag/AgCl. This result demonstrates the feasibility of improving the PEC performance of dendritic α-Fe₂O₃ through partial oxidation. Furthermore, surface modification with Pt was employed in this study to further investigate the potential for enhancing the stability of α-Fe₂O₃.

2. Materials and Methods

Materials and Chemicals: Sodium sulfate (Na₂SO₄, 99%, Aladdin Reagent Inc., Shanghai, China), ferrous sulfate heptahydrate (FeSO₄∙7H₂O, analytically pure, Sinopharm Group Chemical Reagent Co., Ltd., Shanghai, China), sulfuric acid (H₂SO₄, analytically pure, Luoyang Chemical Reagent Factory, Luoyang, China), potassium hydroxide (KOH, 82.0%, Tianjin Huadong Reagent Factory, Tianjin, China), chloroplatinic acid (H₂PtCl₆, 99.0%, Shanghai Conto Chemical Co., Shanghai, China), and ethanol (CH₃CH₂OH, 99.7%, Guangdong Fine Chemicals, Guangdong, China) were used without further purification. All aqueous solutions were prepared with deionized water. The commercial indium-doped tin oxide-coated glass (ITO, thickness 1.1 mm, resistance < 6 Ω, South China Xiang Science & Technology Co., Ltd., Yiyang, China) was cleaned with deionized water and ethanol in a sonication bath (Xiaomei Ultrasonic Instruments, XM-P102H, Kunshan, China), each for 10 min, and dried by N₂ flowing prior to its use.

Preparation of deposition solution: An analytical balance was employed to precisely measure 1.4204 g of Na₂SO₄ and 1.3901 g of FeSO₄·7H₂O, which were subsequently introduced into a 100 mL beaker. To facilitate dissolution, 50 mL of deionized water was added to the beaker. The mixture was then subjected to continuous stirring at a rate of 500 rpm on a magnetic stirrer for a duration of 30 min to ensure complete dissolution of the solid components. The resulting solution was carefully transferred to a 100 mL volumetric flask and filled to the mark. The pH of the solution was meticulously adjusted to 2.5 using a 0.5 M H₂SO₄ aqueous solution. This procedure yielded a deposition solution with 0.05 M FeSO₄, 0.1 M Na₂SO₄, and a pH of 2.5.

Preparation of the dendritic Fe, α-Fe₂O₃, α-Fe₂O₃@Fe, and Pt-α-Fe₂O₃@Fe films: Electrochemical deposition was carried out in a conventional three-electrode cell system using a CHI660e potentiostat (CH Instruments, Inc., Shanghai, China). The commercial indium-doped tin oxide-coated glass (ITO, 25 × 10 × 1.1 mm, resistance ≤ 6 Ω/cm², South China Science & Technology Company Limited, Shenzhen, China) was used as the working electrode. The ITO substrate was dipped into the deposition solution vertically, and the deposition area was 1.0 cm² (1 cm × 1 cm; the deposition area was fixed by tape). A platinum sheet and Ag/AgCl in a saturated KCl electrode were used as the counter and reference electrodes, respectively. All potentials in this work were measured versus the Ag/AgCl electrode. All the electrodeposition experiments were carried out at room temperature (24 °C) without stirring or any external gas bubbling. The dendritic Fe films were deposited onto ITO substrates in a 5 mL deposition solution at −1.4 V vs. Ag/AgCl for 300 s. The dendritic α-Fe₂O₃ films were obtained by annealing the Fe films under air at 500 °C for 2 h (heating speed 5 °C/min) in the box furnace. The partially oxidized dendritic Fe films were obtained by controlling the calcination temperature at 300 °C for different amounts of time, and the obtained partially oxidized Fe film was named α-Fe₂O₃@Fe. For the preparation of Pt-α-Fe₂O₃@Fe films, the α-Fe₂O₃@Fe film was immerged in 1 mM H₂PtCl₆ for different times (1 s, 10 s and 30 s). The samples were donated as xs-Pt-α-Fe₂O₃@Fe (x = 1, 10 and 30).

Photoelectrochemical measurements: The three-electrode PEC water-splitting device was employed to test the performance of PEC water splitting. Specifically, the electrolytic cell was a 5 cm × 5 cm × 5 cm quartz cell, with α-Fe₂O₃/ITO as the working electrode, the platinum sheet as the counter electrode, and Ag/AgCl as the reference electrode, and the electrolyte solution a 40 mL 1.0 M KOH solution. A xenon lamp (model CEL-CEL-PE-300L-3A, Beijing China Education AuLight Technology (CEAuLight) Co., Ltd., Beijing, China) was employed as the light source, providing a light intensity of 1 sun (AM 1.5, 100 mW/cm²). The light intensity of the solar simulator (1 sun) was quantified using an irradiance meter. Current–voltage (I-V) curves were recorded using linear scanning voltammetry (LSV) with a scan rate of 0.01 V/s and a voltage range of −0.2 to 0.6 V. The I-V curves were obtained under dark, illuminated, and chopped light conditions (with an on/off cycle of 1 s). To investigate the photocurrent stability and response, i-t curves were recorded using chronoamperometry to generate the photoresponse profiles of the samples. The samples were evaluated at a potential of +0.55 V vs. Ag/AgCl and a light frequency of 0.05 Hz (with a 20 s light-on/off cycle). The scan rate was 0.05 V/s, and the scan duration was 200 s. Ultraviolet-visible diffuse reflectance spectroscopy (UV-vis DRS, Shimadzu UV-3600, Shimadzu Corporation, Kyoto, Japan) was used to characterize the optical absorption properties, band gap and band edge position of the samples. BaSO₄ was used as the reference sample with an integrating sphere. The scanning wavelength range was 200–800 nm.

Characterization: The crystallinity and crystal structure of the samples were characterized by X-ray diffraction (XRD, Bruker D8 Advance, Karlsruhe, Germany) using a Cu Kα source. The morphologies and elemental composition of the samples were analyzed using a scanning electron microscope (SEM, ZEISS Sigma 300, Jena, Germany). X-ray photoelectron spectroscopy (XPS, Thermo ESCALAB 250XI, Carlsbad, CA, USA) was performed using Al Kα radiation.

3. Results

3.1. Synthesis Principle of α-Fe₂O₃@Fe

The applied potential and the pH of the deposition solution are identified as critical factors influencing the properties of the final product. During the electrodeposition process in the three-electrode system, as shown in Figure 1a, two competing reactions occur on the surface of the working electrode, as defined following Equations (1) and (2):

Hydrogen evolution: 2H⁺ + 2e⁻ → H₂

(1)

Iron reduction: Fe²⁺ + 2e⁻ → Fe

(2)

Depending on the experimental conditions, either reaction can dominate the deposition process. According to previous work [22], the optimum pH for this reaction is 2.47, so in this experiment, the pH of the deposition solution was controlled to be around 2.5. The composition of the deposition solution was 0.1 M Na₂SO₄ and 0.05 M FeSO₄, and different external potentials were applied to investigate the effect of different potentials on electrodeposition.

3.2. Systematic Performance Testing and Characterization of Target Materials

In an initial exploratory study, we selected deposition potentials of −1.3 V, −1.4 V, and−1.5 V to identify the optimal condition for electrodeposition. By monitoring the deposition process and examining the surface morphology of the deposited products (as shown in Figure 1b), we observed the following trends: When the deposition potential was set to −1.3 V, the deposition rate was relatively slow. Upon completion of the deposition process, only a thin, silver-colored layer of Fe was observed on the surface of the ITO glass. The amount of Fe deposited, as assessed visually, appeared insufficient, indicating that a higher deposition potential would be necessary. In contrast, when the deposition potential was increased to −1.4 V, the deposition rate accelerated significantly. After deposition, a uniform and dense Fe film was formed on the ITO glass surface. This film exhibited good adhesion, with no visible flaking. Visually, the Fe film appeared black, suggesting a more substantial deposition as observed in the previous work [16]. When the deposition potential was set to −1.5 V, the deposition rate was further increased. However, after the formation of a uniform Fe film on the ITO surface, the film began to warp and gradually flake off as the deposition process continued. By the end of the deposition phase, the Fe film on the ITO glass surface was non-uniform. Considering the above observations, it was concluded that −1.4 V is the optimal deposition potential for our experimental setup. This potential not only ensures a suitable deposition rate but also yields a more uniform and adherent Fe film. Therefore, −1.4 V was selected as the deposition potential for all subsequent experiments.

SEM images of the samples (Figure 2a,b) reveal that those deposited for 300 s exhibit a three-dimensional (3D) dendritic structure. This morphology significantly enhances the specific surface area of the material, thereby providing a greater number of active sites and facilitating the PEC water-splitting reaction. A comparison of the dendritic structures before and after annealing (Figure 2c,d) indicates minimal changes, confirming the feasibility of employing a deposition–annealing sequence to prepare dendritic α-Fe₂O₃. As shown in Figure 2c, flocculent structures are observed at the base of the dendrites. These structures arise from the simultaneous hydrogen evolution reaction occurring during the deposition of dendritic Fe on the working electrode surface. This reaction generates OH⁻ ions around the electrode, which subsequently react with Fe²⁺ in the deposition solution to form flocculent Fe(OH)₂ precipitates. A comparison of Figure 2e–h highlights that the dendrites of samples treated with H₂PtCl₆ become coarser and exhibit spherical particles on their surfaces. These particles are identified as platinum nanoparticles attached to the α-Fe₂O₃ surface, indicating successful surface modification. Furthermore, the energy dispersive spectrometer (EDS) analysis of the Pt-α-Fe₂O₃@Fe sample demonstrates that the Fe, O, and Pt elements coexist and are uniformly distributed in Pt-α-Fe₂O₃ (Figure 3b–e). This result indicates that Pt has been uniformly dispersed on the surface of α-Fe₂O₃@Fe. In the element content diagram of the sample (Figure 3a), the content of Pt is 0.15 wt%. The relatively low Pt content is due to the short immersion time of α-Fe₂O₃@Fe in the H₂PtCl₆ solution. However, this outcome still successfully confirms that Pt has been loaded onto the surface of α-Fe₂O₃@Fe.

The obtained samples were subjected to XRD analysis to elucidate their crystalline phases, as shown in Figure 4. The XRD peaks of the Fe film were indexed with JCPDS No. 87-0722. The intensity of the Fe peaks decreased significantly after annealing, with only a weak peak remaining at an annealing time of 1 h. As the annealing time increased further, the Fe peaks disappeared entirely, while the α-Fe₂O₃ peaks emerged. This transformation may be attributed to the formation of amorphous iron oxide, which is undetectable by XRD due to its lack of long-range crystalline order. The crystal structure of α-Fe₂O₃ obtained after annealing at 500 °C for 2 h matches the standard card of α-Fe₂O₃ (JCPDS No. 89-8104) [23,24,25] with the following unit cell parameters: a = b = 5.023 Å, c = 13.078 Å, and α = β = 90°, γ = 120°. The 2θ values of 33.25° and 54.23° correspond to the (104) and (116) diffraction peaks, respectively. From the XRD patterns, it is evident that with increasing annealing time, the (104) peak initially intensified and then weakened, remaining at a relatively low intensity, while the (116) peak gradually strengthened but also remained at a lower intensity. This behavior may be due to the compositional changes induced by annealing, which likely rendered the material less crystalline. Consequently, the detected α-Fe₂O₃ peaks were weaker, reflecting the reduced crystallinity of the material.

During the deposition process, the pH near the working electrode increases, causing Fe²⁺ to react with OH⁻, resulting in the precipitation of Fe(OH)₂. Consequently, Fe²⁺ remains present in the sample. Peak I in Figure 5a corresponds to the characteristic peak of Fe²⁺, with binding energies of Fe 2p_3/2 at 710.6 eV and Fe 2p_1/2 at 723.7 eV. Peak II represents the characteristic peak of Fe³⁺, indicating that oxidation has occurred on the sample surface, forming α-Fe₂O₃. The binding energies of Fe 2p_3/2 and Fe 2p_1/2 are 711.5 eV and 725.1 eV, respectively. Additionally, Peak III corresponds to the characteristic peak of FeOOH, with binding energies of Fe 2p_3/2 at 713.2 eV and Fe 2p_1/2 at 726.7 eV. This matches the data reported by Zhang et al. [26], which suggests that FeOOH was generated during the deposition of the sample. Similarly, Peaks I, II, and III in Figure 5c,e correspond to the chemical states of Fe²⁺, Fe³⁺, and FeOOH, respectively. In Figure 5a,c,e, no singlet Fe peaks were observed in the XPS spectra of the partially oxidized samples; however, weak Fe peaks were detected in the XRD plots. This is due to the shallow probing depth of XPS, which only measures surface elements, whereas XRD, with a greater probing depth, reveals that the surface of the samples is oxidized to α-Fe₂O₃, while a small amount of Fe remains in the interior. Therefore, it can be suggested that the α-Fe₂O₃/Fe structure obtained after annealing may be a core–shell structure, as shown in Figure 5. Figure 5b,d,f show the XPS spectra of O 1s. The XPS spectra of O 1s consist of three peaks: Peak I corresponds to the lattice oxygen of α-Fe₂O₃. Peak II may originate from FeOOH or -OH groups adsorbed on the sample surface, and Peak III may originate from oxygen vacancies on the sample surface [27]. Additionally, a comparison of these three spectra reveals that the proportion of Peak I in the O 1s spectra gradually increases with the degree of oxidation. Similarly, a comparison of Figure 5a,c,e shows that the proportion of Fe³⁺ peaks increases as the degree of oxidation deepens. This suggests that the α-Fe₂O₃ content in the samples increases with prolonged annealing time. The peak of Pt could not be observed in the full spectrum of the Pt-α-Fe₂O₃@Fe/ITO sample, which is due to the small amount of Fe remaining in the sample after partial oxidation, and therefore the sample contains less Pt after H₂PtCl₆ immersion. Peak I in Figure 6 corresponds to the characteristic peak of Pt⁰, indicating that Fe displaced Pt monomers during the modification process, with binding energies of Pt 4f_7/2 at 71.5 eV and Pt 4f_5/2 at 74.7 eV. Peak II corresponds to the characteristic peak of Pt²⁺, which is attributed to the partial reduction of Pt⁴⁺ to Pt²⁺ during the immersion process. The binding energies of Pt 4f_7/2 and Pt 4f_5/2 are 73.6 eV and 75.7 eV, respectively. These values are the same as those found by Aricò et al. [28].

The same sample was used to determine the optimal oxidative annealing time. The sample was annealed at 300 °C for 1 h in a muffle furnace, then immediately removed and cooled to room temperature for PEC performance testing. Following the test, the samples were cleaned with deionized water and ethanol, and then annealed again in a muffle furnace at 300 °C for 1 h and cooled to room temperature for PEC performance testing again. These steps were repeated until the optimal oxidative annealing time was determined. After identifying the optimal annealing time, the sample was annealed at 500 °C for 2 h in a muffle furnace to achieve complete oxidation. Figure 7a illustrates the LSV curves of the sample under varying annealing times with light illumination or under dark conditions. It indicates that the photocurrent density of the sample annealed at 300 °C for 6 h is higher than that of samples under the other annealing conditions, with the potential over +0.38 V vs. Ag/AgCl, suggesting that partial oxidation is an effective strategy for improving the PEC performance of the dendritic α-Fe₂O₃ materials. To better understand the relative magnitudes of the photoresponse currents at different annealing times, the currents at +0.55 V vs. Ag/AgCl were recorded for various annealing durations, as shown in Figure 7b. It also shows that the photocurrent density of the sample annealed at 300 °C for 6 h is higher than that of samples under the other annealing conditions.

Figure 7c shows the trend of the photoresponse current as a function of annealing time, revealing that the photoresponse current of dendritic α-Fe₂O₃ initially increases and then decreases with extended annealing. From 0 to 1 h, Fe was gradually oxidized to α-Fe₂O₃, resulting in a gradual increase in the photoresponse current of the sample. As the annealing time increased, the photoresponse current decreased. This may be attributed to the decreased Fe content resulting from the oxidation of metallic Fe. As the degree of annealing increases, α-Fe₂O₃ becomes amorphous, leading to an increase in the light-response current of the sample. Once the annealing time exceeded a certain threshold, the crystallinity of the sample remained stable. Continuing annealing at this point led to a decrease in Fe content, resulting in reduced sample conductivity and increased e⁻-h⁺ recombination, which caused the photoresponse current to decline. The changes in the structure of the sample during the annealing process are shown in Figure 8.

The sample achieved a maximum photoresponse current of 281.1 μA cm⁻² at an annealing time of 6 h. This is significantly lower than the photocurrent of vertically aligned nanotubes deposited on anodized aluminum oxide (AAO) via electrodeposition (2.2 mA cm⁻²), as determined by Mao et al. [29]. This difference may be attributed to the longer length of the dendritic α-Fe₂O₃, which does not effectively absorb incident light, and the higher rate of e⁻—h+ recombination.

To further enhance the PEC performance of partially oxidized dendritic α-Fe₂O₃@Fe, we explored modifying the samples with a 1 mM H₂PtCl₆ solution to displace any Fe potentially present on the material’s surface. The samples, which were annealed at 300 °C for 6 h, were immersed in H₂PtCl₆ for the desired time (1 s, 10 s and 30 s); rinsed with deionized water immediately after removal; and then placed in anhydrous ethanol for additional soaking. PEC tests were performed on samples with different immersion times to determine the optimal immersion time. The photocurrent densities of samples prepared at different immersion times are shown in Figure 9a. For the soaked samples, the 1s-Pt-α-Fe₂O₃@Fe sample has the best performance with a photocurrent of 195 µA/cm². However, the photocurrent densities of all soaked α-Fe₂O₃@Fe samples are lower than that of the unsoaked sample. All immersed samples exhibited a sensitive photoresponse. Photoresponse current measurements were performed at +0.55 V vs. Ag/AgCl for the immersed samples. The test results are shown in Figure 9b. The photoresponse currents of the samples treated with H₂PtCl₆ immersion were consistently lower than those of the unimmersed samples, and they gradually decreased with increasing immersion time. However, the photoresponse currents of samples with immersion times of 1 s and 10 s were higher than those of the fully oxidized samples, suggesting that partial oxidation combined with H₂PtCl₆ immersion can enhance performance. The photoresponse current of the samples gradually decreased with prolonged immersion time, becoming lower than that of the fully oxidized samples after 30 s of immersion. The decrease in the photoresponse current after H₂PtCl₆ immersion can be attributed to the highly acidic nature of H₂PtCl₆, with a pH of 1.2 for the 1 mM solution used in the experiments. This acidity may react with Fe and α-Fe₂O₃, reducing the amount of α-Fe₂O₃ and thereby decreasing the photoresponse current of the samples. Additionally, as Pt is only adhered to the surface of the sample, it may detach during testing, further affecting the photoresponse current and, consequently, the PEC performance. As shown in Figure 9c, after 2 h of continuous operation, the sample treated with H₂PtCl₆ exhibited the best stability, while the stability of the partially oxidized and fully oxidized samples was lower. The photoresponse current of the surface-modified samples was higher than that of the fully oxidized samples, and after 1.5 h of continuous operation, the photoresponse current of the surface-modified samples was higher than that of the partially oxidized samples. These results indicate that surface modification with Pt is a feasible approach for improving the samples. Furthermore, we analyzed the effect of sample band gap on photocurrent density. Figure 9d presents the UV-vis DRS and Tauc plots of different samples. The band gap energy (E_bg) values of the three samples are derived from the Tauc plots. The E_bg values of α-Fe₂O₃@Fe(300 °C, 6 h), α-Fe₂O₃(500 °C, 2 h), and 1s-Pt-α-Fe₂O₃@Fe are 2.48 eV, 2.51 eV, 2.45 eV, respectively. These values show negligible differences with a maximum deviation of only 0.06 eV. The inset UV-vis absorption spectrum reveals nearly identical absorption intensity and trends for all samples in the visible light region (400–800 nm). This further proves their similar light absorption capacity. The band gap difference exerts little influence on the magnitude of the photocurrent response. The variation in photocurrent is possibly attributed to other factors such as α-Fe₂O₃@Fe surface structure and carrier transport efficiency.

Furthermore, the α-Fe₂O₃@Fe(300 °C, 6 h) sample was characterized after a 2 h stability test, as illustrated in Figure 10. The results show that the dendritic morphology of α-Fe₂O₃@Fe(300 °C, 6 h) is well preserved, with no obvious structural change. XRD pattern analysis reveals that the characteristic diffraction peaks of α-Fe₂O₃@Fe(300 °C, 6 h) remain clear and sharp after the reaction, with no new impurity peaks generated, no significant shift in peak positions and no obvious attenuation in peak intensities, indicating the excellent crystallographic-phase stability of the sample. High-resolution XPS spectra of the Fe 2p and O 1s tests confirm that the chemical valence states of Fe and O for the α-Fe₂O₃@Fe(300 °C, 6 h) sample remain unchanged after the 2 h stability test, with no obvious variation in the binding energy and peak shape of each characteristic peak. All the above characterization results consistently demonstrate that the α-Fe₂O₃@Fe(300 °C, 6 h) sample possesses outstanding structural, crystallographic and surface chemical stability during the photochemical reaction process.

4. Conclusions

In this study, the PEC water-splitting performance of dendritic α-Fe₂O₃ was enhanced through partial oxidation. The photoresponse current of dendritic α-Fe₂O₃@Fe, obtained through partial oxidation (281.1 μA cm⁻²), was 2.23 times higher than that of dendritic α-Fe₂O₃, which was synthesized through complete oxidation (125.8 μA cm⁻²), at +0.55 V vs. Ag/AgCl. These results demonstrate the feasibility of enhancing the PEC performance of dendritic α-Fe₂O₃ through partial oxidation. Furthermore, surface modification was employed in this study to enhance the photoresponse current of α-Fe₂O₃. However, the high acidity of the H₂PtCl₆ solution used in the experiment degraded the original dendritic α-Fe₂O₃, leading to a decrease in photoresponse current rather than an increase, thereby reducing the PEC water-splitting performance of α-Fe₂O₃. Despite this, the photoresponse current of the sample remained higher than that of the fully oxidized sample for shorter immersion times. In future studies, the use of a less acidic potassiumchloroplatinate solution will be explored, along with surface modification of α-Fe₂O₃ using Au, graphene, or other materials. While this study has limitations, it offers valuable insights for the preparation of simple PEC materials and suggests potential avenues for further improvement.