# Facile Synthesis ofZnxCd1-xS Solid Solution Microspheres through Ultrasonic Spray Pyrolysis for Improved Photocatalytic Activity

Authors: Jianhui Huang; Wenting Lin; Liyan Xie; Wingkei Ho
Journal: Journal of Nanomaterials
 (2017)

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## Abstract

NanocrystalZnxCd1-xS solid solutions were successfully prepared using a facile and reproducible method of ultrasonic spray pyrolysis with Cd(Ac)2·2H2O, ZnCl2, and thiourea as precursors. Scanning electron microscopy and transmission electron microscopy images show that the prepared particles possess microspherical morphology. The band gaps of the solid solutions can be tuned by changing the constituent stoichiometries of Cd and Zn. The X-ray diffraction peaks gradually shift to small angle, and the absorption edge shifts to long wavelength with increasing Cd molar fraction in the solid solution. The sample prepared at the Cd/Zn ratio of 1 : 1 displays the optimal activity by using the photocatalytic degradation of methyl orange in the aqueous solution as model reactions under visible light irradiation. This study provides an effective route to prepare spherical ternary photocatalysts with mesoporous structure for further investigations and practical applications.


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## Body

## 1. Introduction

The controlled fabrication, characterization, and application of semiconductor nanomaterials with functional properties have attracted significant interest owning to their novel properties and promising applications in electrical, optoelectronic, and photochemical fields. The band gap energy of a semiconductor nanostructure is an important parameter for their applications. Band gap tuning has attracted considerable attention particularly in the region of photocatalysis, which requires suitable band gap and band position. Changing the size of nanostructured semiconductors is a common method used to tune their band gap due to the quantum confinement effect [1–3]. However, the physical and chemical properties of semiconductors are significantly influenced by their sizes; hence, changing the sizes of single-component semiconductor nanostructures has limited applications because of the possible alterations in the properties of the material. Doping with guest elements is another commonly utilized method, but both dopant type and concentration are difficult to control [4, 5]. Upon this, ternary semiconductor materials have gained considerable attention as their properties could be controlled by their morphology, particle size, and constituent stoichiometries. For example, ZnxCd1-xS [6, 7], a ternary II–VI semiconductor material, is formed using the solid solution of CdS with a narrow band gap of 2.4 eV [8, 9] and ZnS with a wide band gap of 3.7 eV [10]. Consequently, ZnxCd1-xS nanocrystals can form a series of semiconductors, whose band gap can be continuously tunable and cover the absorption light range from visible to ultraviolet [11, 12]. Up to now, the ZnxCd1-xS have been extensively researched in the organic pollutant degradation as efficient photocatalyst.Currently, various strategies are employed in the synthesis ofZnxCd1-xS nanostructures including chemical precipitation methods [13–15], hydrothermal or solvothermal reactions [10, 16–19], and chemical reduction processes [20]. In many cases, the synthesized ZnxCd1-xS were applied to the degradation of organic dyes [10, 15–17] such as methyl orange (MO), which is genotoxic [21] and carcinogenic [22] and difficult to degrade using conventional treatment processes. However, these traditional synthesis methods usually require severe conditions, such as high temperature, high pressure, toxic agent, or complicated equipment. In addition, most of them cannot be used for continuous fabrication, thereby limiting their application for mass production. Thus, a continuous method for synthesis of ZnxCd1-xS with special nanostructures and high yield must be developed to improve the design of high-performance materials for various applications.In this paper, we report a convenient, new method for continuous synthesis ofZnxCd1-xS microspheres through ultrasonic spray pyrolysis. The synthesized ZnxCd1-xS microspheres exhibit composition-dependent band gap energies and light absorption properties. The synthesized ZnxCd1-xS could be used to efficiently degrade organic pollutants in water.


## 2. Experimental Section

### 2.1. Catalyst Preparation

For synthesis ofZnxCd1-xS (0<x<1), 4x mmol ZnCl2, 4(1–x) mmol cadmium acetate [Cd(CH3COO)2·2H2O], and 20 mmol thiourea [CS(NH2)2] were added to 200 mL of deionized water under magnetic stirring to form a transparent colorless solution. The solution was nebulized by an ultrasonic atomizer (YUYUE402AI, Shanghai) at 1.7 MHz ± 10% and carried by air through a quartz tube with a flow rate of 10 L/min in a furnace thermostated at 500°C. The quartz reaction tube is 1 m in length with a diameter of 3.5 cm. The products were collected in a percolator with distilled water, separated by centrifugation, and washed thoroughly with distilled water and ethanol. The product was vacuum dried at 80°C for 2 h. A series of ZnxCd1-xS microspheres were synthesized by adjusting the ratio of the reactants, namely, ZnCl2 and Cd(CH3COO)2·2H2O (Table 1). The ZnxCd1-xS powder was obtained with a yield of 50~90% which depended on the constituent stoichiometries of ZnxCd1-xS.Table 1
Composition (Zn/Cd molar ratio) of the reactant solutions and the resultingZnxCd1-xS microspheres.
Samples
ZnS
Z
n
0.75
C
d
0.25
S
Z
n
0.50
C
d
0.5
0
S
Z
n
0.25
C
d
0.75
S
CdS
Molar ration of Zn/Cd in precursor
1 : 0
3 : 1
1 : 1
1 : 3
0 : 1
x of ZnxCd1-xS in producta
—
0.73
0.47
0.24
0.01
Abortion edge (nm)
335
390
454
484
525
Band gap (eV)
3.7
3.2
2.7
2.6
2.4
aThe value of x in product was detected by energy dispersive X-ray spectroscopy.


### 2.2. Characterization

The crystal structures and phase states of the synthesized materials were determined by X-ray diffractometry (XRD) on a Bruker D8 Advance X-ray diffractometer with Cu Ka radiation (λ = 1.54178 Å) at a scanning rate of 0.05° 2 θ/s and the scanning range was 10–80°. The morphologies of samples were observed with a scanning electron microscopy (JEOL JSM-6300F) operated at an accelerating voltage of 25 kV. Transmission electron microscopy (TEM) images were measured by using a Philips CM-120 electron microscopy instrument. UV–vis diffuse reflection spectroscopy (DRS) was performed on a Varian Cary 100 Scan UV-visible system equipped with Labsphere diffuse reflectance accessory using BaSO4 as the reference material. The reflection spectra were converted to absorbance spectra by Kubelka–Munk method. Brunauer–Emmett–Teller (BET) surface areas and pore volume were determined by N2 adsorption/desorption isotherms measurements at 77 K by using an automated nitrogen adsorption analyzer (ASAP 2020, Micromeritics, America). The samples were degassed under vacuum at 120°C and kept for 5 h before data acquisition.


### 2.3. Evaluation of Photocatalytic Activity

The photocatalytic activities of theZnxCd1-xS were evaluated by degrading of methyl orange (MO) in aqueous solution under visible light irradiation. In the typical photocatalytic degradation experiment process, the tested catalyst (40 mg) was suspended in a 100 mL Pyrex glass vessel containing MO aqueous solution (80 mL, 10 ppm) to produce a suspension at room temperature with the magnetic stirring. The suspension was stirred in darkness for 2 h to achieve the adsorption equilibrium. The 300 W halogen lamp (Philips Electronics) with a 420 nm cutoff filter was used as visible light source which was positioned beside a cylindrical reaction vessel with a flat side. The system was water cooled to maintain the temperature. In a certain time, 3 mL of the reaction suspension was collected and centrifuged at 6000 rpm for 3 min to remove the catalyst. The residual pollution concentration was collected and analyzed using a Varian Cary 50 Scan UV/vis spectrophotometer.


## 2.1. Catalyst Preparation

For synthesis ofZnxCd1-xS (0<x<1), 4x mmol ZnCl2, 4(1–x) mmol cadmium acetate [Cd(CH3COO)2·2H2O], and 20 mmol thiourea [CS(NH2)2] were added to 200 mL of deionized water under magnetic stirring to form a transparent colorless solution. The solution was nebulized by an ultrasonic atomizer (YUYUE402AI, Shanghai) at 1.7 MHz ± 10% and carried by air through a quartz tube with a flow rate of 10 L/min in a furnace thermostated at 500°C. The quartz reaction tube is 1 m in length with a diameter of 3.5 cm. The products were collected in a percolator with distilled water, separated by centrifugation, and washed thoroughly with distilled water and ethanol. The product was vacuum dried at 80°C for 2 h. A series of ZnxCd1-xS microspheres were synthesized by adjusting the ratio of the reactants, namely, ZnCl2 and Cd(CH3COO)2·2H2O (Table 1). The ZnxCd1-xS powder was obtained with a yield of 50~90% which depended on the constituent stoichiometries of ZnxCd1-xS.Table 1
Composition (Zn/Cd molar ratio) of the reactant solutions and the resultingZnxCd1-xS microspheres.
Samples
ZnS
Z
n
0.75
C
d
0.25
S
Z
n
0.50
C
d
0.5
0
S
Z
n
0.25
C
d
0.75
S
CdS
Molar ration of Zn/Cd in precursor
1 : 0
3 : 1
1 : 1
1 : 3
0 : 1
x of ZnxCd1-xS in producta
—
0.73
0.47
0.24
0.01
Abortion edge (nm)
335
390
454
484
525
Band gap (eV)
3.7
3.2
2.7
2.6
2.4
aThe value of x in product was detected by energy dispersive X-ray spectroscopy.


## 2.2. Characterization

The crystal structures and phase states of the synthesized materials were determined by X-ray diffractometry (XRD) on a Bruker D8 Advance X-ray diffractometer with Cu Ka radiation (λ = 1.54178 Å) at a scanning rate of 0.05° 2 θ/s and the scanning range was 10–80°. The morphologies of samples were observed with a scanning electron microscopy (JEOL JSM-6300F) operated at an accelerating voltage of 25 kV. Transmission electron microscopy (TEM) images were measured by using a Philips CM-120 electron microscopy instrument. UV–vis diffuse reflection spectroscopy (DRS) was performed on a Varian Cary 100 Scan UV-visible system equipped with Labsphere diffuse reflectance accessory using BaSO4 as the reference material. The reflection spectra were converted to absorbance spectra by Kubelka–Munk method. Brunauer–Emmett–Teller (BET) surface areas and pore volume were determined by N2 adsorption/desorption isotherms measurements at 77 K by using an automated nitrogen adsorption analyzer (ASAP 2020, Micromeritics, America). The samples were degassed under vacuum at 120°C and kept for 5 h before data acquisition.


## 2.3. Evaluation of Photocatalytic Activity

The photocatalytic activities of theZnxCd1-xS were evaluated by degrading of methyl orange (MO) in aqueous solution under visible light irradiation. In the typical photocatalytic degradation experiment process, the tested catalyst (40 mg) was suspended in a 100 mL Pyrex glass vessel containing MO aqueous solution (80 mL, 10 ppm) to produce a suspension at room temperature with the magnetic stirring. The suspension was stirred in darkness for 2 h to achieve the adsorption equilibrium. The 300 W halogen lamp (Philips Electronics) with a 420 nm cutoff filter was used as visible light source which was positioned beside a cylindrical reaction vessel with a flat side. The system was water cooled to maintain the temperature. In a certain time, 3 mL of the reaction suspension was collected and centrifuged at 6000 rpm for 3 min to remove the catalyst. The residual pollution concentration was collected and analyzed using a Varian Cary 50 Scan UV/vis spectrophotometer.


## 3. Results and Discussion

### 3.1. Structure

Figure1 shows the XRD patterns of the as-prepared ZnS, ZnxCd1-xS, and CdS samples. The size-broadening effects can be found in all of the XRD patterns, indicating the finite size of the samples. For CdS and ZnxCd1-xS samples, the XRD patterns show strong characteristic peaks of (100), (002), (101), (102), (110), (103), and (112), which can be indexed as wurtzite-phase structure. For ZnS sample, the XRD pattern mainly reflects three strong peaks of (111), (220), and (311), which can be indexed as a zincblende structure with weak wurtzite. The diffraction peaks of CdS and ZnxCd1-xS gradually shift to larger angles with increasing Zn content. This finding also indicates that no phase separation occurs during nucleation of ZnS or CdS in the ZnxCd1-xS samples [23].Figure 1
X-ray diffraction patterns of CdS,ZnxCd1-xS, and ZnS samples.The lattice constantsa and c for the hexagonal phase of ZnxCd1-xS are calculated using the following equation[24]:(1)1d=43h2+hk+k2a2+l2c2.As shown in Figure2, the value of lattice constants “a” and “c” exhibits nearly linear relationship to Zn composition in the region of 0–0.75. The linear relationship almost obeys the empirical formulations of Vegard’s law [25–27], which suggests that the Zn/Cd ratio in the produced ZnxCd1-xS is almost the same as the ratio of the reactants. This trend also confirms that the as-prepared samples underwent homology formation without separating ZnS and CdS phases.Figure 2
Composition dependence of the cell constantsa (▲) and c (■) axis values of ZnxCd1-xS spheres as a function of Zn content (x). The solid line was calculated using Vegard’s law.


### 3.2. Morphology

Figures3(a), 3(b), and 3(c) depict the SEM images of the as-prepared ZnS, CdS, and Zn0.50Cd0.50S, respectively. All samples prepared with ultrasonic spray pyrolysis consist entirely of spheres, with size ranging from 100 nm to 1.0 μm. During preparation, the use of ultrasonic nebulizer endows the samples with a spherical morphology, which could generate aerosol containing Zn and Cd ions as well as thiourea. These aerosols would serve as microreactors when carried into a tubular reactor with constant air flow rate under pyrolysis conditions. At high temperatures, water in aerosols evaporates quickly. Thiourea in the droplet decomposes and releases H2S, which would quickly react with Zn and Cd ions in the aerosols to generate spherical products. The product dimension is determined by the size of droplets in the aerosol, which could be adjusted by controlling the nebulizing condition.Figure 3
Scanning electron microscopy (SEM) and transmission electron microscopy (TEM) images of the prepared samples: (a) SEM of CdS, (b) SEM of ZnS, (c) SEM of Zn0.50Cd0.50S, (d) TEM of Zn0.50Cd0.50S, and (e) energy dispersive X-ray analysis spectra of Zn0.50Cd0.50S.
(a)
(b)
(c)
(d)
(e)The typical high-magnified TEM image of the Zn0.50Cd0.50S sphere shows that the prepared spheres are composed of small nanoparticles and exhibit porous structure (Figure 3(d)). The porous surface with nanosized crystal structure improves adsorptivity, which is vital for catalytic applications. The composition of the Zn0.50Cd0.50S sphere was determined by energy dispersive X-ray spectroscopy (EDX). The results indicate that the as-prepared samples contain Zn, Cd, and S, and some of the Cu signal originates from the substrate (Figure 3(e)). Moreover, the Zn/Cd ratio in the produced ZnxCd1-xS microspheres is almost identical to that in the precursor solution (Table 1). This finding suggests that Zn and Cd in the precursor have reacted completely. These results are consistent with the result deduced with Vegard’s law. Excess thiourea in the precursor supplies sufficient sulfides to ensure that Zn2+ and Cd2+ react completely. Hence, the composition of ZnxCd1-xS can be easily and accurately adjusted using the proposed synthesis method.


### 3.3. UV–Vis Diffuse Reflectance Spectroscopy and Band Structure

An optimal photocatalytic material exhibits appropriate band position and band gap that absorbs light in the visible range. Figure4(a) shows the UV-visible absorption spectra of samples prepared with different ratios of Zn/Cd. The spectra indicate a typical semiconductor absorption behavior. The absorption edges of the samples gradually red shift from 335 nm to 525 nm with increasing Cd content, indicating the narrowing of the band gaps. The inset in Figure 4 represents the suspension of the samples whose color changes from white to orange. Hence, the range of light absorption can be adjusted from ultraviolet to blue-green light. The band gaps calculated from the onset of the absorbance edge spectra for each catalyst are presented in Table 1. All the samples of ZnxCd1-xS show band gaps between CdS (2.4 eV) and ZnS (3.7 eV). This large shift in the absorbance edge should be attributed to the changes in the composition rather than the quantum size effects. The compositional variation of ZnxCd1-xS solid solutions affects their band gap, because the replacement of Cd cations by Zn in the crystal lattice modifies the position of the conduction band through hybridization of the Cd 5s5p level with the negative Zn 4s4p level [28, 29].Figure 4
(a) Diffuse reflectance UV–vis spectra and the aqueous solution image (inset) of CdS,ZnxCd1-xS, and ZnS samples. (b) Conduction and valence band edge potentials of ZnxCd1-xS obtained by theoretical calculation.
(a)
(b)Figure4(b) shows the estimated ECB and EVB edge potentials of ZnxCd1-xS microspheres calculated using (2) and (3), respectively [30, 31]:(2)ECB=XCd1-xXZnxXS11/2-12Eg+E0,(3)EVB=ECB+Eg,where XCd, XZn, and XS are 4.3, 4.45, and 6.22 eV, respectively, which correspond to the absolute electronegativities of the constituent atoms, namely, Cd, Zn, and S, respectively. ECB and EVB are the conduction band minimum and valence band maximum of ZnxCd1-xS, respectively. Eg is the bandgap energy of ZnxCd1-xS which was determined by UV–vis diffuse reflectance spectra (DRS), and E0 = −4.5 eVVAS at pH = 0 [30]. The results indicate that the band position can be tuned by changing the constituent stoichiometries of ZnxCd1-xS. Taking Cd0.50Zn0.50S microspheres, for example, the ECB (−0.65 eV) and EVB edge levels (−0.65 eV) are more negative and positive than those of CdS. Hence, Cd0.50Zn0.50S can be excited by visible light, and its photogenerated charge carriers possess stronger redox ability than that of CdS. Therefore, Cd0.50Zn0.50S may have promising photocatalytic performance for highly efficient organic pollutant degradation.


### 3.4. BET Surface Areas

Figure5 shows the nitrogen adsorption–desorption isotherms and Barrett–Joyner–Halenda (BJH) pore size distribution plots of Cd0.50Zn0.50S. Nitrogen adsorption measurements demonstrate that the prepared Zn0.50Cd0.50S exhibits type IV isotherm behavior, which is representative of mesoporous solids. The specific surface of Zn0.50Cd0.50S calculated by multipoint BET method is 51 m2/g. The BJH pore size analysis (utilizing the isotherm desorption branch) shows that the sphere has a wide pore size distribution, ranging from 0 nm to 80 nm and peaking at 10 nm with a pore volume of 0.13/g (Figure 5(b)).Figure 5
N2 physisorption results at 77 K of Zn0.50Cd0.50S. (a) Adsorption–desorption isotherms (open and filled symbols correspond to the adsorption and desorption branches, resp.). (b) Pore size distributions derived from the desorption branches using the Barrett–Joyner–Halenda method.
(a)
(b)


### 3.5. Photocatalytic Performance

The photocatalytic activity ofZnxCd1-xS nanoparticles was evaluated by degradation of MO molecules in water. The control experiment was performed before the test without using any photocatalyst. Figure 6 shows the changes in the concentration of MO in the presence of photocatalysts and under irradiation of visible light (λ > 420 nm). Figure 6(a) shows that the main absorption peak of MO (λ = 464 nm) nearly disappears after 4 h of irradiation in the presence of Zn0.50Cd0.50S, which indicates that MO in water is almost completely degraded. The control experiment indicates that MO is stable under the testing conditions without photocatalyst. The concentration of MO is almost invariable in the dark situation indicating that the adsorption equilibrium had been achieved after being stirred in darkness for 2 h. Some comparative experiments were conducted to investigate the liquid-phase photocatalytic activity under different conditions (Figure 6(b)). The y-axis of degradation is Ct/C0. Ct is the absorption of MO at each irradiated time interval at a wavelength of 464 nm. C0 is the absorption of the starting concentration upon reaching the adsorption–desorption equilibrium. Under identical conditions, ZnxCd1-xS shows considerably higher activity than that of CdS, ZnS, and mechanically mixed CdS and ZnS. Thus, the visible photocatalytic activity of ZnxCd1-xS could be ascribed to the solid solution formation between CdS and ZnS. In addition, the test shows that the activities of the samples are influenced by their compositions. The photocatalytic conversion of degraded MO over Zn0.50Cd0.50S after 4 h is about 96%, which is higher than that of Zn0.25Cd0.75S and Zn0.75Cd0.25S; this difference may be ascribed to the appropriate band gap and band position of Zn0.50Cd0.50S. The prepared Zn0.50Cd0.50S was also applied to the degradation of other dyes such as congo red (10 ppm, 80 mL). The peak at wavelength of 488 nm is used to evaluate the degradation of congo red. The result is shown in Figure 7 which indicates that the photocatalytic conversion ratio of congo red was up to 97% in 120 min in the presence of Zn0.50Cd0.50S. The control experiment indicates that the congo red is stable without Zn0.50Cd0.50S under irradiation or with Zn0.50Cd0.50S in the dark. The result also proved that the prepared Zn0.50Cd0.50S is effective in degrading organic dye in water.Figure 6
The concentration changes of methyl orange under different conditions.
(a)
(b)Figure 7
The concentration changes of congo red under different conditions.Figure8 shows the durability of Zn0.50Cd0.50S microspheres for the degradation of MO under the same reaction conditions. Zn0.50Cd0.50S microspheres were recovered by being centrifuged without any treatment. The results indicate that the photocatalytic activity of Zn0.50Cd0.50S did not decrease significantly after three successive cycles. The activity of the photocatalyst was maintained effectively. The slight decrease of MO degradation rate can be attributed to the reduction of photocatalyst in each sample collection. These results demonstrate that the Zn0.50Cd0.50S microspheres prepared by ultrasonic spray pyrolysis are stable. In the further study, we also prepared ZnxCd1-xS by hydrothermal processes under optimal conditions according to the literature [10] and tested its photocatalytic activity in our conditions. The Zn0.50Cd0.50S prepared by ultrasonic spray pyrolysis method shows improved activity which is higher than the samples prepared by hydrothermal process.Figure 8
Catalyst cycling in the photocatalytic degradation of methyl orange in the presence of Zn0.50Cd0.50S.


## 3.1. Structure

Figure1 shows the XRD patterns of the as-prepared ZnS, ZnxCd1-xS, and CdS samples. The size-broadening effects can be found in all of the XRD patterns, indicating the finite size of the samples. For CdS and ZnxCd1-xS samples, the XRD patterns show strong characteristic peaks of (100), (002), (101), (102), (110), (103), and (112), which can be indexed as wurtzite-phase structure. For ZnS sample, the XRD pattern mainly reflects three strong peaks of (111), (220), and (311), which can be indexed as a zincblende structure with weak wurtzite. The diffraction peaks of CdS and ZnxCd1-xS gradually shift to larger angles with increasing Zn content. This finding also indicates that no phase separation occurs during nucleation of ZnS or CdS in the ZnxCd1-xS samples [23].Figure 1
X-ray diffraction patterns of CdS,ZnxCd1-xS, and ZnS samples.The lattice constantsa and c for the hexagonal phase of ZnxCd1-xS are calculated using the following equation[24]:(1)1d=43h2+hk+k2a2+l2c2.As shown in Figure2, the value of lattice constants “a” and “c” exhibits nearly linear relationship to Zn composition in the region of 0–0.75. The linear relationship almost obeys the empirical formulations of Vegard’s law [25–27], which suggests that the Zn/Cd ratio in the produced ZnxCd1-xS is almost the same as the ratio of the reactants. This trend also confirms that the as-prepared samples underwent homology formation without separating ZnS and CdS phases.Figure 2
Composition dependence of the cell constantsa (▲) and c (■) axis values of ZnxCd1-xS spheres as a function of Zn content (x). The solid line was calculated using Vegard’s law.


## 3.2. Morphology

Figures3(a), 3(b), and 3(c) depict the SEM images of the as-prepared ZnS, CdS, and Zn0.50Cd0.50S, respectively. All samples prepared with ultrasonic spray pyrolysis consist entirely of spheres, with size ranging from 100 nm to 1.0 μm. During preparation, the use of ultrasonic nebulizer endows the samples with a spherical morphology, which could generate aerosol containing Zn and Cd ions as well as thiourea. These aerosols would serve as microreactors when carried into a tubular reactor with constant air flow rate under pyrolysis conditions. At high temperatures, water in aerosols evaporates quickly. Thiourea in the droplet decomposes and releases H2S, which would quickly react with Zn and Cd ions in the aerosols to generate spherical products. The product dimension is determined by the size of droplets in the aerosol, which could be adjusted by controlling the nebulizing condition.Figure 3
Scanning electron microscopy (SEM) and transmission electron microscopy (TEM) images of the prepared samples: (a) SEM of CdS, (b) SEM of ZnS, (c) SEM of Zn0.50Cd0.50S, (d) TEM of Zn0.50Cd0.50S, and (e) energy dispersive X-ray analysis spectra of Zn0.50Cd0.50S.
(a)
(b)
(c)
(d)
(e)The typical high-magnified TEM image of the Zn0.50Cd0.50S sphere shows that the prepared spheres are composed of small nanoparticles and exhibit porous structure (Figure 3(d)). The porous surface with nanosized crystal structure improves adsorptivity, which is vital for catalytic applications. The composition of the Zn0.50Cd0.50S sphere was determined by energy dispersive X-ray spectroscopy (EDX). The results indicate that the as-prepared samples contain Zn, Cd, and S, and some of the Cu signal originates from the substrate (Figure 3(e)). Moreover, the Zn/Cd ratio in the produced ZnxCd1-xS microspheres is almost identical to that in the precursor solution (Table 1). This finding suggests that Zn and Cd in the precursor have reacted completely. These results are consistent with the result deduced with Vegard’s law. Excess thiourea in the precursor supplies sufficient sulfides to ensure that Zn2+ and Cd2+ react completely. Hence, the composition of ZnxCd1-xS can be easily and accurately adjusted using the proposed synthesis method.


## 3.3. UV–Vis Diffuse Reflectance Spectroscopy and Band Structure

An optimal photocatalytic material exhibits appropriate band position and band gap that absorbs light in the visible range. Figure4(a) shows the UV-visible absorption spectra of samples prepared with different ratios of Zn/Cd. The spectra indicate a typical semiconductor absorption behavior. The absorption edges of the samples gradually red shift from 335 nm to 525 nm with increasing Cd content, indicating the narrowing of the band gaps. The inset in Figure 4 represents the suspension of the samples whose color changes from white to orange. Hence, the range of light absorption can be adjusted from ultraviolet to blue-green light. The band gaps calculated from the onset of the absorbance edge spectra for each catalyst are presented in Table 1. All the samples of ZnxCd1-xS show band gaps between CdS (2.4 eV) and ZnS (3.7 eV). This large shift in the absorbance edge should be attributed to the changes in the composition rather than the quantum size effects. The compositional variation of ZnxCd1-xS solid solutions affects their band gap, because the replacement of Cd cations by Zn in the crystal lattice modifies the position of the conduction band through hybridization of the Cd 5s5p level with the negative Zn 4s4p level [28, 29].Figure 4
(a) Diffuse reflectance UV–vis spectra and the aqueous solution image (inset) of CdS,ZnxCd1-xS, and ZnS samples. (b) Conduction and valence band edge potentials of ZnxCd1-xS obtained by theoretical calculation.
(a)
(b)Figure4(b) shows the estimated ECB and EVB edge potentials of ZnxCd1-xS microspheres calculated using (2) and (3), respectively [30, 31]:(2)ECB=XCd1-xXZnxXS11/2-12Eg+E0,(3)EVB=ECB+Eg,where XCd, XZn, and XS are 4.3, 4.45, and 6.22 eV, respectively, which correspond to the absolute electronegativities of the constituent atoms, namely, Cd, Zn, and S, respectively. ECB and EVB are the conduction band minimum and valence band maximum of ZnxCd1-xS, respectively. Eg is the bandgap energy of ZnxCd1-xS which was determined by UV–vis diffuse reflectance spectra (DRS), and E0 = −4.5 eVVAS at pH = 0 [30]. The results indicate that the band position can be tuned by changing the constituent stoichiometries of ZnxCd1-xS. Taking Cd0.50Zn0.50S microspheres, for example, the ECB (−0.65 eV) and EVB edge levels (−0.65 eV) are more negative and positive than those of CdS. Hence, Cd0.50Zn0.50S can be excited by visible light, and its photogenerated charge carriers possess stronger redox ability than that of CdS. Therefore, Cd0.50Zn0.50S may have promising photocatalytic performance for highly efficient organic pollutant degradation.


## 3.4. BET Surface Areas

Figure5 shows the nitrogen adsorption–desorption isotherms and Barrett–Joyner–Halenda (BJH) pore size distribution plots of Cd0.50Zn0.50S. Nitrogen adsorption measurements demonstrate that the prepared Zn0.50Cd0.50S exhibits type IV isotherm behavior, which is representative of mesoporous solids. The specific surface of Zn0.50Cd0.50S calculated by multipoint BET method is 51 m2/g. The BJH pore size analysis (utilizing the isotherm desorption branch) shows that the sphere has a wide pore size distribution, ranging from 0 nm to 80 nm and peaking at 10 nm with a pore volume of 0.13/g (Figure 5(b)).Figure 5
N2 physisorption results at 77 K of Zn0.50Cd0.50S. (a) Adsorption–desorption isotherms (open and filled symbols correspond to the adsorption and desorption branches, resp.). (b) Pore size distributions derived from the desorption branches using the Barrett–Joyner–Halenda method.
(a)
(b)


## 3.5. Photocatalytic Performance

The photocatalytic activity ofZnxCd1-xS nanoparticles was evaluated by degradation of MO molecules in water. The control experiment was performed before the test without using any photocatalyst. Figure 6 shows the changes in the concentration of MO in the presence of photocatalysts and under irradiation of visible light (λ > 420 nm). Figure 6(a) shows that the main absorption peak of MO (λ = 464 nm) nearly disappears after 4 h of irradiation in the presence of Zn0.50Cd0.50S, which indicates that MO in water is almost completely degraded. The control experiment indicates that MO is stable under the testing conditions without photocatalyst. The concentration of MO is almost invariable in the dark situation indicating that the adsorption equilibrium had been achieved after being stirred in darkness for 2 h. Some comparative experiments were conducted to investigate the liquid-phase photocatalytic activity under different conditions (Figure 6(b)). The y-axis of degradation is Ct/C0. Ct is the absorption of MO at each irradiated time interval at a wavelength of 464 nm. C0 is the absorption of the starting concentration upon reaching the adsorption–desorption equilibrium. Under identical conditions, ZnxCd1-xS shows considerably higher activity than that of CdS, ZnS, and mechanically mixed CdS and ZnS. Thus, the visible photocatalytic activity of ZnxCd1-xS could be ascribed to the solid solution formation between CdS and ZnS. In addition, the test shows that the activities of the samples are influenced by their compositions. The photocatalytic conversion of degraded MO over Zn0.50Cd0.50S after 4 h is about 96%, which is higher than that of Zn0.25Cd0.75S and Zn0.75Cd0.25S; this difference may be ascribed to the appropriate band gap and band position of Zn0.50Cd0.50S. The prepared Zn0.50Cd0.50S was also applied to the degradation of other dyes such as congo red (10 ppm, 80 mL). The peak at wavelength of 488 nm is used to evaluate the degradation of congo red. The result is shown in Figure 7 which indicates that the photocatalytic conversion ratio of congo red was up to 97% in 120 min in the presence of Zn0.50Cd0.50S. The control experiment indicates that the congo red is stable without Zn0.50Cd0.50S under irradiation or with Zn0.50Cd0.50S in the dark. The result also proved that the prepared Zn0.50Cd0.50S is effective in degrading organic dye in water.Figure 6
The concentration changes of methyl orange under different conditions.
(a)
(b)Figure 7
The concentration changes of congo red under different conditions.Figure8 shows the durability of Zn0.50Cd0.50S microspheres for the degradation of MO under the same reaction conditions. Zn0.50Cd0.50S microspheres were recovered by being centrifuged without any treatment. The results indicate that the photocatalytic activity of Zn0.50Cd0.50S did not decrease significantly after three successive cycles. The activity of the photocatalyst was maintained effectively. The slight decrease of MO degradation rate can be attributed to the reduction of photocatalyst in each sample collection. These results demonstrate that the Zn0.50Cd0.50S microspheres prepared by ultrasonic spray pyrolysis are stable. In the further study, we also prepared ZnxCd1-xS by hydrothermal processes under optimal conditions according to the literature [10] and tested its photocatalytic activity in our conditions. The Zn0.50Cd0.50S prepared by ultrasonic spray pyrolysis method shows improved activity which is higher than the samples prepared by hydrothermal process.Figure 8
Catalyst cycling in the photocatalytic degradation of methyl orange in the presence of Zn0.50Cd0.50S.


## 4. Conclusion

A facile and aerosol-assisted synthesis strategy was developed to prepareZnxCd1-xS microspheres by using Cd(CH3COO)2·2H2O, ZnCl2, and CS(NH2)2 as precursors. The composition dependence of the UV–vis spectra shows continuous red shift with increased Cd content. The photocatalytic activity tests show that samples prepared at the Cd/Zn ratio of 1 : 1 possess the optimal activity for MO degradation under visible light. The conversion ratio of MO degradation is about 96%. In this work, a new convenient route to synthesize ternary nonintegral stoichiometry compound ZnxCd1-xS microspheres is presented which exhibits potential for fabrication of other ternary semiconductors as photocatalysts and optoelectronic materials.



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*Source: 6356021-2017-05-14.xml*