Fe₃O₄-TiO₂ Thin Films in Solar Photocatalytic Processes

Abstract

The optical properties of 5wt% Fe₃O₄-TiO₂ thin films were evaluated in detail with the aim of proposing a mechanism for solar photocatalytic processes and highlighting the advantages over the use of bare TiO₂. The results showed that the incorporation of 5wt% Fe₃O₄ enhanced the optical properties by a redshift to a wavelength in the visible range, reducing the anatase/rutile band gap energy from 3.2 eV to 2.8 eV. Photoluminescence studies reveal a superior separation efficiency of photoexcited electron-hole pairs when Fe₃O₄ nanoparticles (NPs) are present in the photocatalyst. X-ray photoelectron spectroscopy spectra confirm the presence of Fe₃O₄ and existence of a chemical bonding between TiO₂ and Fe₃O₄ NPs. Moreover, in this study, a mechanism of solar photocatalytic processes involving Fe₃O₄-TiO₂ thin films is proposed and it is supported by experimental results. Finally, solar photocatalytic experiments were carried out, indicating that the effectiveness for the removal of the selected pharmaceutical is considerably improved when the composite material is used as catalyst. Furthermore, it was demonstrated that the photocatalytic activity of the prepared Fe₃O₄-TiO₂ thin films depends on their thickness, achieving the highest pharmaceutical removal yields using the 2 µm thick sample. The stability and reusability of the catalyst was confirmed studying the photocatalytic activity over three cycles.

1. Introduction

In recent years, semiconductor photocatalytic processes have found wide applications in water treatment [1]. Titanium dioxide (TiO₂) has been considered as the most widely used semiconductor oxide photocatalyst due to its attractive attributes, such as low cost, corrosion resistance, excellent chemical stability, non-toxicity and high photocatalytic activity [2]. However, the use of TiO₂ nanoparticles (NPs) in solar photocatalysis for environmental remediation has some technical limitations, such as the high band gap of TiO₂ (~3.2 eV) [3,4], close to UV spectral range. For this reason, this photocatalyst is triggered by near UV radiation. Thus, it takes advantage of only a small range of the solar spectrum (about 3–4%), which limits the potential of solar light as an energy source. Additionally, the photogenerated electron-hole pairs are liable to recombination, resulting in low quantum efficiency of TiO₂ [5].

Moreover, the use of TiO₂ as a photocatalytic material would increase the overall cost if it is utilized in powder form, which constitutes a drawback. This is so due to the necessity of performing an additional filtration stage in order to separate this powder from the water in solutions [6]. Thus, the separation of the semiconductor TiO₂ catalyst after water treatment remains as the major obstacle towards the practicality of this technology [7]. In addition, nanoparticles, dispersed in the medium, can be dangerous due to their possible cytotoxic and inflammatory effects [8,9].

In order to overcome these issues, there are several studies in the literature in which Fe₃O₄-TiO₂ nanoparticles systems have already been investigated. These studies revealed that the presence of Fe₃O₄ enhance the photocatalytic activity of TiO₂ and that modified TiO₂ NPs can be separated from water by means of an external magnetic field [10,11,12,13,14]. It is important to note that composites/heterojunction catalysts enhance the electron-hole separation and prevent charge back transfer [15,16].

However, we consider that modifying TiO₂ with Fe₃O₄ would not lead to a feasible solution, since: (1) the suspended NPs tend to aggregate, especially when high concentrations are used [6] and furthermore, (2) the use of magnetic separation is complicated in real water treatment applications.

Therefore, a more realistic proposal would consist of depositing thin film coatings onto a substrate material [17]. In this sense, it is important to note that there are only few studies about the immobilization of Fe₃O₄-TiO₂ NPs on substrates as thin films, being very few of them those related to its use in photocatalytic processes. For instance, Wei et al. [18] prepared Fe₃O₄-TiO₂ composite films to enhanced the ability to store energy under low operating electric field. Zhang et al. [19] used Fe₃O₄ nanoparticles and molecularly imprinted TiO₂ in the fabrication of a novel photoelectrochemical biosensor. Yeh et al. [20] evaluated the antimicrobial efficiency of immobilized Fe₃O₄/TiO₂ powder on glass substrate. Nevertheless, to the best of our knowledge, no studies have been reported on the use of Fe₃O₄-TiO₂ thin film for solar photocatalytic processes. Therefore, the current work represents a highly innovative study, which could open a new field of application for this particular material.

Thus, the purpose of this paper is to develop a Fe₃O₄-TiO₂ composite material with high photocatalytic activity and good stability and their immobilization on substrates. In this study, thin films are prepared using a “sandwich” type structure [21], which prevents the release of NPs to the medium. Furthermore, the photocatalytic efficiency is evaluated by studying the degradation of an antibiotic, sulfamethoxazole (SFX), in the presence of these films. SFX is a sulphonamide antibiotic, which is one of the common pollutants in surface water [4,22,23,24,25].

The main motivation for using an antibiotic as a contaminant model in solar photocatalytic experiments is that conventional methods implemented in wastewater treatment plants are not efficient enough to remove pharmaceutical contaminants [25,26,27]. Therefore, these pollutants can arrive in rivers, lakes, seas, aquifers and occasionally, they can be found in tap water, although in very small quantities [28]. The presence of pharmaceutical compounds in surface and wastewater, all over the world, involves a significant risk for aquatic ecosystems and for all living beings and the environment [29,30,31]. Considering the effects and consequences to the environment, animals and plants, and regarding the frequency with which pharmaceuticals have been detected in water, it is expected that these types of pollutants will be candidates for future regulations.

Therefore, the research on alternative, resultative and cost-efficient technologies is a field of great interest for all the technological and scientific community.

2. Materials and Methods

2.1. Chemicals

Iron (II) chloride (FeCl₂), iron (III) chloride (FeCl₃) and ammonium hydroxide (NH₄OH) were used to prepare magnetite (Fe₃O₄) NPs. Tetrabutil-ortotitatanate (TBOT) C₁₆H₃₆O₄Ti (98%), acetylacetone C₅H₈O₂ (99.5%), TiO₂ nanoparticles (P25, 99.5%) and ethanol C₂H₆O (99.5%) were used to fabricate sandwich-type structure thin films. SFX and T-Butanol were used in the photocatalytic experiments. These experiments were carried out using MilliQ water.

Acetylacetona and ethanol were received from Merck and Panreac (ITW companies), respectively. The rest of reagents were purchased from Sigma-Aldrich.

2.2. Preparation of Fe₃O₄-TiO₂ Thin Film Photocatalyst

2.2.1. Synthesis of Magnetite Nanoparticles

Magnetite (Fe₃O₄) nanoparticles have been prepared following a classical bottom-up chemical route based on a co-precipitation reaction. With the aim to obtain the mixed (II and III) iron oxide, we have started from Fe²⁺ and Fe³⁺ precursor salts, FeCl₂ and FeCl₃, respectively, and we have promoted the controlled co-precipitation of both salts. Briefly, 0.99 g of FeCl₂ and 2.76 g of FeCl₃ are dissolved in 100 mL of MilliQ water. The solution is placed in a three-necked flask and heated at 80 °C under reflux and with magnetic stirring, in a nitrogen atmosphere, in order to avoid the formation of non-magnetic iron oxide phases. After heating the solution for 10 min, 10 mL of 25% ammonium hydroxide solution is swiftly added to the flask, promoting the fast and homogeneous nucleation step to form the magnetite cores. The solution is still heated, keeping the temperature at 80 °C, for 30 additional minutes, in which the previously formed nuclei continue growing. Once the solution was cooled down to room temperature, it was filtered three times (using a 0.1 μm Millipore membrane), adding ethanol, in order to eliminate the excess of precursor species and/or residues from the reaction. As result, we obtained a magnetic black powder composed by magnetite NPs.

2.2.2. Preparation of Fe₃O₄-TiO₂ Nanoparticles

For preparation, 0.15 g of synthetized Fe₃O₄ NPs were initially dispersed in 10 mL deionized water and kept under ultrasonic irradiation for 30 min. Throughout this procedure, a stable ferrofluid was obtained. Next, the dispersion was added, drop by drop, to 3 g of TiO₂ NPs, forming a slurry that was finally dried at 110 °C for 24 h. Finally, samples were annealed at 400 °C for 30 min. This processing would lead to a 5wt% load of Fe₃O₄ NPs in TiO₂. This concentration value (around 5wt%) has shown to give the best optical and structural properties as well as superior photocatalytic activity in FeTiO₂ samples [32,33,34].

2.2.3. Preparation of Photocatalyst Films

Photocatalyst coatings on flat glass supports were prepared according to a multilayer approach proposed in previous works by scientists of our research group [4,21]. According to the methodology, the structure of the photocatalyzer responds to a “sandwich” approach consisting of two very thin anatase films (~50 nm), obtained by sol gel [35], delimiting a thicker layer obtained from a suspension of TiO₂/Fe₃O₄ nanoparticles.

Anatase films were deposited from a precursor sol prepared by hydrolysis of titanium n-butoxide (TBOT) in a solution containing acetylacetone, ethanol and acidified water (HNO₃, pH = 1) in a molar ratio TBOT:acetylacetone:H₂O:EtOH of 1:0.5:2:35 as described in Blanco et al. (2015) [35]. Dip coating was performed from aged sol at precisely controlled withdrawal speed (100 mm/min) in a homemade apparatus on a microscope slide and the resulting film was subsequently dried at 150 °C for 30 min and annealed at 1°/min until 500 °C, in order to ensure that TiO₂ films is formed by small anatase crystallites while preserving a certain porosity level in the films which provides high surface areas [36].

For the central part of the sandwich coating, a suspension of the Fe₃O₄-TiO₂ nanoparticles in an acetylacetone-ethanol solution (4:1 vol ratio, 40 g/L) was prepared by using high power ultrasounds (20 KHz). Films were dip coated on the top of the previous anatase film at 100 mm/min, layer by layer. After every five depositions, the layers are dried at 150 °C for 30 min and the process is repeated until reaching the total number of nanoparticulated layers are deposited.

Finally, the coating was sealed with a new single anatase thin film prepared as described before. The final photocatalyst is obtained after annealing in air for 1 h at 400 °C. For comparison, a similar non-doped “sandwich” coating was also prepared using a suspension of TiO₂ NPs a precursor of the central layer. The resulting film was used as a reference.

2.3. Photocatalyst Characterization

Magnetite NPs were studied by Transmission Electron Microscopy (TEM) and Scanning-Transmission Electron Microscopy (STEM), using a JEOL JEM-2100 EX TEM and a FEI TALOS F200X STEM microscope, with thermionic effect and field effect electron emission guns, respectively, both working at 200 kV. Both microscopes are located at the facilities of Servicios Centrales de Investigación, Ciencia y Tecnología (SC-ICYT) of the University of Cádiz (UCA). NPs were deposited in TEM holey carbon grids according to a previously stablished method [37]. Dynamic Light Scattering (DLS) was utilized for measuring the hydrodynamic NP size. Measurements were carried out at 25 °C, using a Malvern Zetasizer Nano-ZS (“Malvern Instruments”, Worcestershire, U.K.), with a 1 cm path cell. This equipment also allows for the Z-potential to be measured which evaluate colloidal solutions stability, as well as NP surface charge.

In order to study the effect of incorporating Fe₃O₄ NPs on the optical properties of TiO₂ NPs and estimate their energy band gap, UV-Vis absorbance and diffuse reflectance measurements were carried out using an Agilent Cary 5000 UV-Vis-NIR double-beam spectrophotometer. The spectra in the 200 to 800 nm range were registered in an integrating sphere. The resulting diffuse reflectance spectra were transformed into apparent absorption spectra using the Kubelka-Munk function (F(R)). The direct and indirect optical band gap of the materials was determined through the construction of Tauc plots by plotting (F(R)hν)ⁿ against (hν), with n = 2 or n = ½, for direct and indirect transitions, respectively. The optical band gap was obtained by extrapolating the linear part of this plot to the energy axis. Furthermore, the photoluminescence spectra were obtained using a Fluorolog-QM spectrometer (Horiba) equipped with a continuous 75 W Xenon arc lamp, double monochromators at the excitation and the emission and a photomultiplier tube detector (PMT-920IS). Temperature controlled experiments were performed with a cryostat (CS204-FMX-1SS, ARSCRYO) that can be operated between 4 and 350 K.

X-ray photoelectron spectroscopy (XPS) was recorded using a Kratos Axis Ultra DLD spectrometer. XPS measurements were performed using a monochromatic Al Kα radiation at 1486.6 eV and X-ray power of 150 W. The analyser was operated in constant analyser energy transmission (CAE) mode, with pass energy of 80 eV and 20 eV for the survey scan spectrum and for high-resolution core levels, respectively. Surface charging effects were compensated by making use of the Kratos coaxial neutralization system. The binding energy (BE) scale was calibrated with respect to the C 1 s signal at 284.8 eV. XPS data analysis was performed by using CasaXPS Software, version 2.3.19rev1.1 m (Neal Fairley, Casa Software Ltd., Teignmouth, Devon, UK).

Morphology and thickness of prepared thin films was followed by Scanning Electron Microscopy (SEM), recording cross-section images obtained using the secondary electron detector of a FEI Nova NanoSEM 450 scanning microscope (also located at the UCA-SC-ICYT facilities), with field effect electron emission gun, working at a voltage and a distance of 20 kV 4.6 mm, respectively.

Atomic Force Microscopy (AFM) images were obtained with a DI Veeco Nanoscope Multimode IIIa equipment using Bruker TESP-V2 probes and working in tapping mode. AFM images were processed with the open-source software Gwyddion [38].

2.4. Photocatalytic Experiments

Experiments were carried out using a custom-made photocatalytic system, consisting of a magnetic-stirred reactor exposed to sunlight, equipped with a recirculating peristaltic pump (Selecta Percom N-M) and coupled to an Avantes fiber optic UV-Vis-NIR spectrometer (Ocean Optics DT-Mini-2GS light source) that allows continuous monitoring [4].

For each experiment, 20 mL of an aqueous solution of SFX was charged into the photoreactor (5.6 mm diameter). SFX initial concentration was 5 ppm. A Fe₃O₄-TiO₂ thin film (2.5 × 2.8 cm²) was also place into the reactor. Experiments were conducted at Campus de Puerto Real, University of Cadiz (Spain, local latitude 36°31′ N) on sunny days. A radiometer UV34 (PCE Ibérica, Spain) was used to measure the intensity of solar radiation.

Absorbance measurements were determined using a UV-Vis-NIR fibre optic spectrometer and its evolution over radiation dose was monitored due to a peristaltic pump that recirculated (6 mL/min) the solution treated by solar photocatalysis.

Cumulative UV dose was calculated as shown in Equation (1).

$${\mathrm{Q}}_{\mathrm{UVn}}={\mathrm{Q}}_{\mathrm{UVn}-1}+\sum \left({\mathrm{UV}}_{\mathrm{n}}·\Delta \mathrm{t}\right)\frac{{\mathrm{V}}_{\mathrm{i}}}{{\mathrm{V}}_{\mathrm{T}}}$$

(1)

where Q_UVn, Q_UVn−1 is the cumulative irradiated UV energy received at times n and n − 1, respectively; Δt_n the time interval between two sampling times; UV_n the average incident radiation for each time interval (W/m²); Vi the illuminated volume of the reactor and V_T the total volume of the reactor.

Experimental results can also be expressed using t_30W (see Equation (2)). It is a normalized value that indicates the time spent on the experiment in the hypothetically situation of a constant UV radiation intensity of 30 W/m², during its development [39]. A UV intensity of 30 W/m² resembles conditions around a sunny noon in the vicinity of Cádiz.

$$t_{30Wn}=t_{30Wn-1}+\sum \left(\frac{U{V}_n}{30}·\Delta t\right)\frac{V_i}{V_T}$$

(2)

where t_30Wn t_30Wn−1 are the normalised illumination time of samples at times n and n − 1, respectively.

3. Results and Discussion

3.1. Fe₃O₄ and Fe₃O₄-TiO₂ NPs Morphology, Size, Crystallinity and Composition

Figure 1a corresponds to a SEM micrograph, showing a general view of the synthetized magnetite NPs. This image and others alike were utilized as a first indication of the quality of the synthetized NPs and to calculate the average particle size. Micrograph reveals the formation of relatively small nanoparticles with homogeneous size distribution. Although the strong magnetic character of the material leads to the NP aggregation, the higher atomic number of iron gives a good contrast that allows distinguishing the formation of approximately spherical particles whose concentration is high enough for performing a statistical study on the size distribution. In this sense, the histogram of this magnitude is presented in Figure 1b. As it can be observed, the experimental particle size distribution fits well with a Gaussian distribution. This fit indicates a NP average size of 8.7 nm with a small standard deviation (1.1 nm). NP crystalline structures can be observed in High Resolution TEM (HRTEM) images, as the ones in Figure 1c and, at higher magnification, Figure 1d. The averaged experimental distances between crystalline planes are 3.00 and 3.43 Å, respectively. These distances best agree with those of the theoretical ones for ($\overline{1}$11) and (200) planes of magnetite [40]. These measured planes have been labelled and marked in the figure.

On the other hand,

Table 1. Average hydrodynamic size, polydispersity index and Z-Potential values for Fe₃O₄ NPs.

DLS Size (nm)	PDI	Z Potential (mV)
68.7	0.3	23.7

shows the average hydrodynamic size, PDI (polydispersity index) and Z-Potential values for magnetite NPs. As expected, the hydrodynamic size determined by the DLS technique is significantly higher in comparison with the one obtained by TEM. This effect is assigned to the presence of extra hydrate layers in aqueous medium. Moreover, some agglomeration of the nanoparticles in aqueous solutions is expected due to the magnetism of magnetite NPs. However, this average hydrodynamic size, together with the relatively high value of the Z-potential, indicates the NPs colloidal stability. In addition, the positive value of the Z-potential suggests the presence of positive charge at the NP surface, which could promote subsequent crosslinking with the matrix.

In order to find out whether or not the utilized TiO² doping process produce a material in which the magnetite NPs are actually imbibed in the titanium oxide matrix, small volumes of Fe₃O₄-TiO₂ were deposited on holey-carbon TEM grids, for their compositional study. One of these volumes is presented in Figure 2a, which corresponds to a TEM micrograph obtained in Diffraction Contrast-Bright Field (BF) mode. The darker areas correspond to orientations of the material (TiO₂) along which the electron beam is parallel to high atomic density crystallographic planes. This doped TiO₂ volume was later observed using STEM techniques, such as High Angle Annular Dark Field (HAADF) and Energy Dispersive X-ray spectroscopy (EDX), as presented in Figure 2b,c. HAADF images intensity highly depends on the atomic mass and thickness of the material. Therefore, and taking into consideration the small size of the NPs and roughness and irregularity of the TiO₂ volume under study, it is difficult to distinguish these NPs in HAADF images. EDX spectra maps, on the other hand, easily revealed the positions of such particles in the titanium oxide matrix, as it can be observed in Figure 2c. In this map, red spots correspond to Fe characteristic X-rays emitted from the material, and green dots correspond to Ti-signal. Weaker Fe signals from the volume could be explained by different particle sizes or, more probably, because of the high possibility of the NP being totally contained inside the TiO₂ volume. This was corroborated by EDX point spectra taken from the NPs. Figure 2d shows one of such spectra, obtained from the region “1” indicated in Figure 2a with a red square. This spectrum presents a Fe-peak, corresponding to the NP, and a Ti-peak (since the STEM probe interacts with a certain volume surrounding the NP). EDX point spectrum in Figure 2e, taken from the region labelled as “2” in Figure 2a, proves that the Fe-peak in the previous spectrum is not due to sample contamination. Cu-peak in both spectra comes from the Cu mesh of the utilized TEM grid. It can be concluded, thus, from this EDX map, that the utilized process indeed produces a Fe₃O₄-TiO₂ slurry, with NPs randomly distributed in the TiO₂. HRTEM images were obtained in order to investigate possible changes in the TiO₂ structure. In this sense, images such as the one in Figure 2f (obtained from the region labelled as “3” in Figure 2a) and, at higher magnification, 2g allow measuring averaged lattice distances of 2.36 and 3.52 Å, which are in good agreement well with the theoretical distances for (110) and (101) for the atomic planes of the anatase phase of TiO₂ [41]. The dashed lines in the figure are representative of the indicated lattice distances. Neither of the HRTEM images recorded shows, in any case, a change in the TiO₂ crystalline structure, indicating the absence of a possible phase change or measurable stress due to the introduction of NPs.

3.2. Thin Film Characterization

3.2.1. Optical Properties: UV-Vis Spectra, Bandgap Energy and Photoluminescence Studies

The catalysts were deposited in the form of thin films. Figure 3 shows the UV-Vis absorption spectra of Fe₃O₄-TiO₂ and TiO₂ photocatalysts, where it is possible to assign some common features in the spectral range beyond 300 nm, despite the strong absorption of the substrate at this wavelength. TiO₂ spectrum shows a strong absorption corresponding to the absorption edge of semiconductor TiO₂ below 400 nm but, in the spectral range above 420 nm, shows very little absorption. Conversely, spectrum corresponding to Fe₃O₄-TiO₂ sample exhibits a broad absorption across the whole visible spectrum, as was previously described in the literature [42].

Optical band gap energy determination of the doped catalyst and its components were evaluated from UV-Vis diffuse reflectance spectra by applying the Kubelka-Munk (K-M) function [21,43]. The K-M function, F(R), establishes a relationship between absorbed, scattered and diffused reflected light by the sample, and is defined as:

$$F\left(R\right)=\frac{{\left(1-R\right)}^2}{2R}$$

(3)

where R is the wavelength dependent sample diffuse reflectance, measured with the spectrophotometer integrating sphere. The use of this model for this kind of coating has been justified by considering the granular structure for these optically rough films [36].

Thus, the Tauc method can be applied to the function (F(R)*E)^m versus the photon energy, E, with m = 1/2 or m = 2 for indirect or direct interband transitions, respectively. The (F(R)*E)^m function will present a linear region for E values close to E_g where the relationship (F(R)*E)^m = k(E − E_g) applies. In this way, the gap energy of Fe₃O₄-TiO₂ thin film, E_g, can be obtained from the extrapolation to zero of the linear regression in this region of the plot. Both direct and indirect bandgaps (

Table 2. Measurements of indirect and direct bandgap for different materials in this work.

Material	Indirect Eg (eV)	Direct Eg (eV)
TiO2	3.19 ± 0.05	3.61 ± 0.06
Fe3O4-TiO2	2.79 ± 0.05	3.31 ± 0.04
Fe3O4	0.93 ± 0.01	2.85 ± 0.06

) calculated in this way from plots using m = 1/2 and m = 2, respectively, are collected in Table 2.

It can be noticed that materials shown in Table 2 exhibit an indirect bandgap smaller than the direct band gap, suggesting that the fundamental bandgap for these materials could be considered as an indirect bandgap [44,45]. The direct or indirect nature of the bandgap transition is an essential parameter of semiconductors for photocatalytic applications. Thus, when a semiconductor has an indirect bandgap and the electric dipole transition from valence band maximum to conduction band minimum is allowed, then the electron-hole pairs recombine with a lower probability [46].

As it can be seen in Table 2, the calculated indirect bandgap of TiO₂ is nearly 3.2 eV but it is reduced when Fe₃O₄ NPs are included in the material. The small indirect energy gap obtained for magnetite NPs is consistent with the fact that Fe₃O₄-TiO₂ materials present absorption in the visible spectrum region.

This lower bandgap energy of the doped material is due to the fact that the presence of Fe₃O₄ NPs introduce a series of localized occupied states into the bandgap of TiO₂ lattice [47].

Narrowing the bandgap of TiO₂ is an important strategy to enhance its photocatalytic activity. It has been shown that TiO₂ surface loading with Fe₃O₄ nanoparticles can be used to enhance the electron-hole pairs generation efficiency to stimulate photocatalytic reaction [48].

PL studies were conducted to elucidate the effect of the electron-hole annihilation on the photocatalytic properties. The steady state photoluminescence spectra of synthesized photocatalysts were registered using an excitation wavelength of 325 nm and different temperatures (77,206 and 273 K). Our results showed (Figure 4) that pure TiO₂ exhibits the highest PL emission intensity, what can be directly related to a high electron-hole recombination rate [49]. PL intensity of Fe₃O₄-TiO₂ was significantly smaller, indicating a noteworthy lower recombination rate, i.e., a superior separation efficiency of the photoexcited electron-hole pairs [49]. Thus, the addition of Fe₃O₄ nanoparticles on the surface of TiO₂ can significantly reduce the electron-hole pairs recombination by accepting the electrons from TiO₂ [48].

3.2.2. Composition, Structure and Morphology

X-ray photoelectron spectroscopy was carried out in order to investigate the electronic features and elemental composition of the prepared materials. Figure 5 shows the survey scan XPS spectrum of Fe₃O₄-TiO₂ thin films, which contains O 1 s, Ti 2p and Fe 2p peaks.

High Resolution XPS signal and their deconvolutions are presented in Figure 6a–c:

O 1s: a high-resolution O 1s XPS spectrum is deconvoluted into four peaks.

From those computationally obtained peaks, the ones centred at energies of 529.8 and 530.4 eV can be assigned to the oxygen in the lattice Ti-O and to the oxygen in Fe-O, respectively. The peak located at 531.6 eV is related to the oxygen atoms in ‘bridging’ hydroxyl groups that are bound to titanium or iron atoms (Me-OH) [50]. Two types of hydroxyl groups are defined in the literature [51,52]: one of them, referred to as a ‘bridging’ hydroxyl, is attributed to O₂⁻ anions in the bulk structure of the material. The other one, which called ‘terminal’ and resides at an acidic site, is attributed to chemisorbed OH groups on the sample surface. As can be deduced from spectrum shown in Figure 6a, no terminal hydroxyl groups were detected in the fabricated material.

The O atom in the bridge OH should be energetically favourable to attract positive holes, because it has negative charge. Consequently, a certain fraction of trapped holes probably release ^•OH into bulk solution [53].

Fe 2p: in order to confirm the presence of Fe₃O₄, the elemental and valence state analysis were performed using XPS. Figure 6b shows the core-level XPS spectra of Fe 2p corresponding to Fe₃O₄. The peaks located at 711 and 724.6 eV are associated to Fe(III) 2p_3/2 and Fe(III) 2p_1/2, respectively. Peaks at 709.3 eV and 722.5 eV can be assigned to Fe (II) 2p_3/2 and Fe(II) 2p_1/2, respectively. These results are in agreement with Fe 2p XPS spectrum of Fe₃O₄ reported in the literature [54]. Moreover, the area ratio of Fe³⁺/Fe²⁺ is about 0.50, which is consistent with the stoichiometry of Fe₃O₄ [55].

Ti 2p: the core-level XPS spectra of Ti 2p is fitted with three peaks. Peaks located at 458.6 eV and 464.4 eV can be assigned to Ti⁴⁺, confirming the main valence state of + 4 for Ti. Moreover, the energy difference between Ti2p_1/2 and Ti2p_3/2 is 5.8 eV, which is associated to the TiO₂ standard binding energy value [56]. Additionally, the calculated peak that corresponds to the Ti in the Ti-O-Fe bond is centred at an energy of 459.7 eV. It is worth noting that the existence of this peak, which is a necessary result of the deconvolution of the experimental XPS signal, is proof of the existence of a chemical bonding between TiO₂ and Fe₃O₄ NPs [50,56].

Once the composition of the Fe₃O₄-TiO₂ thin film was analysed by XPS, and taking into account the expected influence of the thickness in the photocatalysis experiments, the photocatalysts with 5, 10 and 15 layers deposited were prepared, and SEM in the cross section was performed to get thickness measurements. Samples were called “1 µm:Fe₃O₄-TiO₂”, “1.5 µm:Fe₃O₄-TiO₂” and “2 µm:Fe₃O₄-TiO₂”, according to their nominal thicknesses. SEM micrographs of the prepared photocatalysts are shown in Figure 7. These images allowed to obtain the experimental thicknesses of the Fe₃O₄-TiO₂ layer for each sample: (0.97 ± 0.03), (1.51 ± 0.04) and (1.99 ± 0.02) µm, respectively. These experimental values are in very good agreement with the nominal ones.

SEM images in Figure 7 indicates, beside the spatial scale, the expected 1, 1.5 and 2 μm thicknesses for each case. Note that, due to sample orientation and the clivationmethod followed in order to observe the materials in the SEM microscope, images in Figure 7 shows not only the layers profiles, but also, in the cases of Figure 7b and c, the surface of the preparations. Such surface can be distinguished from the profile by the intensity contrast in the image.

Surface roughness of the titanium oxide layer for these three photocatalysts samples (1 µm:Fe₃O₄-TiO₂, 1.5 µm:Fe₃O₄-TiO₂ and 2 µm:Fe₃O₄-TiO₂) was also determined, using atomic force microscopy (Figure 8). Measurements were repeated in three different locations on their surfaces. These measurements and their averaged values are collected in

Table 3. Root mean square, RMS (nm) of Fe₃O₄-TiO₂ thin films.

Sample	Measurement	RMS (nm)
1 µm:Fe3O4-TiO2	1	25.6
	2	23.4
	3	21.5
	Mean ± s.d	23.5 ± 2.1
1.5 µm:Fe3O4-TiO2	1	20.2
	2	18.8
	3	15.9
	Mean ± s.d.	18.3 ± 2.2
2 µm:Fe3O4-TiO2	1	20.6
	2	24.8
	3	20.2
	Mean ± s.d.	21.9 ± 2.5

. The values in this table reveal that, the appearance of surface, in all cases, is similar and quite homogeneous, having a roughness which seems to be independent of the layer thickness. It means that this method of fabrication would allow using even thicker layers without a modification in the surface roughness, which is an important factor that influences the physical behaviour of TiO₂ -based thin films [57].

3.3. Proposed Mechanism

Based on Equations (4) and (5) and using the experimental band gap energies (see Table 2), the valence band energy, E_VB, of TiO₂ and Fe₃O₄ can be calculated to be 2.91 eV and 1.74 eV, respectively.

$$E_{CB}=\chi -E^c-0.5E_g$$

(4)

$$E_g=E_{VB}-E_{CB}$$

(5)

being the absolute electronegativities ($\chi$) of TiO₂ and Fe₃O₄ 5.81 eV and 5.77 eV, respectively, and E^C = 4.5 eV is the scaling factor relating the normal hydrogen electrode scale (NHE) to absolute vacuum scale [58].

As can be seen in Figure 9, when Fe₃O₄-TiO₂ is solar irradiated (see Solar spectrum shown in the embedded Figure [59]), the different steps that take place during the photocatalytic process are:

• Electron-hole pairs are produced in TiO₂ and Fe₃O₄ nanoparticles.
• Electrons can be easily transferred from the conduction band (CB) of TiO₂ to the CB of Fe₃O₄. It is a consequence of the positive energy difference between conduction bands of Fe₃O₄ and TiO₂ (3.19 and 0.93 eV, respectively).
• The transferred electrons would then migrate to the surface of Fe₃O₄ to further assist to oxygen reduction to form superoxide radical anion during photocatalysis [60].
• Additionally, electrons in the conduction band of TiO₂ will further react with molecular oxygen O₂ dissolved to also form the superoxide radical anion O₂^·− [61].
• Superoxide radical anion could recombine to yield hydrogen peroxide that can react with Fe(II) generated by the electrons transferred from the TiO₂ to Fe₃O₄, via a Fenton reaction, to generate ^·OH and Fe(III) [62].
• On the other hand, holes located in the valence band of TiO₂ are transferred to the surface of TiO₂ generating hydroxyl radicals because of the oxidation of water or surface hydroxyl species [60].
• Radiation corresponding to wavelength range above 388 nm (E < 3.2 eV) is not energetic enough to excite TiO₂ and generate electron-hole pairs, whereas Fe₃O₄ could be easily activated in this spectral range and produces charge carriers. Subsequently, the photogenerated electrons should be involved in the processes previously described in the step 3 of this proposed mechanism.
• The holes that are accumulated in the valence band of Fe₃O₄ will react with OH⁻ species existing on the surface of the catalyst, producing reactive hydroxyl radicals (^·OH).

Most of the considerations made in the proposed mechanism could be supported by experimental results. Thus, PL studies revealed a superior separation efficiency of the photoexcited electron-hole pairs in Fe₃O₄-TiO₂ NPs. Results obtained from the deconvolution of the high-resolution O 1s XPS show that positive holes generate hydroxyl radicals. In addition, as can be seen in Figure 10, absorption bands can be related to the energy levels proposed.

On the other side, the determined optical bandgap (Table 2) is originated by electronic coupling between the wide band gap of TiO₂ and the narrow band gap of Fe₃O₄ [63].

Thus, via the proposed mechanism, it can be deduced that in Fe₃O₄-TiO₂ material, not only the amount of photogenerated electron-hole pairs are increased, but also the separation efficiency of the photoexcited charges is enhanced. It is essential due to photocatalytic activity of photocatalysts which mainly depend on the extent of electron-hole pairs production and separation efficiency of these charge carriers [64].

3.4. Photocatalytic Experiments

Photocatalytic degradation of SFX is selected as a probe reaction to evaluate the photocatalytic activity of the so-prepared Fe₃O₄-TiO₂ thin films. Solar photocatalysis experiments were performed treating 5 mg·L⁻¹ aqueous solutions of SFX. The goal of photocatalytic experiments was not only to evaluate whether the incorporation of Fe₃O₄ NPs enhance the photocatalytic activity or not, but also to study the influence of thickness of the thin films on the SFX removal rates. Thus, in order to compare the effectiveness of Fe₃O₄-TiO₂ films with that of pure TiO₂, solar photocatalysis experiments were carried out using thin films with a similar thickness (~2 µm). Experimental results show that SFX follows first order kinetics according to Equation (6), in which t_30W can be calculated from experimental data by using Equation (2).

$$ln\frac{C}{C_0}=-k{t}_{30W}$$

(6)

From this fitting process, pseudo-first order constants for TiO₂ and Fe₃O₄-TiO₂ thin film were calculated to be 6.95·10⁻³ min⁻¹ and 1.35·10⁻² min⁻¹, respectively. As expected from the previously exposed optical characterization, when the composite material is used, the removal performance is considerably improved when solar photocatalytic processes are applied. Moreover, adsorption experiments indicated that SFX does not adsorb on the TiO₂ and Fe₃O₄-TiO₂ photocatalyst surface. These results are in agreement with the literature [22]. In addition, direct photolysis contribution is negligible. Thus, no elimination of SFX was observed when it was exposed to solar radiation, without the presence of the photocatalyst. In conclusion, it can be accepted that free radical oxidation is the main way of oxidation and, as was described in Section 3.3, hydroxyl radicals can be generated by different pathways.

In order to prove that the elimination is due to the presence of hydroxyl radicals, an experiment was carried out in the presence of T-butanol. T-Butanol is a very commonly used hydroxyl radical scavenger in aqueous matrices [24]. Results show that the presence of t-butanol completely inhibits the SFX removal.

On the order hand, in addition to the Fe₃O₄-TiO₂ film with a thickness of 2 µm, thin Fe₃O₄-TiO₂ films with thickness of around 1 and 1.5 µm were also prepared, as was mentioned above. Photocatalysis efficiency of these three samples is evaluated in Figure 11, in which the normalized concentration of SFX versus UV dose is represented. The presented results were calculated as an average value of the three repeated experiments per photocatalyst. Under solar irradiation, the concentration of the selected pharmaceutical evolves according to Equation (6) for all the cases and the calculated pseudo-first order constants are shown in

Table 4. Values of the apparent pseudo-first order rate constant using thin films with different thicknesses in the oxidation of SFX in water.

Sample	Thickness (µm)	k (10−2 min−1)
1 µm:Fe3O4-TiO2	0.97 ± 0.03	0.62 ± 0.004
1.5 µm:Fe3O4-TiO2	1.51 ± 0.04	1.03 ± 0.004
2 µm:Fe3O4-TiO2	1.99 ± 0.02	1.35 ± 0.003

. In view of the Figure 11 and Table 4, it is evident that a higher removal degree is achieved as the thickness of the Fe₃O₄-TiO₂ film increases in the studied range.

As an example, for an accumulated radiation dose of 150 Wh/m² (t_30w = 300 min), elimination yields of 84.2, 95.4 and 98.3% were reached, when 1 µm:Fe₃O₄-TiO₂; 1.5 µm:Fe₃O₄-TiO₂ and 2 µm:Fe₃O₄-TiO₂ were used, respectively. Furthermore, differences observed when 1.5 µm:Fe₃O₄-TiO₂ and 2 µm:Fe₃O₄-TiO₂ samples were used are less significant than those observed when comparing the results obtained with the 1 and 1.5 µm thick samples, which may be due to the existence of a critical film thickness.

Taking into account that there is no elimination of SFX by adsorption or direct photolysis, the presence of light and photocatalyst are necessary.

Experimental results obtained (Figure 11) demonstrate that activity is governed by the catalyst film thickness. This result allows us to conclude that all the deposited material participates in the solar photocatalysis process.

Finally, in order to check the stability of the fabricated thin films, solar photocatalytic experiments were carried out reusing one of these films. Specifically, the 1.5 µm:Fe₃O₄-TiO₂ photocatalyst was used in three consecutive reactions and no decrease in SFX elimination efficiency was observed.

4. Conclusions

The main conclusions of this work are:

Magnetite NPs and TiO₂, as examined by electron microscopy, were of crystalline nature, and the utilized method to dope TiO₂ resulted in imbibed magnetite NPs, randomly distributed in the titanium oxide. NPs size was (8.7 ± 1.1) nm. XPS confirmed the presence of Fe₃O₄ and the chemical bonding between TiO₂ and Fe₃O₄ NPs.

The process to obtain the modified titanium oxide layer for the “sandwich” structure was well controlled, and tested for thicknesses between 1 and 2 µm.

The calculated indirect bandgap is reduced when Fe₃O₄ NPs are included in the material. The small indirect energy gap obtained for magnetite NPs is consistent with the fact that Fe₃O₄-TiO₂ materials present absorption in the visible spectrum region.

The proposed mechanism of Fe₃O₄-TiO₂ thin films in solar photocatalytic processes could be supported by experimental results. It was determined that, in Fe₃O₄-TiO₂ material, not only are the number of photogenerated electron-hole pairs increased, but also the separation efficiency of the photoexcited charges is enhanced. Solar photocatalytic experiments evidenced the effectiveness improvement when modified thin films are used. Thus, pseudo-first order constants for TiO₂ and Fe₃O₄-TiO₂ 2 µm thin films were calculated to be 6.95·10⁻³ min⁻¹ and 1.35·10⁻² min⁻¹, respectively.

Regarding the thickness of the fabricated thin films, AFM measurements revealed that surface roughness seems to be independent of the number of deposited layers. However, a higher removal degree is achieved as the thickness of the Fe₃O₄-TiO₂ film increases in the studied range.

Finally, experiments reusing 1.5 µm:Fe₃O₄-TiO₂ photocatalyst structures evidenced the stability of the fabricated thin films.