# Synthesis and Photocatalytic Properties of Co-Doped Zn1-xCoxMn2O Hollow Nanospheres

Authors: Long Ma; Zhiqiang Wei; Xueliang Zhu; Jiahao Liang; Xudong Zhang
Journal: Journal of Nanomaterials
 (2019)

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## Abstract

A series of Co-doped Zn1-xCoxMn2O nanocrystals with a spinel structure were successfully prepared by hydrothermal method, and the influence of Co doping concentration on the microstructure, morphology, elemental composition, and optical and photocatalytic properties of the samples was characterized. The experimental results show that all samples exhibit a tetragonal structure, Co2+ ions are successfully substituted for the lattice site of Zn2+ to generate ZnMn2O4 nanocrystals, and the crystalline size decreases as Co-doped concentration increase. The morphologies are loose hollow microsphere structures. The band gap of Zn1−xCoxMn2O samples is smaller than that of pure ZnMn2O4 and has been red shifted. The photocatalytic activity of doped Zn1−xCoxMn2O4 samples is obviously higher than that of pure ZnMn2O4 samples for the photodegradation of MO under visible light irradiation. All these results demonstrate that Co-doped spinel ZnMn2O4 nanocrystals are a meaningful choice for photocatalytic degradation of the pollutants.


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## Body

## 1. Introduction

In recent decades, with the development of modern industry, the growth of population, and the acceleration of urbanization, the increased pollution of natural water and air has become one of the major challenges that the modern human society and the ecological system are is facing and the main pollution sources are nondegradable and toxic artificial dyes [1–4]. The toxic compounds in water media cause serious harm to human health. Nanoscale semiconductor photocatalysts have attracted extensive research interest in the field of environmental restoration owing to their potential value, such as nontoxic, inexpensive, strong oxidizing activity, and chemical stability [5–8].Spinel structure ZnMn2O4 belongs to I41/amd space group, and with a narrow band gap of 1.86 eV [9, 10]. ZnMn2O4 nanocrystals possess unique properties that are quite different from those of the bulk solid state due to their surface effect, quantum size effect, small size effect, and quantum tunnelling effect [11, 12]. Spinel structure ZnMn2O4 nanocrystals have attracted considerable attention due to their novel properties and broad application prospect in the gas sensor [13], photocatalyst [14], supercapacitor electrode [15, 16], lithium ion battery anode [17], energy storage [18], nonvolatile memory [19], etc. In recent years, some researchers have studied transition metal ion-doped ZnMn2O4 nanocrystals to obtain the desired crystal structure and energy band structure by providing extra positive carriers in the host material [20]. The crystal structure and energy band structure of semiconductor materials can be modified to improve their physical properties by controlling the preparation process, changing the type and amount of doped elements [21, 22]. In addition, transition metal ion configuration doping can significantly improve the separation rate of photoinduced carriers in semiconductor photocatalysts, inhibit the recombination of photoinduced electron hole pairs, and greatly improve photocatalytic activity [23]. Unfortunately, as far as we know, there are few reports about the influence of doping concentration on the photocatalytic performance of the transition metal-ion doped ZnMn2O4 nanostructure. Therefore, the main purpose of this study is to study the effect of doping concentration on the microstructure and photocatalytic activity.In this work, Co-dopedZn1−xCoxMn2O nanocrystals with different ratios (x=0, 0.1, 0.3, and 0.5) were successfully synthesized by hydrothermal method. The influence of Co doping concentration on the microstructure, morphology, elemental composition, and optical properties of the samples was investigated by X-ray diffraction (XRD), field emission scanning electron microscopy (FESEM), X-ray energy dispersive spectrometry (XEDS), ultraviolet-visible spectroscopy (UV-Vis), and Fourier transform infrared spectroscopy (FT-IR), and the photocatalytic activity of Zn1−xCoxMn2O nanocrystals was evaluated by the photodegradation of MO dye in aqueous solution under UV light irradiation.


## 2. Material and Methods

### 2.1. Synthesis

A facile hydrothermal method was used to synthesizeZn1−xCoxMn2O4 (x=0, 0.1, 0.3, and 0.5) nanocrystals. In a typical experiment, zinc nitrate (Zn(NO3)2·6H2O, AR, Tianjin Kaixin Chemical Industry Co. Ltd.), manganese nitrate (Mn(NO3)2·6H2O, AR, Tianjin Kemeiou Reagent Co. Ltd.), cobalt nitrate (Co(NO3)2·6H2O, AR, Shanghai Zhongqin Reagent Co. Ltd.), polyethylene glycol-400 (PEG-400, AR, Shandong West Asia Chemical Reagent Co. Ltd.), absolute ethyl alcohol (AR, China Pharmaceutical Group Reagent Co. Ltd), and citric acid (AR, Tianjin Kemeiou Reagent Co. Ltd.) were used in this study without any further purification. According to the chemical formula of Zn1-xCoxMn2O4 (x=0, 0.1, 0.3, and 0.5) and the molar ratio of metal cations, the stoichiometric quantities of zinc nitrate, cobalt nitrate, and manganese nitrate as precursors were weighed. Zn(NO3)2, Mn(NO3)2, and Co(NO3)2 were mixed in distilled water and magnetically stirred at room temperature for 30 min. Meanwhile, appropriate amounts of citric acid and PEG-400 were dripped into the above-mixed solution under magnetic stirring for 3 hours. Subsequently, the resulting solution was transferred to a 100 mL Teflon-lined stainless steel autoclave. The hydrothermal reaction process was conducted at 180°C for 24 h in an oven and then cooled to room temperature naturally. Finally, the resultant precipitate was separated centrifugally, washed several times with distilled water and absolute alcohol, respectively, and then dried at 60°C in a vacuum oven for 10 h. Thus, Zn1−xCoxMn2O4 nanocrystals were collected and used for further study. By comparison, Zn1−xCoxMn2O4 nanoparticles with different ratios (x=0, 0.1, 0.3, and 0.5) were also prepared using the abovementioned procedure.


### 2.2. Characterization

The crystal structure of the as-obtained samples was examined by X-ray diffractometer (XRD) using the CuKα source (λ=1.54056 Å), the scanning rate 0.005°/s, and step size 0.02°. The morphology of the samples was investigated using a field emission scanning electron microscope (SEM) (JEOL JSM-6701F) equipped with an X-ray energy dispersive spectroscopy (XEDS). The ultraviolet-visible (UV-Vis) diffuse reflectance spectra (DRS) of the products were recorded on a UV-Vis spectrophotometer (PERSEE TU-1901) using BaSO4 as reference. Fourier transform infrared spectroscopy (FT-IR) studies were measured by a Nexus 670 FT-IR spectrometer in the range of 4000–400 cm-1.


### 2.3. Photocatalytic Activity Test

The photocatalytic property of the samples was evaluated by measuring the degradation of methyl orange (MO) aqueous solution in a cylindrical glass vessel under simulated sunlight, and the reaction vessel was kept at a constant temperature using a circulating cooling system. The reaction solution was irradiated with the light source of a 300 W xenon lamp, and the distance between the solution surface and the light source was kept at 30 cm to avoid thermal effect. In this work, 20 mg of the as-synthesized samples was dispersed into a 100 mL MO aqueous solution (the initial MO aqueous solution concentration was 10 mg/L). The mixed suspensions were magnetically stirred for 30 min in the dark to reach the adsorption-desorption equilibrium between the photocatalyst and organic dye MO. During the photocatalytic process, about 2.5 mL of the reaction solution was collected from the container at predetermined intervals (30, 60, 90, 120, and 150 min) and the solid catalyst powder was separated and recovered by external magnetism field method. Then, the concentration of residual MO in the solution was determined by detecting the adsorption and degradation performance using an UV-visible spectrophotometer.


## 2.1. Synthesis

A facile hydrothermal method was used to synthesizeZn1−xCoxMn2O4 (x=0, 0.1, 0.3, and 0.5) nanocrystals. In a typical experiment, zinc nitrate (Zn(NO3)2·6H2O, AR, Tianjin Kaixin Chemical Industry Co. Ltd.), manganese nitrate (Mn(NO3)2·6H2O, AR, Tianjin Kemeiou Reagent Co. Ltd.), cobalt nitrate (Co(NO3)2·6H2O, AR, Shanghai Zhongqin Reagent Co. Ltd.), polyethylene glycol-400 (PEG-400, AR, Shandong West Asia Chemical Reagent Co. Ltd.), absolute ethyl alcohol (AR, China Pharmaceutical Group Reagent Co. Ltd), and citric acid (AR, Tianjin Kemeiou Reagent Co. Ltd.) were used in this study without any further purification. According to the chemical formula of Zn1-xCoxMn2O4 (x=0, 0.1, 0.3, and 0.5) and the molar ratio of metal cations, the stoichiometric quantities of zinc nitrate, cobalt nitrate, and manganese nitrate as precursors were weighed. Zn(NO3)2, Mn(NO3)2, and Co(NO3)2 were mixed in distilled water and magnetically stirred at room temperature for 30 min. Meanwhile, appropriate amounts of citric acid and PEG-400 were dripped into the above-mixed solution under magnetic stirring for 3 hours. Subsequently, the resulting solution was transferred to a 100 mL Teflon-lined stainless steel autoclave. The hydrothermal reaction process was conducted at 180°C for 24 h in an oven and then cooled to room temperature naturally. Finally, the resultant precipitate was separated centrifugally, washed several times with distilled water and absolute alcohol, respectively, and then dried at 60°C in a vacuum oven for 10 h. Thus, Zn1−xCoxMn2O4 nanocrystals were collected and used for further study. By comparison, Zn1−xCoxMn2O4 nanoparticles with different ratios (x=0, 0.1, 0.3, and 0.5) were also prepared using the abovementioned procedure.


## 2.2. Characterization

The crystal structure of the as-obtained samples was examined by X-ray diffractometer (XRD) using the CuKα source (λ=1.54056 Å), the scanning rate 0.005°/s, and step size 0.02°. The morphology of the samples was investigated using a field emission scanning electron microscope (SEM) (JEOL JSM-6701F) equipped with an X-ray energy dispersive spectroscopy (XEDS). The ultraviolet-visible (UV-Vis) diffuse reflectance spectra (DRS) of the products were recorded on a UV-Vis spectrophotometer (PERSEE TU-1901) using BaSO4 as reference. Fourier transform infrared spectroscopy (FT-IR) studies were measured by a Nexus 670 FT-IR spectrometer in the range of 4000–400 cm-1.


## 2.3. Photocatalytic Activity Test

The photocatalytic property of the samples was evaluated by measuring the degradation of methyl orange (MO) aqueous solution in a cylindrical glass vessel under simulated sunlight, and the reaction vessel was kept at a constant temperature using a circulating cooling system. The reaction solution was irradiated with the light source of a 300 W xenon lamp, and the distance between the solution surface and the light source was kept at 30 cm to avoid thermal effect. In this work, 20 mg of the as-synthesized samples was dispersed into a 100 mL MO aqueous solution (the initial MO aqueous solution concentration was 10 mg/L). The mixed suspensions were magnetically stirred for 30 min in the dark to reach the adsorption-desorption equilibrium between the photocatalyst and organic dye MO. During the photocatalytic process, about 2.5 mL of the reaction solution was collected from the container at predetermined intervals (30, 60, 90, 120, and 150 min) and the solid catalyst powder was separated and recovered by external magnetism field method. Then, the concentration of residual MO in the solution was determined by detecting the adsorption and degradation performance using an UV-visible spectrophotometer.


## 3. Results and Discussion

### 3.1. Structural Characterization

Figure1 depicts the XRD patterns of pure ZnMn2O4 and Co-doped Zn1-xCoxMn2O4 samples. The diffraction peaks of all samples can be well indexed to single-phase ZnMn2O4 tetragonal structures (space group: I41/amd, a=b=0.5722 nm, and c=0.9326 nm), which are in agreement with the reported values of JCPDS card no. 71-2499 [24]. No extra diffraction peaks of other impurity phases such as metal oxides or metal clusters are detected when the doping atomic percentage ranges from 10% to 50% from the XRD patterns, indicating that all Co ions are assumed to be successfully incorporated into Zn2+ ion sites without changing the parent ZnMn2O4 structure. The crystallite size of the samples is calculated from the full width at half maximum (FWHM) and the peak position using the most intense diffraction peak (211) by the following Scherrer formula: D=Kλ/Bcosθ, where D represents the crystallite size, K=0.9 is the Scherrer constant, λ is the wavelength of X-ray (CuKα, 1.54056 Å), θ is the Bragg diffraction angle, and B is FWHM in radians of the (211) plane. The crystallite sizes for Zn1−xCoxMn2O4 (x=0, 0.1, 0.3, and 0.5) are 36, 33, 31, and 29 nm; it is clear that the crystallite size gradually decreases with the increase of the Co doping amount.Figure 1
XRD patterns ofZn1−xCoxMn2O4 samples.


### 3.2. Morphological Studies

The SEM image of the pure ZnMn2O4 sample is showed in Figure 2(a). It is clearly visible that the morphology of pure ZnMn2O4 is a regular porous microsphere architecture mainly composed of many nanoparticles, with the diameter of the rough and porous microspheres ranging from 300 to 500 nm, with the average diameter of about 400 nm. Figure 2(b) presents the SEM image of the Zn0.7Co0.3Mn2O4 sample, showing a loose and irregular microsphere morphology composed of massive nanoparticles. With the increase of the Co doping content, the edges of the microsphere become looser and hollower and some stacked microspheres appear in breakage and exhibit hollow microspheres. The hollow microspheres grow bigger in size and rougher and irregular in morphology. This loose hollow microsphere structure contributes to improving the electrochemical performance.Figure 2
SEM images of (a) pure ZnMn2O4 and (b) Zn0.7Co0.3Mn2O4 samples.
(a)
(b)Figure3(a) shows the XEDS patterns of the pure ZnMn2O4 sample to further clarify the chemical components of the as-prepared samples. It is easily found that pure ZnMn2O4 mainly exhibits the peak characteristic of Zn, Mn, and O elements. Figure 3(b) obviously confirms the presence of Co elements besides Zn, Mn, and O elements for the Zn0.7Co0.3Mn2O4 sample, whereas the spectrum of pure ZnMn2O4 does not find the presence of Co elements. The XEDS results further verify XRD , which indicates that Co-doped ZnMn2O4 nanocrystals were successful synthesized by hydrothermal method and Co2+ is successfully substituted as dopant in the ZnMn2O4 matrix. It is evident that the synthesize condition helps to further study the influence of Co doping concentration on the properties of Zn1−xCoxMn2O4 nanocrystals.Figure 3
XEDS patterns of (a) pure ZnMn2O4 and (b) Zn0.7Co0.3Mn2O4 samples.
(a)
(b)


### 3.3. UV-Vis DRS Results

The optical properties of the samples are investigated by UV-Vis DRS. Figure4(a) shows the absorption spectra of Zn1−xCoxMn2O4 samples. From Figure 4(a), Co-doped Zn1−xCoxMn2O4 samples show the similar absorption property as that of the pure ZnMn2O4 except that the absorption edge slightly shifts to a short wavelength with increasing Co content. The drift of the absorption edge revealed the interaction between Co ions and ZnMn2O4. For Zn1−xCoxMn2O4 nanocrystals with a direct band structure, according to the Tauc rule [25]: αhν2=Ahν–Eg, the optical band gap Eg is evaluated from the linear intercept of the ahv2 versus hv plots as displayed in Figure 4(b). Consequently, the band gaps for Zn1−xCoxMn2O4 (x=0, 0.1, 0.3, and 0.5) are calculated to be 2.21, 2.07, 2.02, and 1.98 eV, respectively. Furthermore, the band gap of the Co-doped ZnMn2O4 samples smaller than that of pure ZnMn2O4 and the band gap energy gradually decrease with the increase of Co concentration. This is manifested by the presence of a redshift in the band gap energy for Co-doped Zn1−xCoxMn2O4 nanocrystals.Figure 4
(a) UV-Vis diffuse reflectance spectra and (b)αhν2 versus hν curves of Zn1−xCoxMn2O4 samples.
(a)
(b)


### 3.4. FT-IR Spectra

The chemical structure ofZn1−xCoxMn2O4 samples was investigated using FT-IR, and the results were shown in Figure 5, wherein all of the samples exhibit very similar FT-IR absorption bands. A broad absorption band at 3410 cm-1 in the spectrum of Zn1−xCoxMn2O4 nanocrystals corresponds to O-H stretching vibrations of chemically bonded hydroxyl groups. The peak that appeared at 2923 cm-1 attributed to the vibrational absorption peaks corresponding to the C-H bonds [26], and the peak at 1542 cm-1 was caused by the C=O stretching vibrations of the remaining carbonyl groups in the compound [27]; the band at 1367 cm-1 can be assigned to the organic compounds of PEG-400 or alcohol induced in the process of preparation and test, and the presence of the peak at 1084 cm-1 is owing to C–O stretching vibrations [26]. It is noteworthy that two distinct peaks that appear at 505 and 622 cm-1 are dependent on the formation of metal–oxygen bonds of tetrahedral and octahedral sites, i.e., Zn–O and Mn–O bonds [28]; these bands confirm the formation of spinel compounds for Zn1−xCoxMn2O4 nanocrystals. The corresponding peak position of the Fourier infrared spectrum of the sample did not change with the increase of the Co doping concentration, which is also consistent with the XRD data, indicating that Co2+ was successfully doped into the ZnMn2O4 lattice.Figure 5
FT-IR spectra ofZn1−xCoxMn2O4 samples.


### 3.5. Photocatalytic Performance

In order to study the influence of Co doping concentration on the degradation efficiency, MO dye was selected as target pollutant for evaluating the photocatalytic activity ofZn1−xCoxMn2O4 nanocrystals. Figure 6(a) depicts the MO degradation of Zn1−xCoxMn2O4 samples with different doping ratios versus time (t) under simulated sunlight irradiation. Blank experiment was performed without any catalyst, it was found that there was no obvious self-degradation in the MO dye aqueous solution under visible light irradiation for 180 min, the blank experiment suggested that MO has good stability without catalyst, and the spontaneous photolysis can be negligible under visible light illumination. It is worth noting that the concentration of the MO dye slightly decreased when the reaction mixture is stirred for 30 min without light illumination, because Zn1−xCoxMn2O4 nanocrystals possess a larger specific surface area and can adsorb the MO dye well. The degradation rate of pure ZnMn2O4 is about 57% after xenon lamp irradiation for 150 mins, while the photocatalytic activity of Zn1−xCoxMn2O4 samples is obviously higher than that of pure ZnMn2O4 samples, and the decolorization rates are 69%, 75%, and 82%. It is obvious that the photocatalytic performance increases with the increase of Co doping amount and Co2+ ions replaced the lattice site of Zn2+ to generate single-phase ZnMn2O4 nanocrystal results in the effective separation of photoinduced electron-hole pairs to improve the photocatalytic activity.Figure 6
(a) Photocatalytic degradation of MO over time and (b) first-order kinetic curves ofZn1−xCoxMn2O4 samples.
(a)
(b)To better compare the photocatalytic efficiency forZn1−xCoxMn2O4 nanocrystals of MO decolorization, the kinetic study was performed using a first-order kinetic equation: lnCt/C0=k, where k represents reaction rate constant (h−1), t is the irradiation time, and Ct and C0 denote the initial concentration and the reaction concentration, respectively, of MO after light irradiation. The first-order kinetics of Zn1−xCoxMn2O4 nanocrystals for photocatalytic decolorization of MO as shown in Figure 6(b) and the k values for Zn1−xCoxMn2O4 (x=0.1, 0.3, and 0.5) are 0.470, 0.545, and 0.658 h-1, respectively; these values demonstrate that doped Zn1−xCoxMn2O4 nanocrystals have a higher efficiency than that of pure samples (k=0.336 h-1). The improvement of photocatalytic efficiency is mainly due to the fact that Co-doped Zn1−xCoxMn2O4 nanocrystals possess smaller particle size and larger specific surface area and Co2+ can adjust the crystal structure and energy band structure, which accelerate the migration of the photogenerated electron-hole pairs toward its surface and prevent the electron-hole pairs from recombination.The stability and reusability for the Zn0.5Co0.5Mn2O4 sample were evaluated by cyclic experiments of photocatalytic degradation of MO under the same conditions. As shown in Figure 7, the degradation efficiency of the Zn0.5Co0.5Mn2O4 sample exhibits a minor decrease from 82% to 79.5% after five consecutive cycles of photocatalytic experiments and the repetition rate is still maintained at 80%. The little decreases may relate to the particle aggregation of the sample after a long time reaction. Hence, Zn1−xCoxMn2O4 nanocrystals possess excellent photocatalytic active and good stability; these results demonstrate that Co-doped ZnMn2O4 nanocrystals possess good application prospects in photocatalytic degradation of pollutants.Figure 7
Photocatalytic cycle stability of Zn0.7Co0.3Mn2O4 samples.Under simulated sunlight irradiation, the electrons (e−) in the valence band (VB) of ZnMn2O4 can be excited to its conduction band (CB), while the holes (h+) is generated in VB of ZnMn2O4. Zn1−xCoxMn2O4 nanocrystals can effectively promote the generation of photoinduced electron-hole pairs owing to the reduction of average grain size and the band gap for Co-doped Zn1−xCoxMn2O4 nanocrystals. The electrons at VB are excited to transition to CB, thus forming a hole in VB and generated an electron-hole pair (equation (1)). Electrons react with dissolved oxygen in the solution to form superoxide radicals (•O2-). At the same time, photoinduced holes react with water to generate •OH, H+ (equation (2)). Meanwhile, H+ further reacts with oxygen to form H2O2 (equation (3)). Obviously, hydrogen peroxide reacts with O2- to produce •OH, OH-, and O2 (equation (4)). As strong oxidants, •OH reacts strongly with organic pollutants and promote the decomposition of organic pollutants. Finally, •OH and O2- oxidize MO to CO2, H2O, and other small molecule compounds (equation (5)) [3].Under simulated sunlight irradiation, the photocatalytic decolorization reaction of the photoinduced electron-hole transport forZn1−xCoxMn2O4 nanocrystals is as follows [29]:
(1)Zn1−xCoxMn2O4+hv⟶Zn1−xCoxMn2O4e−+Zn1−xCoxMn2O4h+,(2)Zn1−xCoxMn2O4h++H2O⟶Zn1−xCoxMn2O4+O•H+H+,Zn1−xCoxMn2O4e−+O2⟶Zn1−xCoxMn2O4+O2•−,(3)O2+H+⟶H2O2,(4)H2O2+O2•−⟶O•H+OH−+O2,(5)O•H,O2•−+organicmolecules⟶H2O+CO2+mineralacids.


## 3.1. Structural Characterization

Figure1 depicts the XRD patterns of pure ZnMn2O4 and Co-doped Zn1-xCoxMn2O4 samples. The diffraction peaks of all samples can be well indexed to single-phase ZnMn2O4 tetragonal structures (space group: I41/amd, a=b=0.5722 nm, and c=0.9326 nm), which are in agreement with the reported values of JCPDS card no. 71-2499 [24]. No extra diffraction peaks of other impurity phases such as metal oxides or metal clusters are detected when the doping atomic percentage ranges from 10% to 50% from the XRD patterns, indicating that all Co ions are assumed to be successfully incorporated into Zn2+ ion sites without changing the parent ZnMn2O4 structure. The crystallite size of the samples is calculated from the full width at half maximum (FWHM) and the peak position using the most intense diffraction peak (211) by the following Scherrer formula: D=Kλ/Bcosθ, where D represents the crystallite size, K=0.9 is the Scherrer constant, λ is the wavelength of X-ray (CuKα, 1.54056 Å), θ is the Bragg diffraction angle, and B is FWHM in radians of the (211) plane. The crystallite sizes for Zn1−xCoxMn2O4 (x=0, 0.1, 0.3, and 0.5) are 36, 33, 31, and 29 nm; it is clear that the crystallite size gradually decreases with the increase of the Co doping amount.Figure 1
XRD patterns ofZn1−xCoxMn2O4 samples.


## 3.2. Morphological Studies

The SEM image of the pure ZnMn2O4 sample is showed in Figure 2(a). It is clearly visible that the morphology of pure ZnMn2O4 is a regular porous microsphere architecture mainly composed of many nanoparticles, with the diameter of the rough and porous microspheres ranging from 300 to 500 nm, with the average diameter of about 400 nm. Figure 2(b) presents the SEM image of the Zn0.7Co0.3Mn2O4 sample, showing a loose and irregular microsphere morphology composed of massive nanoparticles. With the increase of the Co doping content, the edges of the microsphere become looser and hollower and some stacked microspheres appear in breakage and exhibit hollow microspheres. The hollow microspheres grow bigger in size and rougher and irregular in morphology. This loose hollow microsphere structure contributes to improving the electrochemical performance.Figure 2
SEM images of (a) pure ZnMn2O4 and (b) Zn0.7Co0.3Mn2O4 samples.
(a)
(b)Figure3(a) shows the XEDS patterns of the pure ZnMn2O4 sample to further clarify the chemical components of the as-prepared samples. It is easily found that pure ZnMn2O4 mainly exhibits the peak characteristic of Zn, Mn, and O elements. Figure 3(b) obviously confirms the presence of Co elements besides Zn, Mn, and O elements for the Zn0.7Co0.3Mn2O4 sample, whereas the spectrum of pure ZnMn2O4 does not find the presence of Co elements. The XEDS results further verify XRD , which indicates that Co-doped ZnMn2O4 nanocrystals were successful synthesized by hydrothermal method and Co2+ is successfully substituted as dopant in the ZnMn2O4 matrix. It is evident that the synthesize condition helps to further study the influence of Co doping concentration on the properties of Zn1−xCoxMn2O4 nanocrystals.Figure 3
XEDS patterns of (a) pure ZnMn2O4 and (b) Zn0.7Co0.3Mn2O4 samples.
(a)
(b)


## 3.3. UV-Vis DRS Results

The optical properties of the samples are investigated by UV-Vis DRS. Figure4(a) shows the absorption spectra of Zn1−xCoxMn2O4 samples. From Figure 4(a), Co-doped Zn1−xCoxMn2O4 samples show the similar absorption property as that of the pure ZnMn2O4 except that the absorption edge slightly shifts to a short wavelength with increasing Co content. The drift of the absorption edge revealed the interaction between Co ions and ZnMn2O4. For Zn1−xCoxMn2O4 nanocrystals with a direct band structure, according to the Tauc rule [25]: αhν2=Ahν–Eg, the optical band gap Eg is evaluated from the linear intercept of the ahv2 versus hv plots as displayed in Figure 4(b). Consequently, the band gaps for Zn1−xCoxMn2O4 (x=0, 0.1, 0.3, and 0.5) are calculated to be 2.21, 2.07, 2.02, and 1.98 eV, respectively. Furthermore, the band gap of the Co-doped ZnMn2O4 samples smaller than that of pure ZnMn2O4 and the band gap energy gradually decrease with the increase of Co concentration. This is manifested by the presence of a redshift in the band gap energy for Co-doped Zn1−xCoxMn2O4 nanocrystals.Figure 4
(a) UV-Vis diffuse reflectance spectra and (b)αhν2 versus hν curves of Zn1−xCoxMn2O4 samples.
(a)
(b)


## 3.4. FT-IR Spectra

The chemical structure ofZn1−xCoxMn2O4 samples was investigated using FT-IR, and the results were shown in Figure 5, wherein all of the samples exhibit very similar FT-IR absorption bands. A broad absorption band at 3410 cm-1 in the spectrum of Zn1−xCoxMn2O4 nanocrystals corresponds to O-H stretching vibrations of chemically bonded hydroxyl groups. The peak that appeared at 2923 cm-1 attributed to the vibrational absorption peaks corresponding to the C-H bonds [26], and the peak at 1542 cm-1 was caused by the C=O stretching vibrations of the remaining carbonyl groups in the compound [27]; the band at 1367 cm-1 can be assigned to the organic compounds of PEG-400 or alcohol induced in the process of preparation and test, and the presence of the peak at 1084 cm-1 is owing to C–O stretching vibrations [26]. It is noteworthy that two distinct peaks that appear at 505 and 622 cm-1 are dependent on the formation of metal–oxygen bonds of tetrahedral and octahedral sites, i.e., Zn–O and Mn–O bonds [28]; these bands confirm the formation of spinel compounds for Zn1−xCoxMn2O4 nanocrystals. The corresponding peak position of the Fourier infrared spectrum of the sample did not change with the increase of the Co doping concentration, which is also consistent with the XRD data, indicating that Co2+ was successfully doped into the ZnMn2O4 lattice.Figure 5
FT-IR spectra ofZn1−xCoxMn2O4 samples.


## 3.5. Photocatalytic Performance

In order to study the influence of Co doping concentration on the degradation efficiency, MO dye was selected as target pollutant for evaluating the photocatalytic activity ofZn1−xCoxMn2O4 nanocrystals. Figure 6(a) depicts the MO degradation of Zn1−xCoxMn2O4 samples with different doping ratios versus time (t) under simulated sunlight irradiation. Blank experiment was performed without any catalyst, it was found that there was no obvious self-degradation in the MO dye aqueous solution under visible light irradiation for 180 min, the blank experiment suggested that MO has good stability without catalyst, and the spontaneous photolysis can be negligible under visible light illumination. It is worth noting that the concentration of the MO dye slightly decreased when the reaction mixture is stirred for 30 min without light illumination, because Zn1−xCoxMn2O4 nanocrystals possess a larger specific surface area and can adsorb the MO dye well. The degradation rate of pure ZnMn2O4 is about 57% after xenon lamp irradiation for 150 mins, while the photocatalytic activity of Zn1−xCoxMn2O4 samples is obviously higher than that of pure ZnMn2O4 samples, and the decolorization rates are 69%, 75%, and 82%. It is obvious that the photocatalytic performance increases with the increase of Co doping amount and Co2+ ions replaced the lattice site of Zn2+ to generate single-phase ZnMn2O4 nanocrystal results in the effective separation of photoinduced electron-hole pairs to improve the photocatalytic activity.Figure 6
(a) Photocatalytic degradation of MO over time and (b) first-order kinetic curves ofZn1−xCoxMn2O4 samples.
(a)
(b)To better compare the photocatalytic efficiency forZn1−xCoxMn2O4 nanocrystals of MO decolorization, the kinetic study was performed using a first-order kinetic equation: lnCt/C0=k, where k represents reaction rate constant (h−1), t is the irradiation time, and Ct and C0 denote the initial concentration and the reaction concentration, respectively, of MO after light irradiation. The first-order kinetics of Zn1−xCoxMn2O4 nanocrystals for photocatalytic decolorization of MO as shown in Figure 6(b) and the k values for Zn1−xCoxMn2O4 (x=0.1, 0.3, and 0.5) are 0.470, 0.545, and 0.658 h-1, respectively; these values demonstrate that doped Zn1−xCoxMn2O4 nanocrystals have a higher efficiency than that of pure samples (k=0.336 h-1). The improvement of photocatalytic efficiency is mainly due to the fact that Co-doped Zn1−xCoxMn2O4 nanocrystals possess smaller particle size and larger specific surface area and Co2+ can adjust the crystal structure and energy band structure, which accelerate the migration of the photogenerated electron-hole pairs toward its surface and prevent the electron-hole pairs from recombination.The stability and reusability for the Zn0.5Co0.5Mn2O4 sample were evaluated by cyclic experiments of photocatalytic degradation of MO under the same conditions. As shown in Figure 7, the degradation efficiency of the Zn0.5Co0.5Mn2O4 sample exhibits a minor decrease from 82% to 79.5% after five consecutive cycles of photocatalytic experiments and the repetition rate is still maintained at 80%. The little decreases may relate to the particle aggregation of the sample after a long time reaction. Hence, Zn1−xCoxMn2O4 nanocrystals possess excellent photocatalytic active and good stability; these results demonstrate that Co-doped ZnMn2O4 nanocrystals possess good application prospects in photocatalytic degradation of pollutants.Figure 7
Photocatalytic cycle stability of Zn0.7Co0.3Mn2O4 samples.Under simulated sunlight irradiation, the electrons (e−) in the valence band (VB) of ZnMn2O4 can be excited to its conduction band (CB), while the holes (h+) is generated in VB of ZnMn2O4. Zn1−xCoxMn2O4 nanocrystals can effectively promote the generation of photoinduced electron-hole pairs owing to the reduction of average grain size and the band gap for Co-doped Zn1−xCoxMn2O4 nanocrystals. The electrons at VB are excited to transition to CB, thus forming a hole in VB and generated an electron-hole pair (equation (1)). Electrons react with dissolved oxygen in the solution to form superoxide radicals (•O2-). At the same time, photoinduced holes react with water to generate •OH, H+ (equation (2)). Meanwhile, H+ further reacts with oxygen to form H2O2 (equation (3)). Obviously, hydrogen peroxide reacts with O2- to produce •OH, OH-, and O2 (equation (4)). As strong oxidants, •OH reacts strongly with organic pollutants and promote the decomposition of organic pollutants. Finally, •OH and O2- oxidize MO to CO2, H2O, and other small molecule compounds (equation (5)) [3].Under simulated sunlight irradiation, the photocatalytic decolorization reaction of the photoinduced electron-hole transport forZn1−xCoxMn2O4 nanocrystals is as follows [29]:
(1)Zn1−xCoxMn2O4+hv⟶Zn1−xCoxMn2O4e−+Zn1−xCoxMn2O4h+,(2)Zn1−xCoxMn2O4h++H2O⟶Zn1−xCoxMn2O4+O•H+H+,Zn1−xCoxMn2O4e−+O2⟶Zn1−xCoxMn2O4+O2•−,(3)O2+H+⟶H2O2,(4)H2O2+O2•−⟶O•H+OH−+O2,(5)O•H,O2•−+organicmolecules⟶H2O+CO2+mineralacids.


## 4. Conclusion

(1)
Co-dopedZn1−xCoxMn2O4 nanocrystals with different ratios (x=0, 0.1, 0.3, and 0.5) were successfully synthesized via a facile hydrothermal method. All samples exhibit single-phase spinel tetragonal with good crystallization. Co2+ ions are successfully substituted for the lattice site of Zn2+ to generate single-phase ZnMn2O4 nanocrystals
(2)
The morphologies of all the samples are loose hollow microsphere structures. The crystalline size decreases as Co-doped concentration increase. The energy band gap of Co-dopedZn1−xCoxMn2O4 nanocrystalline is smaller than that of pure ZnMn2O4 has been red shifted
(3)
The photocatalytic activity of dopedZn1−xCoxMn2O4 samples is obviously higher than that of pure ZnMn2O4 samples for the photodegradation of MO under visible light irradiation. Co-doped ZnMn2O4 nanocrystals can act as a potential photocatalyst for photocatalytic degradation of the pollutants



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*Source: 4257270-2019-05-09.xml*