# Light-Driven Preparation, Microstructure, and Visible-Light Photocatalytic Property of Porous Carbon-Doped TiO2

Authors: Xiao-Xin Zou; Guo-Dong Li; Jun Zhao; Juan Su; Xiao Wei; Kai-Xue Wang; Yu-Ning Wang; Jie-Sheng Chen
Journal: International Journal of Photoenergy
 (2012)

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## Abstract

Highly porous carbon-doped TiO2 (C-TiO2) has been prepared, for the first time, through a light-driven approach using crystalline titanium glycolate (TG) as the single-source precursor. Although the nonthermally prepared porous C-TiO2 is amorphous, it shows a remarkable visible-light photocatalytic activity higher than that of nitrogen-doped TiO2 (N-TiO2) due to its significant surface area (530 m2/g) and pore-rich structure. X-ray photoelectron, electron paramagnetic resonance, and UV-Vis diffuse reflectance spectroscopy reveal that the as-prepared porous C-TiO2 photocatalyst contains Ti–O–C bonds which result in visible-light absorption of the material at wavelengths less than 550 nm. Furthermore, it is discovered that the Ti–O–C bonds in the as-prepared C-TiO2 is easily transformed to coke-type species under mild thermal treatment (200°C). The resulting coke-containing porous TiO2 is an even better visible-light photocatalyst, almost twice as effective as N-TiO2, because of its stronger visible-light absorption. The Ti–O–C and the coke-containing porous TiO2 materials follow two different mechanisms in the visible-light photocatalysis process for degradation of methylene blue.


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## Body

## 1. Introduction

The elimination of hazardous organic pollutants from the environment has become a major and perennial issue. Heterogeneous photocatalysis proves to be a green and efficient approach to photodecompose organic pollutants by solar energy [1]. For this application, typical photocatalysts commonly used are semiconductor metal oxides and sulfides such as TiO2, ZnO, CdS, and ZnS, among which titanium dioxide is regarded as the most promising material due to its chemical stability, nontoxicity, and low cost [2]. However, the widespread use of TiO2 is limited by its wide bandgap energy, which causes the catalyst to exploit only a very small proportion (about 3~5%) of solar radiation. Therefore, it is highly desired to develop strategies of shifting the photo-responsive range of TiO2 to visible spectral region. One of the most efficient strategies is to dope the TiO2 compound with nonmetals. Since the pioneering work reported by Asahi on nitrogen-doped TiO2 (N-TiO2) [3], nonmetal-doped TiO2 has attracted a great deal of attention [4–9], for the nonmetal doping can lead to formation of intragap localized states or bandgap narrowing, improving the visible-light photocatalytic activity of the material considerably. In particular, carbon-doped TiO2 (C-TiO2) turns out to be remarkably effective under visible-light irradiation [10–21], and there has been report that C-TiO2 is even superior to N-TiO2 in visible-light photocatalysis [21].Introduction of porous structures, which increases the surface area of the photocatalyst to a great extent, is believed to be an effective approach to further enhance the photocatalytic performance of C-TiO2. The large surface area in combination with the porous feature can facilitate the diffusion and adsorption of reactant molecules [22, 23], offer more surface-active sites [24, 25], and enhance light-harvesting [24, 25]. Moreover, the transfer path of photogenerated charges from bulk to surface can be shortened, and as a result, the recombination of the photogenerated charges is greatly suppressed [25].To our knowledge, only a few reports have demonstrated the preparation of porous C-TiO2 visible-light photocatalysts [26–31], and the carbon-doping was usually accomplished through calcination or hydrothermal treatment using organic species as the carbon sources. In this paper, we report a facile light-driven preparation route [32] that leads to the successful formation of highly porous C-TiO2 material without any thermal treatment, using crystalline titanium glycolate (TG) as the single-source precursor. The as-prepared porous C-TiO2 containing only Ti–O–C bonds exhibits distinct visible-light photocatalytic activity. In view of the amorphous feature of the as-prepared C-TiO2, the superior photocatalytic activity can be attributed to the C-doping in combination with the large surface area (530 m2/g) of the solid, which is unprecedented among the C-TiO2 photocatalytic materials reported so far. Furthermore, it is found that the carbon in Ti–O–C bonds in the as-prepared porous C-TiO2 is transformed to coke species after mild thermal treatment, and the resulting coke-containing porous TiO2 shows visible-light photocatalytic performance, even superior over the as-prepared C-TiO2. The photocatalysis processes for the Ti–O–C and the coke-containing porous TiO2 materials follow two different mechanisms.


## 2. Experimental

### 2.1. Materials

Absolute ethanol, ethylene glycol, titanium sulfate, urea, methylene blue (MB), and aqueous ammonia were purchased from Beijing Chemical Factory. All the reagents were of analytical grade and used as received. Titaniumn-butoxide was purchased from Tianjin Guangfu Fine Chemical Research Institute. Deionized water was used throughout.


### 2.2. Synthesis of Titanium Glycolate (TG)

The TG precursor was prepared on a large scale according to the reported procedure with minor modifications [33]. Typically, titanium n-butoxide (15 mL) was added to ethylene glycol (150 mL) and heated at 180°C for 2 hours under vigorous stirring to form the TG compound. After cooling down to room temperature, the white TG precipitate was washed several times with ethanol and dried in an oven at 60°C.


### 2.3. Light-Driven Preparation of Porous C-TiO2

The TG precursor (4.0 g) was dispersed in water (400 mL) and then exposed to the UV-light irradiation for 2 h. After the irradiation, the color of the solid sample turned from white (TG) to intense blue because of the presence of Ti3+ [32]. Finally, the blue solid product was separated from the mixture and dried in air, the O2 molecules of which oxidize the Ti3+ to Ti4+. The obtained light yellow TiO2 product, designated C-TiO2(UV), was amorphous and porous on the basis of X-ray diffraction and adsorption measurement. The elemental analysis indicated that the content of carbon in the material was 1.08 wt%. The UV-light source used in the experiment was a 400 W high-pressure mercury lamp (main output at 313 nm).


### 2.4. Control Experiments

The as-prepared porous C-TiO2(UV) was heated at 200°C and 500°C in air for 2 h, respectively, and the corresponding products were designated C-TiO2(200) and TiO2(500). The brown sample C-TiO2(200) contained 0.86 wt% carbon, and the white sample TiO2(500) was carbon-free on the basis of elemental analysis. The N-TiO2 containing 2.3 wt% nitrogen was prepared through a previously reported method using urea as the nitrogen source [34], and more characterization results about this sample are provided (see XRD in Figure S1, UV-Vis in Figure S2, and XPS in Figure S3 in Supplementary Material available online at doi:10.1155/2012/720183).


### 2.5. Photocatalytic Activity

The photocatalytic activity was assessed in aqueous solution in a water-cooled quartz cylindrical cell. Generally, the reaction mixture in the cell was maintained at about 20°C by a continuous flow of water, and was illuminated with an external light source. The visible-light source was a 500 W Xe lamp (main output > 400 nm), with a glass optical filter used to cut off the short wavelength part (λ < 420 nm).The as-prepared C-TiO2(UV) photocatalyst (0.3 g) was mixed with an aqueous solution of methylene blue (MB) (300 mL, 1 × 10−5mol/L). The aqueous system was magnetically stirred in dark for at least 2 h to establish an adsorption/desorption equilibrium of MB on the particle surface of the material and then subjected to visible-light irradiation. Each reaction cycle lasted for about 4 h during which oxygen was bubbled through the solution. At given irradiation time intervals, a series of aqueous solution samples (3 mL) were collected and separated from the suspended catalyst particles for analysis. The concentration of the MB was determined on a UV-Vis spectrophotometer by monitoring its characteristic absorption at 665 nm. For comparison, the photocatalytic activities of C-TiO2(200), TiO2(500), and N-TiO2 were also measured under the same condition. The weights of all the catalyst samples were identical (0.3 g). Considering that MB can absorb visible light above 600 nm, a cutoff filter (λ > 600 nm) was used to ensure that only MB was excited, and as a result, there was no significant change in the MB concentration after 4 h irradiation even in the presence of C-TiO2(UV) or C-TiO2(200).


### 2.6. General Characterization

The powder X-ray diffraction (XRD) patterns were recorded on a Rigaku D/Max 2550 X-ray diffractometer with Cu Kα radiation (λ = 1.5418 Å) whereas the TEM images were obtained on a JEOL JSM-3010 TEM microscope. The UV-Vis diffuse reflectance spectra were recorded on a Perkin-Elmer Lambda 20 UV/Vis spectrometer, and the absorbance spectra were obtained from the reflectance spectra by means of Kubelka-Munk transformation. The IR spectra were acquired on a Bruker IFS 66 v/S FTIR spectrometer. The carbon contents of the obtained samples were determined through elemental analysis on a Perkin-Elmer 2400 elemental analyzer. The IR spectra were acquired on a Bruker IFS 66 v/S FTIR spectrometer whereas the X-ray photoelectron spectra (XPS) were recorded on a VG ESCALAB MK II electron spectrometer. The nitrogen adsorption and desorption isotherms were measured using a Micromeritics ASAP 2020 M system. The electron paramagnetic resonance (EPR) spectra were recorded on a JEOL JES-FA 200 EPR spectrometer. The concentration of MB was analyzed with a Shimadzu UV-2450 spectrophotometer.


## 2.1. Materials

Absolute ethanol, ethylene glycol, titanium sulfate, urea, methylene blue (MB), and aqueous ammonia were purchased from Beijing Chemical Factory. All the reagents were of analytical grade and used as received. Titaniumn-butoxide was purchased from Tianjin Guangfu Fine Chemical Research Institute. Deionized water was used throughout.


## 2.2. Synthesis of Titanium Glycolate (TG)

The TG precursor was prepared on a large scale according to the reported procedure with minor modifications [33]. Typically, titanium n-butoxide (15 mL) was added to ethylene glycol (150 mL) and heated at 180°C for 2 hours under vigorous stirring to form the TG compound. After cooling down to room temperature, the white TG precipitate was washed several times with ethanol and dried in an oven at 60°C.


## 2.3. Light-Driven Preparation of Porous C-TiO2

The TG precursor (4.0 g) was dispersed in water (400 mL) and then exposed to the UV-light irradiation for 2 h. After the irradiation, the color of the solid sample turned from white (TG) to intense blue because of the presence of Ti3+ [32]. Finally, the blue solid product was separated from the mixture and dried in air, the O2 molecules of which oxidize the Ti3+ to Ti4+. The obtained light yellow TiO2 product, designated C-TiO2(UV), was amorphous and porous on the basis of X-ray diffraction and adsorption measurement. The elemental analysis indicated that the content of carbon in the material was 1.08 wt%. The UV-light source used in the experiment was a 400 W high-pressure mercury lamp (main output at 313 nm).


## 2.4. Control Experiments

The as-prepared porous C-TiO2(UV) was heated at 200°C and 500°C in air for 2 h, respectively, and the corresponding products were designated C-TiO2(200) and TiO2(500). The brown sample C-TiO2(200) contained 0.86 wt% carbon, and the white sample TiO2(500) was carbon-free on the basis of elemental analysis. The N-TiO2 containing 2.3 wt% nitrogen was prepared through a previously reported method using urea as the nitrogen source [34], and more characterization results about this sample are provided (see XRD in Figure S1, UV-Vis in Figure S2, and XPS in Figure S3 in Supplementary Material available online at doi:10.1155/2012/720183).


## 2.5. Photocatalytic Activity

The photocatalytic activity was assessed in aqueous solution in a water-cooled quartz cylindrical cell. Generally, the reaction mixture in the cell was maintained at about 20°C by a continuous flow of water, and was illuminated with an external light source. The visible-light source was a 500 W Xe lamp (main output > 400 nm), with a glass optical filter used to cut off the short wavelength part (λ < 420 nm).The as-prepared C-TiO2(UV) photocatalyst (0.3 g) was mixed with an aqueous solution of methylene blue (MB) (300 mL, 1 × 10−5mol/L). The aqueous system was magnetically stirred in dark for at least 2 h to establish an adsorption/desorption equilibrium of MB on the particle surface of the material and then subjected to visible-light irradiation. Each reaction cycle lasted for about 4 h during which oxygen was bubbled through the solution. At given irradiation time intervals, a series of aqueous solution samples (3 mL) were collected and separated from the suspended catalyst particles for analysis. The concentration of the MB was determined on a UV-Vis spectrophotometer by monitoring its characteristic absorption at 665 nm. For comparison, the photocatalytic activities of C-TiO2(200), TiO2(500), and N-TiO2 were also measured under the same condition. The weights of all the catalyst samples were identical (0.3 g). Considering that MB can absorb visible light above 600 nm, a cutoff filter (λ > 600 nm) was used to ensure that only MB was excited, and as a result, there was no significant change in the MB concentration after 4 h irradiation even in the presence of C-TiO2(UV) or C-TiO2(200).


## 2.6. General Characterization

The powder X-ray diffraction (XRD) patterns were recorded on a Rigaku D/Max 2550 X-ray diffractometer with Cu Kα radiation (λ = 1.5418 Å) whereas the TEM images were obtained on a JEOL JSM-3010 TEM microscope. The UV-Vis diffuse reflectance spectra were recorded on a Perkin-Elmer Lambda 20 UV/Vis spectrometer, and the absorbance spectra were obtained from the reflectance spectra by means of Kubelka-Munk transformation. The IR spectra were acquired on a Bruker IFS 66 v/S FTIR spectrometer. The carbon contents of the obtained samples were determined through elemental analysis on a Perkin-Elmer 2400 elemental analyzer. The IR spectra were acquired on a Bruker IFS 66 v/S FTIR spectrometer whereas the X-ray photoelectron spectra (XPS) were recorded on a VG ESCALAB MK II electron spectrometer. The nitrogen adsorption and desorption isotherms were measured using a Micromeritics ASAP 2020 M system. The electron paramagnetic resonance (EPR) spectra were recorded on a JEOL JES-FA 200 EPR spectrometer. The concentration of MB was analyzed with a Shimadzu UV-2450 spectrophotometer.


## 3. Results and Discussion

### 3.1. General Structural Characterization

The powder X-ray diffraction (XRD) patterns of the as-prepared porous TiO2 photocatalysts are presented in Figure 1. The sample C-TiO2(UV) directly obtained by the light-driven technique is noncrystalline on the basis of the X-ray diffraction. After thermal treatment at 200°C, the product, C-TiO2(200), is still dominated by an amorphous phase, whereas at 500°C the obtained material TiO2(500) is identified as pure anatase. The broad XRD peaks for TiO2(500) indicate that this material is composed of nanoparticles and the corresponding particle size, estimated by the Scherrer formula, is about 8 nm.Figure 1
Powder XRD patterns of C-TiO2(UV), C-TiO2(200), and TiO2(500).The specific surface area and the pore structure of the porous TiO2 solids were evaluated through N2 adsorption measurements. In Figure 2, the N2 adsorption/desorption isotherms and the corresponding BJH pore-size distribution for the three samples are presented. It is seen that the N2 adsorption/desorption isotherms (Figure 2(a)) are characteristic type IV curves, demonstrating the presence of a porous structure in all the three materials. For C-TiO2(UV) and C-TiO2(200), the negligible hysteresis loop at high relative pressures (P/P0) indicates that the pore size of these two samples is uniform and small. This result is in agreement with the pore-size distribution measurement (Figure 2(b)), which shows a narrow pore-size distribution with average pore sizes of 1.8 nm and 2.6 nm for C-TiO2(UV) and C-TiO2(200), respectively. Interestingly, the mild thermal treatment at 200°C results in not only obvious loss of BET-specific surface area (from 530 to 340 m2 g−1), but also an unusual increase of pore size (from 1.8 to 2.6 nm) and pore volume (from 0.3 to 1.2 cm3 g−1) (Table 1). In general, surface area, pore size, and pore volume should decrease simultaneously after thermal treatment due to structural shrinkage. The increase of pore size and pore volume of our material after the thermal treatment may result from a structural rearrangement of pore wall of the porous C-TiO2. For TiO2(500), the N2 adsorption measurement leads to a BET surface area of 89 m2 g−1, a pore size of 3.7 nm, and a pore volume of 0.1 cm3 g−1. Obviously, at this treatment temperature, the pore structure of the TiO2 material is damaged to a considerable extent although its crystallinity is increased significantly.Table 1
Surface area, pore size, and pore volume of the TiO2 samples.
SampleSurface area (m2 g−1)Pore size (nm)Pore volume (cm3 g−1)C-TiO2(UV)5301.80.3C-TiO2(200)3402.61.2TiO2(500)893.70.1N-TiO2898.20.2(a) N2 adsorption/desorption isotherms and (b) the corresponding BJH pore size distributions of (Δ) C-TiO2(UV), (■) C-TiO2(200), and (★) TiO2(500).
(a)(b)To further verify the presence of porous structures in the obtained TiO2 samples, TEM and HRTEM have been performed and the corresponding images are presented in Figure 3. The TEM images (Figure 3(a)–3(c)) reveal that both C-TiO2(UV) and C-TiO2(200) possess a uniform worm-like porous structure, while TiO2(500) displays only an irregular porous structure formed by randomly arranged and interconnected nanocrystals. The lattice spacing in Figure 3(d), obtained by HRTEM, is about 0.352 nm, which is in accordance with the distance between (101) crystal planes of the anatase phase.TEM images of (a) C-TiO2(UV), (b) C-TiO2(200), (c) TiO2(500), and (d) HRTEM image of TiO2(500).
(a)(b)(c)(d)


### 3.2. Chemical Nature of Carbon Species

To elucidate the nature of the carbon species in the obtained porous C-TiO2 photocatalysts, infrared (IR) spectroscopy has been performed in combination with electron paramagnetic resonance (EPR) and X-ray photoelectron spectroscopy (XPS).The IR spectra of C-TiO2(UV), C-TiO2(200), and the precursor TG are shown in Figure 4. Upon UV-irradiation of TG, the IR absorption peaks related to organic species in the TG precursor almost completely disappear, and only a very weak absorption at 1067 cm−1, which is associated with the presence of a small quantity of Ti–O–C bonds, remains. The above observation indicates that UV-irradiation of TG leads to the removal of organic species form TG and the formation of a final product C-TiO2(UV) with a nominal formula TiO2 and a small amount of Ti–O–C species. Further mild thermal treatment (200°C) leads to complete elimination of the Ti–O–C absorption. This result demonstrates that the Ti–O–C bonds in C-TiO2(UV) are not thermally stable, and can be easily transformed to other forms of carbon in the TiO2 material.Figure 4
The IR spectra of TG, C-TiO2(UV), and C-TiO2(200).The X-ray photoelectron spectroscopy (XPS) has been used to obtain valuable information about the chemical nature of surface elements for the C-TiO2 materials. Figures 5(a) and 5(b) show the high-resolution C1s spectra of C-TiO2(UV) and C-TiO2(200) samples. The peak at 284.8 eV for both samples are due to adventitious elemental carbon from the XPS instrument [28], and this peak is also observed for the carbon-free TiO2(500) sample. Besides the peak at 284.8 eV, a shoulder peak associated with Ti–O–C bonds at about 285.9 eV is detected for C-TiO2(UV). Furthermore, no peaks appear at around 282 eV (Ti-C bonds) and 288.5 eV (C=O bonds), suggesting that except for Ti–O–C bonds, neither O–Ti–C bonds nor carbonate species are present in C-TiO2(UV). After the mild thermal treatment (at 200°C), the peak of Ti–O–C bonds disappears, and only two weak peaks ascribed to C–O (286.4 eV) and C=O (288.5 eV) bonds are observed for C-TiO2(200). The simultaneous presence of C–O and C=O bonds was considered to be characteristic of carbonate species previously, but the carbonate species were not chromophores in nature [35]. Thus, the strong visible-light response of the brown C-TiO2(200) may arise from other carbon species, which were not detected by XPS. Figure 5(c) shows the high-resolution XPS spectra of Ti2p for C-TiO2(UV), C-TiO2(200), and TiO2(500). It is seen that the XPS spectrum of Ti2p for the TiO2(500) sample exhibit two peaks at 464.4 and 458.8 eV, which are assigned to the 2p1/2 and 2p3/2 core level of Ti4+, respectively. In comparison with XPS peaks of the TiO2(500) sample, an obvious peak shift towards high binding energy (0.2 eV) in the Ti2p spectra of C-TiO2(UV) and C-TiO2(200) is observed. Similar peak shift was also observed in the O1s spectra of C-TiO2(UV) and C-TiO2(200), as demonstrated in Figure 5(d). TiO2(500) gives an XPS peak related to Ti–O–Ti oxygen at 530.0 eV, whereas C-TiO2(UV) and C-TiO2(200) exhibit this XPS peak at 530.3 eV. The above results indicate that the presence of carbon species affect the local chemical circumstances of surface elements (Ti4+ and O2−), and strong interaction between carbon species and surface elements is present.High-resolution XPS spectra of C1s for (a) C-TiO2(UV) and (b) C-TiO2(200); high-resolution XPS spectra of (c) Ti2p and (d) O1s for C-TiO2(UV), C-TiO2(200), and TiO2(500).
(a)(b)(c)(d)To reveal the nature of the remained carbon species in C-TiO2(200), EPR spectroscopy has been employed to examine the C-TiO2(UV) and C-TiO2(200) samples (Figure 6). No EPR signals for paramagnetic species are observed for C-TiO2(UV) whereas C-TiO2(200) shows a distinct singlet signal at g=2.0023 assignable to coke-type carbon species. Similar EPR signals have also been observed for other porous materials containing coke species [30, 36–38]. Taking into account the existence of coke in C-TiO2(200), it is believed that the weak signals of C–O and C=O bonds (Figure 5) observed in this case are derived from the coke through its partial oxidization during the thermal treatment [38]. The XPS signal for the coke itself should be located at 284.8 eV, covered by the adventitious elemental carbon peak from the XPS instrument, and thus cannot be distinguished. From the above results, it is easily concluded that the carbon species (Ti–O–C bonds) in C-TiO2(UV) are driven off from the TiO2 framework during the mild thermal treatment, forming a new type of carbonaceous matter (coke), on the surface of the C-TiO2(200) material. The signal of coke disappears for the carbon-free TiO2(500) sample, which is obtained after thermal treatment of C-TiO2(UV) at 500°C in air, as at this temperature the coke species is completely oxidized and removed from the solid sample.Figure 6
The EPR spectra of C-TiO2(UV) and C-TiO2(200) measured at room temperature.


### 3.3. Photoresponsive Range

The UV-Vis diffuse reflectance spectra (Figure7) demonstrate that the light-yellow C-TiO2(UV) shows two optical absorption thresholds at 385 nm in the ultraviolet region and 550 nm in the visible region. In comparison, no visible-light absorption but an absorption threshold at 400 nm appears for the white TiO2(500). The ultraviolet absorption thresholds for both C-TiO2(UV) and TiO2(500) correspond to the inherent bandgap absorptions of TiO2, and the small difference between these threshold values are due to the difference in crystal structure (amorphous for C-TiO2(UV), anatase for TiO2(500)). The visible-light absorption band between 400 and 550 nm for C-TiO2(UV) arises from the Ti–O–C bonds which form localized occupied states in the bandgap of TiO2, as predicted by density function theory (DFT) calculations [39]. The energies of these intragap states are higher than that of the top of the TiO2 valence band, and as a result, the electron transitions from these intragap states to the TiO2 conduction band absorb energies distinctly lower than the TiO2 bandgap, corresponding to visible-light radiation. For the UV-Vis diffuse reflectance spectrum of the brown C-TiO2 (200), a broad and strong band covering the whole visible region appears and this absorption is attributed to the presence of coke-type species in the material.Figure 7
UV-Vis diffuse reflectance spectra of C-TiO2(UV), C-TiO2(200), and TiO2(500).


### 3.4. Photocatalytic Performance

The photocatalytic performances of the obtained C-TiO2 materials have been evaluated by testing the degradation of methylene blue (MB), which is often used as a model pollutant in semiconductor photocatalysis, under visible light (λ > 420 nm) irradiation. During the whole process of photocatalysis, the reaction system is saturated by oxygen, which can prevent MB from reduction to colorless leuco form (LMB) [40]. For comparison, the photocatalytic performance of N-TiO2 has also been measured under the same condition.It is generally believed that the capacity to adsorb reactant molecules on the surface of a solid material is a key parameter for its photocatalytic activity [41–43]. Therefore, the MB absorption capacities of the obtained samples were assessed before light irradiation, and the results are shown in Figure 8. The obtained sample (0.3 g) was mixed with an aqueous solution of methylene blue (MB) (300 mL, 1 × 10−5mol/L). After the adsorption/desorption equilibration is reached, about 44% and 45% of the dye are removed from the respective aqueous solutions by adsorption on the C-TiO2(UV) and C-TiO2(200) surfaces, while only 11% and 10% of the initial dye are absorbed by TiO2(500) and N-TiO2, respectively. The high adsorption capacities for C-TiO2(UV) and C-TiO2(200) can be attributed to their significant surface areas (530 m2 g−1 for C-TiO2(UV), 340 m2 g−1 for C-TiO2(200)). It is of interest to note that C-TiO2(200) shows an adsorption capacity similar to that of C-TiO2(UV) whereas the surface area of C-TiO2(200) is smaller than that of C-TiO2(UV). This unusual observation can be explained by the fact that the pore volume (1.2 cm3 g−1) of C-TiO2(200) is about 4-times as large as that (0.3 cm3 g−1) of C-TiO2(UV). In addition, it has been reported that coke matter contains polyaromatic structures [30, 36–38], and the π-π interactions between coke and the aromatic rings of MB may also contribute to the adsorption of MB by the TiO2(200) material.Figure 8
The absorption capacity of (A) C-TiO2(UV), (B) C-TiO2(200), (C) TiO2(500), and (D) N-TiO2 for MB.The photocatalytic performances of the samples (Figure9) are measured by the changes of MB concentration (Ct/C0) during the process of photodegradation reaction under visible-light irradiation (λ > 420 nm), where Ct is the concentration of MB at the irradiation time t and C0 is the initial concentration of MB after an adsorption/desorption equilibrium is reached before irradiation. 37%, 50%, and 75% of MB are degraded after 4 h irradiation for N-TiO2, C-TiO2(UV), and C-TiO2(200), respectively. The photocatalytic activities of the two C-doped TiO2 materials are distinctly superior to that of the N-TiO2 sample. In contrast, only slight degradation of MB (<5%) has been observed for TiO2(500) after visible-light irradiation of 4 hours, indicating that the TiO2(500) material is not a good visible-light photocatalyst. In addition, the difference of visible-light photocatalytic performances of the obtained TiO2 materials can be easily explained on the basis of the UV-Vis diffuse reflectance spectra of the samples (Figure 7). The coke-containing C-TiO2(200) and the C-TiO2(UV) with Ti–O–C bonds both absorb visible light, and consequently, they are visible-light responsive in the photocatalytic process. In contrast, the TiO2(500) sample absorbs no visible light, and therefore this material is not photocatalytically active under visible-light irradiation. The higher photocatalytic activity of C-TiO2(200) in comparison with that of C-TiO2(UV) is rationalized by its stronger visible-light absorption. The recycling experiments demonstrate that both C-TiO2(UV) and C-TiO2(200) are rather stable when used as photocatalysts and there is no loss of photocatalytic activity after at least five cycles of degradation testing of MB.Figure 9
The residual fraction of MB in solution as a function of irradiation time with (▲) C-TiO2(UV), (★) C-TiO2(200), (■) TiO2(500), and (●) N-TiO2.Considering that MB can absorb visible light above 600 nm (the absorption peak is at about 665 nm), a cutoff filter (λ > 600 nm) was used to ensure that only MB was excited during the photocatalysis process. Whereas the photocatalysts we used nearly do not absorb the visible light with a wavelength longer than 600 nm. With the use of the cutoff filter, no significant change in MB concentration was observed for the photocatalytic reaction even after 4 h irradiation in the presence of C-TiO2(UV) or C-TiO2(200). This observation indicates that the decoloration of MB under visible light with use of cutoff filter (λ > 420 nm) is attributed to the photocatalytic effect of the obtained C-doped TiO2 samples, rather than MB photosensitization.


### 3.5. Photocatalytic Mechanism

The carbon species in C-TiO2(UV) and C-TiO2(200) are very different in nature, and therefore, they contribute to the photocatalytic performances of the corresponding materials in different manners (Scheme 1).Scheme 1
The photocatalytic mechanisms for C-TiO2(UV) and C-TiO2(200).For C-TiO2(UV), the carbons are incorporated in the TiO2 lattice to form Ti–O–C bonds. As demonstrated earlier by the UV-Vis spectroscopy, the electron transitions from the localized states associated with these Ti–O–C bonds to the TiO2 conduction band absorb visible light, and hence generating electrons and holes upon visible-light irradiation. The photogenerated electrons on the conduction band of TiO2 interact with O2 molecules to form oxidative species such as superoxide radicals which degrade the MB molecules.For C-TiO2(200), the photocatalytic mechanism differs to a certain extent. In this material, there exists coke on the surface of TiO2. As demonstrated previously in the literature [30, 44], the coke itself can be photoexcited under visible-light irradiation, and the excited carbon species inject the photogenerated electrons into the conduction band of TiO2. The injected electrons move to the surface of the TiO2, where they are captured by O2 to form superoxide ions (O2·−), which finally lead to the degradation of MB. In addition, the photogenerated holes located in coke can also directly oxidize and degrade MB.


## 3.1. General Structural Characterization

The powder X-ray diffraction (XRD) patterns of the as-prepared porous TiO2 photocatalysts are presented in Figure 1. The sample C-TiO2(UV) directly obtained by the light-driven technique is noncrystalline on the basis of the X-ray diffraction. After thermal treatment at 200°C, the product, C-TiO2(200), is still dominated by an amorphous phase, whereas at 500°C the obtained material TiO2(500) is identified as pure anatase. The broad XRD peaks for TiO2(500) indicate that this material is composed of nanoparticles and the corresponding particle size, estimated by the Scherrer formula, is about 8 nm.Figure 1
Powder XRD patterns of C-TiO2(UV), C-TiO2(200), and TiO2(500).The specific surface area and the pore structure of the porous TiO2 solids were evaluated through N2 adsorption measurements. In Figure 2, the N2 adsorption/desorption isotherms and the corresponding BJH pore-size distribution for the three samples are presented. It is seen that the N2 adsorption/desorption isotherms (Figure 2(a)) are characteristic type IV curves, demonstrating the presence of a porous structure in all the three materials. For C-TiO2(UV) and C-TiO2(200), the negligible hysteresis loop at high relative pressures (P/P0) indicates that the pore size of these two samples is uniform and small. This result is in agreement with the pore-size distribution measurement (Figure 2(b)), which shows a narrow pore-size distribution with average pore sizes of 1.8 nm and 2.6 nm for C-TiO2(UV) and C-TiO2(200), respectively. Interestingly, the mild thermal treatment at 200°C results in not only obvious loss of BET-specific surface area (from 530 to 340 m2 g−1), but also an unusual increase of pore size (from 1.8 to 2.6 nm) and pore volume (from 0.3 to 1.2 cm3 g−1) (Table 1). In general, surface area, pore size, and pore volume should decrease simultaneously after thermal treatment due to structural shrinkage. The increase of pore size and pore volume of our material after the thermal treatment may result from a structural rearrangement of pore wall of the porous C-TiO2. For TiO2(500), the N2 adsorption measurement leads to a BET surface area of 89 m2 g−1, a pore size of 3.7 nm, and a pore volume of 0.1 cm3 g−1. Obviously, at this treatment temperature, the pore structure of the TiO2 material is damaged to a considerable extent although its crystallinity is increased significantly.Table 1
Surface area, pore size, and pore volume of the TiO2 samples.
SampleSurface area (m2 g−1)Pore size (nm)Pore volume (cm3 g−1)C-TiO2(UV)5301.80.3C-TiO2(200)3402.61.2TiO2(500)893.70.1N-TiO2898.20.2(a) N2 adsorption/desorption isotherms and (b) the corresponding BJH pore size distributions of (Δ) C-TiO2(UV), (■) C-TiO2(200), and (★) TiO2(500).
(a)(b)To further verify the presence of porous structures in the obtained TiO2 samples, TEM and HRTEM have been performed and the corresponding images are presented in Figure 3. The TEM images (Figure 3(a)–3(c)) reveal that both C-TiO2(UV) and C-TiO2(200) possess a uniform worm-like porous structure, while TiO2(500) displays only an irregular porous structure formed by randomly arranged and interconnected nanocrystals. The lattice spacing in Figure 3(d), obtained by HRTEM, is about 0.352 nm, which is in accordance with the distance between (101) crystal planes of the anatase phase.TEM images of (a) C-TiO2(UV), (b) C-TiO2(200), (c) TiO2(500), and (d) HRTEM image of TiO2(500).
(a)(b)(c)(d)


## 3.2. Chemical Nature of Carbon Species

To elucidate the nature of the carbon species in the obtained porous C-TiO2 photocatalysts, infrared (IR) spectroscopy has been performed in combination with electron paramagnetic resonance (EPR) and X-ray photoelectron spectroscopy (XPS).The IR spectra of C-TiO2(UV), C-TiO2(200), and the precursor TG are shown in Figure 4. Upon UV-irradiation of TG, the IR absorption peaks related to organic species in the TG precursor almost completely disappear, and only a very weak absorption at 1067 cm−1, which is associated with the presence of a small quantity of Ti–O–C bonds, remains. The above observation indicates that UV-irradiation of TG leads to the removal of organic species form TG and the formation of a final product C-TiO2(UV) with a nominal formula TiO2 and a small amount of Ti–O–C species. Further mild thermal treatment (200°C) leads to complete elimination of the Ti–O–C absorption. This result demonstrates that the Ti–O–C bonds in C-TiO2(UV) are not thermally stable, and can be easily transformed to other forms of carbon in the TiO2 material.Figure 4
The IR spectra of TG, C-TiO2(UV), and C-TiO2(200).The X-ray photoelectron spectroscopy (XPS) has been used to obtain valuable information about the chemical nature of surface elements for the C-TiO2 materials. Figures 5(a) and 5(b) show the high-resolution C1s spectra of C-TiO2(UV) and C-TiO2(200) samples. The peak at 284.8 eV for both samples are due to adventitious elemental carbon from the XPS instrument [28], and this peak is also observed for the carbon-free TiO2(500) sample. Besides the peak at 284.8 eV, a shoulder peak associated with Ti–O–C bonds at about 285.9 eV is detected for C-TiO2(UV). Furthermore, no peaks appear at around 282 eV (Ti-C bonds) and 288.5 eV (C=O bonds), suggesting that except for Ti–O–C bonds, neither O–Ti–C bonds nor carbonate species are present in C-TiO2(UV). After the mild thermal treatment (at 200°C), the peak of Ti–O–C bonds disappears, and only two weak peaks ascribed to C–O (286.4 eV) and C=O (288.5 eV) bonds are observed for C-TiO2(200). The simultaneous presence of C–O and C=O bonds was considered to be characteristic of carbonate species previously, but the carbonate species were not chromophores in nature [35]. Thus, the strong visible-light response of the brown C-TiO2(200) may arise from other carbon species, which were not detected by XPS. Figure 5(c) shows the high-resolution XPS spectra of Ti2p for C-TiO2(UV), C-TiO2(200), and TiO2(500). It is seen that the XPS spectrum of Ti2p for the TiO2(500) sample exhibit two peaks at 464.4 and 458.8 eV, which are assigned to the 2p1/2 and 2p3/2 core level of Ti4+, respectively. In comparison with XPS peaks of the TiO2(500) sample, an obvious peak shift towards high binding energy (0.2 eV) in the Ti2p spectra of C-TiO2(UV) and C-TiO2(200) is observed. Similar peak shift was also observed in the O1s spectra of C-TiO2(UV) and C-TiO2(200), as demonstrated in Figure 5(d). TiO2(500) gives an XPS peak related to Ti–O–Ti oxygen at 530.0 eV, whereas C-TiO2(UV) and C-TiO2(200) exhibit this XPS peak at 530.3 eV. The above results indicate that the presence of carbon species affect the local chemical circumstances of surface elements (Ti4+ and O2−), and strong interaction between carbon species and surface elements is present.High-resolution XPS spectra of C1s for (a) C-TiO2(UV) and (b) C-TiO2(200); high-resolution XPS spectra of (c) Ti2p and (d) O1s for C-TiO2(UV), C-TiO2(200), and TiO2(500).
(a)(b)(c)(d)To reveal the nature of the remained carbon species in C-TiO2(200), EPR spectroscopy has been employed to examine the C-TiO2(UV) and C-TiO2(200) samples (Figure 6). No EPR signals for paramagnetic species are observed for C-TiO2(UV) whereas C-TiO2(200) shows a distinct singlet signal at g=2.0023 assignable to coke-type carbon species. Similar EPR signals have also been observed for other porous materials containing coke species [30, 36–38]. Taking into account the existence of coke in C-TiO2(200), it is believed that the weak signals of C–O and C=O bonds (Figure 5) observed in this case are derived from the coke through its partial oxidization during the thermal treatment [38]. The XPS signal for the coke itself should be located at 284.8 eV, covered by the adventitious elemental carbon peak from the XPS instrument, and thus cannot be distinguished. From the above results, it is easily concluded that the carbon species (Ti–O–C bonds) in C-TiO2(UV) are driven off from the TiO2 framework during the mild thermal treatment, forming a new type of carbonaceous matter (coke), on the surface of the C-TiO2(200) material. The signal of coke disappears for the carbon-free TiO2(500) sample, which is obtained after thermal treatment of C-TiO2(UV) at 500°C in air, as at this temperature the coke species is completely oxidized and removed from the solid sample.Figure 6
The EPR spectra of C-TiO2(UV) and C-TiO2(200) measured at room temperature.


## 3.3. Photoresponsive Range

The UV-Vis diffuse reflectance spectra (Figure7) demonstrate that the light-yellow C-TiO2(UV) shows two optical absorption thresholds at 385 nm in the ultraviolet region and 550 nm in the visible region. In comparison, no visible-light absorption but an absorption threshold at 400 nm appears for the white TiO2(500). The ultraviolet absorption thresholds for both C-TiO2(UV) and TiO2(500) correspond to the inherent bandgap absorptions of TiO2, and the small difference between these threshold values are due to the difference in crystal structure (amorphous for C-TiO2(UV), anatase for TiO2(500)). The visible-light absorption band between 400 and 550 nm for C-TiO2(UV) arises from the Ti–O–C bonds which form localized occupied states in the bandgap of TiO2, as predicted by density function theory (DFT) calculations [39]. The energies of these intragap states are higher than that of the top of the TiO2 valence band, and as a result, the electron transitions from these intragap states to the TiO2 conduction band absorb energies distinctly lower than the TiO2 bandgap, corresponding to visible-light radiation. For the UV-Vis diffuse reflectance spectrum of the brown C-TiO2 (200), a broad and strong band covering the whole visible region appears and this absorption is attributed to the presence of coke-type species in the material.Figure 7
UV-Vis diffuse reflectance spectra of C-TiO2(UV), C-TiO2(200), and TiO2(500).


## 3.4. Photocatalytic Performance

The photocatalytic performances of the obtained C-TiO2 materials have been evaluated by testing the degradation of methylene blue (MB), which is often used as a model pollutant in semiconductor photocatalysis, under visible light (λ > 420 nm) irradiation. During the whole process of photocatalysis, the reaction system is saturated by oxygen, which can prevent MB from reduction to colorless leuco form (LMB) [40]. For comparison, the photocatalytic performance of N-TiO2 has also been measured under the same condition.It is generally believed that the capacity to adsorb reactant molecules on the surface of a solid material is a key parameter for its photocatalytic activity [41–43]. Therefore, the MB absorption capacities of the obtained samples were assessed before light irradiation, and the results are shown in Figure 8. The obtained sample (0.3 g) was mixed with an aqueous solution of methylene blue (MB) (300 mL, 1 × 10−5mol/L). After the adsorption/desorption equilibration is reached, about 44% and 45% of the dye are removed from the respective aqueous solutions by adsorption on the C-TiO2(UV) and C-TiO2(200) surfaces, while only 11% and 10% of the initial dye are absorbed by TiO2(500) and N-TiO2, respectively. The high adsorption capacities for C-TiO2(UV) and C-TiO2(200) can be attributed to their significant surface areas (530 m2 g−1 for C-TiO2(UV), 340 m2 g−1 for C-TiO2(200)). It is of interest to note that C-TiO2(200) shows an adsorption capacity similar to that of C-TiO2(UV) whereas the surface area of C-TiO2(200) is smaller than that of C-TiO2(UV). This unusual observation can be explained by the fact that the pore volume (1.2 cm3 g−1) of C-TiO2(200) is about 4-times as large as that (0.3 cm3 g−1) of C-TiO2(UV). In addition, it has been reported that coke matter contains polyaromatic structures [30, 36–38], and the π-π interactions between coke and the aromatic rings of MB may also contribute to the adsorption of MB by the TiO2(200) material.Figure 8
The absorption capacity of (A) C-TiO2(UV), (B) C-TiO2(200), (C) TiO2(500), and (D) N-TiO2 for MB.The photocatalytic performances of the samples (Figure9) are measured by the changes of MB concentration (Ct/C0) during the process of photodegradation reaction under visible-light irradiation (λ > 420 nm), where Ct is the concentration of MB at the irradiation time t and C0 is the initial concentration of MB after an adsorption/desorption equilibrium is reached before irradiation. 37%, 50%, and 75% of MB are degraded after 4 h irradiation for N-TiO2, C-TiO2(UV), and C-TiO2(200), respectively. The photocatalytic activities of the two C-doped TiO2 materials are distinctly superior to that of the N-TiO2 sample. In contrast, only slight degradation of MB (<5%) has been observed for TiO2(500) after visible-light irradiation of 4 hours, indicating that the TiO2(500) material is not a good visible-light photocatalyst. In addition, the difference of visible-light photocatalytic performances of the obtained TiO2 materials can be easily explained on the basis of the UV-Vis diffuse reflectance spectra of the samples (Figure 7). The coke-containing C-TiO2(200) and the C-TiO2(UV) with Ti–O–C bonds both absorb visible light, and consequently, they are visible-light responsive in the photocatalytic process. In contrast, the TiO2(500) sample absorbs no visible light, and therefore this material is not photocatalytically active under visible-light irradiation. The higher photocatalytic activity of C-TiO2(200) in comparison with that of C-TiO2(UV) is rationalized by its stronger visible-light absorption. The recycling experiments demonstrate that both C-TiO2(UV) and C-TiO2(200) are rather stable when used as photocatalysts and there is no loss of photocatalytic activity after at least five cycles of degradation testing of MB.Figure 9
The residual fraction of MB in solution as a function of irradiation time with (▲) C-TiO2(UV), (★) C-TiO2(200), (■) TiO2(500), and (●) N-TiO2.Considering that MB can absorb visible light above 600 nm (the absorption peak is at about 665 nm), a cutoff filter (λ > 600 nm) was used to ensure that only MB was excited during the photocatalysis process. Whereas the photocatalysts we used nearly do not absorb the visible light with a wavelength longer than 600 nm. With the use of the cutoff filter, no significant change in MB concentration was observed for the photocatalytic reaction even after 4 h irradiation in the presence of C-TiO2(UV) or C-TiO2(200). This observation indicates that the decoloration of MB under visible light with use of cutoff filter (λ > 420 nm) is attributed to the photocatalytic effect of the obtained C-doped TiO2 samples, rather than MB photosensitization.


## 3.5. Photocatalytic Mechanism

The carbon species in C-TiO2(UV) and C-TiO2(200) are very different in nature, and therefore, they contribute to the photocatalytic performances of the corresponding materials in different manners (Scheme 1).Scheme 1
The photocatalytic mechanisms for C-TiO2(UV) and C-TiO2(200).For C-TiO2(UV), the carbons are incorporated in the TiO2 lattice to form Ti–O–C bonds. As demonstrated earlier by the UV-Vis spectroscopy, the electron transitions from the localized states associated with these Ti–O–C bonds to the TiO2 conduction band absorb visible light, and hence generating electrons and holes upon visible-light irradiation. The photogenerated electrons on the conduction band of TiO2 interact with O2 molecules to form oxidative species such as superoxide radicals which degrade the MB molecules.For C-TiO2(200), the photocatalytic mechanism differs to a certain extent. In this material, there exists coke on the surface of TiO2. As demonstrated previously in the literature [30, 44], the coke itself can be photoexcited under visible-light irradiation, and the excited carbon species inject the photogenerated electrons into the conduction band of TiO2. The injected electrons move to the surface of the TiO2, where they are captured by O2 to form superoxide ions (O2·−), which finally lead to the degradation of MB. In addition, the photogenerated holes located in coke can also directly oxidize and degrade MB.


## 4. Conclusions

An unusual light-driven strategy is explored for the preparation of highly porous C-doped TiO2. It has been demonstrated that the obtained material exhibits high efficiency in visible-light photocatalysis for degradation of methylene blue. The carbon species, which are responsible for the visible-light photocatalytic activity, in the porous C-TiO2 are found to exist in the form of Ti–O–C bonds. The Ti–O–C bonds are thermally nonstable and can be transformed to coke matter after mild thermal treatment at 200°C. The resulting coke-containing TiO2 is proved to be an even better visible-light photocatalyst, almost twice as effective as N-TiO2. Our experiments reveal that both the Ti–O–C bonds and the coke species play a role in visible-light photocatalysis, providing new insights into the origin of visible-light photocatalytic performance of C-TiO2 materials. Moreover, the strategy reported here is anticipated to open vistas for light-driven preparation of inorganic materials with advanced functions.



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*Source: 720183-2012-03-13.xml*