# Synthesis of Nitrogen-Doped ZnS with Camellia Brushfield Yellow Nanostructures for Enhanced Photocatalytic Activity under Visible Light Irradiation

Authors: Gang-Juan Lee; Chi-Lun Hong; Valentina Batalova; Gennady Mokrousov; Jerry Wu
Journal: International Journal of Photoenergy
 (2013)

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## Abstract

Nitrogen modified zinc sulfide photocatalysts were successfully prepared and characterized by X-ray diffraction (XRD), field emission scanning electron microscopy (FE-SEM), high-resolution transmission electron microscopy (HR-TEM), X-ray photoelectron spectroscopy (XPS), and surface area analysis. Thermal decomposition of the semisolid was carried out under nitrogen conditions at 500°C for 2 hours, and a series of nitrogen-doped ZnS photocatalysts were produced by controlling inflow flow rate of nitrogen at 15–140 mL/min. Optical characterizations of the synthesized N-doping ZnS substantially show the shifted photoabsorption properties from ultraviolet (UV) region to visible light. The band gaps of nitrogen-doped ZnS composite catalysts were calculated to be in the range of 2.58~2.74 eV from the absorptions edge position. The 15N/ZnS catalyst shows the highest photocatalytic activity, which results in 75.7% degradation of Orange II dye in 5 hrs by visible light irradiation, compared with pristine ZnS and higher percentage N-doping ZnS photocatalysts.


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## Body

## 1. Introduction

The photocatalytic degradation of organic pollutions present in water and wastewater has been comprehensively investigated with the use of photocatalysts and a solar light simulating source [1]. Since zinc sulfide (ZnS) is an important II–VI semiconductor with a large band gap, it has been extensively studied not only for its application as a photocatalyst but also as a device material for other purposes, such as light-emitting diodes, cathoderay tubes, thin film electroluminescence, reflector, dielectric filter, chemical/biological sensors, and window layers in photovoltaic cells [2]. In addition, zinc sulfide has the direct band gap of 3.68 eV (zinc blend) and 3.80 eV (wurtzite) at 300 K [3]. However, its wide band gap restricts light absorption specifically to the wavelength of UV less than 340 nm, where it can only take advantage of ultraviolet irradiation constituting only 4% of the incoming solar light [4]. Therefore, the development of visible-light-driven photocatalysts by using less energy but more abundant visible light (λ≥420 nm), which accounts for about 43% of the solar spectrum, has recently become a very important topic of research [5]. As visible-light-driven photocatalysts by doping nonmetal ions can provide more active sites and mechanisms on photocatalysts, those have been widely used to improve the visible-light-driven photocatalytic activity [6]. Therefore, in this paper, we attempted to prepare nitrogen-doped ZnS nanostructures using thermal decomposition methods to degrade Orange II dye under visible light irradiation.


## 2. Materials and Methods

### 2.1. Preparation and Modification of Nitrogen-Doped ZnS Photocatalysts

Zinc chloride and potassium thiocyanate were used as the source of zinc and sulfur, respectively. 12.51 g of anhydrous ZnCl2 (Merck) was dissolved in 25 mL of water, and then 50 mL of ethanol (95%) was added by constant stirring (solution A); 20.07 g of potassium thiocyanate (Merck) was separately dissolved in another 25 mL of water (solution B). Under magnetic stirring, solution B was then added drop by drop (30 min) into solution A. The clear solution was stirred for another 30 min, and the solvents were evaporated on a hot plate until they became a semisolid, which was then transferred into a crucible for decomposition. Thermal decomposition of the semisolid was carried out under nitrogen conditions at 500°C for 2 hours. A series of nitrogen-doped ZnS photocatalysts prepared by controlling the inflow flow rate of nitrogen at 15, 30, 70, and 140 mL/min denoted as 15N/ZnS, 30N/ZnS, 70N/ZnS, and 140N/ZnS, respectively, were prepared under nitrogen atmospheric conditions at 500°C. After thermal decomposition at the desired temperature (500°C), the samples were washed with plenty of water and methanol to eliminate the impurities and finally dried in an oven at 60°C overnight.


### 2.2. Characterizations and Instruments

The X-ray diffraction (XRD) patterns were recorded using RigakuUltima III diffractometer (Japan) with Cu-Kα1 radiation, in the scan angle range from 10° to 80°. The morphologies of the catalysts were examined by using JEOL, JSM-7401F field emission scanning electron microscope (FE-SEM). High-resolution transmission electron microscopic (HR-TEM) images were recorded using JEOL JEM-2010 model. Elemental analysis (EA) was conducted using a PerkinElmer CS02010 elemental analyzer. X-ray photoelectron spectroscopy (XPS) measurements were carried out using Physical Electronics PHI 5600 XPS instrument with monochromatic Al-Kα as (1,486.6 eV) excitation source. The UV-visible diffuse reflectance spectra were recorded by a Shimadzu UV-2600 spectrophotometer equipped with an integrated sphere attachment using barium sulfate as a reference. The concentration of the Orange II dye was also determined by UV-2600 spectrophotometer equipped with a universal liquid cell attachment at the wavelength of 485 nm.


### 2.3. Photocatalytic Activity

The photocatalytic experiments of the synthesized composite catalysts were performed in a 500 mL tubular quartz reactor. Catalyst dose and initial dye concentration were maintained at 0.5 g/L and 40 mg/L, respectively. The experiments were carried out at neutral pH under ambient condition. Prior to experiment, the catalyst and dye mixtures were stirred in the dark for 1 hr to achieve adsorption equilibrium of Orange II dye on the surface of the catalysts. For light irradiation, the photocatalytic reactor was illuminated with a 350 W xenon light source, which has a cutoff filter at wavelength 400 nm allowing visible light to pass.


## 2.1. Preparation and Modification of Nitrogen-Doped ZnS Photocatalysts

Zinc chloride and potassium thiocyanate were used as the source of zinc and sulfur, respectively. 12.51 g of anhydrous ZnCl2 (Merck) was dissolved in 25 mL of water, and then 50 mL of ethanol (95%) was added by constant stirring (solution A); 20.07 g of potassium thiocyanate (Merck) was separately dissolved in another 25 mL of water (solution B). Under magnetic stirring, solution B was then added drop by drop (30 min) into solution A. The clear solution was stirred for another 30 min, and the solvents were evaporated on a hot plate until they became a semisolid, which was then transferred into a crucible for decomposition. Thermal decomposition of the semisolid was carried out under nitrogen conditions at 500°C for 2 hours. A series of nitrogen-doped ZnS photocatalysts prepared by controlling the inflow flow rate of nitrogen at 15, 30, 70, and 140 mL/min denoted as 15N/ZnS, 30N/ZnS, 70N/ZnS, and 140N/ZnS, respectively, were prepared under nitrogen atmospheric conditions at 500°C. After thermal decomposition at the desired temperature (500°C), the samples were washed with plenty of water and methanol to eliminate the impurities and finally dried in an oven at 60°C overnight.


## 2.2. Characterizations and Instruments

The X-ray diffraction (XRD) patterns were recorded using RigakuUltima III diffractometer (Japan) with Cu-Kα1 radiation, in the scan angle range from 10° to 80°. The morphologies of the catalysts were examined by using JEOL, JSM-7401F field emission scanning electron microscope (FE-SEM). High-resolution transmission electron microscopic (HR-TEM) images were recorded using JEOL JEM-2010 model. Elemental analysis (EA) was conducted using a PerkinElmer CS02010 elemental analyzer. X-ray photoelectron spectroscopy (XPS) measurements were carried out using Physical Electronics PHI 5600 XPS instrument with monochromatic Al-Kα as (1,486.6 eV) excitation source. The UV-visible diffuse reflectance spectra were recorded by a Shimadzu UV-2600 spectrophotometer equipped with an integrated sphere attachment using barium sulfate as a reference. The concentration of the Orange II dye was also determined by UV-2600 spectrophotometer equipped with a universal liquid cell attachment at the wavelength of 485 nm.


## 2.3. Photocatalytic Activity

The photocatalytic experiments of the synthesized composite catalysts were performed in a 500 mL tubular quartz reactor. Catalyst dose and initial dye concentration were maintained at 0.5 g/L and 40 mg/L, respectively. The experiments were carried out at neutral pH under ambient condition. Prior to experiment, the catalyst and dye mixtures were stirred in the dark for 1 hr to achieve adsorption equilibrium of Orange II dye on the surface of the catalysts. For light irradiation, the photocatalytic reactor was illuminated with a 350 W xenon light source, which has a cutoff filter at wavelength 400 nm allowing visible light to pass.


## 3. Results and Discussion

### 3.1. Characterization of Nitrogen-Doped ZnS Photocatalysts

The crystallinity and crystal phase of pure ZnS and nitrogen-doped ZnS photocatalysts were characterized by XRD as shown in Figure1. The major diffraction peaks of the ZnS (JCPDS card number 36-1450, the lattice parameters of a=3.820 Å and c=6.257 Å) with (100), (002), (101), (110), (103), and (112) planes were apparent for hexagonal wurtzite crystal structure. The (002) peak intensity is stronger than the (100) peak when the nitrogen-doped ZnS composite catalysts were prepared under different conditions. This is due to the change in the stacking sequence of the close packed planes of the ZnS crystal [7]. This observation is supported by the TEM results, and it indicates that nanosheets preferential growth occurs along the c-axis. The remaining peaks are generally broad and probably indicate relatively small dimensions of the materials [8]. The (100), (002), and (101) peaks strongly overlap, implying the formation of well-crystallized ZnS. At the same time, the atmospheric conditions have not influenced the crystal structure of ZnS [7].Figure 1
XRD patterns of nitrogen-doped and bare ZnS.HR-TEM images (Figure2(a)) of the as-synthesized catalysts can further confirm the flowery structure of the microspheres. The clear lattice fringes (Figure 2(b)) also indicate the polycrystalline nature of the petals. The interplanar spacing is 0.31 nm, which corresponds to the (002) plane of wurtzite ZnS. The corresponding selected area electron diffraction (SAED) patterns (Figure 2(c)) with a regular and clear ring diffraction spot array reveal that each petal is polycrystalline. Moreover, the major diffraction ring matches (100), (002), (101), (110), and (112) planes of ZnS phase.Figure 2
(a) HR-TEM images, (b) lattice fringes, and (c) the corresponding SAED pattern of 15N/ZnS.To better understand chemical states of the elements within the catalysts, XPS analyses were performed in this study. The typical XPS results are shown in Figure3. The peaks of S and Zn can be clearly seen in the survey spectra of all catalysts used (Figures 3(b) and 3(c)). The binding energies of S2p3/2 and S2p1/2 at 161.1 eV and 160.2 eV (Figure 3(b)) are consistent with the binding energy values in the literature [9]. Moreover, the binding energy of Zn2p3/2 and Zn2p1/2 is 1020.3 eV and 1043.3 eV (Figure 3(c)), belonging to the Zn2+ oxidation state in ZnS [9]. As for N, the binding energy of N1s at 395.9 eV belongs to atomic β-N (396 eV) [10]. According to the references, N1s peak at 396 eV is attributed to a characteristic peak of substitutional N, resulting from the nitrogen substitution of sulfur in the ZnS lattice [10–12]. In addition, the substitutional doping of N is thought to be the most pronounced because its p states contribute to the band gap narrowing by mixing with S2p states [10]. From the UV-Vis absorption spectra results as shown in Figure 4, the band gap of bare ZnS was calculated as 2.95 eV. The band gap of nitrogen-doped ZnS composite catalysts is between 2.58 and 2.74 eV. Therefore, the redshift in UV-Vis absorption spectra is enhanced by the nitrogen-doped ZnS composite catalysts, which implies the potential absorption to effectively harvest visible light.The survey XPS spectra of (a) 15N/ZnS photocatalysts and the high-resolution XPS spectra of (b) S2p, (c) Zn2p, and (d) N1s of 15N/ZnS photocatalysts.
(a)
(b)
(c)
(d)Figure 4
UV-Vis absorption spectra of as-synthesized photocatalysts.The morphology of nitrogen-doped ZnS composite catalysts was characterized by FE-SEM as shown in Figure5. The zinc isothiocyanate complex thermal decompositions have been carried out at 500°C under nitrogen conditions. The ZnS photocatalysts consist of irregular spheres with an average diameter of 1 μm and seem to facilitate microsphere aggregation. The images in Figures 5(a)–5(e) show that the nitrogen-doped ZnS Camellia Brushfield Yellow-like structure comprises numerous ZnS particles (petals) and the nitrogen-doped ZnS crystallites are self-organized into spherical assemblies, or a Camellia Brushfield Yellow-like morphology, with a puffy appearance. The nitrogen-doped ZnS products are all in this morphology with diameters ranging from 300 to 700 nm. The gap between particles (petals) was observed in the average range of 100 nm. The nitrogen-doped ZnS flower is quite open and puffy with ZnS particles (petals) that have good crystallinity [13]. When the nitrogen flowrate was increased from 15 to 140 mL/min, the morphology of the nitrogen-doped ZnS nanoparticles became more rough as seen in Figures 5(a)–5(e). Figure 5(f) clearly indicates that the flowery structures, from which one can see that dozens of 2D sheets are intercrossed with each other, have been formed throughout their self-assembly mechanisms.FE-SEM images of (a) ZnS, (b) 15N/ZnS, (c) 30N/ZnS, (d) 70N/ZnS, and (e) 140N/ZnS photocatalysts.
(a)
(b)
(c)
(d)
(e)
(f)Furthermore, based on the experimental results, we considered that the formation mechanism of the as-synthesized product of nitrogen-doped ZnS Camellia Brushfield Yellow-like structure could be explained by a synergic effect of Ostwald ripening and the self-assembled mechanism as proposed in Figure6. In the first stage, tiny crystalline nuclei are generated in the mixed solution and grow into nanoparticles. These nanoparticles are built and aggregated into spheres to minimize their surface area through the process known as Ostwald ripening [14, 15]. In the second stage, the thiocyanate ion (SCN-) coordinates with a variety of metal ions. It can form isothiocyanate (M-NCS) complexes that are further decomposed into metal sulfides with high purity [9]. The thermal decomposition of the Zn(SCN)2 complex at 500°C results in weakening of the coordination of Zn-NCS complex, and SO2, CO2, and N2 will be released gradually [15]. Then the crystallized particles grow along the 2D direction, resulting in the formation of nanosheets as shown in Figure 2(a1). As the mass diffusion and Ostwald ripening process proceed, the nanosheets can grow until all the nanoparticles are consumed, accompanied by their self-organization into the Camellia Brushfield Yellow-like structure. In addition, the increase of inflow flowrate of nitrogen until 140 mL/min has resulted in the increase of N atoms in the ZnS structure. According to the energy dispersive system (EDS) results on the catalyst surface, the nitrogen atom concentration of 15N/ZnS, 30N/ZnS, 70N/ZnS, and 140N/ZnS is 5.31%, 7.88%, 12.57%, and 17.98%, respectively. To quantify the impurities of carbon in the ZnS structure, elemental analysis (EA) was used and the carbon impurities were found to be 7.0±0.14% (w/w) in all as-synthesized ZnS powders, which implies that the thermal decomposition at 500°C cannot remove the carbon impurities perfectly in the ZnS structure, but the residual carbon concentration is relatively low. The different morphology of 140N/ZnS can be ascribed to the production of more decomposed products, including SO2, CO2, NO2, and N2, to go off readily from the catalyst surface during the decomposition process [16].Figure 6
Schematic illustration of possible growth mechanism of nitrogen-doped ZnS Camellia Brushfield Yellow-like structure.


### 3.2. Photocatalytic Activity

The photocatalytic activities of the prepared nitrogen-doped ZnS nanoparticles were evaluated for the degradation of Orange II dye under visible light irradiation. Figure7(a) shows the removal percentage of Orange II dye as a function of reaction time using bare and nitrogen-doped ZnS catalysts. The Orange II dye concentration was removed around 5.0% and 5.1% after 300 minutes of visible-light irradiation in the presence of commercial ZnS and as-synthesized bare ZnS, respectively. The optimal degradation ratio of Orange II dye using 15N/ZnS photocatalyst was found to be 75.7% after 300-minute irradiation. However, the increase of nitrogen-doped amount on the ZnS photocatalyst would result in the decrease of dye removal. The efficient removal of Orange II dye using visible-light photocatalysis by nitrogen-doped ZnS can be attributed to the response from occupied N2p localized states slightly above the valence band edge [11]. The decrease in photocatalytic activity observed in the higher nitrogen-doping ZnS, such as 140N/ZnS powder, may be attributed to a change in the crystal structure of the sample caused by the high doping of N in the crystal, though we did not find a noticeable change in XRD. As a result, such a surface roughness can function as traps for photogenerated electrons and holes, reducing the efficiency of photocatalysis [17].(a) Photocatalytic degradation of Orange II dye in the presence of bare and different nitrogen-doped ZnS photocatalysts; (b) plot of ln(C0/Ct) versus time for photocatalytic degradation of Orange II dye in presence of bare and different nitrogen-doped ZnS photocatalysts.
(a)
(b)Furthermore, the decomposition process is modeled as a pseudo-first-order reaction with the kinetics expressed by the equationln(C0/Ct)=kt, where C0 represents the initial concentration, Ct denotes the concentration at a given reaction time (t), and k is the reaction rate constant. From the linear extrapolations as shown in Figure 5(b), the reaction rate constants were calculated as 4.63×10-3 min−1, 3.04×10-3 min−1, 1.41×10-3 min−1, 1.09×10-3 min−1, and 1.80×10-4 min−1, respectively, using 15N/ZnS, 30N/ZnS, 70N/ZnS, 140N/ZnS, and bare ZnS photocatalysts. The results indicate that the N-doping ZnS shows better photocatalytic activity than bare ZnS under visible light irradiation due to the shorter band gap. However, the increase of N-doping will negate the efficiency by its surface roughness.


## 3.1. Characterization of Nitrogen-Doped ZnS Photocatalysts

The crystallinity and crystal phase of pure ZnS and nitrogen-doped ZnS photocatalysts were characterized by XRD as shown in Figure1. The major diffraction peaks of the ZnS (JCPDS card number 36-1450, the lattice parameters of a=3.820 Å and c=6.257 Å) with (100), (002), (101), (110), (103), and (112) planes were apparent for hexagonal wurtzite crystal structure. The (002) peak intensity is stronger than the (100) peak when the nitrogen-doped ZnS composite catalysts were prepared under different conditions. This is due to the change in the stacking sequence of the close packed planes of the ZnS crystal [7]. This observation is supported by the TEM results, and it indicates that nanosheets preferential growth occurs along the c-axis. The remaining peaks are generally broad and probably indicate relatively small dimensions of the materials [8]. The (100), (002), and (101) peaks strongly overlap, implying the formation of well-crystallized ZnS. At the same time, the atmospheric conditions have not influenced the crystal structure of ZnS [7].Figure 1
XRD patterns of nitrogen-doped and bare ZnS.HR-TEM images (Figure2(a)) of the as-synthesized catalysts can further confirm the flowery structure of the microspheres. The clear lattice fringes (Figure 2(b)) also indicate the polycrystalline nature of the petals. The interplanar spacing is 0.31 nm, which corresponds to the (002) plane of wurtzite ZnS. The corresponding selected area electron diffraction (SAED) patterns (Figure 2(c)) with a regular and clear ring diffraction spot array reveal that each petal is polycrystalline. Moreover, the major diffraction ring matches (100), (002), (101), (110), and (112) planes of ZnS phase.Figure 2
(a) HR-TEM images, (b) lattice fringes, and (c) the corresponding SAED pattern of 15N/ZnS.To better understand chemical states of the elements within the catalysts, XPS analyses were performed in this study. The typical XPS results are shown in Figure3. The peaks of S and Zn can be clearly seen in the survey spectra of all catalysts used (Figures 3(b) and 3(c)). The binding energies of S2p3/2 and S2p1/2 at 161.1 eV and 160.2 eV (Figure 3(b)) are consistent with the binding energy values in the literature [9]. Moreover, the binding energy of Zn2p3/2 and Zn2p1/2 is 1020.3 eV and 1043.3 eV (Figure 3(c)), belonging to the Zn2+ oxidation state in ZnS [9]. As for N, the binding energy of N1s at 395.9 eV belongs to atomic β-N (396 eV) [10]. According to the references, N1s peak at 396 eV is attributed to a characteristic peak of substitutional N, resulting from the nitrogen substitution of sulfur in the ZnS lattice [10–12]. In addition, the substitutional doping of N is thought to be the most pronounced because its p states contribute to the band gap narrowing by mixing with S2p states [10]. From the UV-Vis absorption spectra results as shown in Figure 4, the band gap of bare ZnS was calculated as 2.95 eV. The band gap of nitrogen-doped ZnS composite catalysts is between 2.58 and 2.74 eV. Therefore, the redshift in UV-Vis absorption spectra is enhanced by the nitrogen-doped ZnS composite catalysts, which implies the potential absorption to effectively harvest visible light.The survey XPS spectra of (a) 15N/ZnS photocatalysts and the high-resolution XPS spectra of (b) S2p, (c) Zn2p, and (d) N1s of 15N/ZnS photocatalysts.
(a)
(b)
(c)
(d)Figure 4
UV-Vis absorption spectra of as-synthesized photocatalysts.The morphology of nitrogen-doped ZnS composite catalysts was characterized by FE-SEM as shown in Figure5. The zinc isothiocyanate complex thermal decompositions have been carried out at 500°C under nitrogen conditions. The ZnS photocatalysts consist of irregular spheres with an average diameter of 1 μm and seem to facilitate microsphere aggregation. The images in Figures 5(a)–5(e) show that the nitrogen-doped ZnS Camellia Brushfield Yellow-like structure comprises numerous ZnS particles (petals) and the nitrogen-doped ZnS crystallites are self-organized into spherical assemblies, or a Camellia Brushfield Yellow-like morphology, with a puffy appearance. The nitrogen-doped ZnS products are all in this morphology with diameters ranging from 300 to 700 nm. The gap between particles (petals) was observed in the average range of 100 nm. The nitrogen-doped ZnS flower is quite open and puffy with ZnS particles (petals) that have good crystallinity [13]. When the nitrogen flowrate was increased from 15 to 140 mL/min, the morphology of the nitrogen-doped ZnS nanoparticles became more rough as seen in Figures 5(a)–5(e). Figure 5(f) clearly indicates that the flowery structures, from which one can see that dozens of 2D sheets are intercrossed with each other, have been formed throughout their self-assembly mechanisms.FE-SEM images of (a) ZnS, (b) 15N/ZnS, (c) 30N/ZnS, (d) 70N/ZnS, and (e) 140N/ZnS photocatalysts.
(a)
(b)
(c)
(d)
(e)
(f)Furthermore, based on the experimental results, we considered that the formation mechanism of the as-synthesized product of nitrogen-doped ZnS Camellia Brushfield Yellow-like structure could be explained by a synergic effect of Ostwald ripening and the self-assembled mechanism as proposed in Figure6. In the first stage, tiny crystalline nuclei are generated in the mixed solution and grow into nanoparticles. These nanoparticles are built and aggregated into spheres to minimize their surface area through the process known as Ostwald ripening [14, 15]. In the second stage, the thiocyanate ion (SCN-) coordinates with a variety of metal ions. It can form isothiocyanate (M-NCS) complexes that are further decomposed into metal sulfides with high purity [9]. The thermal decomposition of the Zn(SCN)2 complex at 500°C results in weakening of the coordination of Zn-NCS complex, and SO2, CO2, and N2 will be released gradually [15]. Then the crystallized particles grow along the 2D direction, resulting in the formation of nanosheets as shown in Figure 2(a1). As the mass diffusion and Ostwald ripening process proceed, the nanosheets can grow until all the nanoparticles are consumed, accompanied by their self-organization into the Camellia Brushfield Yellow-like structure. In addition, the increase of inflow flowrate of nitrogen until 140 mL/min has resulted in the increase of N atoms in the ZnS structure. According to the energy dispersive system (EDS) results on the catalyst surface, the nitrogen atom concentration of 15N/ZnS, 30N/ZnS, 70N/ZnS, and 140N/ZnS is 5.31%, 7.88%, 12.57%, and 17.98%, respectively. To quantify the impurities of carbon in the ZnS structure, elemental analysis (EA) was used and the carbon impurities were found to be 7.0±0.14% (w/w) in all as-synthesized ZnS powders, which implies that the thermal decomposition at 500°C cannot remove the carbon impurities perfectly in the ZnS structure, but the residual carbon concentration is relatively low. The different morphology of 140N/ZnS can be ascribed to the production of more decomposed products, including SO2, CO2, NO2, and N2, to go off readily from the catalyst surface during the decomposition process [16].Figure 6
Schematic illustration of possible growth mechanism of nitrogen-doped ZnS Camellia Brushfield Yellow-like structure.


## 3.2. Photocatalytic Activity

The photocatalytic activities of the prepared nitrogen-doped ZnS nanoparticles were evaluated for the degradation of Orange II dye under visible light irradiation. Figure7(a) shows the removal percentage of Orange II dye as a function of reaction time using bare and nitrogen-doped ZnS catalysts. The Orange II dye concentration was removed around 5.0% and 5.1% after 300 minutes of visible-light irradiation in the presence of commercial ZnS and as-synthesized bare ZnS, respectively. The optimal degradation ratio of Orange II dye using 15N/ZnS photocatalyst was found to be 75.7% after 300-minute irradiation. However, the increase of nitrogen-doped amount on the ZnS photocatalyst would result in the decrease of dye removal. The efficient removal of Orange II dye using visible-light photocatalysis by nitrogen-doped ZnS can be attributed to the response from occupied N2p localized states slightly above the valence band edge [11]. The decrease in photocatalytic activity observed in the higher nitrogen-doping ZnS, such as 140N/ZnS powder, may be attributed to a change in the crystal structure of the sample caused by the high doping of N in the crystal, though we did not find a noticeable change in XRD. As a result, such a surface roughness can function as traps for photogenerated electrons and holes, reducing the efficiency of photocatalysis [17].(a) Photocatalytic degradation of Orange II dye in the presence of bare and different nitrogen-doped ZnS photocatalysts; (b) plot of ln(C0/Ct) versus time for photocatalytic degradation of Orange II dye in presence of bare and different nitrogen-doped ZnS photocatalysts.
(a)
(b)Furthermore, the decomposition process is modeled as a pseudo-first-order reaction with the kinetics expressed by the equationln(C0/Ct)=kt, where C0 represents the initial concentration, Ct denotes the concentration at a given reaction time (t), and k is the reaction rate constant. From the linear extrapolations as shown in Figure 5(b), the reaction rate constants were calculated as 4.63×10-3 min−1, 3.04×10-3 min−1, 1.41×10-3 min−1, 1.09×10-3 min−1, and 1.80×10-4 min−1, respectively, using 15N/ZnS, 30N/ZnS, 70N/ZnS, 140N/ZnS, and bare ZnS photocatalysts. The results indicate that the N-doping ZnS shows better photocatalytic activity than bare ZnS under visible light irradiation due to the shorter band gap. However, the increase of N-doping will negate the efficiency by its surface roughness.


## 4. Conclusions

In summary, we have successfully synthesized nitrogen-doped ZnS composite catalysts with the Camellia Brushfield Yellow-like structure. The obtained surface and optical characteristics demonstrate that the nitrogen-doped ZnS can act as a good visible-light-driven photocatalyst. Their visible light assisted photocatalytic ability has been shown by the degradation of azo dye Orange II. The effect of nitrogen-doped amount on the photocatalytic on the removal of Orange II dye suggests that 15N/ZnS is the optimum loading for better photocatalytic ability.



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*Source: 801846-2013-10-02.xml*