Materials Sciences and Applications
 Vol.5 No.3(2014), Article ID:43630,12 pages DOI:10.4236/msa.2014.53016

New Preparation Method of Visible Light Responsive Titanium Dioxide Photocatalytic Films

Kaori Nishizawa*, Masahisa Okada, Eiji Watanabe

Materials Research Institute for Sustainable Development, National Institute of Advanced Industrial Science and Technology (AIST), Nagoya, Japan

Email: *k-nishizawa@aist.go.jp

Copyright © 2014 by authors and Scientific Research Publishing Inc.

This work is licensed under the Creative Commons Attribution International License (CC BY).

http://creativecommons.org/licenses/by/4.0/

Received 25 December 2013; revised 29 January 2014; accepted 16 February 2014

ABSTRACT

We report a new and simple preparation method of the visible light responsive Titanium dioxide (TiO2) photocatalytic films using sol-gel method and ultraviolet light (UV) irradiation. Proposed films were prepared on fused silica plates using titanium tetra-isopropoxide, urea, 2-methoxyethanol, water and UV irradiation. The 650˚C-annealed films were carbon-containing anatase type TiO2, not carbon-doped ones. The prepared films absorbed visible light with wavelengths longer than 400 nm. Also, organic dyes were effectively photodegradated by visible light irradiation in the presence of these films.

Keywords:Titanium Dioxide Films; Sol-Gel Method; UV Irradiation; Visible Light Responsive Photocatalyst

1. Introduction

Titanium dioxide (TiO2) has been widely studied for many applications, such as paints, cloth fibers, cosmetics and microelectronics, optical cells, solar energy conversion, photocatalyst for environmental purification and production of hydrogen gas, and so on. This is because TiO2 is a cheap material and shows nontoxicity, high activities and chemical stability. In particular, various anatase type TiO2 powders and films have been fabricated for development of photocatalytic activities such as strong organic degradation and superhydrophilicity [1] -[6] . However, photocatalytic reactions by TiO2 only proceed under ultraviolet (UV) irradiation, but do not proceed under visible light irradiation. That is because the anatase type pure TiO2 only absorbs UV light with wavelength shorter than 380 nm, based on its wide band gap (3.0 - 3.2 eV). However, UV light accounts for only about several % of solar energy. In addition, UV light responsive photocatalysts had been limited for use in the room because there are not a lot of UV lights in the room.

Recently, many attempts to develop the effective photocatalysts for the visible light region have been done [7] -[11] . That is, a lot of visible light responsive TiO2 photocatalysts, whose photocatalytic reaction can proceed under visible light, have been developed by doping something elements to the TiO2 crystal lattice or reduction of TiO2. The shift of the optical response of TiO2 from UV to the visible spectral range will have a profound positive effect on the efficient use of solar energy in photocatalytic reactions and the use in the room. The doping of TiO2 is currently attracting considerable interest as a promising route to extend the optical absorption of this material to visible spectral region. One promising approach to synthesizing visible light active photocatalysts is the substitution of Ti by transition metals, such as V, Cr, Ni, or Fe, and so on [12] -[15] . However, most of these metal-doped TiO2 do not show long-term stability or do not have sufficient activities for wide range of applications. Another promising approach is the doping of nonmetal atoms, such as N, S, or C [16] -[21] . The nonmetal atoms doping have been reported to be more effective for the band gap narrowing of TiO2 than transition metal doping [19] [20] . That is because their impurity levels are near the valence band edge of TiO2. Therefore, they do not act as charge carriers and their roles as recombination centers are minimized compared to the metal doping [13] [19] [20] . As a famous example of nonmetal doping, Asahi and co-workers proposed that substitutionaltype N doping was effective for the band gap narrowing of TiO2 due to the mixing of N 2p with O 2p states in the valence band [16] . As for the investigation of TiO2 modified with C, it has been reported some types of TiO2 such as substitutional C-doped TiO2, interstitial carbonate-doped TiO2 and highly condensed coke-like carbon containing TiO2 and so on [21] -[34] . It is reported that the TiO2 modified with C induce the visible light absorption by band gap narrowing or a role as photosensitizer like organic dyes. In these ways, the design of the electronic structure or the chemical modification of metal oxides was very effective for controlling their optical properties. However, an expensive apparatus was used or there were some safety hazard in these proposed methods.

On the other hand, the sol-gel method is one of the suitable and simple techniques for preparation of metal oxide films. In addition, it is also suited to design the network formation of metal oxide precursors, resulting in materials with special optical and catalytic properties. Furthermore, UV irradiation of metal oxide gel films is effective for the decomposition of organic compounds in the films or improvement of crystallinity of the films, and so on [35] -[38] . In this paper, we report a safety and simple preparation method of the visible light responsive TiO2 photocatalytic films by sol-gel and UV irradiation method.

2. Materials and Methods

2.1. Preparation of TiO2 Precursor Sol Solutions

All chemicals used in this study were of analytical grade and were used without further purification. The preparation methods of TiO2 precursor sol solutions (a)-(d) were as follows: The 0.25 mol/dm3 titanium-tetra-isopropoxide (Ti(O-i-Pr)4) was dissolved in 2-methoxyethanol under dry argon gas. Then urea was added to the solution and it was refluxed at 130˚C for 3 hours. After cooling the solution to room temperature, UV light (250 W ultra-high pressure mercury lamp, 100 mW/cm2 at 365 nm) was irradiated to the sol solution for 4 hours in the air at room temperature. After that, a small amounts of distilled water was added to it and it was stirred for one night. The preparation conditions of sol solutions were shown in Table 1.

2.2. Preparation of TiO2 Films

Fused silica plates (25 × 25 × 1 mm) were used as support substrates. The fused silica plate was dipped into the TiO2 precursor sol solution. The dipped plate was withdrawn from the solution at the rate of 0.5 mm/s. The dip-coated films were dried at room temperature for 30 s and then dried at 100˚C for 30 min. After drying, the films were heated at the rate of 10˚C/min and annealed at 650˚C for 1 hour in the air.

2.3. Characterization

The crystal structures of the films were identified by thin film X-ray diffraction (XRD: MPX, Mac Science)

Table 1. Preparation conditions of TiO2 precursor sol solutions and films.                                         

measurements using CuKα radiation. The acceleration voltage and current were 40 kV and 30 mA, respectively. The UV-visible (UV-vis) absorption spectra of the films were taken on a Hitachi U-4100. Elemental analysis of C, H, and N in the dried and annealed gels was carried out in an elemental analyzer Thermo Finnigan Flash EA 1112. The dried gels were prepared by vacuum drying of the sols at room temperature and the annealed gels were prepared by sintering of the dried gels at 650˚C for 1 hour. X-ray photoelectron spectroscopy measurements of the films were carried out using a Sigmaprobe spectrometer (XPS: Thermo Electron) with MgKα X-ray (hν = 1254 eV) radiation to investigate the surface properties. The shift of the binding energy due to relative surface changing was corrected using the C1s level at 284.5 eV as an internal standard. Ar+ etching was applied to clean the surface of samples and to measure the depth profiles. The estimated etch rate of the ion gun was expected to be about 0.05 nm/s for the TiO2 thin films [39] . 1H-NMR spectra of the TiO2 precursor dried gels were recorded on a Varian INOVA300 spectrometer in CDCl3.

2.4. Photocatalytic Evaluation of TiO2 Films

The photocatalytic activities of prepared TiO2 films were evaluated by examining photodecomposition of methylene blue (MB). The substrates coated with TiO2 films were placed in a 1.0 × 10−2 mmol/dm3 aqueous solution containing MB for 18 hours under dark. Then the solutions were irradiated with visible light (wavelength: 410 - 520 nm). Used lamp was 250 W ultra-high pressure mercury lamp (UHPML: multilight UIV-270, Ushio) and two pieces of glass filters were used for selection of wavelength (No. 3-73 and 7-59, Corning). The concentration change of MB by visible light irradiation was evaluated by monitoring 665 nm absorbance using the UV-vis light spectrometer U-4100 at hourly intervals.

3. Results and Discussion

3.1. Characterization of the TiO2 Films

Figure 1 shows the XRD patterns of TiO2 films (A)-(D) prepared using the sol solutions (a)-(d). For each sample, all peaks were indexed to the anatase phase of TiO2 (JCPDS file No. 21-1272). The average crystallite sizes were calculated using (101) diffraction peaks according to the Scherrer equation. The crystallite sizes of all films were almost the same, ca 18 nm.

Figure 2(a) shows UV-vis absorption spectra of TiO2 films (A)-(D). A strong absorption assigned to the band-band transition can be observed in the ultraviolet region for all samples. In addition, all TiO2 films absorbed not only UV light, but also visible light with wavelength longer than 400 nm. In particular, the absorbance of the TiO2 film (A) prepared using the sol solution (a) was higher than that of the films (B)-(D). Assuming the materials to be an indirect semiconductor, the band gap energies of films were estimated from the intercept of the tangents to the plots of (αhν)1/2 versus photon energy hν as shown in Figure 2(b) [21] . The optical band gap energies of all films estimated from the plots of Figure 2(b) were around 3.2 eV. It is known that the band gap energy of anatase type TiO2 is 3.2 eV. Accordingly, it was expected that the visible light absorptions in these films were not due to band gap narrowing.

The CHN elemental analysis of 650˚C-annealed TiO2 powder samples was carried out in order to examine the reasons of visible light absorption as shown in Table 2. The found values of elemental analysis were C: 0.12% - 0.23%, H: 0.00% and N: 0.00% in all samples. The visible light absorption of TiO2 will be due to carbon species including in the films.

The XPS measurements were carried out to determine the chemical state of elements around the surface of films in details. Figure 3 shows N1s spectra of films (A)-(D). Broad energy bands were observed in the range

Figure 1. XRD patterns of sol-gel derived TiO2 films. (A) TiO2 film which was made from the sol solution (a); (B) TiO2 film which was made from the sol solution (b); (C) TiO2 film which was made from the sol solution (c); (D) TiO2 film which was made from the sol solution (d).                           

Table 2. The CHN elemental analysis of TiO2 annealed at 650˚C.

from 404 to 396 eV before surface etching (etching time 0 s). However, these bands disappeared after surface etching for 20 s (ca. 1 nm etching from the surface). From the results, broad N1s bands around 400 eV can be assigned to adventitious nitrogen species on the surface. Accordingly, it was clear that nitrogen is not included in the films. The results of N1s spectra agreed with those of the elemental analysis. Figure 4 shows C1s spectra of films (A)-(D). Broad energy bands were observed in the range from 290 to 282 eV before surface etching (etching time 0 s). The peaks around 289, 286 and 284.5 eV for all films before surface etching can be assigned to adventitious carbon species, C = O of, C-O and C-C, respectively [21] [25] . After surface etching for 20 s, adventitious carbon species on the surface disappeared and new peaks appeared around 283.5 eV. Accord-

Figure 2. UV-vis absorption spectra (a) and plots of (ahn)1/2 versus photon energy (hn) (b) of sol-gel derived TiO2 films. (A) TiO2 film which was made from the sol solution (a); (B) TiO2 film which was made from the sol solution (b); (C) TiO2 film which was made from the sol solution (c); (D) TiO2 film which was made from the sol solution (d).       

ing to the literatures, it has been reported that there are highly condensed coke-like carbon originated from another C-C species, that is, Ti-alkoxide derived C-C species in the films in the case of sol-gel method using alkoxide precursors [22] [27] . Thus, it was suggested that the new peaks around 283.5 eV were originated from Ti-alkoxide derived C-C species that were different from adventitious carbon species. Furthermore, the peak around 283.5 eV of film (A) was greater than those of films (B)-(D) in the case of surface etching for 20 s. In addition, the peak around 283.5 eV of film (A) after surface etching for 140 s (ca. 7 nm etching from the surface) got larger than that after surface etching for 20 s. From the results of Figures 2, 4 and Table 2, it was found that the visible light absorption got stronger with increasing of the amounts of C species in the sample. These results agreed with an earlier report [20] [27] . On the other hand, new small peaks appeared around 281 eV for all films after etching for 140 s. The peak around 281 eV can be assigned to Ti-C species [21] [24] [25] . It was expected that the oxygen sites of TiO2 lattice were substituted by carbon atoms and Ti-C structures were formed in the

Figure 3. XPS spectra of N1s of sol-gel derived TiO2 films. The digits, 0 s and 20 s, in figures show etching time. (A) TiO2 film which was made from the sol solution (a); (B) TiO2 film which was made from the sol solution (b); (C) TiO2 film which was made from the sol solution (c); (D) TiO2 film which was made from the sol solution (d).       

Figure 4. XPS spectra of C1s of sol-gel derived TiO2 films. The digits, 0 s, 20 s and 140 s, in figures show etching time. (A) TiO2 film which was made from the sol solution (a); (B) TiO2 film which was made from the sol solution (b); (C) TiO2 film which was made from the sol solution (c); (D) TiO2 film which was made from the sol solution (d).

crystal lattice. However, it might not be effective for the visible light absorption because a quantity of Ti-C species formed in the crystal lattice was very few and the formed Ti-C species were not in the surface. Therefore, it was expected that the visible light absorption of TiO2 is due to photosensitization by coke-like carbon formed in the films [20] -[22] [27] [28] . In the literature [21] , it has been reported that two possible pathways ascribed to band gap narrowing by carbon doping and to carbon photosensitization are not involved in the photoreaction for single-nonmetal doped TiO2. The results in this paper accorded with the former report.

3.2. Formation Mechanism of Carbon-Containing TiO2

Formation mechanism of carbon-containing TiO2 will be considered as follows: Ti(O-i-Pr)4 was easy to be hydrolyzed by H2O addition and form precipitations in the solution in the case of using isopropyl alcohol as a reaction solvent. However, Ti(O-i-Pr)4 formed a stable and homogeneous TiO2 precursor sol without precipitating in the solution after H2O addition in the case of using 2-methoxyethanol as a reaction solvent. From these phenolmena, it was expected that Ti(O-i-Pr)4 caused solvent exchange reaction and/or alcoholysis reaction with 2-methoxyethanol, that is, 2-methoxyethanol attached to the titanium metal center [40] -[43] . As a result, the sixcoordinated Ti complexes were formed in the reaction and stabilized for hydrolysis.

Table 3 shows the colors of prepared sol solution and results of the CHN elemental analysis of TiO2 precursor gels dried in a vacuum oven at room temperature. The sol solution prepared without urea remained transparent after H2O addition as shown in Tables 3(b) and (d). It has shown that these solutions are stabilized for hydrolysis. That will be because Ti(O-i-Pr)4 caused solvent exchange reaction and/or alcoholysis reaction with 2-methoxyethanol as described above. Furthermore, the color of sol solution prepared without urea has changed from clear transparent to yellow transparent after UV irradiation (Tables 3(b) and (d)). Considering the ligand field theory, the result may be because division width of the d-orbitals in titanium became narrow by change of ligand field, that is, ligands of titanium fully exchanged from isopropoxides to 2-methoxyethoxides by UV irradiation [44] -[47] . According to 1H-NMR spectra, the doublet peak at 1.25 ppm originated from methyl groups of isopropoxides disappeared by irradiating UV light as shown in Figure 5. From the result, it was suggested that the ligand substitution reaction occurred by UV irradiation. In addition, carbon contents in the dried gel and the annealed TiO2 prepared from sol solution (b) with UV irradiation were more than those in the dried gel and the annealed TiO2 prepared from sol solution (d) without UV irradiation as shown in Tables 2 and 3. It may be because eliminated organic ligands (isopropoxides) were decomposed and condensed as cokes in the gels by UV irradiation.

On the other hand, the rate of hydrolysis and gelation for the sol solutions prepared using urea (Tables 3(a) and (c)) was faster than that for the sol solutions prepared without urea (Tables 3(b) and (d)). In addition, the dried gels prepared with urea have included nitrogen as shown in Tables 3(a) and (c). According to the literatures [48] -[50] , it has been reported that urea coordinates to titanium through weak C=O ® Ti coordination bonding with remaining the carbonyl groups. Therefore, it was expected that the sites coordinated by urea are

Figure 5. 1H-NMR spectra of the TiO2 precursor dried gels prepared without urea. (A) Dried gel before UV irradiation and without H2O addition; (B) Dried gel prepared without UV irradiation and with H2O addition; (C) Dried gel prepared after UV irradiation and without H2O addition; (D) Dried gel prepared after UV irradiation and with H2O addition. 

easy to be hydrolyzed by H2O. Furthermore, nitrogen and carbon contents in the dried gels increased by UV irradiation (Tables 3(a) and (c)). According to 1H-NMR spectra, the ratio of integral value of peak assigned to NH2 groups in urea and that of OCH3 groups in 2-methoxyethoxides became larger by UV irradiation. From the results, in the case of the samples prepared using urea, it was suggested that ligands of titanium changed from 2-methoxyethoxides to urea by UV irradiation. After that, the released organic ligands were decomposed and condensed by UV irradiation, coke-like carbon would have been formed in the gels. About nitrogen, it was expected that urea eliminated by hydrolysis was decomposed after annealing and nitrogen species released completely from the gels. In this way, it was suggested that TiO2 became able to absorb the visible light because the carbon contents in the TiO2 improved by urea addition and UV irradiation.

3.3. Photocatalytic Evaluation of TiO2 Films

In order to evaluate the photocatalytic activities of the prepared TiO2 films toward visible light irradiation, the absorbance change of MB at 665 nm was monitored as a function of visible light irradiation time. Figure 6 shows plots of ln(C/C0) vs irradiation time t, where C0 and C are the concentrations of MB at t = 0 and t = t, respectively. Concentrations of MB were calculated from the absorbance. MB aqueous solutions immersing TiO2

Table 3. The colors of TiO2 precursor sol solution and the CHN elemental analysis of TiO2 precursor gels dried in a vacuum oven at room temperature.

Figure 6. Photocatalytic activities of sol-gel derived TiO2 films under visible light irradiation (wavelength: 410 - 600 nm). Dotted lines show the concentration changes of methylene blue under dark. (A) TiO2 film which was made from the sol solution (a); (B) TiO2 film which was made from the sol solution (b); (C) TiO2 film which was made from the sol solution (c); (D) TiO2 film which was made from the sol solution (d).

films (A)-(D) were clearly photo-bleached by visible light irradiation. The photo-bleaching of MB is caused by photo-oxidative decomposition derived from electron holes on valence band of TiO2 or photo-reduction derived from electrons photo-generated on conduction band of TiO2. Generally, it is reported that photo-reduction is difficult to occur because the electrons photo-generated and excited from valence band to conduction band are trapped by O2 in the air [2] [4] [51] [52] . Therefore, photo-oxidative decomposition is easy to be caused by electron holes on valence band of TiO2 instead. When photo-reduction of MB occurs, a new peak originated from reduction form of MB is observed at 256 nm in the UV-visible absorption spectra. In this experiment, the new peak at 256 nm did not appear together with photo-bleaching of MB. Therefore, the photo-bleaching in this experiment was judged to be due to the photo-oxidative decomposition. The photo-oxidative decomposition of MB in the presence of the TiO2 films obeyed good first-order kinetics. The apparent rate constant was obtained from the slop of the straight line, which was strongly dependent on the visible light absorbance of films as shown in Figure 6. In particular, the decomposition rate of MB in the presence of the film (A) was faster than that of the other films (B)-(D). In this way, the TiO2 films prepared by these methods showed visible light responsive photocatalytic activities.

On the other hand, upon illumination in the absence of the photocatalytic films, the concentration of MB slightly decreased with increasing of visible light irradiation time. This fact meant that MB itself slightly absorbed visible light in this region and was a little photo-bleached. According to the UV-visible absorption spectral measurement of MB, the phenomena were suggested to be due to the photodecomposition of MB. Moreover, the concentration changes of MB aqueous solutions under dark were measured and shown in dotted lines of this figure. Also under dark, the concentration of MB slightly decreased over time in the solution immersing TiO2 films (A)-(D) and without films (blank). From the results, MB has been slightly removed from the liquid phase just by their adsorption on TiO2 films and/or the glass beaker surface. However, their influence can be omitted because the amounts of the photo-absorption of MB itself and the adsorption of MB on the surface are little.

4. Conclusion

Carbon-containing TiO2 films were prepared using the four types of sol solutions. All films were anatase type TiO2 and absorbed visible light with wavelength longer than 400 nm effectively. In addition, the photocatalytic activities of the films under visible light (410 - 520 nm) irradiation were confirmed by evaluation of the MB decomposition. The sol-gel method using urea addition and UV irradiation was simple and effective method for the fabrication of visible light responsive TiO2 photocatalyst.

Acknowledgements

We would like to thank Dr. Masakazu Nishida, National Institute of Advanced Industrial Science and Technology (AIST), for helpful technical advices in relation to 1H-NMR spectral measurement.

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NOTES

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