Scholarly article on topic 'Increase of the Photocatalytic Activity of TiO𝟐 by Carbon and Iron Modifications'

Increase of the Photocatalytic Activity of TiO𝟐 by Carbon and Iron Modifications Academic research paper on "Chemical sciences"

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International Journal of Photoenergy
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Academic research paper on topic "Increase of the Photocatalytic Activity of TiO𝟐 by Carbon and Iron Modifications"

Hindawi Publishing Corporation International Journal of Photoenergy Volume 2008, Article ID 721824, 15 pages doi:10.1155/2008/721824

Review Article

Increase of the Photocatalytic Activity of TiO2 by Carbon and Iron Modifications

Beata Tryba

Department of Chemical Technology and Engineering, Faculty of chemical Engineering, Szczecin University of Technology, ul. Pulaskiego 10, Szczecin 70-322, Poland

Correspondence should be addressed to Beata Tryba, Received 27 August 2007; Accepted 23 November 2007 Recommended by M. Sabry A. Abdel-Mottaleb

Modification of TiO2 by doping of a residue carbon and iron can give enhanced photoactivity of TiO2. Iron adsorbed on the surface of TiO2 can be an electron or hole scavenger and result in the improvement ofthe separation of free carriers. The presence of carbon can increase the concentration of organic pollutants on the surface of TiO2 facilitating the contact of the reactive species with the organic molecules. Carbon-doped TiO2 can extend the absorption of the light to the visible region and makes the photocatalysts active under visible-light irradiation. It was proved that TiO2 modified by carbon and iron can work in both photocatalysis and photo-Fenton processes, when H2O2 is used, enhancing markedly the rate of the organic compounds decomposition such as phenol, humic acids and dyes. The photocatalytic decomposition of organic compounds on TiO2 modified by iron and carbon is going by the complex reactions of iron with the intermediates, what significantly accelerates the process of their decomposition. The presence of carbon in such photocatalyst retards the inconvenient reaction of OH radicals scavenging by H2O2, which occurs when Fe-TiO2 photocatalyst is used.

Copyright © 2008 Beata Tryba. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.


The photocatalytic process with using TiO2 photocatalyst is very promising for application in the water purification because many organic compounds can be decomposed and mineralized by the proceeding oxidation and reduction processes on TiO2 surface. The most commonly tested compounds for decomposition through the photocatalysis are phenols, chlorophenols, pesticides, herbicides, benzenes, alcohols, dyes, pharmaceutics, humic acids, organic acids, and others.

TiO2 is the most commonly used photocatalyst, because it is nontoxic, chemically stable, cheap, and very efficient. However, it has some disadvantages: one of this is a relatively high value of the bandgap, around 3.2 eV, which limits its using to the UV light, high dispersion in the water which causes difficulties in sedimentation, and sensitivity to the recombination of photoinduced electrons and holes, which decreases its photocatalytic activity. Many efforts of researchers are focused on the enhancing the photoactivity of TiO2 by improving the separation between free carriers, increasing the adsorption abilities of the photocatalyst surface, or charging

one photocatalyst by another when the mixture of two photocatalysts is used.


2.1. Carbon-doped TiO2 visible ligh-active photocatalysts

Recently, modification of TiO2 by C doping towards obtaining the visible light-active photocatalyst has been reported [1-9]. The narrowing of the bandgap, the anodic shift of the quasi-Fermi potential, the visible-light absorption, and the transfer of photoexcited carriers to the reactive sites at the catalyst surface have been noticed as a result of nonmetal anion doping affecting its visible-light activity.

Sakthivel and Kisch [2] proved that prepared C/TiO2 photocatalyst from TiCl4 and tetrabutylammonium hydroxide was active under artificial solar light and could efficiently decompose tetrachlorophenol with the activity higher than TiO2 and TiO2 doped with nitrogen. In Figure 1, diffuse reflectance spectra of pure and carbon-doped TiO2 are shown [2].

1.5 2 2.5 3 3.5 4

E (eV)

Figure 1: (A) Diffuse reflectance spectra of modified and pure TiO2, (B) plot of transformed Kubelka-Munk function versus the energy of the light absorbed; (a) TiO2, (b) TiO2-2.98%C, (c) TiO2-0.42%C, (d) TiO2-0.03%C.

180 t (min)

Figure 2: (A) Photomineralisation of 4-chlorophenol with artificial visible light (A = 455 nm; TOC0 and TOC( = total organic carbon content at times 0 and t); (B) diffuse indoor daylight degradation of 4-chlorophenol and remazol red on pure and modified TiO2; (a) TiO2, (b) TiO2-2.98%C, (c) TiO2-0.42%C, (d) TiO2-0.03%C.

Two absorption maxima on the UV-Vis spectra have been observed, in the range of UV and Vis, showing that these photocatalysts could be excited with the wavelengths in the visible region.

In Figure 2, the mineralisation of the tetrachlorophenol on these samples is presented.

Shen et al. [4] prepared C/TiO2 photocatalyst through calcination of TiCl4 in air at 350°C and proved that such prepared photocatalyst was active for decomposition of trichloroacetic acid under visible light. Carbon-doped TiO2 can be prepared also by hydrolysis and calcinations of TiCl4 with tetra-n-butyl ammonium hydroxide [7], and by calci-

nations of TiO2 with urea and thiourea [8] or oxidation of TiC at high temperatures [9]. Choi et al. [9] have investigated carbon-doped TiO2, and they claimed that substitution of C for O in the TiO2 leads to a photocatalytic decomposition of methylene blue under visible-light irradiation. Di Valentin et al. [10] reported a theory of in-building of carbon atom in the structure of TiO2, and they showed that carbon atom could replace oxygen atom or titania atom depending on the concentration of oxygen in the structure of TiO2. Replacing of carbon atom with Ti conducts to form the new states in the bandgap. Some oxygen vacancies are formed, which could be responsible for the extending of the photocatalytic activity

Figure 3: Partial geometry of the models for: (a) one substitutional C atom to O (Cs-o), (b) one substitutional C atom Ti (Cs-Ti), (c) one interstitial C atom (C;), and (d) one interstitial C atom nearby an oxygen vacancy (Q + VO) in the anatase TiO2 supercell; the yellow spheres represent O atoms, the small brown spheres represent Ti atoms, and the black represents the carbon impurity.

of C/TiO2 to the visible range. The model proposed by Di Valentin et al. is presented in Figure 3 [10].

Preparation of C/TiO2 photocatalyst by heating of TiO2 with the vapours of n-hexane [11] and ethanol [12], and by mixing of TiO2 with liquid ethanol and heating under pressure [13] has been also reported. Enhanced photoactivity of carbon-doped TiO2 prepared under pressure has been noticed for decomposition of dyes under UV irradiation [13].

Carbon-doped TiO2 electrodes have been prepared by modified sol-gel method from tetraisopropoxide, 2-propanol, and activated carbon at 600°C and were used for electrochemical photooxidation of sodium oxalate; the efficiency of electrode with 5% of doped activated carbon was two times higher than the electrode without carbon doping [14].

Effective photoresponse in the visible-light region was observed in carbon-doped TiO2 [7,15]. Carbon-doped TiO2 nanotube arrays for efficient solar water splitting have been prepared by Park et al. [16]. The synthesised TiO2 -xCx nan-otube arrays showed much higher photocurrent densities and more efficient water splitting under visible-light illumination (>420 nm) than pure TiO2 nanotube arrays.

2.2. TiO2 and activated carbon (AC) composites

Herrmann et al. [17], Arana et al. [18, 19], and Liu et al. [20] have observed the synergistic effect for the mixture of TiO2

with activated carbon (AC). Improving the photocatalytic properties of TiO2/AC composite was explained by the high adsorption of the impurities on the surface of activated carbon and their transfer to TiO2 surface. Carbon/TiO2 microsphere has been prepared by Nagaoka et al. [21], and it was successfully used for decomposition of acetaldehyde through the concentration of the pollutant around TiO2 anchored on the composite surface. In Figure 4, the enhanced pho-toactivity with using TiO2/AC composite is presented under both solar and UV irradiations, for photodecomposition of p-nitrophenol [19].

2.3. Carbon-coated TiO2

Carbon-coated TiO2 photocatalysts have been prepared by calcination of TiO2 with carbon precursor such as (polyvinyl alcohol) (PVA), poly (terephthalate ethylene) (PET), or hy-droxyl propyl cellulose (HPC) at high temperatures, 700-900°C [22-24], or impregnation ofTiO2 with sacharose 400-600°C [25]. Carbon coating TiO2 retarded the phase transformation from anatase to rutile, which usually occurs during heating TiO2 at 700° C and through that improved the crystallinity of anatase phase in TiO2, which was responsible for its high photoactivity. From the other hand, carbon coating reduced the amount of UV radiation reaching the surface of the TiO2 particles. A balance among different factors controlled by the carbon layer on the TiO2 particles was

4.5 -4 -3.5 -3 -2.5 -2 -1.5 -1 -0.5 0

Time (min)

Figure 4: Apparent first-order linear transform ln (n0/n) = f(t) of the p-nitrophenol concentration during its degradation; UV-light: (A)—bare TiO2, (B)—13% AC-TiO2; solar light: (A)—bare TiO2, (□)—13 % AC-TiO2 .

100 200 300

Time of UV irradiation (h)

Figure 6: Color fading of MB solution under UV irradiation in the presence of carbon-coated TiO2 sample (10wt% of carbon) with cycling to use fresh MB solution, concentration of MB = 2.94 x 10"5M.

Figure 5: TEM images of carbon-coated TiO2 prepared from TiO2 and PVA.

required to get high-photocatalytic activity. On the sample prepared at 850° C with a carbon content of about 3.5 wt%, the highest rate constant for methylene blue decomposition was obtained, in which the transition from anatase to rutile was suppressed, and carbon layer was thin enough to transmit UV rays [24]. The TEM images of carbon-coated TiO2 are presented in Figure 5 [23].

Carbon-coated TiO2 samples showed high adsorption and high photoactivity towards methylene blue decomposition [22-25], however in case of phenol, reactive black 5 or iminoctadine triacetate decomposition was slower than on unmodified TiO2 [23]. In Figure 6, there is shown a cycling decomposition of methylene blue on carbon-coated TiO2 prepared from powders of TiO2 and PVA at 900° C with ratio of TiO2/PVA = 50/50 in weight [22].

Coating of carbon changes the nature of TiO2 from hy-drophilic to hydrophobic and results in lower adsorption of water on the photocatalyst surface and lower formation of OH radicals in comparison with TiO2. Probably in case of methylene blue, decomposition is going by the direct oxidation pathway, therefore high adsorption of methylene blue on the carbon-coated TiO2 improved its photocatalytic activity.

2.4. TiO2 loaded carbon

TiO2 can be loaded on the activated carbon (AC) [2635], carbon fibers [36], carbon nanotube [37], exfoliated graphite [38, 39] with efficient adsorption and decomposition of organic compounds such as phenol, 4-chlorophenol, methyl orange, methylene blue, iminoctadine triacetates, oils, dichloromethane, and so forth. In Figure 7, TiO2 loaded on different carbon structures is presented.

TiO2 loaded carbon spheres have been prepared by hydrolysis of TiOSO4 under hydrothermal conditions. Adsorption and decomposition of methylene blue on TiO2 loaded carbon spheres are presented in Figure 8 [28]. It can be observed saturation with methylene blue adsorption on carbon spheres (CS), and no change in methylene blue concentration with UV irradiation, whereas on anatase loaded carbon spheres (Ti/CS) methylene blue could be adsorbed in the dark and decomposed with UV irradiation in the cycles.

Tryba et al. [29] have reported preparation of TiO2 loaded AC from the tetraorthotitanate solution. Higher removal of organic compounds has been achieved by combination of adsorption, which occurred in the pores of activated carbon, with decomposition on the anatase particles. Decreas in adsorption has been observed after TiO2 mounting, because mounted TiO2 particles blocked the entrance to the pores of AC, however these TiO2 particles could decompose the adsorbed organic molecules in the pores of AC, enhancing the total removal of the pollutant [29].

El-Sheikh et al. [34] have prepared TiO2 loaded AC by different methods: chemical vapour deposition (CVD), direct air-hydrolysis (DAH), and high-temperature impregnation (HTI), among those methods, CVD gave the best bounding of TiO2 with the carbon surface; anatase particles were placed in the pores of activated carbon.

Tsumura et al. have mounted TiO2 on the exfoliated graphite [38]. High sorption of oil and its decomposition under UV irradiation have been observed.

Figure 7: TiO2 loaded on (a) carbon spheres [28], (b) activated carbon [28], (c) granular activated carbon [35], (d) carbon nanotubes [37], (e) carbon fibers [36], and (f) exfoliated graphite [38].

3. TIO2 MODIFIED BY IRON 3.1. Preparation methods

There are few methods of Fe doping to TiO2. The sol-gel method has been widely used for preparation of Fe-doped TiO2 from TiCl4 or titania alkoxide and an iron precursor like FeCl3, Fe(NO3)3 -9H2O, or Fe(III)-acetyloacetonate [4047]. Wang et al. [40] have reported that preferable preparation of Fe-doped TiO2 to get the uniform distribution of the dopant ions on TiO2 particles is hydrolysis of a homogeneous mixture of organic titanium and organic iron precursors in isopropyl alcohol. Preparation of Fe-doped TiO2 by hydrolysis of TiCl4 with FeCl3 appeared to be less favourable than using Fe(III)-acetyloacetonate as an iron precursor. Fe doping from microemulsion of Ti tetraisopropoxide with an aqueous solution of iron and further calcinations has been reported by Adan et al. [48], Fe-doped TiO2 can be obtained also through the calcination of FexTiS2 [49-51], plasma oxidative pyrolysis [52], one-step flame spray pyrolysis (FSP) [53], coprecipitation and immersion [46], and by the wet impregnation method from Fe(III) acetylacetonate [54] or Fe(NO3)3-9H2O [42].

Navio has been reported that impregnation with Fe(III)-acetyloacetonate gives more homogeneous distribution of iron for each mixed oxide sample on the particle surfaces but

UV irradiation

100 80 -60 40 20 -

Sample Ti/CS

30 Time (h)

Figure 8: Changes in relative concentration of MB in the solution in which pristine carbon spheres (CS) and anatase loaded one (Ti/CS) were dispersed.

not between particles in comparison with impregnation with Fe(NO3)3-9H2O [54].

Recently, doping of Fe to TiO2 by the ultrasonic-induced hydrolysis reaction of tetrabutyl titanate (Ti(OC4H9)4) in a ferric nitrate aqueous solution has been reported in [55].

The mechanical alloying on the solid state reaction of hematite, Fe2O3, and titanium has been also sufficiently used for introducing of iron to TiO2 lattice [56].

TiO2/Fe thin film has been prepared by metal (Fe) plasma ion implantation [57, 58] and by magnetron sputtering method [59].

Using a simple sol-gel method, a novel magnetic photo-catalyst was produced by immobilisation ofTiO2 nanocrystal on Fe-filled carbon nanocapsules. TiO2-coated Fe-CNC displayed good performance in the removal of NO gas under UV exposure [60].

Fe-doped TiO2 nanotubes with small diameter of 10 nm were obtained by hydrothermal method [61].

3.2. Visible-light activity of fe-doped TiO2

It has been found that the addition of transition metals to TiO2 can improve the photocatalytic activity of the photo-catalyst by UV irradiation and extend its use in the visible region of the electromagnetic spectrum. It has been observed the red shift in the UV-Vis spectra due to the introduction of the 3d electron state of Fe3+, 3d5, in the conduction band of TiO2 [40, 44, 48, 49, 58, 59, 62-65].

The absorbance of visible light is higher for higher amount of doped iron, as it is presented in Figure 9 [48].

This implies that iron-doped TiO2 may be photocatalyti-cally reactive under visible-light irradiation. Navio et al. have reported that the photodegradation of oxalic acid under visible irradiation, not occurring with TiO2, could be observed for Fe-doped TiO2 using 5% Fe-containingsamples [54]. Na-har et al. reported that Fe-doped TiO2 was responsive to the visible-light activity of phenol degradation [49]. Teoh et al. have reported that by flame spray pyrolysis a stable Fe-TiO2 photocatalyst can be prepared and at the ratio of Fe/Ti = 0.05 it has high activity towards oxalic acid mineralisation under visible light [53]. Wang et al. have reported that for Fe(III) doping in TiO2 > 0.05 at.%, decomposition of methyl orange under UV irradiation has been lower than on un-doped TiO2, but under visible-light irradiation the Fe(III)-doped TiO2 with an intermediate iron doping concentration of «1 at.% had the highest photocatalytic reactivity due to the narrowing of bandgap so that it could effectively absorb the light with longer wavelength [52]. Chen and Peng have reported the preparation of magnetic-nanometer titanium dioxide/ferriferous oxide (TiO2/Fe3O4) composite photocatalyst with the particles size of 30-50 nm, which appeared to be very active under visible light and highly effective in discoloring of wastewater [66].

It has been investigated that Fe/TiO2 particles had a higher hydrophilic property compared with TiO2 [65, 67].

TiO2/Fe thin film has been demonstrated to have antimicrobial activity after being irradiated with visible light [68].

3.3. Enhancement of photocatalytic activity of TiO2 by iron doping

It is generally accepted that Fe(III) centres form shallow charge trapping sites within the TiO2 matrix as well as on the particle surface through the replacement of Ti(IV) by Fe(III)



350 450

Wavelength (nm)

TiFe-1.5 TiFe-3.5 TiFe-5.1

Figure 9: UV-Vis spectra of Fe-doped TiO2 with different iron content.

Fe(III) + e~ ^ Fe(II)*



Fe(III) + h+ ^ Fe(IV)*

Semiconductor (TiO2)

Figure 10: Scheme of mechanism of TiO2 photocatalysis with modifications by Fe(III) ion doping (CB—conduction band, VB— valence band).

[69]. Based on the favourable energy levels, Fe(III) centres may act either as an electron or a hole trap (see Figure 10); so that photogenerated charge carriers are temporarily separated more effectively [40].

Wang et al. [40] have reported that enhancement of the quantum yield by Fe(III) doping TiO2 can be explained by assuming that the Fe(III) centre acts predominately as a shallow electron trap from which the electron is transferred to molecular oxygen more rapidly than the undoped TiO2.

However, it was proved that the photoactivity of Fe/TiO2 catalyst is dependent on the way of preparation and the amount and state of iron.

Wang et al. [40] have reported that the highest quantum yield has been obtained when Fe(III)-acetyloacetonate precursor was used and for the optimal doping levels 0.25 and 0.5 atom %. They have also reported that above-mentioned optimal doping level, some of the Fe(III) dopants might act as shallow hole traps leading to an enhanced recombination of the trapped charge carriers.

Navio et al. [42] have also observed that at the some conditions and for the certain quantity of Fe(III), the dopant can be a center of recombination. They prepared Fe/TiO2 by an impregnation of TiO2 with Fe(NO3)3-9H2O and by the solgel method from TiCl4 and Fe(NO3)3 - 9H2O. They have been reported that Fe/TiO2 prepared by the sol-gel method was less active than TiO2 due to the fact that dopants acted more as recombination centres than a trap sites for charge transfer and the obtained photocatalysts had the lower amount of surface hydroxyl groups and a lower anatase-to-rutile ratio compared with TiO2 precursor sample. They proved that the existence of separated hematite or pseudobrookite (Fe2TiO5) phases in samples containing more than 2% iron could decrease the activity [42]. It has been also proved that the excess of deposited iron on TiO2 can form Fe(OH)2+, which has the greater adsorption to the incidence light than TiO2 in the range of 290-400 nm, and can cause decreasing of the Fe/TiO2 photoactivity [69]. The low temperature of calcinations, such as 300°C in Fe/TiO2 preparation appeared to be favoured taking into account its photoactivity [70].

Different amount of doped Fe(III) to TiO2 has been reported to affect the enhanced photoactivity of photocatalyst, dependent on the way of preparation and degradation compound.

Adan et al. [48] reported the enhancement of photocat-alytic activity of Fe-doped TiO2 for doping levels up to ca. 1 wt%, which was attributable to the introduction of Fe3+ cations into the anatase structure. Nahar et al. [49] reported that the molar ratio of 0.005 Fe content in Fe-doped TiO2 was the optimum for degradation rate of phenol under both the UV and visible-light irradiations. Hung et al. [44] also found that 0.005 mol% of iron ions can enhance the photo-catalytic activity, while too great an amount will make the iron ions become recombination centres for the electron-hole pairs and reduce the photocatalytic activity. Chen et al. [47] and Feng et al. [71] have found the highest pho-tocatalytic activity of Fe-doped TiO2 for 0.05 at.% Fe(III). The photocatalytic decomposition of Rhodamine B. on the nanosize Fe(III)-doped TiO2 catalysts prepared by the hydrothermal method with TiCl4 as the precursor was higher than on TiO2, and the optimal results have been obtained for the 0.1% Fe(III)-doped TiO2 [72]. For photocatalytic oxidation of nitrite to nitrate, the most photoactive sample was found to beTiO2 doped with 0.5 wt% of iron [73]. Themeso-porous nanocrystalline Fe-doped TiO2 samples prepared by ultrasonic method exhibited enhanced photocatalytic activity towards oxidation of acetone in air at a small amount of doped Fe3+ ions in TiO2 particles. The found optimal atomic ratio of Fe to Ti was 0.25 The high activities of the Fe-doped TiO2 powders could be attributed to the results of the syner-getic effects of Fe-doping, large BET specific surface area, and small crystallite size [55]. Zhang et al. [74] reported that the

films with low-iron concentrations performed better photocatalytic activity than the pure TiO2 film, and the best doped iron concentration was 0.58 at.%.

Wang et al. have reported that the formation of surface defects in Fe-doped TiO2 affects the high-photocatalytic activity of this photocatalyst [43, 75]. They reported that when the Fe content increased in Fe-doped TiO2 prepared by the sol-gel method, the isolated Fe2O3, Fe3O4, and FeO species were observed and Ti-O-Fe species were formed, which increased the surface defects ofthe Ti/Fe particles and led to the higher activity of the catalyst than bare TiO2 for the degradation of tetracycline [75]. They also reported that the concentration of titanium defects remained almost constant below 400°C but decreased as the calcination temperature was higher than 600°C due to the decrease of the hydroxyls in the crystalline structure. Below 400°C of calcination, all the samples had some brookite and a majority of anatase phase. when the temperature was 800°C , Fe2TiO5 was produced in the sample containing 5 wt% Fe by a reaction between interstitial iron ions and lattice titanium ions, and in the 10 wt% Fe sample through a reaction of hematite with titania phases. [43].

Egerton et al. have investigated that photoelectrocatalytic disinfection of Escherichia coli by an iron doped TiO2 sol-gel electrode was more efficient than disinfection by the corresponding undoped electrode. The optimum disinfection rate corresponded to the replacement of «0.1% of the Ti atoms by Fe [76].

Some researchers have been observed that doping Fe to TiO2 can be detrimental or not affect the enhancement activity of the photocatalysts [77, 78].

Fe2O3 can work as a photocatalyst and can decompose some organic compounds like aniline [79]. However, the mixture of Fe2O3 and TiO2 has been reported to be less active than original TiO2 [80,81].

3.4. Mechanisms of organic compounds decomposition by Fe-doped TiO2

Wang et al. [82] detected by cryo-TEM that Fe(III)-doped TiO2 prepared by hydrolysis of TiCl4 with Fe(III)-acetyloa-cetonate as an iron precursor forms three-dimentional networks with nanoparticles of 2-4 nm, which act as antenna systems in photocatalysis, leading to an enhanced photocat-alytic activity of the colloidal preparation. HRTEm image of such prepared particles is shown in Figure 11, and the scheme of this working system is presented in Figure 12 [82].

Once the energy has reached the particle with the adsorbed target molecule, the latter will act as a hole trap thus inducing the separation of the original excitation [82].

Arana et al. [83] have studied the photocatalytic degradation of maleic acid by using Fe-doped TiO2 (0.15, 0.5, 2, and 5% w/w in Fe) catalysts. They observed that catalysts with the lowest Fe content (0.15 and 0.5%) showed a considerably better catalytic behaviour than nondoped TiO2 and catalysts with higher Fe contents. Maleic acid molecules interacted with the surface of the lowest Fe-containing catalysts and as a consequence; iron atoms were extracted from the catalyst surface as photoactive Fe3+~ maleic acid complexes.

Figure 11: HRTEM image of 0.5 at % Fe(III)-dopedTiO2 nanopar-ticles.


Figure 12: The scheme of increased photocatalytic activity through energy/exciton transfer in aggregated photocatalyst particles (antenna effect). A and D represent electron and hole scavengers, respectively.

When this complex was degraded, the resulting Fe2+ ions reacted with TiO2 holes (h+) and the iron return to the catalyst surface as Fe2O3. In catalysts with low-Fe content (0.15 and 0.5% w/w in Fe), this process occurs in a fast way. On the contrary, in catalysts with high-Fe content (2 and 5% w/w in Fe), the formation of less photoactive complexes seems to predominate [83].

These authors have studied also the photocatalytic degradation of formic acid by Fe-doped TiO2 calcined at 773 and 1073 K [84]. For 773 K calcined catalyst, results suggested that Fe was extracted through the formation of a [Fe-OOCH]2+ complex by which formic acid degrades. Fe2+ ions that remain in solution after formic acid degradation went back to the catalyst surface and were oxidised by photogenerated holes. In this way, the catalyst was reactivated becoming ready for a new degradation process. The formation of hydrogen-carbonates on the TiO2 catalyst through OH radicals insertion was inhibited, and the formation of [Fe-OOCH]2+ complex was favoured. A markedly lower capacity for the formic acid degradation has been determined for the 1073 K calcined catalysts, because of its lower surface area and the major presence of lower-active phases such as rutile andFe2TiO5 [84].

The formation of intermediate products over the pho-tocatalytic decomposition was found to be important in the further oxidation processes.

Arana et al. [85] have proved that the mechanism of ethanol decomposition on Fe-TiO2 was gone by the formation of ethoxides on the catalyst surface that were oxidised to acetate by radicals O2'- and • OH. However, the forma-

Figure 13: Photochemical cycle of combined system iron-TiO2.

tion, an acetaldehyde as an intermediate product, caused that their catalytic activity progressively decreased over time, whereas on Pd-TiO2 and Cu-TiO2, formed ethyleneglycol caused faster degradation [85].

It has been also reported that the formation of a ternary compound HQ-Fe-H2O2 in phenol decomposition or formation of an intermediate, highly-oxidised and unstable form of Fe [Fe(IV)] in the case of chlorophenol decomposition were responsible for fast degradation of phenol and chlorophenol, respectively [86, 87].

The synergistic effect has been observed when a mixture of TiO2 and iron has been used for oxidative photodegradation of monuron (3-(4-chlorophenyl)-1,1- dimethylurea). In a suspension of TiO2 (24 mg L-1) with addition of Fe(III) (3 X 10-4 mol L-1), the measured rate constant was similar to that obtained in a suspension of TiO2 with a concentration more than 20 times higher (500mg L-1). The optimisation of the photocatalytic systems was obtained when each pho-tocatalyst plays a specific role: Fe(III) as a main OH radicals source and TiO2 as an oxidizing agent of Fe(II) to Fe(III) favouring the photocatalytic cycle Fe(III)/Fe(II). This proposed mechanism is presented in Figure 13 [88].

The following are photochemical reactions conducted to production of OH radicals:

Fe(OH)2+Fe2+ +* OH,

and the reaction occurring in the dark (Fenton reaction):

Fe2+ + H2O2 — Fe3+ + OH~. (2)

It has been already established that the formation of H2O2 is negligible in homogeneous photocatalysis with Fe(III). The reactions between iron and TiO2 appear to be essential:

Fe11 + HO; + H+

.III .

■ H2O2,

Fe11 +; OH — Fe111 + OH-

The reaction (4) is detrimental for pollutant degradation. It has been reported that Fe(III) could easily adsorb on the surface of TiO2, and Fe(II) cations were not adsorbed, therefore the reoxidation of Fe(II) by holes is unlikely. In the absence of oxygen Fe(III), cations react with the electron at the surface of TiO2, allowing the formation of the active species h+ and *OH. However, it was proved that *OH radicals are more efficiently formed via the photodissociation of Fe(OH)2+, which was found to be responsible for fast degradation of monuron [88].

Ranjit and Viswanathan [45] reported that the photocat-alytic activity of the iron-doped catalysts could be explained in terms of the heterojunction formed between the Fe/TiO2 and a-Fe2O3 phases for the sol-gel-derived catalyst.


As it was described above, carbon-coated TiO2 showed high photoactivity towards decomposition of methylene blue but the other organic compounds were poorly decomposed on these photocatalysts, therefore the preparation of carbon-coated TiO2 has been modified to obtain carbon-coated TiO2 with doped iron. For this purpose, poly(ethylene tereph-thalate) (PET) was impregnated with oxalic acid solution (FeC2O4) and then was mixed with powder TiO2 and heat treated at different temperatures, 400-800°C, under flow of Ar [89]. The obtained samples are consisted from anatase phase, contained carbon from 7.5 to 15.5 wt%, and an iron from 0.34 to 0.67 wt%, mostly in the form of Fe(II) [89]. Such prepared samples did not show the enhanced photo-catalytic activity towards phenol decomposition under UV irradiation, even though the sample prepared at 400°C exhibited high adsorption of phenol on its surface, around 30 ■ 10-5 mol/g, which was much higher than on the other samples, which showed adsorption of phenol in the range of 35-10-5 mol/g. However, high acceleration of the phenol decomposition has been observed on the sample prepared at 400°C, when 0.03mol/L, H2O2 was added to the reaction mixture; see Figure 14 [89]. This could be caused by occurring photo-Fenton reactions, in which Fe2+ is oxidised to Fe3+ with H2O2 yielding in OH radicals. Increase of OH radicals production after H2O2 addition on samples contained iron was confirmed by OH radicals measurements [89-91].

The high-decomposition rate of phenol was obtained only on the sample, which showed high adsorption of phenol, although this sample contained the lowest content of Fe(II) in comparison with the other samples. Increase of OH radicals formation on samples with iron was not proportional to the decomposition rate of phenol under UV irradiation with H2O2. It has been proved that, in case of the sample prepared at 400°C, some complexes were formed, which were responsible for fast degradation of phenol [91]. The FTIR studies indicated that hydroquinone was more likely adsorbed on Fe-C-TiO2 and could play a key role in the process of phenol decomposition, as reported by Chen and Pig-natello [86] that some hydroquinones formed in the phenol decomposition could reduce iron and accelerate in this way the rate of phenol decomposition by the formation of a ternary HQ-Fe-H2O2 complex [93]. Cycling decomposi-

Time (h)

Carbon-coated TiO2


\ Fe-modified

carbon-coated TiO2

1 2 3 4 5 6

Time (h)

Figure 14: Phenol decomposition on commercial TiO2-ST-01 and modified TiO2 by carbon and iron at 400°C, (a) under UV irradiation and (b) under UV with addition of H2O2.

tion of phenol under UV and H2O2 was performed on Fe-modified carbon-coated TiO2 photocatalyst heat treated at 400°C. For those measurements, photocatalyst was mounted on the adhesive tape and fixed to the metal grid, which was placed inside the reactor. For cycling performance, the metal grid with fixed photocatalyst each time was put to the fresh phenol solution with concentration of 2.1 ■ 10-4 mol/L; the results are presented in Figure 15.

A good performance of the phenol decomposition with cycling suggests that an iron present in the sample could follow the processes ofoxidation and reduction, being reused in Fenton reactions and photodegradation ofphenol. It is worth to add that in this case no pH adjustment was needed as it is usually applied in photo-Fenton process, and not any leaching of iron occurred.

In the further investigations on TiO2 modified by carbon and iron photocatalysts, the preparation method was changed, the powder of TiO2 was impregnated with FeC2O4

-С Сч

1 Cycle 1 Cycle 2 Cycle 3 Cycle 4 Cycle 5

: \ 1 \.

Ci = 0.0193g/L Ci = 0.0191 g/L Ci = 0.0205 g/L Ci = 0.0255 g/L Ci = 0.0223 g/L

Time (h)

Figure 15: Cycling decomposition of phenol under UV irradiation and H2O2 on Fe-modified carbon-coated TiO2 photocatalyst heat treated at 400° C.

solution and heated at 400-800°C under flow of Ar, but not any polymer was added. The obtained Fe-C-TiO2 samples contained a residue carbon, 0.2-3.3 wt%, which came from the carbonisation of oxalate [90]. A residue carbon did not prevent the transformation of anatase to rutile, which occurred at 700° C, with increasing the heat treatment temperature FeTiO3 phase (ilmenite) appeared. The highest photoac-tivity for phenol decomposition under UV and H2O2 had the sample prepared at 500°C, which contained 2.4 wt% of residue carbon, 0.70 wt% of Fe(II), 0.96 wt% of Fe(III), and did not have FeTiO3 phase. The phenol decomposition on this sample was much faster than in the case of previous experiments, in which PET was used for preparation, phenol was decomposed after 2 hours of UV irradiation, and after 3 hours of UV irradiation not any ring products of phenol decomposition were detected [90, 91].

It was proved that in case of TiO2 modified by FeC2O4 and heated at 550°C in air (Fe-TiO2), FeTiO3 phase is formed, which exhibits higher photocatalytic activity than pure TiO2 for phenol decomposition under UV irradiation, but with H2O2 addition this activity decreases, proportional to the decreasing of OH radicals formation, due to the scavenging effect:

H2O2 +; OH

Formed in this reaction, HO* radicals are known to have lower potential of oxidation than * OH [91]. This scavenging effect has been observed to occur also on TiO2. In Figure 16, formation of OH radicals on TiO2, Fe-TiO2, and Fe-C-TiO2 samples is presented [91].

In Figure 17, phenol decomposition on these samples is presented [91].

It can be observed that phenol decomposition is going through the radical reaction on TiO2 and Fe-TiO2 photocat-alysts, whereas by the surface reactions on Fe-C-TiO2.

The cycling decomposition ofphenol on Fe-C-TiO2 sample prepared at 500°C has been performed in the circulated flow reactor [94]. For this purpose, the photocatalyst has been pasted on the cotton material with a suspension of the powdered photocatalyst with aqueous solution of sodium silicate (Na2SiO3) and was placed inside the reactor on the inner walls, along the UV lamp. Circulated phenol solution was

140 120 100

¿3 60

Time of UV irradiation (h)



80 70 60 50

" 30 20 10 0

Time of UV irradiation (h)

♦ TiO2 + H2O2 ■ Fe-TiO2+H2O2

▲ Fe-C-TiO2+H2O2 • H2O2

Figure 16: Formation of OH radicals on TiO2, Fe-TiO2, and Fe-C-TiO2 prepared at 500°C, (a) under UV and (b) under UV with H2O2.

irradiated with UV for some cycles, and with UV and H2O2, as shown in Figure 18 [94].

Adsorption and following decomposition of phenol on immobilised Fe-C-TiO2 photocatalyst can be observed under UV irradiation, but under UV with addition of H2O2 acceleration of phenol decomposition is observed with stable amount of decomposed phenol, over 90% and mineralisation degree around 50% [94].

It has been proved that preparation of Fe-C-TiO2 from the other TiO2 precursor of anatase structure at the same conditions as described above gives similar results; the highest photocatalytic activity under UV irradiation with H2O2

♦ TÍO2 A Fe-C-TiO2 ■ Fe-TiO2

Time of UV irradiation (h)

234 Time of UV irradiation (h)

♦ TiO2 + H2O2 ■ Fe-TiO2 + H2O2

Fe-C-TiO2 + H2O2 H2O2

Figure 17: Phenol decomposition on TiO2, Fe-TiO2, and Fe-C-TiO2 prepared at 500°C, (a) under UV and (b) under UV with H2O2.

has the sample prepared at 500°C [95]. The high photoactiv-ity of Fe-C-TiO2 sample prepared at 500°C has been found for decomposition of phenol, humic acids, and different dyes, like acid red, methylene blue, and reactive black 5. It has been found that FeTiO3 phase is detrimental in pho-tocatalytic activity of Fe-C-TiO2 photocatalysts under UV with H2O2, and the low temperatures of preparation such as 500°C led to obtain the samples with high amount of paramagnetic iron on the surface, not built in TiO2 lattice, which probably facilitates proceeding of the photo-Fenton reactions, in which iron is oxidised and reduced with cy-

Cycle 1 .-••^-Cycle 2 yCycle 3

Cj = 0.03 g/L C¡ = 0.03 g/L Cj = 0.03 g/L

400 600

Time (m)

<b Cycle 1 Cycle 2 Cycle 3

. \ TOCN 1 tocN 1 TOO

Phenol \ Phenol\ PhenolN.

Cj = 0.03 g/L ^ Cj = 0.03 g/LN Cj = 0.03 g/LN

0 200 400 600 800

Time (m)

Figure 18: Cycling decomposition ofphenol on immobilised Fe-C-TiO2 prepared at 500°C. (a) under UV, (b) under UV with H2O2.

cling. The EPR spectra of Fe-C-TiO2 samples prepared from anatase and FeC2O4 [95] are presented in Figure 19.

In obtained EPR spectra, some peaks can be observed, in anatase type TiO2 a maximum at 344 MT, g = 1.93, which is assigned to Ti3+ ions associated to oxygen vacancies [96, 97], this peak was also observed in Fe-C-TiO2 samples and was higher intensity in samples heated at higher temperatures. Some peaks assigned to Fe3+ ions were observed: in Fe-C-TiO2 samples prepared from anatase at temperature 500 and 600°C, a broad peak with maximum at around 434 MT, g = 1.53 assigned to paramagnetic Fe3+ ions, peaks with maximum at around 330 and 310 M (g « 2) assigned to Fe3+ ions in octahedral symmetry in anatase [48, 96], and two broad peaks at the range of 133 to 272 MT assigned to Fe3+ ions substituting for Ti4+ in the TiO2 rutile lattice [96].


Modification of TiO2 by carbon can enhance its photocat-alytic activity: doped C can extend the light absorption to the visible range and give photocatalytic activity under visible light by the narrowing of the bandgap; carbon coated

500 400 300 200 100 0

-100 200 300 400

Magnetic field (mT)

Figure 19: EPR spectra of TiO2 and Fe-C-TiO2 samples prepared from anatase and Fe-C2O4 at 500-800°C.

TiO2 as well as TiO2/AC composites can enhance the concentration of the organic compounds on the surface of the photocatalyst and accelerate the process of their decomposition through the transfer of the adsorbed molecules to the TiO2 surface; TiO2 loaded carbon can also work as a photo-catalyst, on which the molecules are adsorbed in the pores of carbon and then they undergo the photocatalytic decomposition with UV irradiation.

Doping Fe(III) to TiO2 causes formation of shallow charge trapping sites within the TiO2 matrix and on the particle surface through the replacement of Ti(IV) by Fe(III). Fe(III) centres may act either as an electron or a hole trap. At high concentration of Fe(III) in Fe-doped TiO2 Fe(III), ions can act as a recombination centres. The photocatalytic activity of Fe-doped TiO2 has been found to depend strongly on the preparation method, iron precursor, and the amount and state of iron, generally insignificant amount of doped iron has a positive effect in the enhancement of the photocatalytic activity of Fe-doped TiO2, whereas amount of doped iron >2 wt% has been detrimental. It has been observed the red shift in the UV-Vis spectra of Fe-doped TiO2 photocatalysts due to the introduction of the 3d electron state of Fe3+, 3d5, in the conduction band of TiO2, what makes these photocat-alysts active under visible light.

TiO2 modified by carbon and iron can work in both pho-tocatalysis and photo-Fenton processes, when H2O2 is used, enhancing markedly the rate of the organic compounds decomposition. The photocatalytic decomposition of organic compounds on TiO2 modified by iron and carbon is going by the complex reactions of iron with the intermediates, what significantly accelerate the process of their decomposition. A good performance of cycling decomposition of phenol has been obtained on immobilised Fe-C-TiO2 photocat-alyst, what suggests that an iron present in the sample could follow the processes of oxidation and reduction, being reused in Fenton reactions and photodegradation of phenol. The additional advantage of using this photocatalyst for the decomposition of organic compounds is the fact that no pH adjustment is needed, and it was observed that there was not any leaching of iron from this photocatalyst.


This work was supported by the research Project no.

1T09D00730 for 2006-2009.


[1] S. U. M. Khan, M. Al-Shahry, and W. B. Ingler, "Efficient photochemical water splitting by a chemically modified n-TiO2," Science, vol. 297, no. 5590, pp. 2243-2245, 2002.

[2] S. Sakthivel and H. Kisch, "Daylight photocatalysis by carbon-modified titanium dioxide," Angewandte Chemie International Edition, vol. 42, no. 40, pp. 4908-4911, 2003.

[3] C. Lettmann, K. Hildenbrand, H. Kisch, W. Macyk, and W. F. Maier, "Visible light photodegradation of 4-chlorophenol with a coke-containing titanium dioxide photocatalyst," Applied Catalysis B, vol. 32, no. 4, pp. 215-227, 2001.

[4] M. Shen, Z. Wu, H. Huang, Y. Du, Z. Zou, and P. Yang, "Carbon-doped anatase TiO2 obtained from TiC for pho-tocatalysis under visible light irradiation," Materials Letters, vol. 60, no. 5, pp. 693-697, 2006.

[5] H. Irie, Y. Watanabe, and K. Hashimoto, "Carbon-doped anatase TiO2 powders as a visible-light sensitive photocata-lyst," Chemistry Letters, vol. 32, no. 8, pp. 772-773, 2003.

[6] J. Matos, J. Laine, and J.-M. Herrmann, "Effect of the type of activated carbons on the photocatalytic degradation of aqueous organic pollutants by UV-irradiated titania," Journal of Catalysis, vol. 200, no. 1, pp. 10-20, 2001.

[7] K. M. Reddy, B. Baruwati, M. Jayalakshmi, M. M. Rao, and S. V. Manorama, "S-, N- and C-doped titanium dioxide nanoparticles: synthesis, characterization and redox charge transfer study," Journal of Solid State Chemistry, vol. 178, no. 11, pp. 3352-3358, 2005.

[8] T. Tachikawa, S. Tojo, K. Kawai, et al., "Photocatalytic oxidation reactivity of holes in the sulfur- and carbon-doped TiO2 powders studied by time-resolved diffuse reflectance spectroscopy," Journal of Physical Chemistry B, vol. 108, no. 50, pp. 19299-19306, 2004.

[9] Y. Choi, T. Umebayashi, and M. Yoshikawa, "Fabrication and characterization of C-doped anatase TiO2 photocatalysts," Journal of Materials Science, vol. 39, no. 5, pp. 1837-1839, 2004.

[10] C. Di Valentin, G. Pacchioni, and A. Selloni, "Theory of carbon doping of titanium dioxide," Chemistry of Materials, vol. 17, no. 26, pp. 6656-6665, 2005.

[11] M. Janus, B. Tryba, M. Inagaki, and A. W. Morawski, "New preparation of a carbon-TiO2 photocatalyst by carbonization of и-hexane deposited on TiO2," Applied Catalysis B, vol. 52, no. 1, pp. 61-67, 2004.

[12] M. Janus, M. Inagaki, B. Tryba, M. Toyoda, and A. W. Morawski, "Carbon-modified TiO2 photocatalyst by ethanol carbonisation," Applied Catalysis B, vol. 63, no. 3-4, pp. 272276, 2006.

[13] M. Janus, M. Toyoda, M. Inagaki, B. Tryba, and A. W. Morawski, "Preparation of TiO2/C photocatalyst by ethanol modification of hydrolysed titania TiO(OH)2 in a pressure reactor," Journal of Advanced Oxidation Technologies, vol. 10, no. 2, pp. 1-7, 2007.

[14] T. A. Egerton, M. Janus, and A. W. Morawski, "New TiO2/C sol-gel electrodes for photoelectrocatalytic degradation of sodium oxalate," Chemosphere, vol. 63, no. 7, pp. 1203-1208, 2006.

[15] H. Wang and J. P. Lewis, "Effects of dopant states on pho-toactivity in carbon-doped TiO2," Journal of Physics Condensed Matter, vol. 17, no. 21, pp. L209-L213, 2005.

[16] J. H. Park, S. Kim, and A. J. Bard, "Novel carbon-doped TiO2 nanotube arrays with high aspect ratios for efficient solar water splitting," Nano Letters, vol. 6, no. 1, pp. 24-28, 2006.

[17] J. Matos, J. Laine, and J-M. Herrmann, "Association of activated carbons of different origins with titania in the photocat-alytic purification of water," Carbon, vol. 37, no. 11, pp. 18701872, 1999.

[18] J. Araña, J. M. Dona-Rodríguez, E. Tello Rendon, et al., "TiO2 activation by using activated carbon as a support—part I. Surface characterisation and decantability study," Applied Catalysis B, vol. 44, no. 2, pp. 161-172, 2003.

[19] J. Araña, J. M. Dona-Rodríguez, E. Tello Rendon, et al., "TiO2 activation by using activated carbon as a support—part II. Photoreactivity and FTIR study," Applied Catalysis B, vol. 44, no. 2, pp. 153-160, 2003.

[20] S. X. Liu, X. Y. Chen, and X. Chen, "A TiO2/AC composite photocatalyst with high activity and easy separation prepared by a hydrothermal method," Journal of Hazardous Materials, vol. 143, no. 1-2, pp. 257-263, 2007.

[21] S. Nagaoka, Y. Hamasaki, S.-I. Ishihara, et al., "Preparation of carbon/TiO2 microsphere composites from cellulose/TiO2 mi-crosphere composites and their evaluation," Journal of Molecular Catalysis A, vol. 177, no. 2, pp. 255-263, 2002.

[22] T. Tsumura, N. Kojitani, I. Izumi, N. Iwashita, M. Toyoda, and M. Inagaki, "Carbon coating of anatase-type TiO2 and pho-toactivity," Journal of Materials Chemistry, vol. 12, no. 5, pp. 1391-1396, 2002.

[23] B. Tryba, A. W. Morawski, T. Tsumura, M. Toyoda, and M. Inagaki, "Hybridization of adsorptivity with photocatalytic activity—carbon-coated anatase," Journal of Photochemistry and Photobiology A, vol. 167, no. 2-3, pp. 127-135, 2004.

[24] M. Inagaki, F. Kojin, B. Tryba, and M. Toyoda, "Carbon-coated anatase: the role of the carbon layer for photocatalytic performance," Carbon, vol. 43, no. 8, pp. 1652-1659, 2005.

[25] L. Lin, W. Lin, Y. X. Zhu, et al., "Uniform carbon-covered titania and its photocatalytic property," Journal of Molecular Catalysis A, vol. 236, no. 1-2, pp. 46-53, 2005.

[26] X. Zhang, M. Zhou, and L. Lei, "Preparation of photocatalytic TiO2 coatings of nanosized particles on activated carbon by AP-MOCVD," Carbon, vol. 43, no. 8, pp. 1700-1708, 2005.

[27] Y. Li, X. Li, J. Li, and J. Yin, "Photocatalytic degradation of methyl orange by TiO2-coated activated carbon and kinetic study," Water Research, vol. 40, no. 6, pp. 1119-1126, 2006.

[28] M. Toyoda, Y. Nanbu, T. Kito, M. Hirano, and M. Inagaki, "Preparation and performance of anatase-loaded porous carbons for water purification," Desalination, vol. 159, no. 3, pp. 273-282, 2003.

[29] B. Tryba, A. W. Morawski, and M. Inagaki, "Application of TiO2-mounted activated carbon to the removal of phenol from water," Applied Catalysis B, vol. 41, no. 4, pp. 427-433, 2003.

[30] T. Torimoto, Y. Okawa, N. Takeda, and H. Yoneyama, "Effect of activated carbon content in TiO2-loaded activated carbon on photodegradation behaviors of dichloromethane," Journal of Photochemistry and Photobiology A, vol. 103, no. 1-2, pp. 153-157, 1997.

[31] B. Tryba, A. W. Morawski, M. Toyoda, and M. Inagaki, "TiO2-mounted activated carbon for the elimination of organic pollutants in water," Water Research, vol. 4, pp. 35-42, 2003.

[32] Z. Ding, X. Hu, P. L. Yue, G. Q. Lu, and P. F. Greenfield, "Synthesis of anatase TiO2 supported on porous solids by chemical vapor deposition," Catalysis Today, vol. 68, no. 1-3, pp. 173182, 2001.

[33] C. H. Ao and S. C. Lee, "Enhancement effect of TiO2 immobilized on activated carbon filter for the photodegradation of pollutants at typical indoor air level," Applied Catalysis B, vol. 44, no. 3, pp. 191-205, 2003.

[34] A. H. El-Sheikh, A. P. Newman, H. Al-Daffaee, S. Phull, N. Cresswell, and S. York, "Deposition of anatase on the surface of activated carbon," Surface and Coatings Technology, vol. 187, no. 2-3, pp. 284-292, 2004.

[35] D.-K. Lee, S.-C. Kim, I.-C. Cho, S.-J. Kim, and S.-W. Kim, "Photocatalytic oxidation of microcystin-LR in a fluidized bed reactor having TiO2-coated activated carbon," Separation and Purification Technology, vol. 34, no. 1-3, pp. 59-66, 2004.

[36] R. Yuan, J. Zheng, R. Guan, and Y. Zhao, "Surface characteristics and photocatalytic activity of TiO2 loaded on activated carbon fibers," Colloids and Surfaces A: Physicochemical and Engineering Aspects, vol. 254, no. 1-3, pp. 131-136, 2005.

[37] A. Jitianu, T. Cacciaguerra, R. Benoit, S. Delpeux, F. Beguin, and S. Bonnamy, "Synthesis and characterization of carbon nanotubes-TiO2 nanocomposites," Carbon, vol. 42, no. 5-6, pp. 1147-1151,2004.

[38] T. Tsumura, N. Kojitani, H. Umemura, M. Toyoda, and M. Inagaki, "Composites between photoactive anatase-type TiO2 and adsorptive carbon," Applied Surface Science, vol. 196, no. 1-4, pp. 429-436, 2002.

[39] H. Yamashita, M. Harada, A. Tanii, J. Misaka, H. Nakao, and M. Anpo, "Design of TiO2/activated carbon fiber systems by an ionized cluster beam method and their application for the photocatalytic water purification," Molecular Crystals and Liquid Crystals, vol. 388, no. 1, pp. 39-44, 2002.

[40] C. Wang, C. Bottcher, D. W. Bahnemann, and J. K. Dohrmann, "A comparative study of nanometer sized fe(III)-doped TiO2 photocatalysts: synthesis, characterization and activity," Journal ofMaterials Chemistry, vol. 13, pp. 2322-2329, 2003.

[41] J. A. Navio, G. Colon, M. Macias, C. Real, and M. I. Litter, "Iron-doped titania semiconductor powders prepared by a sol-gel method—part I: synthesis and characterization," Applied Catalysis A, vol. 177, no. 1, pp. 111-120, 1999.

[42] J. A. Navio, J. J. Testa, P. Djedjeian, J. R. Padron, D. Rodriguez, and M. I. Litter, "Iron-doped titania powders prepared by a sol-gel method—part II: photocatalytic properties," Applied Catalysis A, vol. 178, no. 2, pp. 191-203, 1999.

[43] J. A. Wang, R. Limas-Ballesteros, T. Lopez, et al., "Quantitative determination of titanium lattice defects and solid-state reaction mechanism in iron-doped TiO2 photocatalysts," Journal of Physical Chemistry B, vol. 105, no. 40, pp. 9692-9698, 2001.

[44] W.-C. Hung, S.-H. Fu, J.-J. Tseng, H. Chu, and T.-H. Ko, "Study on photocatalytic degradation of gaseous dichloromethane using pure and iron ion-doped TiO2 prepared by the sol-gel method," Chemosphere, vol. 66, no. 11, pp. 2142-2151, 2007.

[45] K. T. Ranjit and B. Viswanathan, "Synthesis, characterization and photocatalytic properties of iron-doped TiO2 catalysts," Journal of Photochemistry and Photobiology A, vol. 108, no. 1, pp. 79-84, 1997.

[46] M. Shui, L.-H. Yue, and Z.-D. Xu, "Photocatalytic activity of iron doping TiO2 prepared by several methods," Acta Physico-Chimica Sinica, vol. 17, no. 3, p. 285, 2001.

[47] X.-Q. Chen, J.-Y. Yang, and J.-S. Zhang, "Preparation and photocatalytic properties of Fe-doped TiO2 nanoparticles," Journal of Central South University of Technology, vol. 11, no. 2, pp. 161-165, 2004.

[48] C. Adán, A. Bahamonde, M. Fernández-García, and A. Martinez-Arias, "Structure and activity of nanosized iron-doped anatase TiO2 catalysts for phenol photocatalytic degradation," Applied Catalysis B, vol. 72, no. 1-2, pp. 11-17, 2007.

[49] M. S. Nahar, K. Hasegawa, and S. Kagaya, "Photocatalytic degradation of phenol by visible light-responsive iron-doped TiO2 and spontaneous sedimentation of the TiO2 particles," Chemosphere, vol. 65, no. 11, pp. 1976-1982, 2006.

[50] M. S. Nahar, K. Hasegawa, S. Kagaya, and S. Kuroda, "Comparative assessment of the efficiency of Fe-doped TiO2 prepared by two doping methods and photocatalytic degradation of phenol in domestic water suspensions," Science and Technology of Advanced Materials, vol. 8, no. 4, pp. 286-291, 2007.

[51] N. Uekawa, Y. Kurashima, K. Kakegawa, and Y. Sasaki, "Preparation and nonstoichiometric property of wide compositional Fe(III)-doped TiO2 (anatase)," Journal of Materials Research, vol. 15, no. 4, pp. 967-973, 2000.

[52] X. H. Wang, J.-G. Li, H. Kamiyama, Y. Moriyoshi, and T. Ishigaki, "Wavelength-sensitive photocatalytic degradation of methyl orange in aqueous suspension over iron(III)-doped TiO2 nanopowders under UV and visible light irradiation," Journal of Physical Chemistry B, vol. 110, no. 13, pp. 68046809, 2006.

[53] W. Y. Teoh, R. Amal, L. Madler, and S. E. Pratsinis, "Flame sprayed visible light-active Fe-TiO2 for photomineralisation of oxalic acid," Catalysis Today, vol. 120, no. 2, pp. 203-213,2007.

[54] J. A. Navio, G. Colon, M. I. Litter, andG. N. Bianco, "Synthesis, characterization and photocatalytic properties of iron-doped titania semiconductors prepared from TiO2 and iron (III) acetylacetonate," Journal of Molecular Catalysis A, vol. 106, no. 3, pp. 267-276, 1996.

[55] M. Zhou, J. Yu, and B. Cheng, "Effects of Fe-doping on the photocatalytic activity of mesoporous TiO2 powders prepared by an ultrasonic method," Journal of Hazardous Materials, vol. 137, no. 3, pp. 1838-1847, 2006.

[56] C. H. Lee, S. H. Lee, S. J. Lee, J. S. Kim, and Y. S. Kwon, "Fabrication of Fe-TiO2 nano-composite powders by mechanical alloying," Journal of Ceramic Processing Research, vol. 4, no. 3, pp. 122-125, 2003.

[57] K. S. Yao, D. Y. Wang, J. J. Yan, L. Y. Yang, and W. S. Chen, "Photocatalytic effects of TiO2/Fe thin film irradiated with visible light on cellular surface ultrastructure and genomic DNA of bacteria," Surface and Coatings Technology, vol. 201, no. 15, pp. 6882-6885, 2007.

[58] H. Yamashita, M. Harada, J. Misaka, M. Takeuchi, B. Nep-polian, and M. Anpo, "Photocatalytic degradation of organic compounds diluted in water using visible light-responsive metal ion-implanted TiO2 catalysts: Fe ion-implanted TiO2," Catalysis Today, vol. 84, no. 3-4, pp. 191-196, 2003.

[59] J. O. Carneiro, V. Teixeira, A. Portinha, et al., "Iron-doped photocatalytic TiO2 sputtered coatings on plastics for self-cleaning applications," Materials Science and Engineering B, vol. 138, no. 2, pp. 144-150, 2007.

[60] H.-C. Huang, G.-L. Huang, H.-L. Chen, and Y.-D. Lee, "Immobilization of TiO2 nanoparticles on Fe-filled carbon nanocapsules for photocatalytic applications," Thin Solid Films, vol. 515, no. 3, pp. 1033-1037, 2006.

[61] X.-C. Song, L.-H. Yue, B. Liu, G. Han, W.-X. Chen, and Z.-D. Xu, "Preparation of Fe-doped TiO2 nanotubes with small di-

ameter by hydrothermal method," Chinese Journal of Inorganic Chemistry, vol. 19, no. 8, pp. 899-901, 2003.

[62] C. Wang, Q. Li, and R. Wang, "Synthesis and characterization of mesoporous iron-doped TiO2," Journal of Materials Science, vol. 39, no. 5, pp. 1899-1901, 2004.

[63] D. H. Kim, H. S. Hong, S. J. Kim, J. S. Song, and K. S. Lee, "Photocatalytic behaviors and structural characterization of nanocrystalline Fe-doped TiO2 synthesized by mechanical alloying," Journal of Alloys and Compounds, vol. 375, no. 1-2, pp. 259-264, 2004.

[64] R. S. Sonawane, B. B. Kale, and M. K. Dongare, "Preparation and photo-catalytic activity of Fe-TiO2 thin films prepared by sol-gel dip coating," Materials Chemistry and Physics, vol. 85, no. 1,pp. 52-57, 2004.

[65] M. Kang, "Synthesis of Fe/TiO2 photocatalyst with nanometer size by solvothermal method and the effect of H2O addition on structural stability and photodecomposition of methanol," Journal of Molecular Catalysis A, vol. 197, no. 1-2, pp. 173-183, 2003.

[66] J.-Y. Chen and T.-Z. Peng, "Preparation and properties of a magnetic-nanometer TiO2/Fe3O4 composite photocatalyst," Acta Chimica Sinica, vol. 62, no. 20, pp. 2093-2097, 2004.

[67] H. Jiang and L. Gao, "Enhancing the UV inducing hy-drophilicity of TiO2 thin film by doping Fe ions," Materials Chemistry and Physics, vol. 77, no. 3, pp. 878-881, 2003.

[68] K. S. Yao, D. Y. Wang, J. J. Yan, L. Y. Yang, and W. S. Chen, "Photocatalytic effects ofTiO2/Fe thin film irradiated with visible light on cellular surface ultrastructure and genomic DNA of bacteria," Surface and Coatings Technology, vol. 201, no. 15, pp. 6882-6885, 2007.

[69] M.I. Litter and J. A. Navio, "Photocatalytic properties of iron-doped titania semiconductors," Journal of Photochemistry and Photobiology A, vol. 98, no. 3, pp. 171-181, 1996.

[70] X.-H. Qi, Z.-H. Wang, Y.-Y. Zhuang, Y. Yu, and J.-L. Li, "Study on the photocatalysis performance and degradation kinetics of X-3B over modified titanium dioxide," Journal of Hazardous Materials, vol. 118, no. 1-3, pp. 219-225, 2005.

[71] J. Feng, R. S. K. Wong, X. Hu, and P. L. Yue, "Discoloration and mineralization of Orange II by using Fe3+-doped TiO2 and bentonite clay-based Fe nanocatalysts," Catalysis Today, vol. 98, no. 3, pp. 441-446, 2004.

[72] P.-F. Yan, D.-R. Zhou, J.-Q. Wang, L.-B. Yang, D. Zhang, and H.-G. Fu, "Preparation ofiron-dopedTiO2 nanocrystal by hydrothermal method and its photocatalytic properties," Chemical Journal of Chinese Universities, vol. 23, no. 12, p. 2321,2002.

[73] A. Milis, J. Peral, X. Domenech, and J. A. Navio, "Heterogeneous photocatalytic oxidation of nitrite over iron-doped TiO2 samples," Journal of Molecular Catalysis, vol. 87, no. 1, pp. 67-74, 1994.

[74] W. Zhang, Y. Li, S. Zhu, and F. Wang, "Surface modification of TiO2 film by iron doping using reactive magnetron sputtering," Chemical Physics Letters, vol. 373, no. 3-4, pp. 333-337, 2003.

[75] X.-B. Yu, G.-H. Wang, and H.-X. Li, "The promoting effect on the activities of Fe doped TiO2 photocatalysts," Chemical Research in Chinese Universities, vol. 17, no. 2, pp. 187-192, 2001.

[76] T. A. Egerton, S. A. M. Kosa, and P. A. Christensen, "Pho-toelectrocatalytic disinfection of E. coli suspensions by iron doped TiO2," Physical Chemistry Chemical Physics, vol. 8, no. 3, pp. 398-406, 2006.

[77] L. Palmisano, M. Schiavello, A. Sclafani, C. Martin, I. Martin, and V. Rives, "Surface properties of iron-titania pho-tocatalysts employed for 4-nitrophenol photodegradation in

aqueous TiO2 dispersion," Catalysis Letters, vol. 24, no. 3-4, pp. 303-315, 1994.

[78] E. Piera, M. I. Tejedor-Tejedor, M. E. Zorn, and M. A. Anderson, "Relationship concerning the nature and concentration of Fe(III) species on the surface of TiO2 particles and photo-catalytic activity of the catalyst," Applied Catalysis B, vol. 46, no. 4, pp. 671-685, 2003.

[79] C. Karunakaran and S. Senthilvelan, "Fe2O3-photocatalysis with sunlight and UV light: oxidation of aniline," Electrochemistry Communications, vol. 8, no. 1, pp. 95-101, 2006.

[80] M. Sadeghi, W. Liu, T.-G. Zhang, P. Stavropoulos, and B. Levy, "Role of photoinduced charge carrier separation distance in heterogeneous photocatalysis: oxidative degradation of CH3OH vapor in contact with Pt/TiO2 and cofumed TiO2-Fe2O3," Journal of Physical Chemistry, vol. 100, no. 50, pp. 19466-19474, 1996.

[81] J. C. Crittenden, J. Liu, D. W. Hand, and D. L. Perram, "Photo-catalytic oxidation of chlorinated hydrocarbons in water," Water Research, vol. 31, no. 3, pp. 429-438, 1997.

[82] C. Wang, C. Bottcher, D. Bahnemann, and J. Dohrmann, "In situ electron microscopy investigation of Fe(III)-doped TiO2 nanoparticles in an aqueous environment," Journal of Nanoparticle Research, vol. 6, no. 1, pp. 119-122, 2004.

[83] J. Arana, O. González Díaz, M. Miranda Saracho, J. M. Doa Rodríguez, J. A. Herrera Melián, and J. Perez Peña, "Maleic acid photocatalytic degradation using Fe-TiO2 catalysts. Dependence of the degradation mechanism on the Fe catalysts content," Applied Catalysis B, vol. 36, no. 2, pp. 113-124, 2002.

[84] J. Arana, O. González Díaz, M. Miranda Saracho, J. M. Doa Rodríguez, J. A. Herrera Melián, and J. Perez Pena, "Photocatalytic degradation of formic acid using Fe/TiO2 catalysts: the role of Fe3+/Fe2+ ions in the degradation mechanism," Applied Catalysis B, vol. 32, no. 1-2, pp. 49-61, 2001.

[85] J. Araña, J. M. Doa Rodríguez, O. González Díaz, et al., "Gasphase ethanol photocatalytic degradation study with TiO2 doped with Fe, Pd and Cu," Journal of Molecular Catalysis A, vol. 215, no. 1-2, pp. 153-160, 2004.

[86] R. Chen and J. J. Pignatello, "Role of quinone intermediates as electron shuttles in fenton and photoassisted fenton oxidations of aromatic compounds," Environmental Science and Technology, vol. 31, no. 8, pp. 2399-2406, 1997.

[87] M. Pera-Titus, V. García-Molina, M. A. Banos, J. Giménez, and S. Esplugas, "Degradation of chlorophenols by means of advanced oxidation processes: a general review," Applied Catalysis B, vol. 47, no. 4, pp. 219-256, 2004.

[88] H. Mest'ánková, G. Mailhot, J. Jirkovy, J. Krysa, and M. Bolte, "Mechanistic approach of the combined (iron-TiO2) photo-catalytic system for the degradation of pollutants in aqueous solution: an attempt of rationalisation," Applied Catalysis B, vol. 57, no. 4, pp. 257-265, 2005.

[89] B. Tryba, M. Toyoda, A. W. Morawski, and M. Inagaki, "Modification of carbon-coated TiO2 by iron to increase adsorptivity and photoactivity for phenol," Chemosphere, vol. 60, no. 4, pp. 477-484, 2005.

[90] B. Tryba, A. W. Morawski, M. Inagaki, and M. Toyoda, "Effect of the carbon coating in Fe-C-TiO2 photocatalyst on phenol decomposition under UV irradiation via photo-Fenton process," Chemosphere, vol. 64, no. 7, pp. 1225-1232, 2006.

[91] B. Tryba, A. W. Morawski, M. Inagaki, and M. Toyoda, "The kinetics of phenol decomposition under UV irradiation with and without H2O2 on TiO2, Fe-TiO2 and Fe-C-TiO2 photocat-alysts," Applied Catalysis B, vol. 63, no. 3-4, pp. 215-221, 2006.

[92] B. Tryba, A. W. Morawski, M. Inagaki, and M. Toyoda, "Mechanism of phenol decomposition on Fe-C-TiO2 and Fe-TiO2 photocatalysts via photo-Fenton process," Journal of Photochemistry and Photobiology A, vol. 179, no. 1-2, pp. 224-228, 2006.

[93] B. Tryba, M. Inagaki, M. Toyoda, and A. W. Morawski, "FTIR studies of the surface of TiO2, Fe-TiO2 and Fe-C-TiO2 photocatalysts in phenol oxidation via the photo-fenton process," Journal of Advanced Oxidation Technologies, vol. 10, no. 1, pp. 25-30, 2007.

[94] B. Tryba, "Immobilization of TiO2 and Fe-C-TiO2 photocatalysts on the cotton material for application in a flow photocatalytic reactor for decomposition of phenol in water", Journal of Hazardous Materials, vol. 151, no. 2-3, pp. 623-627, 2008.

[95] B. Tryba, "Effect of TiO2 precursor on the photoactivity of Fe-C-TiO2 photocatalysts for Acid Red (AR) decomposition", Journal of Advanced Oxidation Technologies, vol. 10, no. 2, pp. 267-272, 2007.

[96] J. Soria, J. C. Conesa, V. Augugliaro, L. Palmisano, M. Schi-avello, and A. Sclafani, "Dinitrogen photoreduction to ammonia over titanium dioxide powders doped with ferric ions," Journal of Physical Chemistry, vol. 95, no. 1, pp. 274-282, 1991.

[97] T. Berger, M. Sterrer, O. Diwald, et al., "Light-induced charge separation in anatase TiO2 particles," Journal of Physical Chemistry, vol. 109, no. 13, pp. 6061-6068, 2005.

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