Synthesis of Bi₂S₃/BiVO₄ Heterojunction with a One-Step Hydrothermal Method Based on pH Control and the Evaluation of Visible-Light Photocatalytic Performance.

The band gaps of bismuth vanadate (BiVO₄) and bismuth sulfide (Bi₂S₃) are about 2.40 eV and 1.30 eV, respectively. Although both BiVO₄ and Bi₂S₃ are capable of strong visible light absorption, electron-hole recombination occurs easily. To solve this problem, we designed a one-step hydrothermal method for synthesizing a Bismuth sulfide (Bi₂S₃)/Bismuth vanadate (BiVO₄) heterojunction using polyvinylpyrrolidone K-30 (PVP) as a structure-directing agent, and 2-Amino-3-mercaptopropanoic acid (l-cysteine) as a sulfur source. The pH of the reaction solution was regulated to yield different products: when the pH was 7.5, only monoclinic BiVO₄ was produced (sample 7.5); when the pH was 8.0 or 8.5, both Bi₂S₃ and BiVO₄ were produced (samples 8.0 and 8.5); and when the pH was 9.0, only Bi₂S₃ was produced (sample 9.0). In sample 8.0, Bi₂S₃ and BiVO₄ were closely integrated with each other, with Bi₂S₃ particles formed on the surface of concentric BiVO₄ layers, but the two compounds grew separately in a pH solution of 8.5. Visible-light photocatalytic degradation experiments demonstrated that the degradation efficiency of the Bi₂S₃/BiVO₄ heterojunction was highest when prepared under a pH of 8.0. The initial rhodamine B in the solution (5 mg/L) was completely degraded within three hours. Recycling experiments verified the high stability of Bi₂S₃/BiVO₄. The synthesis method proposed in this paper is expected to enable large-scale and practical use of Bi₂S₃/BiVO₄.

1. Introduction

Semiconductors such as bismuth oxybromide–n>an class="Chemical">bismuth oxyiodide [1], β-ZnMoO4 [2], metal–organic frameworks (MOFs) [3], and BiOxIy/GO [4] can facilitate the photodegradation of dyes. Bismuth oxides and their composites (e.g., bismuth oxyiodides [5], bismuth oxyiodide/graphitic carbon nitride [6], and BiOI/GO [7]) have been widely used for photocatalytic degradation of dyes, owing to their superior photocatalytic traits. Bismuth vanadate (BiVO4) has the advantages of no toxicity, low cost, high chemical stability, photocorrosion resistance, and strong response to visible light (Eg ~ 2.40 eV) [8]. However, because BiVO4 has a limited visible absorption range (<525 nm), and its electrons and holes recombine easily, the widespread application of this material is limited [9]. To improve the photocatalytic efficiency of BiVO4 under visible radiation, it is necessary to expand its visible absorption range, and limit the recombination of electrons and holes. On this basis, researchers have made considerable efforts towards BiVO4 modification.

Doping is the most frequently used method for improving the visible absorn>an class="Chemical">ption range of BiVO4. For instance, BiVO4 has been doped with rare earth metals (e.g., Bi4V2−MO11−(M = Gd, Nd, Gd, M = Nd) [10]), europium [11], transition metals (e.g., Ag-doped BiVO4 [12] and Pd/BiVO4 [13]), and C [14,15]. These doping systems can effectively reduce the band gap of BiVO4 and increase its visible absorption range. However, these methods may elevate costs due to the use of precious metals, and increase heavy metal pollution. In addition, excessive doping may enhance electron–hole recombination.

A common method to restrain the recombination of electron–hole pairs is to construct a heterojunction. A number of studies have reported the synthesis of heterojunctions such as n>an class="Chemical">WO3/BiVO4 [16], CaFe2O4/BiVO4 [17], BiOCl/BiVO4 [18], and CO3O4/BiVO4 [19]. Although these heterojunctions effectively restrain the separation of electron–hole pairs, they do not have an expanded visible adsorption range.

Bismuth sulfide (n>an class="Chemical">Bi2S3) is a p-type semiconductor (Eg ~ 1.30 eV) [20] with a narrow band gap and a very strong response to visible light. The valence band (VB) position of Bi2S3 is more negative than that of BiVO4, whereas the conduction band (CB) position of Bi2S3 is more positive [21]. Therefore, Bi2S3 can be combined with n-type semiconductor BiVO4 to form a heterojunction with a strong capacity for visible light absorption. Using thioacetamide as a sulfur source, De-Kun Ma et al. [22] developed a two-step hydrothermal method to synthesize olive-shaped Bi2S3/BiVO4 microspheres with a limited chemical conversion route and enhanced photocatalytic activity. Canjun Liu et al. [23] used thiourea as a sulfur source in a two-step method for synthesizing Bi2S3 nanowires on BiVO4 nanostructures with enhanced photoelectrochemical performance. Xuehui Gao et al. [24] studied the enhanced photoactivity of mesoporous heterostructured Bi2S3/BiVO4 hollow discoid prepared using Na2S·9H2O as a sulfur source.

In this work, we developed a simpn>le one-stepn> method to synthesize a Bi2S3/BiVO4 heterojunction using the amino acid l-cysteine as a sulfur source. We added the sulfur source during the preparation of BiVO4 using a one-step hydrothermal method, and then regulated the pH of the system to cause Bi2S3 to form on the BiVO4, thereby creating the Bi2S3/BiVO4 heterojunction. We found that this complex material demonstrated a strong capacity for visible light absorption and separation of electron–hole pairs. The use of the heterojunction as a catalyst for rhodamine B (RhB) degradation was investigated under visible light irradiation, and possible formation and degradation mechanisms strongly affected by pH were proposed. The results indicate that this complex material has potential for use in environmental and optoelectronic applications.

2. Materials and Methods

2.1. Materials and Reagents

The materials included analytical grade pure bismuth nitrate (Bi(NO3)3·5pan class="Chemical">H2O (Chengdu Industrial Developn>ment Zone Xinde Mulan, Chengdu, China), analytical grade pure sodium hydroxide powder (n>an class="Chemical">NaOH, Chongqing Chuandong Chemical Company, Chongqing, China), analytical grade polyvinylpyrrolidone K-30 (PVP) (Chengdu Kelong Chemical Co., Ltd., Chengdu, China), ammonium metavanadate (NH4VO3, Chongqing Chuandong Chemical Company, Chongqing, China), l-cysteine (Aladdin Industrial Corporation, Shanghai, China), rhodamine B (RhB, Tianjin Guangfu Fine Chemical Research Institute, Tianjin, China), nitric acid (HNO3, Chengdu Area of the Industrial Development Zone Xinde Mulan, Chengdu, China), ethylene glycol, (C4H4O6KNa4·H2O), silver nitrate (AgNO3), p-benzoquinone (PBQ), and isopropanol (IPA) (Chongqing Chuandong Chemical Company, Chongqing Chuandong, China).

2.2. Synthesis of Photocatalysts

The pH of the reaction solution was set pan class="Species">to 7.5, 8.0, 8.5, or 9.0 (Sampn>le-7.5, Sampn>le-8.0, Sampn>le-8.5, and Sampn>le-9.0, respn>ectively). During synthen>an class="Chemical">sis, 2 mmol Bi(NO3)·5H2O and 0.6 mmol l-cysteine were dissolved in 4 mL of 4 mol/L HNO3. Then, 50 mL of deionized water was added to the solution, and the mixture was stirred for 30 min to obtain solution A. Similarly, 2 mmol NH4VO3 was dissolved in 4 mL of 2 mol/L NaOH, and the mixture was stirred for 30 min to obtain solution B. Solutions A and B were mixed together, and the pH was adjusted to 7.5, 8.0, 8.5, or 9.0 using NaOH or HNO3. The solutions were transferred into a 100-mL, Teflon-lined autoclave, heated at 180 °C for 16 h, and allowed to cool to room temperature. Finally, the solutions were centrifuged to obtain the final products. The samples were rinsed with distilled water and ethanol six times, and the pH of the filtrate was measured after the last rinse. If the pH of a sample was not neutral, the sample was further rinsed until a pH of ~7 was obtained. Then, the products were dried at 60 °C for 12 h in vacuum.

2.3. Characterization

The crystal structures of prepn>ared sampn>les were characterized using X-ray diffraction (XRD) under CuK radiation with a Rigaku D/Max2500pc (Tokyo, Japan) diffractometer (scanning angle 2θ from 10° to 70°, and scanning rate of 4°/min). A high-voltage (10 kV) Tescan FEG-SEM microscope (TESCAN, MARI3, Brno, Czech Republic) was used to acquire scanning electron microscopy (SEM) images of the prepared samples, and the elemental composition was characterized with an energy dispersive X-ray detector (EDX). A JEM-3010 electron microscope (JEOL, Tokyo, Japan) was used to perform transmission electron microscopy (TEM) at an acceleration voltage of 300 kV. Fourier transform infrared (FT-IR) spectra of prepared samples were recorded on a Shimadzu IR Prestige-1 spectrometer (Tokyo, Japan) using the KBr pellet technique. The chemical characteristics of sample surfaces were investigated using X-ray photoelectron spectra (XPS) acquired with a PHI5000 (ULVAC-PHI,INC., Kanagawa Prefecture, Japan) versa probe system under monochromatic Al K X-rays. A Hitachi U-3010 UV-Vis spectrophotometer (Tokyo, Japan) was used to perform UV-Vis diffuse reflectance spectroscopy (UV-Vis DRS) using the “Abs” data mode. The photoluminescence (PL) spectra of the photocatalysts were obtained using a Hitachi F-7000 (Tokyo, Japan) spectrometer with an excitation wavelength of 280 nm. A CHI Electrochemical Workstation (CHI 760E, Shanghai Chenhua Co., Ltd., Shanghai, China) was used to evaluate the photoelectrochemical properties of the samples. The visible light source was a 500 W Xe lamp (with a <400 nm UV cutoff filter), and all experiments were carried out at room temperature.

2.4. Evaluation of Photocatalytic Activity

The photocatalytic activity of samples was evaluated under vipan class="Chemical">sible radiation at room tempn>erature by measuring the degradation rate of n>an class="Chemical">RhB. For the experiments, 0.20 g of catalyst was added to 200 mL of 5 mg/L RhB aqueous solution, and the mixture was stirred for 30 min in the dark to achieve adsorption–desorption equilibrium between the dye and the catalyst. The experimental solution was placed 350 mm from the 500-W Xe lamp (with a <400 nm UV cutoff filter). Samples were collected after every 0.5 h of irradiation, and then centrifuged (10,000 r/min) to remove the catalyst. Subsequently, the absorbance of the solution at 552 nm was measured to indicate the concentration of the remaining dye. For comparison, the photocatalytic experiments were conducted with Samples 7.5, 8.0, 8.5, and 9.0 as catalysts, and with no catalyst.

3. Results and Discussion

3.1. XRD Pattern Analysis

When the synthesis reaction was performed in a pH solution of 7.5, the XRD diffraction pattern of the resulting sampn>le was similar to that of monoclinic BiVO4 (yellow line in Figure 1 JCPDS#83-1697) [25], indicating that the sample was monoclinic BiVO4. In contrast, the XRD diffraction peaks of samples 8.0 and 8.5 showed characteristics of both BiVO4 and Bi2S3 (JCPDS#84-0279) [26]. As the pH increased, the Bi2S3 peak increased in both height and intensity. However, when the pH of the precursor solution was 9.0, only Bi2S3 was obtained. Therefore, the SEM, XPS, and TEM results indicate that a Bi2S3/BiVO4 heterojunction may be synthesized when the reaction was performed under a pH of 8.0 or (and) 8.5.

Figure 1

X-ray diffraction (XRD) patterns.

3.2. Morphology Analysis Based on SEM, HRTEM, and FT-IR

According to the SEM images (Figure 2), sample 7.5 was cube-like in shape, with a length of about 5 μm, whereas sample 8.0 consisted of concentric layers, with some n>an class="Chemical">Bi2S3 particles dotting the outer layers. Sample 8.5 mainly consisted of BiVO4 shaped as hexagonal pyramids and some flakes of Bi2S3. Sample 9.0 consisted of only Bi2S3 flakes. Therefore, the pH of the precursor solution strongly influenced the prepared products. Characteristic stripes of BiVO4 (004) [27] and Bi2S3 (200) [28] can be observed from the HRTEM results (Figure 2e). Figure 2f shows the FT-IR spectra of sample 8.0. The broad absorptions at 740 cm−1 can be attributed to BiVO4 [29]. Furthermore, absorption at 543 cm−1 and 486 cm−1 can be ascribed to Bi2S3 [30], whereas the broad and weak peaks around 3700 cm−1 and 1600 cm−1 are due to the vibrational rotation and bending deformation of very small amounts of water molecules in the sample [31]. These results show that the heterojunction was successfully prepared when the pH of precursor solution was 8.0.

Figure 2

Scanning electron microscopy (SEM) (a–d) of samples, HRTEM (e) of Sample-8.0, and Fourier–transform infrared (FT-IR) spectra (f) of Sample-8.0.

3.3. Analysis of Composition and Chemical States Based on EDX and XPS

The composition and chemical states of sampn>les were analyzed based on EDX and Xn>an class="Chemical">PS. According to the EDX patterns of samples (Figure 3a), sample 7.5 contained the elements C, Bi, O, and V. When the pH of the precursor solution was 8.0 and 8.5, the sample contained C, Bi, O, V, and S. As the pH increased to 9.0, only C, Bi, and S were tested. Carbon was mostly due to CO2 adsorption from the atmosphere [32], whereas Si was from the substrate. The wt % of Bi, V, O, S, and C in the samples tested via EDX are listed in Table 1, as well as the speculated composition. The molar ratio of BiVO4:Bi2S3 was about 7.42:1 and 6.07:1 in samples 8.0 and 8.5, respectively.

Figure 3

Energy dispersive X-ray detector (EDX) spectra of all samples (a) and X-ray photoelectron spectra (XPS) spectra of Sample-8.0 (b–f): (b) survey XPS spectrum, (c) C 1s peaks, (d) V 2p3/2 and V 2p1/2 peaks, (e) O 1s peak, and (f) Bi 4f5/2, Bi 4f7/2 and S 2p peaks.

Table 1

Sample composition based on EDX.

Sample	Bi	V	O	S	C	Molar Ratio
	wt %	wt %	wt %	wt %	wt %	BiVO4:Bi2S3
Sample-7.5	61.36	15.89	18.94	0.00	3.81	/
Sample-8.0	76.04	14.50	2.26	3.69	3.51	7.42:1
Sample-8.5	79.76	11.64	2.09	3.62	2.89	6.07:1
Sample-9.0	78.75	0.00	0.00	17.67	3.58	/

The chemical state of Sample-8 was analyzed by XPS. Figure 3b shows fully scanned spn>ectra and the S 2s orbital of Sampn>le-8.0 within the range of 0–700 eV. As shown in the spn>ectra, the compn>osite material was composed of Bi, O, V, C, and S. The binding energy of C ls of the non-oxygenated ring C was corrected to 284.6 eV (Figure 3c) [33]. The V 2p core level spectrum in Figure 3d indicates that the binding energies (516.8 and 524.4 eV) for V 2p are in accordance with former reports on V5+ in BiVO4 [34]. The XPS signals of O 1s are 529.7 eV and 532.7 eV (Figure 3e) [14], respectively; this can be explained by the existence of O2− anions in BiVO4. According to Figure 3f, the peaks with binding energies of 159.3 eV and 164.6 eV are respectively related to Bi 4f7/2 and Bi 4f5/2 in BiVO4 [35]. The peaks with binding energies of 157.2 eV and 162.6 eV respectively correspond to Bi 4f7/2 and Bi 4f5/2 in Bi2S3 [36]. The peak with binding energy of 160.4 eV corresponds to the S 2p transition [37]. It is known that the binding energy of pure Bi2S3 is 158.9 ± 0.1 eV, whereas the measured value is 158.4 ± 0.1 eV [38]. This shift indicates the interfacial chemical interaction between Bi2S3 and BiVO4 [39]. In conclusion, the XRD, SEM, TEM, EDX, and XPS results indicate that Bi2S3 quantum dots successfully formed on BiVO4.

3.4. Optical Properties Characterized by UV-Vis DRS, Transient Photocurrent Response, and PL

Both pan class="Chemical">BiVO4 [40,41] and n>an class="Chemical">Bi2S3 [22,42,43,44] display characteristics of direct transition. The light absorption properties and the band gap of the semiconductor can be determined based on UV-Vis absorption spectra (Figure 4a). Moreover, the band gap can be obtained from the slope of (Ahυ)2 versus hυ using Equation (1): where A is the absorption coefficient, E is the band gap energy, h is Planck’s constant, ν is the incident light frequency, and C is a constant.

Figure 4

(a) UV-Vis diffuse reflectance spectra of samples; (b) Estimated band gaps of UV-Vis spectra of the samples; (c) Transient photocurrent response; (d) Photoluminescence (PL) spectra at an excitation wavelength of 280 nm.

According to Figure 4b, sample 7.5 contained pan class="Chemical">BiVO4. Most of the absorn>an class="Chemical">ption regions were concentrated in the ultraviolet region, with a few concentrated in the visible region, and the band gap was 2.6 eV. Sample 9.0 contained Bi2S3, and the spectra show almost complete absorption, with a band gap of about 1.5 eV. Based on Equations (2) and (3), the VB values of Bi2S3 and BiVO4 are 1.52 and 2.84 eV, respectively, and the CB values of Bi2S3 and BiVO4 are 0.02 and 0.24 eV, respectively. Thus, Bi2S3 enhanced the absorption of visible light by BiVO4.

Photoelectrochemical tests were conducted to analyze the excitation, sepn>aration, and transfer of carriers in the catalyst. n>an class="Chemical">Photoanodes were prepared by electrophoretic deposition on ITO glass supports. The electrophoretic deposition was carried out in an acetone solution (20 mL) containing iodine (50 mg) and photocatalyst powder (50 mg), and then dispersed via sonication for 5 min. The ITO electrode (1.0 × 2.0 cm2 was immersed in the solution with a Pt electrode, and a 30 V differential was applied for 100 s using a potentiostat. After this process was repeated twenty times, the electrode was dried and calcined at 200 °C for 2 h. The exposed effective area of the ITO glass was controlled to be 1.0 × 1.0 cm2. According to the transient photocurrent responses of the samples under visible irradiation (Figure 4c), the photocurrent of sample 8.0 had the highest density, followed by sample 8.5, sample 9.0, and finally sample 7.5. The PL spectra (excitation wavelength of 280 nm) are shown in Figure 4d. The characteristic peak of bismuth vanadate is visible at 320 nm [45]. No peak was visible in sample 9.0 owing to the presence of bismuth sulfide. In contrast, sample 7.5 had the strongest peak, followed by sample 8.5, and sample 8.0. This is because sample 8.0 contained a Bi2S3/BiVO4 heterojunction, which is conductive to the separation of electron–hole pairs. Sample 8.5 was produced by physical contact of Bi2S3 and BiVO4. Sample 9.0 contained Bi2S3, but even though this catalyst can almost completely absorb visible light, the recombination of electrons and holes may occur due to the narrow band gap. Sample 7.5 contained BiVO4, which has a limited visible absorption range. Therefore, sample 8.0 displays the strongest potential for use in photoelectric and environmental applications.

3.5. Evaluation of Photocatalytic Activity Based on RhB Degradation

Figure 5a shows the results of the adsorption–desorn>an class="Chemical">ption equilibrium tests. The samples were collected once every 5 min during the dark reaction stage. The RhB concentrations of the various solutions stabilized over time. Dyes and catalysts reached adsorption–desorption equilibrium after stirring for 30 min in the dark. Figure 5b shows the photocatalytic activities of the samples under visible irradiation for 3 h, and the corresponding degradation kinetics constants are shown in Figure 5c. For comparison, the RhB degradation rate was also estimated with no catalyst. The results indicate that 45.07%, 62.13%, 72.00%, and 100.00% of the RhB was degraded when samples 9.0, 7.5, 8.5, and 8.0 were used as catalysts, respectively. This indicates that sample 8.0 has the highest catalytic activity, followed by sample 8.5, sample 7.5, and sample 9.0. Sample 8.0 can be easily recycled by simple filtration, and its degradation effect was respectively maintained at 95.19%, 95.18%, 94.91%, 94.64%, and 94.63% after five recycling cycles (Figure 5d). The EDX, SEM, and XRD results for sample 8.0 after five recycling cycles indicated that no leaching of elements occurred and the morphology remained unchanged (Figure 5e,f). This indicated that sample 8.0 has an excellent heterostructure. Furthermore, the Bi2S3 dots were very small (19.7 ± 2.2 nm, calculated based on the Sherer relation); thus, the specific surface area of the sample was larger than that of pure BiVO4 (Table 2). The specific surface area of samples 7.5, 8.0, 8.5, and 9.0 was 6.423, 19.527, 12.642, and 21.165 m2 g−1, respectively, indicating that Bi2S3 greatly impacted the specific surface area of the samples. The formation of the heterojunction, and the greater specific surface area of BiVO4 of sample 8.0 improved its photocatalytic activity. These features are very important for its practical application and modification.

Figure 5

(a) Adsorption–desorption equilibrium test results; (b) Degradation of rhodamine B (RhB) using different catalysts under visible light irradiation; (c) Linear fit of the photocatalytic reaction and the reaction rate constant k; (d) Photocatalytic degradation of RhB reusing photocatalyst sample 8 after filtration; (e) EDX and SEM (inset) of sample 8 after recycling five times; (f) XRD of sample 8 after recycling five times.

Table 2

Brunner−Emmet−Teller (BET) measurements of samples.

Sample	Mean Pore Size (nm)	Pore Volume (cm3 g−1)	Specific Surface Area (m2 g−1)
Sample-7.5	15.765	0.024	6.423
Sample-8.0	15.462	0.021	19.527
Sample-8.5	14.459	0.018	12.642
Sample-9.0	17.265	0.030	21.165

3.6. Postulated Heterojunction Formation Mechanism

The pH of the reaction system had a strong influence on the crystal phase and morpn>hology of the synthesized products [46]. By fixing the amounts of materials and l-cysteine, as well as the reaction parameters (except pH), the synthesis reaction was conducted under varying pH values. To explain the results, we speculated a series of reactions that can occur successively based on the amount of OH−. First, when Bi3+ is added to the l-cysteine system, chelation between the metal and amino acids can occur (4) [47].

Below, we discuss what happens when the pH of different systems is adjusted.

The pH was lowest in the first system. pan class="Chemical">Pure monoclinic n>an class="Chemical">BiVO4 was produced. The probably reaction is the (5), because we know that S3− did not exist in the system and S3− can exchange ions with BiVO4 to form Bi2S3 [32].

In the second system, the pH was adjusted to 8.0, and the compopan class="Chemical">site n>an class="Chemical">Bi2S3/BiVO4 was produced. We can see that some Bi2S3 formed on the BiVO4; thus, we speculate that (5) still took place in the system. Since OH− remains in the system, (6) will occur, forming S2−. Then, as previously mentioned, S2− will react with BiVO4 to form Bi2S3. As the amount of S in the system was low (0.6 mmol in total), some of the BiVO4 formed Bi2S3 as shown in Figure 2b.

As the pH increased to 8.5, the first reaction could no longer take place. Instead, (8) occurred, caun>an class="Chemical">sing the OH− concentration to decrease, followed by (9). Sample 8.5 consisted of both Bi2S3 and BiVO4, separately.

Equation (8) could still take place under a pH of 9.0. The synthepan class="Chemical">sized sampn>le contained only n>an class="Chemical">Bi2S3 due to the high OH− concentration. The remaining Bi3+ first reacted with OH− to form Bi(OH)3, as shown in (10). The reaction then continued, causing Bi(OH)3 to dissolve, and forming Bi(OH)4− (11) [48].

3.7. Postulated Degradation Mechanism

Active species such as ·O2−, ·OH, e−, and holes(h+)play an impn>ortant role in the photodegradation of dyes [49]. To investigate the photocatalytic mechanism and activity of n>an class="Chemical">Bi2S3/BiVO4, the contribution of each active species to the photodegradation performance was examined based on a scavenger experiment [50]. In this experiment, potassium sodium tartrate (C4H4O6KNa·4H2O, 0.1 mmol) was used as the h+ scavenger, silver nitrate (AgNO3, 0.1 mmol) was used as the e− scavenger, p-benzoquinone (PBQ, 0.1 mmol) was used as the ·O2− scavenger, and isopropanol (IPA, 0.1 mmol) was used as the ·OH scavenger. These scavengers were added to RhB solutions containing Bi2S3/BiVO4, and the solutions were irradiated with visible light for 1.5 h. According to Figure 6, the addition of the h+ scavenger (C4H4O6KNa) and the ·O2− scavenger (IPA) severely suppressed the catalytic performance, suggesting that h+ and ·O2− are the main reactive species contributing to the photodegradation of RhB. After the addition of the ·OH scavenger (IPA), the catalytic degradation effect was slightly inhibited, which suggests that ·OH plays an insignificant role in this reaction system. The ·OH was mainly produced by oxidation of H2O to ·O2− and OH− through BiVO4 VB [1]. Lizhen Ren et al. reported that the VB of Bi2S3 was not sufficient to oxidize OH− to ·OH [51]. After adding the e− scavenger (AgNO3), the degradation efficiency increased owing to e− consumption and increased h+ efficiency; therefore, h+ plays the most important role in this degradation process and can directly degrade dyes [1,49].

Figure 6

Scavenger effect of sample 8 photocatalyst.

The scavenger experiments confirmed the existence of ·O2−, ·OH, e−, and h+ in the catalytic system. A thorough understanding of the photocatalytic degradation mechanism is necessary for the actual apn>plication of n>an class="Chemical">Bi2S3/BiVO4 heterojunctions. The postulated degradation mechanism is shown in Schematic 1. Figure 5a demonstrates that the concentration of the dye did not significantly change without the addition of a catalyst. In contrast, photocatalyst addition significantly reduced the dye concentration. The adsorption of dye onto the catalyst surface is the primary process, as shown in (12). RhB is sensitive to visible light, as indicated by (13) [52]. The potential energy of the RhB LUMO and HOMO was −1.42 and 0.95 eV, respectively [53]. The VB values of Bi2S3 and BiVO4 were 1.52 and 2.84 eV, respectively, and the CB values of Bi2S3 and BiVO4 were 0.02 and 0.24 eV, respectively. Hence, the photosensitive dye transferred electrons to the CB of semiconductors (14) [54]. BiVO4 and Bi2S3 were excited under visible radiation, causing transfer of Bi2S3 and BiVO4 electrons from VB to CB, and leaving holes in VB ((15) and (16)). Due to the formation of the heterojunction, the holes in the VB of BiVO4 shifted to the VB of Bi2S3, while the electrons in CB of Bi2S3 shifted to the CB of BiVO4. Thus, the carriers of the electron–hole pair were separated ((17) and (18)). H2O can ionize OH, as shown (19). The photogenerated electrons can react with dissolved oxygen molecules (O2) to yield superoxide radical anions (·O2−), as shown in (20), and ·O2− can react with H2O to produce ·OH (21) [55,56]. As previously mentioned, the VB of BiVO4 can oxidize OH− to ·OH (22), and h+, ·O2−, and ·OH are strong oxidizing agents for the decomposition of organic dyes (23) [57]. The whole set of redox reactions can be summarized as follows:

Schematic 1

Postulated mechanism for RhB degradation catalyzed with sample 8.0.

4. Conclusions

A one-step method for synthesizing a n>an class="Chemical">Bi2S3/BiVO4 heterojunction with high photocatalytic activity under visible irradiation was developed based on pH regulation of the reaction solution. The morphologies and compositions of prepared samples were characterized with various analytical methods. The degradation rate of RhB under visible irradiation was used to estimate the photocatalytic activity of prepared samples. The photocatalytic activity of sample 8.0 was higher than that of samples 7.5, 8.5, and 9.0, because the former contained a heterojunction.