# Solvothermal Synthesis and Photocatalytic Properties of Nitrogen-Doped SrTiO3 Nanoparticles

Authors: Uyi Sulaeman; Shu Yin; Tsugio Sato
Journal: Journal of Nanomaterials
 (2010)

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## Abstract

Perovskite-type nitrogen-doped SrTiO3 nanoparticles of 50–80 nm in diameter were successfully synthesized by the solvothermal of Ti(OC3H7)4, SrCl2·6H2O, and hexamethylenetetramine in KOH aqueous solution. Nitrogen-doped SrTiO3 showed excellent photocatalytic activity under both UV and visible light irradiation, that is, the photocatalytic activity of N-doped SrTiO3 for DeNOx reaction was greater than that of SrTiO3 and commercial TiO2 (Degussa P25) in both visible light region (>510 nm) and UV light region (>290 nm). The excellent visible light photocatalytic activity of this substance was caused by generating a new band gap that absorbs visible light.


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## Body

## 1. Introduction

Strontium titanate is one of the excellent photocatalysts that could be used in water splitting for hydrogen energy production and degradation of organic contaminant under ultraviolet irradiation. Unfortunately, the photocatalytic activity is not high application in visible light because of relatively large band gap energy of 3.2 eV. Therefore, to extend the absorption range of strontium titanate towards the visible range is essential work to generate visible light responsive photocatalyst. It is a great challenge to synthesize the catalyst which is active under visible light irradiation to use sun light. The research of photocatalyst in the field of visible light region has attracted many researchers [1–5]. Doping with metal or nonmetal ion to SrTiO3 material could extend its optical absorption edge towards the visible light range and generate the photocatalytic activity in visible light.  Many studies have focused on nitrogen doping due to well-responsive photocatalytic activity in visible light. It is well known that the substituting of oxygen ion by nitrogen ion can generate the new band gap of photocatalyst [6]. The photocatalytic activity of the catalysts may depend on the preparation method due to the difference in the specific surface area, particle size, and crystallinity of the catalyst. Nitrogen-doped SrTiO3 could be prepared by the mechanochemical reaction of SrTiO3 [6–8] using doping sources such as hexamethylenetetramine, urea, ammonium carbonate, and thiourea, and using a high energy planetary ball mill and agate mortar. However, the mechanochemical reaction tends to generate stress on the surface of the product and leads to depressing the photocatalytic activity. Therefore, we synthesized the N-doped SrTiO3 nanoparticles using solvothermal reaction in KOH aqueous solution to obtain the fine particles and high specific surface area. The visible responsive photocatalyst could be enhanced by this method.


## 2. Experimental

### 2.1. Preparation

Titanium tetraisopropoxide Ti(OC3H7)4 and SrCl2·6H2O were used as starting materials, hexamethylenetetramine (HMT) as a source of nitrogen, and KOH as a mineralizer. All of them were reagent grade and used without further purification. After dissolving titanium tetraisopropoxide, Ti(OC3H7)4 in 10 mL 2-propanol, SrCl2 aqueous solution was added dropwise to Ti(OC3H7)4 2-propanol solution with stirring continuously, and then 0–6 gram of HMT and 20 mL of 2 M KOH aqueous solution were added in turn. The mixed solution was placed into a stainless steel autoclave inserted with a Teflon container. After that, the autoclave was heated at 200°C for 3 hours. After cooling the autoclave to room temperature, the powder product was separated by centrifugation, washed with distilled water and acetone three times, respectively, then dried in vacuum at 60°C overnight.


### 2.2. Characterization

The powder product was characterized by X-ray diffraction analysis (XRD, Shimadzu XD-D1) using graphite-monochromized CuKα radiation. Microstructures were observed by scanning electron  microscope  (FE-SEM, Hitachi, S-4800) and transmission electron micrograph (TEM, JEOL JEM-2010). The specific surface areas were determined by the nitrogen adsorption at 77 K (BET, Quantachrome NOVA 4200 e). The vibration spectra were characterized by FTIR (FTS 7000 series, DIGILIB). The UV-vis diffuse reflectance spectra were measured at room temperature with a UV-vis spectrophotometer (Shimadzu UV-2450) in the range 250–800 nm. Binding energies of the samples were analyzed at room temperature by X-ray photoelectron spectroscopy (Perkin-Elmer PHI 5600).


### 2.3. Photocatalytic Activity Evaluation

The photocatalytic activity for the NOx destruction was determined by measuring the concentration of NOx gas at the outlet of the reactor during the photoirradiation of a constant flow of a mixed gas containing 1 ppm NOx–50 vol.% air (balance N2). The photocatalyst sample was placed in a hollow of 20 mm length × 15 mm width × 0.5 mm depth on a glass holder plate and set in the bottom centre of the reactor. A 450 W high-pressure mercury arc was used as the light source. The wavelength of the irradiation light was controlled by selecting filters, that is, Pyrex glass for λ> 290 nm, Kenko L41 Super Pro (W) filter for λ> 400 nm, and Fuji, tri-acetyl cellulose filter for λ> 510 nm.  The concentration of NOx was determined using an NOx analyzer (Yanaco, ECL-88A).


## 2.1. Preparation

Titanium tetraisopropoxide Ti(OC3H7)4 and SrCl2·6H2O were used as starting materials, hexamethylenetetramine (HMT) as a source of nitrogen, and KOH as a mineralizer. All of them were reagent grade and used without further purification. After dissolving titanium tetraisopropoxide, Ti(OC3H7)4 in 10 mL 2-propanol, SrCl2 aqueous solution was added dropwise to Ti(OC3H7)4 2-propanol solution with stirring continuously, and then 0–6 gram of HMT and 20 mL of 2 M KOH aqueous solution were added in turn. The mixed solution was placed into a stainless steel autoclave inserted with a Teflon container. After that, the autoclave was heated at 200°C for 3 hours. After cooling the autoclave to room temperature, the powder product was separated by centrifugation, washed with distilled water and acetone three times, respectively, then dried in vacuum at 60°C overnight.


## 2.2. Characterization

The powder product was characterized by X-ray diffraction analysis (XRD, Shimadzu XD-D1) using graphite-monochromized CuKα radiation. Microstructures were observed by scanning electron  microscope  (FE-SEM, Hitachi, S-4800) and transmission electron micrograph (TEM, JEOL JEM-2010). The specific surface areas were determined by the nitrogen adsorption at 77 K (BET, Quantachrome NOVA 4200 e). The vibration spectra were characterized by FTIR (FTS 7000 series, DIGILIB). The UV-vis diffuse reflectance spectra were measured at room temperature with a UV-vis spectrophotometer (Shimadzu UV-2450) in the range 250–800 nm. Binding energies of the samples were analyzed at room temperature by X-ray photoelectron spectroscopy (Perkin-Elmer PHI 5600).


## 2.3. Photocatalytic Activity Evaluation

The photocatalytic activity for the NOx destruction was determined by measuring the concentration of NOx gas at the outlet of the reactor during the photoirradiation of a constant flow of a mixed gas containing 1 ppm NOx–50 vol.% air (balance N2). The photocatalyst sample was placed in a hollow of 20 mm length × 15 mm width × 0.5 mm depth on a glass holder plate and set in the bottom centre of the reactor. A 450 W high-pressure mercury arc was used as the light source. The wavelength of the irradiation light was controlled by selecting filters, that is, Pyrex glass for λ> 290 nm, Kenko L41 Super Pro (W) filter for λ> 400 nm, and Fuji, tri-acetyl cellulose filter for λ> 510 nm.  The concentration of NOx was determined using an NOx analyzer (Yanaco, ECL-88A).


## 3. Results and Discussion

### 3.1. Solvothermal Synthesis of N-Doped SrTiO3

Nitrogen-doped SrTiO3 was successfully synthesized by solvothermal reaction in KOH aqueous solution using tetraisopropoxide, Ti(OC3H7)4, and SrCl2·6H2O as the starting material and hexamethylenetetramine (HMT) as nitrogen source. It is well known that HMT could be degraded into ammonia and formaldehyde by heating in water above 70°C [9]. The ammonia is the key factor of nitrogen doping in catalyst synthesis. By the solvothermal reaction synthesis, ammonia could react with the starting material to produce the catalyst from bottom up. The ammonia decomposed from HMT was absorbed on the surface of developing and growing strontium titanate nanocrystal and reacted with activated strontia-titania surface, then generating the nitrogen doping in the solvothermal reaction. The yellow crystalline of N-doped SrTiO3 could be obtained. The reaction for the synthesis of N-doped SrTiO3 (1) can be described as
(1)Ti(OC3H7)4+2H2O→TiO2+4C3H7OHSrCl2·6H2O+2KOH→Sr(OH)2+2KCl+6H2OSr(OH)2+TiO2→SrTiO3+H2OC6H12N4+6H2O→6HCHO+4NH3SrTiO3+yNH3→SrTiO3-3y/2Ny□y/2+3y2H2O(□:latticedefect).


### 3.2. XRD Characterization

Figure1 shows the XRD pattern of undoped and N-doped SrTiO3 by solvothermal reactions at 200°C for 3 hours with variation of HMT content. All diffraction peaks could be assigned to the perovskite-type structure of SrTiO3 with cubic symmetry (JCPDS no. 79-0176). The diffraction peak position for N-doped SrTiO3 shifted to higher angle as shown in the insert of Figure 1. It indicated that the lattice constant decreased with nitrogen doping. Since the radius of O2- (1.40 Å) is smaller than N3- (1.71 Å), the decrease of lattice constant of SrTiO3 with nitrogen doping may be due to the formation of anion vacancy for charge compensation as SrTiO3-3y/2Ny□y/2(□:latticedefect).Figure 1
XRD patterns of sample prepared by solvothermal method, SrTiO3 (a), N-doped SrTiO3 with HMT of 1 gram (b), 2 gram (c), and 4 gram (d). The insert indicates the (110) peak shift due to nitrogen doping.The average crystallite sizes calculated by Scherrer’s Equation (2) using the full width at half maximum (FWHM) of the most intense peak (110) are also listed in Table 1 together with the specific surface areas
(2)D=0.9λBcosθ,
where D is the average crystallite size or particle size, λ the X-ray wavelength (0.15418 nm), θ the Bragg angle, and B the FWHM. The samples consisted of nanoparticles of 35–48 nm in diameter and specific surface area of 20.5–31.7 m2 g-1 and did not change so much with nitrogen doping and following calcination.Table 1
Crystallite size and surface area of SrTiO3 and N-doped SrTiO3.
PhotocatalystCrystal size (nm)Specific surface area (m2/g)SrTiO34029.51 gram of HMT4320.52 gram of HMT3828.54 gram of HMT3527.94 gram of HMT calcined at200°C3425.84 gram of HMT calcined at300°C3529.64 gram of HMT calcined at400°C4831.7


### 3.3. Morphology

The images of SEM of SrTiO3 and nitrogen-doped SrTiO3 are shown in Figure 2. The sample consisted of sphere particles with the particles size around 50–80 nm, which is slightly larger than those calculated by Scherrer’s equation (see Table 1). The particle size is uniform, and no agglomeration could be observed (Figure 3). Table 1 shows that the specific surface area of catalyst is not well correlated with the crystal size.  Usually, the smaller the particle size, the higher the specific surface area. In this case, because of the organic compound adsorbed on the surface, the irregular correlation between the surface area and particle size was obtained.SEM images of SrTiO3 (a) and N-doped SrTiO3 synthesized by solvothermal reaction with 4 gram of HMT (b).
(a)(b)TEM images of SrTiO3 (a) and N-doped SrTiO3 synthesized by solvothermal reaction with 4 gram of HMT (b).
(a)(b)


### 3.4. DRS and FTIR

The UV-Vis absorption spectra of SrTiO3 and N-doped SrTiO3determined by diffuse reflectance analysis are shown in Figure 4(a).  SrTiO3 showed an absorption edge at 386 nm corresponding to the band gap energy 3.21 eV.  On the other hand, N-doped SrTiO3 showed new absorption edges, around 400–550 nm.  The absorption edges at 400–550 nm may be corresponding to the nitrogen-doped SrTiO3 as the electric transition from N2p to Ti3d. The absorption spectra at visible region were increased by increasing of HMT content in the reaction. The absorption spectra are also broad in the higher of wavelength more then 550 nm. It presumed that the absorption above 550 nm is due to oxygen vacancy. The replacing of O2- with N3- in N-doped SrTiO3 would result in the formation of anion defects for the charge compensation. Justicia and coworkers reported that the anion defects may lead to high visible light absorption ability of the sample [10]. Therefore, the anion defects formed by nitrogen doping seemed to contribute to the formation of the new band gaps of the sample.UV-vis DRS of SrTiO3 and N-doped SrTiO3 synthesized by solvothermal method with 1–4 gram of HMT (a) and FTIR spectra of SrTiO3 and N-doped SrTiO3 with 4 gram of HMT (b).
(a)(b)Figure4(b) shows FTIR spectra of SrTiO3 and N-doped SrTiO3 with 4 gram of HMT.  Broad absorption in the range of 500–900 cm-1 may be attributed to TiO6 octahedron stretching vibration [11, 12], and absorption at  3200–3400 is characteristic of OH- stretching vibration of surface hydroxyl group,  and little peak of 1630 cm-1 has been assigned to H–O–H bending vibration of physically adsorbed water [13, 14]. The vibration of Ti–N could not be observed because of small amount of nitrogen ion which replaced the oxygen ion.


### 3.5. XPS Analysis

Figure5 shows the global XPS spectrum and the detailed spectra of three areas in the XPS profile. The shift of binding energy was calibrated using C1s level at 284.6 eV as the internal standard. The energy peaks of Sr, C, Ti, O, and N could be observed from the global spectrum. The XPS spectrum for the titanium exhibits two different signals of Ti 2p3/2 and Ti 2p1/2 with binding energies at 457.8 eV and 463.3 eV, respectively. The peak position of Ti 2p3/2 corresponds to that of the Ti4+ oxidation state [15, 16]. The XPS spectra of O1s were observed at 529.1 eV which is the characteristic of metallic oxides [17].  The peak N1s could be observed at 399.2 eV which is assigned as nitrogen physically adsorbed on the surface. After sputtering, small peak at 397.5 could be observed which is assigned as the nitrogen-doped SrTiO3 [18]. The amount of nitrogen atomic fraction (N/Ti) after sputtering, 0.032, was lower than that before sputtering operation (0.064).XPS spectra of N-doped SrTiO3 synthesized by solvothermal method with 2 gram of HMT, calcined at 200°C in air: (a) global spectrum; (b) Ti2p; (c) O1s; (d) N1s, Ar+ sputtering was carried out at 3 kV for 3 minutes.
(a)(b)(c)(d)


### 3.6. Photocatalytic Activity

Figure6(a) shows the photocatalytic activities of SrTiO3 and N-doped SrTiO3 for the NOx elimination under irradiation of visible light (λ> 510 nm) (λ> 400 nm) and UV light (λ> 290 nm together with those of commercial TiO2 (Degussa P25). The mechanism of photocatalytic activity of NOx elimination is related to the electron/hole pairs formed by the photoexitation of catalyst.  In the presence of oxygen, the electron in the conduction band is trapped by the molecular oxygen to form ·O2-, which can generate active ·OOH radicals. The NOx reacts with ·OOH, O2, and very small amount of H2O in the air to produce HNO2 or HNO3 [19–21].Photocatalytic activities of SrTiO3 and N-doped SrTiO3 (with 4 gram of HMT) for the oxidative destruction of NOx under irradiation of various wavelength lights together with those of commercial TiO2 (a); photocatalytic activities of  N-doped SrTiO3 prepared with variation of HMT content for the oxidative destruction of NOx (b).
(a)(b)As expected from the large band gap energy, the photocatalytic activities of both SrTiO3 and commercial TiO2 under visible light irradiation (λ> 510 nm) were quite low, but N-doped SrTiO3 showed excellent activity. It was also notable that N-doped SrTiO3 showed photocatalytic activity superior to both SrTiO3 and commercial TiO2 even under UV-light irradiation (λ> 290 nm), indicating that the visible light responsive photocatalytic activity was induced without loss of the activity under UV-light irradiation by the solvothermal nitrogen doping in SrTiO3.Figure6(b) shows the effect of HMT concentration on the photocatalytic abilities. The optimum photocatalytic ability could be achieved at 4 gram of HMT and the addition of excess amount of HMT (up to 6 gram) resulted in decreasing the photocatalytic ability a little. The increase of the photocatalytic activity in the initial stage of nitrogen doping may be due to the positive effect to increase the visible light absorption ability, and the decrease of it by the excess amount of HMT addition may be due to the negative effect to increase the amount of lattice defects which act as the recombination center of photoinduced electrons and holes.Figure7 shows the effect of temperature on the photocatalytic ability. The photocatalytic ability under UV-light irradiation (λ> 290 nm and 400 nm) did not change so much even after heating at 400°C. In contrast, the activity under visible light irradiation was almost constant up to 200°C but greatly decreased by calcination above 300°C. It is because of the release of nitrogen ion doped in the lattice at high temperature.Figure 7
Photocatalytic activities of N-doped SrTiO3 with 4 gram of HMT followed by calcination at various temperatures.


## 3.1. Solvothermal Synthesis of N-Doped SrTiO3

Nitrogen-doped SrTiO3 was successfully synthesized by solvothermal reaction in KOH aqueous solution using tetraisopropoxide, Ti(OC3H7)4, and SrCl2·6H2O as the starting material and hexamethylenetetramine (HMT) as nitrogen source. It is well known that HMT could be degraded into ammonia and formaldehyde by heating in water above 70°C [9]. The ammonia is the key factor of nitrogen doping in catalyst synthesis. By the solvothermal reaction synthesis, ammonia could react with the starting material to produce the catalyst from bottom up. The ammonia decomposed from HMT was absorbed on the surface of developing and growing strontium titanate nanocrystal and reacted with activated strontia-titania surface, then generating the nitrogen doping in the solvothermal reaction. The yellow crystalline of N-doped SrTiO3 could be obtained. The reaction for the synthesis of N-doped SrTiO3 (1) can be described as
(1)Ti(OC3H7)4+2H2O→TiO2+4C3H7OHSrCl2·6H2O+2KOH→Sr(OH)2+2KCl+6H2OSr(OH)2+TiO2→SrTiO3+H2OC6H12N4+6H2O→6HCHO+4NH3SrTiO3+yNH3→SrTiO3-3y/2Ny□y/2+3y2H2O(□:latticedefect).


## 3.2. XRD Characterization

Figure1 shows the XRD pattern of undoped and N-doped SrTiO3 by solvothermal reactions at 200°C for 3 hours with variation of HMT content. All diffraction peaks could be assigned to the perovskite-type structure of SrTiO3 with cubic symmetry (JCPDS no. 79-0176). The diffraction peak position for N-doped SrTiO3 shifted to higher angle as shown in the insert of Figure 1. It indicated that the lattice constant decreased with nitrogen doping. Since the radius of O2- (1.40 Å) is smaller than N3- (1.71 Å), the decrease of lattice constant of SrTiO3 with nitrogen doping may be due to the formation of anion vacancy for charge compensation as SrTiO3-3y/2Ny□y/2(□:latticedefect).Figure 1
XRD patterns of sample prepared by solvothermal method, SrTiO3 (a), N-doped SrTiO3 with HMT of 1 gram (b), 2 gram (c), and 4 gram (d). The insert indicates the (110) peak shift due to nitrogen doping.The average crystallite sizes calculated by Scherrer’s Equation (2) using the full width at half maximum (FWHM) of the most intense peak (110) are also listed in Table 1 together with the specific surface areas
(2)D=0.9λBcosθ,
where D is the average crystallite size or particle size, λ the X-ray wavelength (0.15418 nm), θ the Bragg angle, and B the FWHM. The samples consisted of nanoparticles of 35–48 nm in diameter and specific surface area of 20.5–31.7 m2 g-1 and did not change so much with nitrogen doping and following calcination.Table 1
Crystallite size and surface area of SrTiO3 and N-doped SrTiO3.
PhotocatalystCrystal size (nm)Specific surface area (m2/g)SrTiO34029.51 gram of HMT4320.52 gram of HMT3828.54 gram of HMT3527.94 gram of HMT calcined at200°C3425.84 gram of HMT calcined at300°C3529.64 gram of HMT calcined at400°C4831.7


## 3.3. Morphology

The images of SEM of SrTiO3 and nitrogen-doped SrTiO3 are shown in Figure 2. The sample consisted of sphere particles with the particles size around 50–80 nm, which is slightly larger than those calculated by Scherrer’s equation (see Table 1). The particle size is uniform, and no agglomeration could be observed (Figure 3). Table 1 shows that the specific surface area of catalyst is not well correlated with the crystal size.  Usually, the smaller the particle size, the higher the specific surface area. In this case, because of the organic compound adsorbed on the surface, the irregular correlation between the surface area and particle size was obtained.SEM images of SrTiO3 (a) and N-doped SrTiO3 synthesized by solvothermal reaction with 4 gram of HMT (b).
(a)(b)TEM images of SrTiO3 (a) and N-doped SrTiO3 synthesized by solvothermal reaction with 4 gram of HMT (b).
(a)(b)


## 3.4. DRS and FTIR

The UV-Vis absorption spectra of SrTiO3 and N-doped SrTiO3determined by diffuse reflectance analysis are shown in Figure 4(a).  SrTiO3 showed an absorption edge at 386 nm corresponding to the band gap energy 3.21 eV.  On the other hand, N-doped SrTiO3 showed new absorption edges, around 400–550 nm.  The absorption edges at 400–550 nm may be corresponding to the nitrogen-doped SrTiO3 as the electric transition from N2p to Ti3d. The absorption spectra at visible region were increased by increasing of HMT content in the reaction. The absorption spectra are also broad in the higher of wavelength more then 550 nm. It presumed that the absorption above 550 nm is due to oxygen vacancy. The replacing of O2- with N3- in N-doped SrTiO3 would result in the formation of anion defects for the charge compensation. Justicia and coworkers reported that the anion defects may lead to high visible light absorption ability of the sample [10]. Therefore, the anion defects formed by nitrogen doping seemed to contribute to the formation of the new band gaps of the sample.UV-vis DRS of SrTiO3 and N-doped SrTiO3 synthesized by solvothermal method with 1–4 gram of HMT (a) and FTIR spectra of SrTiO3 and N-doped SrTiO3 with 4 gram of HMT (b).
(a)(b)Figure4(b) shows FTIR spectra of SrTiO3 and N-doped SrTiO3 with 4 gram of HMT.  Broad absorption in the range of 500–900 cm-1 may be attributed to TiO6 octahedron stretching vibration [11, 12], and absorption at  3200–3400 is characteristic of OH- stretching vibration of surface hydroxyl group,  and little peak of 1630 cm-1 has been assigned to H–O–H bending vibration of physically adsorbed water [13, 14]. The vibration of Ti–N could not be observed because of small amount of nitrogen ion which replaced the oxygen ion.


## 3.5. XPS Analysis

Figure5 shows the global XPS spectrum and the detailed spectra of three areas in the XPS profile. The shift of binding energy was calibrated using C1s level at 284.6 eV as the internal standard. The energy peaks of Sr, C, Ti, O, and N could be observed from the global spectrum. The XPS spectrum for the titanium exhibits two different signals of Ti 2p3/2 and Ti 2p1/2 with binding energies at 457.8 eV and 463.3 eV, respectively. The peak position of Ti 2p3/2 corresponds to that of the Ti4+ oxidation state [15, 16]. The XPS spectra of O1s were observed at 529.1 eV which is the characteristic of metallic oxides [17].  The peak N1s could be observed at 399.2 eV which is assigned as nitrogen physically adsorbed on the surface. After sputtering, small peak at 397.5 could be observed which is assigned as the nitrogen-doped SrTiO3 [18]. The amount of nitrogen atomic fraction (N/Ti) after sputtering, 0.032, was lower than that before sputtering operation (0.064).XPS spectra of N-doped SrTiO3 synthesized by solvothermal method with 2 gram of HMT, calcined at 200°C in air: (a) global spectrum; (b) Ti2p; (c) O1s; (d) N1s, Ar+ sputtering was carried out at 3 kV for 3 minutes.
(a)(b)(c)(d)


## 3.6. Photocatalytic Activity

Figure6(a) shows the photocatalytic activities of SrTiO3 and N-doped SrTiO3 for the NOx elimination under irradiation of visible light (λ> 510 nm) (λ> 400 nm) and UV light (λ> 290 nm together with those of commercial TiO2 (Degussa P25). The mechanism of photocatalytic activity of NOx elimination is related to the electron/hole pairs formed by the photoexitation of catalyst.  In the presence of oxygen, the electron in the conduction band is trapped by the molecular oxygen to form ·O2-, which can generate active ·OOH radicals. The NOx reacts with ·OOH, O2, and very small amount of H2O in the air to produce HNO2 or HNO3 [19–21].Photocatalytic activities of SrTiO3 and N-doped SrTiO3 (with 4 gram of HMT) for the oxidative destruction of NOx under irradiation of various wavelength lights together with those of commercial TiO2 (a); photocatalytic activities of  N-doped SrTiO3 prepared with variation of HMT content for the oxidative destruction of NOx (b).
(a)(b)As expected from the large band gap energy, the photocatalytic activities of both SrTiO3 and commercial TiO2 under visible light irradiation (λ> 510 nm) were quite low, but N-doped SrTiO3 showed excellent activity. It was also notable that N-doped SrTiO3 showed photocatalytic activity superior to both SrTiO3 and commercial TiO2 even under UV-light irradiation (λ> 290 nm), indicating that the visible light responsive photocatalytic activity was induced without loss of the activity under UV-light irradiation by the solvothermal nitrogen doping in SrTiO3.Figure6(b) shows the effect of HMT concentration on the photocatalytic abilities. The optimum photocatalytic ability could be achieved at 4 gram of HMT and the addition of excess amount of HMT (up to 6 gram) resulted in decreasing the photocatalytic ability a little. The increase of the photocatalytic activity in the initial stage of nitrogen doping may be due to the positive effect to increase the visible light absorption ability, and the decrease of it by the excess amount of HMT addition may be due to the negative effect to increase the amount of lattice defects which act as the recombination center of photoinduced electrons and holes.Figure7 shows the effect of temperature on the photocatalytic ability. The photocatalytic ability under UV-light irradiation (λ> 290 nm and 400 nm) did not change so much even after heating at 400°C. In contrast, the activity under visible light irradiation was almost constant up to 200°C but greatly decreased by calcination above 300°C. It is because of the release of nitrogen ion doped in the lattice at high temperature.Figure 7
Photocatalytic activities of N-doped SrTiO3 with 4 gram of HMT followed by calcination at various temperatures.


## 4. Conclusions

Perovskite-type N-doped SrTiO3 powder was successfully synthesized by solvothermal method using HMT as nitrogen source. The products consisted of spherical nanoparticles of 50–80 nm in diameter. N-doped SrTiO3 showed excellent photocatalytic activity under both UV and visible light irradiation, that is, the photocatalytic activity of N-doped SrTiO3 for DeNOx reaction was greater than that of SrTiO3 or TiO2 (Degussa P-25) in both visible light region (>510 nm) and UV light region (<290 nm). The high visible light photocatalytic activity of this substance is caused by a generation of a new band gap that absorbs visible light.



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*Source: 629727-2010-09-02.xml*