# The Contrastive Research in the Photocatalytic Activity of BiOBr Synthesized by Different Reactants

Authors: Wang Ling-Li; Ma Wan-Hong; Wang Shu-Lian; Zhang Yu; Jia Man-Ke; Li Rui-Ping; Zhang Ai-Qing; Huang Ying-Ping
Journal: Journal of Nanomaterials
 (2012)

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## Abstract

BiOBr nanoplates, marked asα-BiOBr and β-BiOBr, were synthesized via hydrothermal method using cetylpyridinium bromide (CPB) and NaBr as reactants, respectively. X-Ray Diffraction (XRD), transmission electron microscope (TEM), N2 adsorption/desorption, UV-visible diffuse reflectance spectroscopy (UV-Vis DRS), and cyclic voltammetry (CV) were employed to characterize the obtained BiOBr. The results showed that α-BiOBr and β-BiOBr can absorb visible light and both the band gaps of them were about 2.76 eV. Under visible light irradiation, the photodegradation of organic dye sulforhodamine (SRB) and salicylic acid (SA) using α-BiOBr and β-BiOBr as the catalysts was carried out. The reaction kinetic constants of the degradation of SRB by α-BiOBr and β-BiOBr were 0.00602 min−1 and 0.0047 min−1, respectively, which indicated that the photocatalytic activity of α-BiOBr was higher than that of β-BiOBr. The UV-Vis DRS and total organic carbon (TOC) were also monitored, and the TOC removal rate of α-BiOBr and β-BiOBr was 86% and 48%, respectively. At the same time, hydrogen peroxide (H2O2) and active radicals were measured and analyzed, which showed that the main active species was OH∙ during the photocatalytic reaction.


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## Body

## 1. Introduction

The bismuth oxyhalides (BiOX, X = F, Cl, Br, I) are a new family of semiconductor materials which have unique electronic structures, good optical properties, and catalytic performances, thus attract the interest of researchers [1, 2]. Among them, the band gap of BiOBr [3–5] belongs to the visible region, so it is able to effectively use sunlight to degrade pollutants and overcome the shortage of the first-generation catalyst represented by TiO2 such as a low efficiency of solar energy and the strictly limited practical applications [6–8]. BiOBr is a semiconductor with highly anisotropic layered structure, and its electronic structure and band structure have been calculated through the DFT (density functional theory) method [9] and the TB-LMTO (tight-binding linear muffin-tin orbital) method [10]. The results indicated that BiOBr was the indirect transition band gap semiconductor, which in favor of hole-electron effective separation and charge transfer, so that BiOBr revealed a high photocatalytic activity.The photocatalytic activity of semiconductor has a strong dependence on its particle size and morphology, so the synthesis of nanoparticles with a small size and shape is significant. Nowadays, the common methods to prepare nano-BiOBr include hydrolysis method [11], soft-template method [12, 13], hydrothermal method [14, 15], and high-temperature solid-state method [16]. Introducing templates in preparation of catalysts is an effective technology to control the size and morphology. Templates provide a microreactor to control the prepared materials with same size and single scattered pore structure. So selecting a suitable template to synthesis BiOBr is an effective method to improve its catalytic activity. Cetyltrimethyl ammonium bromide (CTAB) [17, 18] is the most universal templates introduced in synthesis systems because it can be regarded as bromine sources and template simultaneously. But CPB which has the semblable effect with CTAB is seldom used to synthesis BiOBr. Herein, CPB is served as template and bromine sources to prepare BiOBr which compared with BiOBr synthesized using NaBr as bromine source, and the products were denoted as α-BiOBr and β-BiOBr. The physical properties of products were characterized, and the photocatalytic activities of the two products were contrasted via degrading sulforhodamine (SRB) and salicylic acid (SA) under visible light irradiation. In the end, the photocatalytic mechanism of BiOBr photocatalysis was inferred via analyzing the active species during the catalytic process.


## 2. Experimental

### 2.1. Reagents and Instruments

Bismuth nitride (Bi(NO3)3·5H2O) NaBr and CPB were of A.R. grade from the Beijing Chemical Factory (China). The dye sulforhodamine-B was of spec-pure grade (Across). Horseradish peroxidase (POD) was purchased from Lizhudongfeng Biologic Technique, and N, N-diethylphenylenediamine (DPD) reagent was purchased from Merck. Other chemicals were of reagent grade and used without further purification. Deionized and doubly distilled water was used throughout the investigation. The following were also used.JEM-2010 transmission electron microscopy (TEM) (Japan, JEOL); N/C 2100 TOC analyzer (Germany, Jena); F-4500 fluorescence spectrometer (Japan, Hitachi); Lambda25 UV-visible spectrophotometer (U.S., PE); PHs-P pH meter (Mettler-Toledo Instruments Co., Ltd.); U-3010 UV spectrophotometer (Japan, Hitachi); 360 FTIR spectrometer (USA, Nicolet); ASAP 2020 model BET surface area and pore size analyzer (USA, Micrometritics); D8ADVANCE X-ray diffraction (Germany); ESR 300E spectrometer (Germany, Bruker); High performance liquid chromatograph (USA, Waters); AUTOLAB Electrochemical workstation (China, Chenhua).


### 2.2. Preparation of Nano-BiOBr

Bi(NO3)3 · 5H2O solution was added dropwise to CPB solution (nBi:nBr=2:3). The mix solution was stirred for 60 min and then transferred to a Teflon-lined autoclave to react for 17 h at 170°C. When it was cooled to the room temperature, the product was centrifuged and washed with water and ethanol for many times, respectively, dried in a vacuum box for 5 h, thus the photocatalyst was obtained and denoted as α-BiOBr.As the above method, only CPB was converted into the same amount of NaBr, and other conditions did not be changed. The obtained product was recorded asβ-BiOBr.


### 2.3. Characterization

X-ray diffraction (XRD) patterns were conducted on a DMAX 2500 diffractometer equipped with a CuKα radiation at a scanning speed of 5°/min ranging from 5 to 80°. Transmission electron microscopy (TEM) patterns were performed on a JEOL JEM-2010 electron microscope with a field emission gun operating at 200 kV. N2 adsorption-desorption isotherms were performed with a Quanta chrome Autosorb1-C system at 196°C; the data were analyzed by the BET method. The UV-Vis spectroscopy was recorded at room temperature on a Hitachi UV-3010 spectrophotometer from 200 to 800 nm.Cyclic voltammetry (CV) was carried out using Pt wire as the counter electrode, calomel electrode as the reference electrode, and glassy carbon electrode daubed BiOBr thin film as the working electrode. The electrolyte used was a solution of 0.2 mol/L Na2SO4. The measurements were conducted on AUTOLAB Electrochemical Workstation. The potential scan range was from −1.0 V to +1.0 V. The scan rate was 50 mv/s and scan cycle was 4 times.


### 2.4. Photocatalytic Processes and Analytical Methods

The degradation of organic dye SRB was utilized to characterize the photocatalytic activity of the various photocatalysts. 50 mL of 1.5 × 10−5 mol/L SRB aqueous solution containing 10 mg BiOBr was added in 70 mL cylindrical rigid glass. The pH was adjusted to 3 with HClO4 solution (1.0 mol/L). Prior to irradiation, the suspension was stirred for 1 h to achieve adsorption/desorption equilibrium. The system was irradiated under visible light (λ>420 nm). And the solution was sampled at diverse intervals. The liquid was centrifuged and the absorbance of the liquid was measured on a spectrophotometer (maximum absorbance at 565 nm). The A/A0~t curve was plotted to the wavelength, where A0, A were absorbance of SRB at the initial and at reaction time t, respectively.Determination of H2O2 [19]: 30 uL of 0.1% POD solution, 1 mL of KH2PO4-NaOH buffer solution (pH 6.8), 150 uL of 1.0% DPD solution, and 1 mL of reaction solution collected at different time intervals were added successively to 10 mL colorimetric tubes. The volume was constant at 5 mL. After centrifugation, the absorbance was determined at 510 nm.The oxidative active radicals produced in the process of reaction were measured with the ESR method [20]. DMPO was used to capture paramagnetic species, and the ESR signals were recorded at room temperature. In order to reduce the experimental error, the same root quartz capillary was used during the whole process of measuring ESR. The measured parameters of free radicals were gained by direct measuring magnetic field and microwave frequency.The TOC changes in different photocatalytic response time were measured with the N/C 2100TOC.The infrared spectroscopy (IR) of photocatalytic reaction solution for 0 h, 1 h, 4 h, 8 h was evaporated in rotary evaporator with potassium bromide at 60°C. Then the samples were dried and measured on an infrared spectrometer.Photocatalytic degradation of SA: in 70 mL glass cylindrical hard, 25 mL SA that contained 20 mg BiOBr was placed in dark 2 h to achieve the adsorption/desorption equilibrium. Then the solution was illuminated in visible light (λ>420 nm) and carried out at different intervals. The concentration changes of samples were analyzed by high performance liquid chromatography analysis with a Waters 2998 photodiode array (PDA) detector and a C18 reverse-phase column (4.6 mm i.d. × 150 mm, kromasil). The mobile phase was methanol and phosphate (0.01 moL/L, pH 3.5), and the ratio was 45 : 55. The inject volume of the sample was 20 μL and the flow rate was 0.70 mL/min. The detection wavelength was 278 nm.


## 2.1. Reagents and Instruments

Bismuth nitride (Bi(NO3)3·5H2O) NaBr and CPB were of A.R. grade from the Beijing Chemical Factory (China). The dye sulforhodamine-B was of spec-pure grade (Across). Horseradish peroxidase (POD) was purchased from Lizhudongfeng Biologic Technique, and N, N-diethylphenylenediamine (DPD) reagent was purchased from Merck. Other chemicals were of reagent grade and used without further purification. Deionized and doubly distilled water was used throughout the investigation. The following were also used.JEM-2010 transmission electron microscopy (TEM) (Japan, JEOL); N/C 2100 TOC analyzer (Germany, Jena); F-4500 fluorescence spectrometer (Japan, Hitachi); Lambda25 UV-visible spectrophotometer (U.S., PE); PHs-P pH meter (Mettler-Toledo Instruments Co., Ltd.); U-3010 UV spectrophotometer (Japan, Hitachi); 360 FTIR spectrometer (USA, Nicolet); ASAP 2020 model BET surface area and pore size analyzer (USA, Micrometritics); D8ADVANCE X-ray diffraction (Germany); ESR 300E spectrometer (Germany, Bruker); High performance liquid chromatograph (USA, Waters); AUTOLAB Electrochemical workstation (China, Chenhua).


## 2.2. Preparation of Nano-BiOBr

Bi(NO3)3 · 5H2O solution was added dropwise to CPB solution (nBi:nBr=2:3). The mix solution was stirred for 60 min and then transferred to a Teflon-lined autoclave to react for 17 h at 170°C. When it was cooled to the room temperature, the product was centrifuged and washed with water and ethanol for many times, respectively, dried in a vacuum box for 5 h, thus the photocatalyst was obtained and denoted as α-BiOBr.As the above method, only CPB was converted into the same amount of NaBr, and other conditions did not be changed. The obtained product was recorded asβ-BiOBr.


## 2.3. Characterization

X-ray diffraction (XRD) patterns were conducted on a DMAX 2500 diffractometer equipped with a CuKα radiation at a scanning speed of 5°/min ranging from 5 to 80°. Transmission electron microscopy (TEM) patterns were performed on a JEOL JEM-2010 electron microscope with a field emission gun operating at 200 kV. N2 adsorption-desorption isotherms were performed with a Quanta chrome Autosorb1-C system at 196°C; the data were analyzed by the BET method. The UV-Vis spectroscopy was recorded at room temperature on a Hitachi UV-3010 spectrophotometer from 200 to 800 nm.Cyclic voltammetry (CV) was carried out using Pt wire as the counter electrode, calomel electrode as the reference electrode, and glassy carbon electrode daubed BiOBr thin film as the working electrode. The electrolyte used was a solution of 0.2 mol/L Na2SO4. The measurements were conducted on AUTOLAB Electrochemical Workstation. The potential scan range was from −1.0 V to +1.0 V. The scan rate was 50 mv/s and scan cycle was 4 times.


## 2.4. Photocatalytic Processes and Analytical Methods

The degradation of organic dye SRB was utilized to characterize the photocatalytic activity of the various photocatalysts. 50 mL of 1.5 × 10−5 mol/L SRB aqueous solution containing 10 mg BiOBr was added in 70 mL cylindrical rigid glass. The pH was adjusted to 3 with HClO4 solution (1.0 mol/L). Prior to irradiation, the suspension was stirred for 1 h to achieve adsorption/desorption equilibrium. The system was irradiated under visible light (λ>420 nm). And the solution was sampled at diverse intervals. The liquid was centrifuged and the absorbance of the liquid was measured on a spectrophotometer (maximum absorbance at 565 nm). The A/A0~t curve was plotted to the wavelength, where A0, A were absorbance of SRB at the initial and at reaction time t, respectively.Determination of H2O2 [19]: 30 uL of 0.1% POD solution, 1 mL of KH2PO4-NaOH buffer solution (pH 6.8), 150 uL of 1.0% DPD solution, and 1 mL of reaction solution collected at different time intervals were added successively to 10 mL colorimetric tubes. The volume was constant at 5 mL. After centrifugation, the absorbance was determined at 510 nm.The oxidative active radicals produced in the process of reaction were measured with the ESR method [20]. DMPO was used to capture paramagnetic species, and the ESR signals were recorded at room temperature. In order to reduce the experimental error, the same root quartz capillary was used during the whole process of measuring ESR. The measured parameters of free radicals were gained by direct measuring magnetic field and microwave frequency.The TOC changes in different photocatalytic response time were measured with the N/C 2100TOC.The infrared spectroscopy (IR) of photocatalytic reaction solution for 0 h, 1 h, 4 h, 8 h was evaporated in rotary evaporator with potassium bromide at 60°C. Then the samples were dried and measured on an infrared spectrometer.Photocatalytic degradation of SA: in 70 mL glass cylindrical hard, 25 mL SA that contained 20 mg BiOBr was placed in dark 2 h to achieve the adsorption/desorption equilibrium. Then the solution was illuminated in visible light (λ>420 nm) and carried out at different intervals. The concentration changes of samples were analyzed by high performance liquid chromatography analysis with a Waters 2998 photodiode array (PDA) detector and a C18 reverse-phase column (4.6 mm i.d. × 150 mm, kromasil). The mobile phase was methanol and phosphate (0.01 moL/L, pH 3.5), and the ratio was 45 : 55. The inject volume of the sample was 20 μL and the flow rate was 0.70 mL/min. The detection wavelength was 278 nm.


## 3. Results and Discussion

### 3.1. Characterization of Catalyst

#### 3.1.1. XRD Analysis

Figure1 shows the XRD patterns of BiOBr. It showed that the diffraction peaks of α-BiOBr and β-BiOBr accorded well with the diffraction peak of P4/nmm BiOBr (JCPDS 073-2061). No impurity peak in the XRD patterns indicates the high purity of the samples. Furthermore, the intense peak intensity of two products illustrates the high crystallinity of products and the as-prepared α-BiOBr was better crystallized than β-BiOBr.Figure 1
X-Ray diffraction pattern of BiOBr. (a)β-BiOBr; (b) α-BiOBr.


#### 3.1.2. TEM Analysis

The TEM images of the products are shown in Figure2. From Figure 2(a), α-BiOBr is layered nanosheet with uniform morphology and smooth surface and, the width of α-BiOBr is approximately 150 nm. Figure 2(b) shows that β-BiOBr is also neat and smooth layered nanopiece. The size of β-BiOBr is approximately 400 nm, bigger than α-BiOBr. This may attribute to that the surfactant CPB can form a reactor with specific size and morphology in the preparation process, which can control the particle size and morphology of the products in some extent.TEM images of BiOBr.
(a)
α-BiOBr
(b)
β-BiOBr


#### 3.1.3. BET Analysis

The surface area is an important key on the photocatalytic activities of the photocatalysts generally, the smaller size of the photocatalyst, the larger specific surface area, and the more active sites on granular surface, thus the activity of catalyst can be improved. Figure3 shows the nitrogen adsorption-desorption isothermal curves of BiOBr prepared by two methods. The curves of two products in low pressure region are quite gentle. The adsorption increased slowly with the increase of P/P0 indicating N2 monolayer adsorption on hole wall in this stage. When P/P0 was 0.9–1.0, the adsorption sharply increased and produced sudden jump, which was caused by the capillary condensing phenomenon of N2 in the mesoporous. The slope of N2 adsorption curve in this stage could be served to measure the homogeneity of mesoporous, and the greater the absolute value of the curve slope, the narrower the pore distribution [21]. Both the slopes of curves (a) and (b) were very great, accounting for that the pore diameter distributions of them were narrow. The curves in two pictures were similar which indicated that the morphology, pore size, and surface area of two products were similar, but the specific surface area of α-BiOBr and β-BiOBr are different, which were about 4.706 m2/g and 0.8524 m2/g, respectively. So α-BiOBr had a larger specific surface area, which may be beneficial to reduce the electron-hole recombination.N2 adsorption-desorption isotherms of BiOBr.
(a)
α-BiOBr
(b)
β-BiOBr


#### 3.1.4. UV-Vis Diffuse Reflectance Spectral Analysis

The UV-Vis diffuse reflectance spectral ofα-BiOBr and β-BiOBr in the range of 200–700 nm was shown in Figure 4. The absorption peaks of products are steep and had strong absorption, which indicates that the absorption band of BiOBr is not attributed to the transition from impurity band to the conduction band but directly internally converted from the valence band to the conduction band [22]. Both The absorption threshold of α-BiOBr and β-BiOBr was 450 nm, and the band gap of them was 2.76 eV calculated by the formula of λg=1239.18/Eg.Figure 4
UV-Vis diffuse reflectance spectral ofα-BiOBr and β-BiOBr.


### 3.2. Photodegradation of SRB by BiOBr

#### 3.2.1. Comparison of Degrading SRB with BiOBr Prepared by Different Methods

Under the identical conditions, SRB was degraded byα-BiOBr and β-BiOBr (Figure 5). SRB cannot be degraded by the two catalysts in absence of light (curve b and c) or under visible light without catalysts (curve a). However, SRB can be degraded in presence of the two catalysts under visible light, and the degradation efficiency of α-BiOBr was far better than that of β-BiOBr. The reaction kinetic constants of photodegradation of SRB by α-BiOBr and β-BiOBr were 0.00602 min−1 (curve e) and 0.0047 min−1 (curve d), respectively.Figure 5
Photocatalytic degradation of SRB in different systems, (SRB) = 1.5 × 10−5 mol/L, (BiOBr) = 0.2 g/L, pH = 3, (a) SRB/Vis; (b) β-BiOBr/SRB/Dark; (c) α-BiOBr/SRB/Dark; (d) β-BiOBr/SRB/Vis; (e) α-BiOBr/SRB/Vis.


#### 3.2.2. The Optimization of Degrading SRB

Photocatalytic reactions mainly occur on the surface of the catalyst, therefore the intrinsic characteristic of the surface determines the photocatalytic activity. But reactions also can be significantly affected by surroundings. The influences of catalyst dosage and pH on the degradation of SRB byα-BiOBr were discussed. The solution pH has great effect on the surface charge of catalyst, pollutants molecules charge, adsorption of contaminants on catalyst surface, hydroxyl concentration, and so on, which affect the degradation efficiency. Figure 6 showed the degradation of SRB under different pHs. α-BiOBr had the best catalytic activity when pH was about 2. With the increase of pH, the degradation rates reduced gradually, but the activity reduced when pH was less than 2. In addition, catalyst in the neutral and alkaline solution hardly degraded SRB. This showed at the catalytic activity of BiOBr in acidic environment was far better than that in the neutral and alkaline conditions. The probable reason was that the isoelectric point of the BiOBr is in the acidic range and its surface is negatively charged. BiOBr cannot combine dye easily when pH is larger, so the degradation rates were very small in basic and neutral solution. Figure 7 showed the influence of catalyst dosage on the catalytic efficiency. The degradation rates increased with the catalytic concentration. When the dosage was 0.8 g/L, BiOBr had the best catalytic efficiency. If the amount of catalyst continued to increase, the degradation rate unchanged and even decreased. It may be attributed to active centers provided by BiOBr increase with the amount of catalyst, so BiOBr can absorb more photons and pollutants to efficiently degrade SRB. However, when the catalyst dosage is too much, the scattering effect enhances and the efficient absorption of light reduces, so the degradation efficiency declines [23].Figure 6
Effect of pH, (SRB) = 1.5 × 10−5 mol/L, (BiOBr) = 0.2 g/L.Figure 7
Effect of catalyst dosage, (SRB) = 1.5 × 10−5 mol/L, pH = 2.


#### 3.2.3. Degradation of SRB under the Optimum Conditions

The degradation of SRB under the optimum conditions (pH = 2, [BiOBr] = 0.8 g/L) was presented in Figure8. The characteristic absorption peak (λ=565 nm) of SRB decreased constantly and showed a blue shift, which demonstrated that the conjugated structure of SRB decreased and the molecule suffered destruction. After 150 min, the absorption of SRB in visible light disappeared completely and the decoloration rate reached 100%.Figure 8
Temporal UV-Vis spectra changes of SRB, (SRB) = 1.5 × 10−5 mol/L, (BiOBr) = 0.8 g/L, pH = 2.


#### 3.2.4.  Cyclic Photocatalytic Degradation of SRB

The stability and reusability of semiconductors are important parameters to measure their practical value. In order to discuss the stability and repeatable usability of BiOBr,α-BiOBr was used to circularly degrade SRB under the optimum conditions (Figure 9). After recycling for 5 times, the degradation efficiency of SRB did not reduce obviously. BiOBr could completely degrade SRB after 100 min, which indicated BiOBr has good stability, reusability, and application potential.Figure 9
The degradation curve of SRB during multicycle degradation process, (SRB) = 1.5 × 10−5 mol/L, (BiOBr) = 0.8 g/L, pH = 2.


### 3.3. The Measurement of Intermediate Products during the Degradation of SRB

#### 3.3.1. The Measurement of H2O2

The change of H2O2 in the degradation of SRB by α-BiOBr and β-BiOBr was measured by DPD method. As shown in Figure 10, H2O2 did not generate in the dark in presence of α-BiOBr and β-BiOBr (curve c and d). Under visible light irradiation, BiOBr was stimulated to produce electrons and holes, which reacted with dissolved oxygen and water adsorbed on the surface of catalysts to produce H2O2. At the beginning of reaction, H2O2 was accumulated and then gradually consumed to resolve into OH∙ which had better oxidizability to degrade SRB. During the accumulation stage, the generation rate of H2O2 in α-BiOBr/SRB system (curve b) is larger than that in β-BiOBr/SRB system (curve a). The degradation rate of SRB in the former system is larger than that in the latter system, so H2O2 is consumed more rapidly and the total amount of H2O2 is less.Figure 10
Changes of H2O2 during the degradation process of SRB, (a) β-BiOBr/SRB/Vis; (b) α-BiOBr/SRB/Vis; (c) α-BiOBr/SRB/Dark; (d) β-BiOBr/SRB/Vis, (SRB) = 1.5 × 10−5 mol/L, (BiOBr) = 0.8 g/L, pH = 2.


#### 3.3.2. The Measurement of Active Species

The oxidation species involved in photocatalytic oxidation reaction are mainlyOH∙ and O2∙-, which have high oxidation potential and can oxidize almost all organic compounds. The ESR technology is a very effective method to measure the short life of the radicals. Figure 11 showed the characteristic signal peak of DMPO–OH∙ and DMPO–O2∙- in different systems. The characteristic quartet peaks of DMPO–OH∙ adducts with an intensity ratio of 1 : 2 : 2 : 1 appeared, which showed that OH∙ is generated in the catalytic oxidation process of SRB by BiOBr, and that the catalytic mechanism mainly involved the OH∙ oxidation mechanism. The ESR signals of DMPO–O2∙- adducts were also observed in the system under visible radiation (Figure 11), but the intensity of the signal was faint, which indicated that O2∙- was also produced under visible light, but the main oxidation species was OH∙.ESR signals of the DMPO-OH∙ adducts (a) and DMPO-O2∙- adducts (b).
(a)
(b)


#### 3.3.3. The Deep Mineralization of SRB

Figure12 showed the changes of total organic carbon (TOC) in the degradation process of SRB. From the results, the TOC value gradually reduced. Under the same reaction conditions, the TOC removal rates of SRB degraded with α-BiOBr and β-BiOBr are 86% and 48%, respectively, after 900 min, which demonstrated that BiOBr prepared with CPB has a better mineralization of pollutants.Figure 12
TOC removals during the degradation process of SRB, (a)α-BiOBr/SRB/Vis; (b) β-BiOBr/SRB/Vis, (SRB) = 3.0 × 10−5 mol/L, (BiOBr) = 0.8 g/L, pH = 2.


#### 3.3.4. IR Analysis

Figure13 presented the IR spectrum of SRB degraded by α-BiOBr in different photocatalytic reaction time. It is known that the bands at 1460, 1500, 1580, and 1600 cm−1 are corresponded to the stretching vibration of benzenes in SRB molecules and the band at 1649 cm−1 is due to the vibration of C–N stretching. The band at 1460~1508 cm−1 is caused by the vibration of the heterocycles in dye molecules. The band at 1330 cm−1 is due to the vibration of C–Ar peak, and the bands at 1120 cm−1 and 665~620 cm−1 are attributed to the vibration of the –SO3 − functional groups. With the increase of reaction time, some characteristic peaks of SRB disappeared, and new peaks at 1650 cm−1 and 1400 cm−1, attributed to the vibration of C=O expansive and diethylamine–CH3, appeared gradually. The results showed that the conjugate structure of SRB was damaged during the process of catalytic degradation and further demonstrated that SRB was not only simply discolored, but also deeply degrade.Figure 13
IR analysis of degrading SRB, (SRB) = 3.0 × 10−5 mol/L, (BiOBr) = 0.8 g/L, pH = 2.


#### 3.3.5. CV Analysis

Cyclic voltammetry provides a wealth of information in researching electrode process via analyzing the shape of the scanning curve [24], which can account for the photocatalytic phenomenon. Figure 14 was the current-voltage curves of two products under the same condition. α-BiOBr had two pairs of redox peaks. The oxidation potential was 0.126 V and 0.407 V and reduction potential was 0.259 V and 0.441 V. While β-BiOBr only had a pair of redox peak. The oxidation and reduction peaks were 0.259 V and 0.436 V, respectively. This showed that there are two different electronic transfer between the two different valence states of α-BiOBr which may react two redox reactions; while β-BiOBr only react one redox reaction. And it also showed that the transformation of electrons on α-BiOBr surface is more easy than that on β-BiOBr, thus the photocatalytic activity of α-BiOBr is higher than β-BiOBr.The cyclic voltammetry of BiOBr.
(a)
α-BiOBr
(b)
β-BiOBr


### 3.4. Photocatalytic Degradation of Salicylic Acid

Salicylic acid (SA) is a kind of small colorless molecule which has no absorption in visible light, so it is usually used to characterize the visible photoreactivity of photocatalysts. The degradation of SA was under the illumination of visible light (λ≥420 nm) and the concentration of it was measured by HPLC (Figure 15). Curve a showed that SA was not photodissociated under visible irradiation. Curve b and c showed that α-BiOBr and β-BiOBr can adsorb little amount of SA. Curve d and e represented the degradation of SA by α-BiOBr and β-BiOBr under visible light. After 8 h, the degradation rates of SA by α-BiOBr and β-BiOBr were 97% and 37.3%, respectively. The results further indicated that α-BiOBr had a better catalytic activity than β-BiOBr and could be stimulated effectively by visible light to degrade small molecular pollutants.Figure 15
Photodegradation of SA, (a) SA/Vis; (b)β-BiOBr/SA/Dark; (c) α-BiOBr/SA/Dark; (d) β-BiOBr/SA/Vis; (e) α-BiOBr/SA/Vis, (SA) = 5 m mol/L, (BiOBr) = 0.8 g/L.


## 3.1. Characterization of Catalyst

### 3.1.1. XRD Analysis

Figure1 shows the XRD patterns of BiOBr. It showed that the diffraction peaks of α-BiOBr and β-BiOBr accorded well with the diffraction peak of P4/nmm BiOBr (JCPDS 073-2061). No impurity peak in the XRD patterns indicates the high purity of the samples. Furthermore, the intense peak intensity of two products illustrates the high crystallinity of products and the as-prepared α-BiOBr was better crystallized than β-BiOBr.Figure 1
X-Ray diffraction pattern of BiOBr. (a)β-BiOBr; (b) α-BiOBr.


### 3.1.2. TEM Analysis

The TEM images of the products are shown in Figure2. From Figure 2(a), α-BiOBr is layered nanosheet with uniform morphology and smooth surface and, the width of α-BiOBr is approximately 150 nm. Figure 2(b) shows that β-BiOBr is also neat and smooth layered nanopiece. The size of β-BiOBr is approximately 400 nm, bigger than α-BiOBr. This may attribute to that the surfactant CPB can form a reactor with specific size and morphology in the preparation process, which can control the particle size and morphology of the products in some extent.TEM images of BiOBr.
(a)
α-BiOBr
(b)
β-BiOBr


### 3.1.3. BET Analysis

The surface area is an important key on the photocatalytic activities of the photocatalysts generally, the smaller size of the photocatalyst, the larger specific surface area, and the more active sites on granular surface, thus the activity of catalyst can be improved. Figure3 shows the nitrogen adsorption-desorption isothermal curves of BiOBr prepared by two methods. The curves of two products in low pressure region are quite gentle. The adsorption increased slowly with the increase of P/P0 indicating N2 monolayer adsorption on hole wall in this stage. When P/P0 was 0.9–1.0, the adsorption sharply increased and produced sudden jump, which was caused by the capillary condensing phenomenon of N2 in the mesoporous. The slope of N2 adsorption curve in this stage could be served to measure the homogeneity of mesoporous, and the greater the absolute value of the curve slope, the narrower the pore distribution [21]. Both the slopes of curves (a) and (b) were very great, accounting for that the pore diameter distributions of them were narrow. The curves in two pictures were similar which indicated that the morphology, pore size, and surface area of two products were similar, but the specific surface area of α-BiOBr and β-BiOBr are different, which were about 4.706 m2/g and 0.8524 m2/g, respectively. So α-BiOBr had a larger specific surface area, which may be beneficial to reduce the electron-hole recombination.N2 adsorption-desorption isotherms of BiOBr.
(a)
α-BiOBr
(b)
β-BiOBr


### 3.1.4. UV-Vis Diffuse Reflectance Spectral Analysis

The UV-Vis diffuse reflectance spectral ofα-BiOBr and β-BiOBr in the range of 200–700 nm was shown in Figure 4. The absorption peaks of products are steep and had strong absorption, which indicates that the absorption band of BiOBr is not attributed to the transition from impurity band to the conduction band but directly internally converted from the valence band to the conduction band [22]. Both The absorption threshold of α-BiOBr and β-BiOBr was 450 nm, and the band gap of them was 2.76 eV calculated by the formula of λg=1239.18/Eg.Figure 4
UV-Vis diffuse reflectance spectral ofα-BiOBr and β-BiOBr.


## 3.1.1. XRD Analysis

Figure1 shows the XRD patterns of BiOBr. It showed that the diffraction peaks of α-BiOBr and β-BiOBr accorded well with the diffraction peak of P4/nmm BiOBr (JCPDS 073-2061). No impurity peak in the XRD patterns indicates the high purity of the samples. Furthermore, the intense peak intensity of two products illustrates the high crystallinity of products and the as-prepared α-BiOBr was better crystallized than β-BiOBr.Figure 1
X-Ray diffraction pattern of BiOBr. (a)β-BiOBr; (b) α-BiOBr.


## 3.1.2. TEM Analysis

The TEM images of the products are shown in Figure2. From Figure 2(a), α-BiOBr is layered nanosheet with uniform morphology and smooth surface and, the width of α-BiOBr is approximately 150 nm. Figure 2(b) shows that β-BiOBr is also neat and smooth layered nanopiece. The size of β-BiOBr is approximately 400 nm, bigger than α-BiOBr. This may attribute to that the surfactant CPB can form a reactor with specific size and morphology in the preparation process, which can control the particle size and morphology of the products in some extent.TEM images of BiOBr.
(a)
α-BiOBr
(b)
β-BiOBr


## 3.1.3. BET Analysis

The surface area is an important key on the photocatalytic activities of the photocatalysts generally, the smaller size of the photocatalyst, the larger specific surface area, and the more active sites on granular surface, thus the activity of catalyst can be improved. Figure3 shows the nitrogen adsorption-desorption isothermal curves of BiOBr prepared by two methods. The curves of two products in low pressure region are quite gentle. The adsorption increased slowly with the increase of P/P0 indicating N2 monolayer adsorption on hole wall in this stage. When P/P0 was 0.9–1.0, the adsorption sharply increased and produced sudden jump, which was caused by the capillary condensing phenomenon of N2 in the mesoporous. The slope of N2 adsorption curve in this stage could be served to measure the homogeneity of mesoporous, and the greater the absolute value of the curve slope, the narrower the pore distribution [21]. Both the slopes of curves (a) and (b) were very great, accounting for that the pore diameter distributions of them were narrow. The curves in two pictures were similar which indicated that the morphology, pore size, and surface area of two products were similar, but the specific surface area of α-BiOBr and β-BiOBr are different, which were about 4.706 m2/g and 0.8524 m2/g, respectively. So α-BiOBr had a larger specific surface area, which may be beneficial to reduce the electron-hole recombination.N2 adsorption-desorption isotherms of BiOBr.
(a)
α-BiOBr
(b)
β-BiOBr


## 3.1.4. UV-Vis Diffuse Reflectance Spectral Analysis

The UV-Vis diffuse reflectance spectral ofα-BiOBr and β-BiOBr in the range of 200–700 nm was shown in Figure 4. The absorption peaks of products are steep and had strong absorption, which indicates that the absorption band of BiOBr is not attributed to the transition from impurity band to the conduction band but directly internally converted from the valence band to the conduction band [22]. Both The absorption threshold of α-BiOBr and β-BiOBr was 450 nm, and the band gap of them was 2.76 eV calculated by the formula of λg=1239.18/Eg.Figure 4
UV-Vis diffuse reflectance spectral ofα-BiOBr and β-BiOBr.


## 3.2. Photodegradation of SRB by BiOBr

### 3.2.1. Comparison of Degrading SRB with BiOBr Prepared by Different Methods

Under the identical conditions, SRB was degraded byα-BiOBr and β-BiOBr (Figure 5). SRB cannot be degraded by the two catalysts in absence of light (curve b and c) or under visible light without catalysts (curve a). However, SRB can be degraded in presence of the two catalysts under visible light, and the degradation efficiency of α-BiOBr was far better than that of β-BiOBr. The reaction kinetic constants of photodegradation of SRB by α-BiOBr and β-BiOBr were 0.00602 min−1 (curve e) and 0.0047 min−1 (curve d), respectively.Figure 5
Photocatalytic degradation of SRB in different systems, (SRB) = 1.5 × 10−5 mol/L, (BiOBr) = 0.2 g/L, pH = 3, (a) SRB/Vis; (b) β-BiOBr/SRB/Dark; (c) α-BiOBr/SRB/Dark; (d) β-BiOBr/SRB/Vis; (e) α-BiOBr/SRB/Vis.


### 3.2.2. The Optimization of Degrading SRB

Photocatalytic reactions mainly occur on the surface of the catalyst, therefore the intrinsic characteristic of the surface determines the photocatalytic activity. But reactions also can be significantly affected by surroundings. The influences of catalyst dosage and pH on the degradation of SRB byα-BiOBr were discussed. The solution pH has great effect on the surface charge of catalyst, pollutants molecules charge, adsorption of contaminants on catalyst surface, hydroxyl concentration, and so on, which affect the degradation efficiency. Figure 6 showed the degradation of SRB under different pHs. α-BiOBr had the best catalytic activity when pH was about 2. With the increase of pH, the degradation rates reduced gradually, but the activity reduced when pH was less than 2. In addition, catalyst in the neutral and alkaline solution hardly degraded SRB. This showed at the catalytic activity of BiOBr in acidic environment was far better than that in the neutral and alkaline conditions. The probable reason was that the isoelectric point of the BiOBr is in the acidic range and its surface is negatively charged. BiOBr cannot combine dye easily when pH is larger, so the degradation rates were very small in basic and neutral solution. Figure 7 showed the influence of catalyst dosage on the catalytic efficiency. The degradation rates increased with the catalytic concentration. When the dosage was 0.8 g/L, BiOBr had the best catalytic efficiency. If the amount of catalyst continued to increase, the degradation rate unchanged and even decreased. It may be attributed to active centers provided by BiOBr increase with the amount of catalyst, so BiOBr can absorb more photons and pollutants to efficiently degrade SRB. However, when the catalyst dosage is too much, the scattering effect enhances and the efficient absorption of light reduces, so the degradation efficiency declines [23].Figure 6
Effect of pH, (SRB) = 1.5 × 10−5 mol/L, (BiOBr) = 0.2 g/L.Figure 7
Effect of catalyst dosage, (SRB) = 1.5 × 10−5 mol/L, pH = 2.


### 3.2.3. Degradation of SRB under the Optimum Conditions

The degradation of SRB under the optimum conditions (pH = 2, [BiOBr] = 0.8 g/L) was presented in Figure8. The characteristic absorption peak (λ=565 nm) of SRB decreased constantly and showed a blue shift, which demonstrated that the conjugated structure of SRB decreased and the molecule suffered destruction. After 150 min, the absorption of SRB in visible light disappeared completely and the decoloration rate reached 100%.Figure 8
Temporal UV-Vis spectra changes of SRB, (SRB) = 1.5 × 10−5 mol/L, (BiOBr) = 0.8 g/L, pH = 2.


### 3.2.4.  Cyclic Photocatalytic Degradation of SRB

The stability and reusability of semiconductors are important parameters to measure their practical value. In order to discuss the stability and repeatable usability of BiOBr,α-BiOBr was used to circularly degrade SRB under the optimum conditions (Figure 9). After recycling for 5 times, the degradation efficiency of SRB did not reduce obviously. BiOBr could completely degrade SRB after 100 min, which indicated BiOBr has good stability, reusability, and application potential.Figure 9
The degradation curve of SRB during multicycle degradation process, (SRB) = 1.5 × 10−5 mol/L, (BiOBr) = 0.8 g/L, pH = 2.


## 3.2.1. Comparison of Degrading SRB with BiOBr Prepared by Different Methods

Under the identical conditions, SRB was degraded byα-BiOBr and β-BiOBr (Figure 5). SRB cannot be degraded by the two catalysts in absence of light (curve b and c) or under visible light without catalysts (curve a). However, SRB can be degraded in presence of the two catalysts under visible light, and the degradation efficiency of α-BiOBr was far better than that of β-BiOBr. The reaction kinetic constants of photodegradation of SRB by α-BiOBr and β-BiOBr were 0.00602 min−1 (curve e) and 0.0047 min−1 (curve d), respectively.Figure 5
Photocatalytic degradation of SRB in different systems, (SRB) = 1.5 × 10−5 mol/L, (BiOBr) = 0.2 g/L, pH = 3, (a) SRB/Vis; (b) β-BiOBr/SRB/Dark; (c) α-BiOBr/SRB/Dark; (d) β-BiOBr/SRB/Vis; (e) α-BiOBr/SRB/Vis.


## 3.2.2. The Optimization of Degrading SRB

Photocatalytic reactions mainly occur on the surface of the catalyst, therefore the intrinsic characteristic of the surface determines the photocatalytic activity. But reactions also can be significantly affected by surroundings. The influences of catalyst dosage and pH on the degradation of SRB byα-BiOBr were discussed. The solution pH has great effect on the surface charge of catalyst, pollutants molecules charge, adsorption of contaminants on catalyst surface, hydroxyl concentration, and so on, which affect the degradation efficiency. Figure 6 showed the degradation of SRB under different pHs. α-BiOBr had the best catalytic activity when pH was about 2. With the increase of pH, the degradation rates reduced gradually, but the activity reduced when pH was less than 2. In addition, catalyst in the neutral and alkaline solution hardly degraded SRB. This showed at the catalytic activity of BiOBr in acidic environment was far better than that in the neutral and alkaline conditions. The probable reason was that the isoelectric point of the BiOBr is in the acidic range and its surface is negatively charged. BiOBr cannot combine dye easily when pH is larger, so the degradation rates were very small in basic and neutral solution. Figure 7 showed the influence of catalyst dosage on the catalytic efficiency. The degradation rates increased with the catalytic concentration. When the dosage was 0.8 g/L, BiOBr had the best catalytic efficiency. If the amount of catalyst continued to increase, the degradation rate unchanged and even decreased. It may be attributed to active centers provided by BiOBr increase with the amount of catalyst, so BiOBr can absorb more photons and pollutants to efficiently degrade SRB. However, when the catalyst dosage is too much, the scattering effect enhances and the efficient absorption of light reduces, so the degradation efficiency declines [23].Figure 6
Effect of pH, (SRB) = 1.5 × 10−5 mol/L, (BiOBr) = 0.2 g/L.Figure 7
Effect of catalyst dosage, (SRB) = 1.5 × 10−5 mol/L, pH = 2.


## 3.2.3. Degradation of SRB under the Optimum Conditions

The degradation of SRB under the optimum conditions (pH = 2, [BiOBr] = 0.8 g/L) was presented in Figure8. The characteristic absorption peak (λ=565 nm) of SRB decreased constantly and showed a blue shift, which demonstrated that the conjugated structure of SRB decreased and the molecule suffered destruction. After 150 min, the absorption of SRB in visible light disappeared completely and the decoloration rate reached 100%.Figure 8
Temporal UV-Vis spectra changes of SRB, (SRB) = 1.5 × 10−5 mol/L, (BiOBr) = 0.8 g/L, pH = 2.


## 3.2.4.  Cyclic Photocatalytic Degradation of SRB

The stability and reusability of semiconductors are important parameters to measure their practical value. In order to discuss the stability and repeatable usability of BiOBr,α-BiOBr was used to circularly degrade SRB under the optimum conditions (Figure 9). After recycling for 5 times, the degradation efficiency of SRB did not reduce obviously. BiOBr could completely degrade SRB after 100 min, which indicated BiOBr has good stability, reusability, and application potential.Figure 9
The degradation curve of SRB during multicycle degradation process, (SRB) = 1.5 × 10−5 mol/L, (BiOBr) = 0.8 g/L, pH = 2.


## 3.3. The Measurement of Intermediate Products during the Degradation of SRB

### 3.3.1. The Measurement of H2O2

The change of H2O2 in the degradation of SRB by α-BiOBr and β-BiOBr was measured by DPD method. As shown in Figure 10, H2O2 did not generate in the dark in presence of α-BiOBr and β-BiOBr (curve c and d). Under visible light irradiation, BiOBr was stimulated to produce electrons and holes, which reacted with dissolved oxygen and water adsorbed on the surface of catalysts to produce H2O2. At the beginning of reaction, H2O2 was accumulated and then gradually consumed to resolve into OH∙ which had better oxidizability to degrade SRB. During the accumulation stage, the generation rate of H2O2 in α-BiOBr/SRB system (curve b) is larger than that in β-BiOBr/SRB system (curve a). The degradation rate of SRB in the former system is larger than that in the latter system, so H2O2 is consumed more rapidly and the total amount of H2O2 is less.Figure 10
Changes of H2O2 during the degradation process of SRB, (a) β-BiOBr/SRB/Vis; (b) α-BiOBr/SRB/Vis; (c) α-BiOBr/SRB/Dark; (d) β-BiOBr/SRB/Vis, (SRB) = 1.5 × 10−5 mol/L, (BiOBr) = 0.8 g/L, pH = 2.


### 3.3.2. The Measurement of Active Species

The oxidation species involved in photocatalytic oxidation reaction are mainlyOH∙ and O2∙-, which have high oxidation potential and can oxidize almost all organic compounds. The ESR technology is a very effective method to measure the short life of the radicals. Figure 11 showed the characteristic signal peak of DMPO–OH∙ and DMPO–O2∙- in different systems. The characteristic quartet peaks of DMPO–OH∙ adducts with an intensity ratio of 1 : 2 : 2 : 1 appeared, which showed that OH∙ is generated in the catalytic oxidation process of SRB by BiOBr, and that the catalytic mechanism mainly involved the OH∙ oxidation mechanism. The ESR signals of DMPO–O2∙- adducts were also observed in the system under visible radiation (Figure 11), but the intensity of the signal was faint, which indicated that O2∙- was also produced under visible light, but the main oxidation species was OH∙.ESR signals of the DMPO-OH∙ adducts (a) and DMPO-O2∙- adducts (b).
(a)
(b)


### 3.3.3. The Deep Mineralization of SRB

Figure12 showed the changes of total organic carbon (TOC) in the degradation process of SRB. From the results, the TOC value gradually reduced. Under the same reaction conditions, the TOC removal rates of SRB degraded with α-BiOBr and β-BiOBr are 86% and 48%, respectively, after 900 min, which demonstrated that BiOBr prepared with CPB has a better mineralization of pollutants.Figure 12
TOC removals during the degradation process of SRB, (a)α-BiOBr/SRB/Vis; (b) β-BiOBr/SRB/Vis, (SRB) = 3.0 × 10−5 mol/L, (BiOBr) = 0.8 g/L, pH = 2.


### 3.3.4. IR Analysis

Figure13 presented the IR spectrum of SRB degraded by α-BiOBr in different photocatalytic reaction time. It is known that the bands at 1460, 1500, 1580, and 1600 cm−1 are corresponded to the stretching vibration of benzenes in SRB molecules and the band at 1649 cm−1 is due to the vibration of C–N stretching. The band at 1460~1508 cm−1 is caused by the vibration of the heterocycles in dye molecules. The band at 1330 cm−1 is due to the vibration of C–Ar peak, and the bands at 1120 cm−1 and 665~620 cm−1 are attributed to the vibration of the –SO3 − functional groups. With the increase of reaction time, some characteristic peaks of SRB disappeared, and new peaks at 1650 cm−1 and 1400 cm−1, attributed to the vibration of C=O expansive and diethylamine–CH3, appeared gradually. The results showed that the conjugate structure of SRB was damaged during the process of catalytic degradation and further demonstrated that SRB was not only simply discolored, but also deeply degrade.Figure 13
IR analysis of degrading SRB, (SRB) = 3.0 × 10−5 mol/L, (BiOBr) = 0.8 g/L, pH = 2.


### 3.3.5. CV Analysis

Cyclic voltammetry provides a wealth of information in researching electrode process via analyzing the shape of the scanning curve [24], which can account for the photocatalytic phenomenon. Figure 14 was the current-voltage curves of two products under the same condition. α-BiOBr had two pairs of redox peaks. The oxidation potential was 0.126 V and 0.407 V and reduction potential was 0.259 V and 0.441 V. While β-BiOBr only had a pair of redox peak. The oxidation and reduction peaks were 0.259 V and 0.436 V, respectively. This showed that there are two different electronic transfer between the two different valence states of α-BiOBr which may react two redox reactions; while β-BiOBr only react one redox reaction. And it also showed that the transformation of electrons on α-BiOBr surface is more easy than that on β-BiOBr, thus the photocatalytic activity of α-BiOBr is higher than β-BiOBr.The cyclic voltammetry of BiOBr.
(a)
α-BiOBr
(b)
β-BiOBr


## 3.3.1. The Measurement of H2O2

The change of H2O2 in the degradation of SRB by α-BiOBr and β-BiOBr was measured by DPD method. As shown in Figure 10, H2O2 did not generate in the dark in presence of α-BiOBr and β-BiOBr (curve c and d). Under visible light irradiation, BiOBr was stimulated to produce electrons and holes, which reacted with dissolved oxygen and water adsorbed on the surface of catalysts to produce H2O2. At the beginning of reaction, H2O2 was accumulated and then gradually consumed to resolve into OH∙ which had better oxidizability to degrade SRB. During the accumulation stage, the generation rate of H2O2 in α-BiOBr/SRB system (curve b) is larger than that in β-BiOBr/SRB system (curve a). The degradation rate of SRB in the former system is larger than that in the latter system, so H2O2 is consumed more rapidly and the total amount of H2O2 is less.Figure 10
Changes of H2O2 during the degradation process of SRB, (a) β-BiOBr/SRB/Vis; (b) α-BiOBr/SRB/Vis; (c) α-BiOBr/SRB/Dark; (d) β-BiOBr/SRB/Vis, (SRB) = 1.5 × 10−5 mol/L, (BiOBr) = 0.8 g/L, pH = 2.


## 3.3.2. The Measurement of Active Species

The oxidation species involved in photocatalytic oxidation reaction are mainlyOH∙ and O2∙-, which have high oxidation potential and can oxidize almost all organic compounds. The ESR technology is a very effective method to measure the short life of the radicals. Figure 11 showed the characteristic signal peak of DMPO–OH∙ and DMPO–O2∙- in different systems. The characteristic quartet peaks of DMPO–OH∙ adducts with an intensity ratio of 1 : 2 : 2 : 1 appeared, which showed that OH∙ is generated in the catalytic oxidation process of SRB by BiOBr, and that the catalytic mechanism mainly involved the OH∙ oxidation mechanism. The ESR signals of DMPO–O2∙- adducts were also observed in the system under visible radiation (Figure 11), but the intensity of the signal was faint, which indicated that O2∙- was also produced under visible light, but the main oxidation species was OH∙.ESR signals of the DMPO-OH∙ adducts (a) and DMPO-O2∙- adducts (b).
(a)
(b)


## 3.3.3. The Deep Mineralization of SRB

Figure12 showed the changes of total organic carbon (TOC) in the degradation process of SRB. From the results, the TOC value gradually reduced. Under the same reaction conditions, the TOC removal rates of SRB degraded with α-BiOBr and β-BiOBr are 86% and 48%, respectively, after 900 min, which demonstrated that BiOBr prepared with CPB has a better mineralization of pollutants.Figure 12
TOC removals during the degradation process of SRB, (a)α-BiOBr/SRB/Vis; (b) β-BiOBr/SRB/Vis, (SRB) = 3.0 × 10−5 mol/L, (BiOBr) = 0.8 g/L, pH = 2.


## 3.3.4. IR Analysis

Figure13 presented the IR spectrum of SRB degraded by α-BiOBr in different photocatalytic reaction time. It is known that the bands at 1460, 1500, 1580, and 1600 cm−1 are corresponded to the stretching vibration of benzenes in SRB molecules and the band at 1649 cm−1 is due to the vibration of C–N stretching. The band at 1460~1508 cm−1 is caused by the vibration of the heterocycles in dye molecules. The band at 1330 cm−1 is due to the vibration of C–Ar peak, and the bands at 1120 cm−1 and 665~620 cm−1 are attributed to the vibration of the –SO3 − functional groups. With the increase of reaction time, some characteristic peaks of SRB disappeared, and new peaks at 1650 cm−1 and 1400 cm−1, attributed to the vibration of C=O expansive and diethylamine–CH3, appeared gradually. The results showed that the conjugate structure of SRB was damaged during the process of catalytic degradation and further demonstrated that SRB was not only simply discolored, but also deeply degrade.Figure 13
IR analysis of degrading SRB, (SRB) = 3.0 × 10−5 mol/L, (BiOBr) = 0.8 g/L, pH = 2.


## 3.3.5. CV Analysis

Cyclic voltammetry provides a wealth of information in researching electrode process via analyzing the shape of the scanning curve [24], which can account for the photocatalytic phenomenon. Figure 14 was the current-voltage curves of two products under the same condition. α-BiOBr had two pairs of redox peaks. The oxidation potential was 0.126 V and 0.407 V and reduction potential was 0.259 V and 0.441 V. While β-BiOBr only had a pair of redox peak. The oxidation and reduction peaks were 0.259 V and 0.436 V, respectively. This showed that there are two different electronic transfer between the two different valence states of α-BiOBr which may react two redox reactions; while β-BiOBr only react one redox reaction. And it also showed that the transformation of electrons on α-BiOBr surface is more easy than that on β-BiOBr, thus the photocatalytic activity of α-BiOBr is higher than β-BiOBr.The cyclic voltammetry of BiOBr.
(a)
α-BiOBr
(b)
β-BiOBr


## 3.4. Photocatalytic Degradation of Salicylic Acid

Salicylic acid (SA) is a kind of small colorless molecule which has no absorption in visible light, so it is usually used to characterize the visible photoreactivity of photocatalysts. The degradation of SA was under the illumination of visible light (λ≥420 nm) and the concentration of it was measured by HPLC (Figure 15). Curve a showed that SA was not photodissociated under visible irradiation. Curve b and c showed that α-BiOBr and β-BiOBr can adsorb little amount of SA. Curve d and e represented the degradation of SA by α-BiOBr and β-BiOBr under visible light. After 8 h, the degradation rates of SA by α-BiOBr and β-BiOBr were 97% and 37.3%, respectively. The results further indicated that α-BiOBr had a better catalytic activity than β-BiOBr and could be stimulated effectively by visible light to degrade small molecular pollutants.Figure 15
Photodegradation of SA, (a) SA/Vis; (b)β-BiOBr/SA/Dark; (c) α-BiOBr/SA/Dark; (d) β-BiOBr/SA/Vis; (e) α-BiOBr/SA/Vis, (SA) = 5 m mol/L, (BiOBr) = 0.8 g/L.


## 4. Conclusions

In summary, we synthesized layered BiOBr with high catalytic activity by using different reactants. CPB not only can be used as bromine sources to prepare BiOBr, but also is served as template to form a reactor with specific size and morphology in the preparation process, which can control the particle size and morphology of the products in some extent. Obviously, BiOBr synthesized by CPB had a better efficiency on degrading SRB and SA under visible irradiation than BiOBr prepared by NaBr which only served as bromine sources. The different products showed different particle size, surface area, and adsorption quantity, which result in different degradation efficiency on pollutants.



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*Source: 619761-2012-09-06.xml*