# Synthesis, Characterization, and Photocatalytic Tests of N-Doped Zinc Oxide: A New Interesting Photocatalyst

Authors: Chiara Gionco; Debora Fabbri; Paola Calza; Maria Cristina Paganini
Journal: Journal of Nanomaterials
 (2016)

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## Abstract

Fast and simple synthetic methods for the preparation of bare and N-doped zinc oxide, involving a stirring or microwave assisted process, are proposed. All samples were characterized by XRD analysis, BET, and DRS-UV-Vis spectroscopy. The photocatalytic activity of these nanostructured oxides was investigated using phenol and 2,4-dichlorophenol as model molecules under UV-A and visible light irradiation. N-doping in ZnO nanostructures provided a significant increase in phenol and 2,4-dichlorophenol degradation rate under Vis light, leading to a degradation rate higher than that obtained with bare ZnO. The release of chlorine as chloride ions from 2,4-dichlorophenol with N-doped ZnO was faster achieved as well and complete dechlorination was reached within 2 h of irradiation (N-doped ZnO) instead of 3 h (bare ZnO).


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## Body

## 1. Introduction

A growing interest toward zinc oxide has arisen, due to its broad range of properties, that is, conductivity, high transparency, piezoelectricity, semiconducting broadband, ferromagnetism at room temperature, magnetic and optical properties, and sensitivity to the chemical species. Additional and particularly attractive features comprise ZnO stability to high-energy radiation, suggesting it as a prime candidate for space applications [1], and ZnO susceptibility to chemical attack (etching) in acidic or basic aqueous solutions, which provides the possibility to produce small size devices [2]. Even if studies began in the thirties and culminated in early eighties [3, 4], later the interest gradually waned, due to the failure in the synthesis of p-type doped ZnO. Actually, its direct band gap (3.37 eV) and large exciton binding energy (60 meV) [5] make this material one of the most promising functional materials for application in photocatalysis and solar cells production [6, 7]. However, owing to this large band gap, the role of doping tuning and controlling the electronic, magnetic, and optical properties of this solid was a key problem [8]; ZnO usually exhibits n-type behavior due to shallow donor impurities [9, 10]. The latest developments in the field of doping and in the possibility to synthesize ZnO in different nanostructured forms make all these applications a concrete goal and convey a renewed interest toward ZnO research. Recently, a synthetic procedure was reported to obtain rare-earth doped ZnO nanomaterials that can be applied in many technologies, such as degradation of pollutants and optoelectronic devices [11–16].Among dopant agents, nitrogen is emerging as a key dopant element in different semiconductor oxides. Considering TiO2, it has been one of the most promising candidates in the development of effective photocatalysts capable of operating efficiently under solar energy irradiation [17–19]. Recently Di Valentin and Pacchioni proposed an interesting comparison between different defective semiconductor oxides and nitrogen-doped oxides; N-doped TiO2, ZnO, and WO3 were presented as some of the most interesting materials [20].In the case of ZnO, the incorporation of N atoms in the oxide lattice is an effective approach to achieve p-type doping of this material; Klingshirn proved that N impurities act as shallow acceptors in ZnO thin films and bulk crystals [21].So far, N impurities in ZnO were obtained by direct synthesisvia chemical vapor deposition (CVD) methods in N2O or NH3 atmosphere [22], by mechanochemical methods [23, 24] or by postsynthesis treatments with NH3 at high temperature [25–27]. N-doped ZnO has been proved to be a good photocatalyst in water oxidation [28] and in the degradation of rhodamine B [29].In this work, we present two new synthetic strategies to prepare zinc oxide and nitrogen-doped zinc oxide, based on microwave assisted or stirring method. We tested the efficiency of these materials on two model molecules, phenol (P) and 2,4-dichlorophenol (2,4-DCP), under UV light and visible light, obtaining interesting results. In most studies P has been used as a molecule probe for photocatalytic tests, whose degradation mechanism is well established [30–33]. The choice of 2,4-DCP as additional model molecule is due to the fact that (a) it is an endocrine disrupting agent, widely used as herbicide, whose presence was detected in surface waters in several countries [34, 35], (b) it is highly soluble in water relative to other polychlorinated phenols, and (c) its simple molecular structure facilitates a greater understanding of the reaction mechanism involving aromatic compounds.


## 2. Materials and Methods

### 2.1. Materials and Reagents

Phenol, 2,4-dichlorophenol, catechol, 1,4-benzoquinone, resorcinol, hydroquinone, and all reactants employed in this work were purchased from Aldrich. Acetonitrile (AC0331 Supergradient HPLC grade eluent) was purchased from Scharlau. All aqueous solutions were prepared with ultrapure water Millipore Milli-Q™. All reactants employed in the synthesis processes, namely, ZnSO4·7H2O, ethylenediamine, ammonia, zinc acetate, and ethanol, were purchased from Aldrich and used without any further purification treatment.


### 2.2. Synthesis of ZnO and N-ZnO

Zinc oxide was synthesized following two different approaches. The first synthetic approach to produce bare ZnO involved a simple stirring process, adapted from [36]. Zinc acetate (2.2 g) and ethylenediamine (0.6 mL) were dissolved in 15 mL of ethanol. The solution was then stirred for 2 hours and dried at 50°C overnight and calcined at 500°C for two hours.Nitrogen-doped ZnO was synthesized by adding to the mother solution urea (0.6 g) and ethanol (15 mL) and the resulting mixture was kept under stirring until a stable sol was obtained. The sol was dried at 50°C overnight and calcined at 500°C for two hours. These samples will be hereafter labeled as ZnO_St and N-ZnO_St.The second method involved a microwave assisted precipitation process adapted from [37]: few drops of ammonia were added to a 0.25 M aqueous solution of ZnSO4·7H2O until the pH is 7 and a white precipitate appeared. The solution was stirred and heated in a domestic microwave oven (2.45 GHz and 800 W) for 1 min. N-ZnO sample was synthesized with the same procedure, adding 0.25 g of urea to the starting aqueous solution of ZnSO4·7H2O. Then, the product (for both samples) was centrifuged at 6000 rpm for 10 min and washed twice with deionized water. Both samples were dried at 50°C for 2 days and later calcined at 500°C for 2 hours. These samples will be hereafter labeled as ZnO_MW and N-ZnO_MW.


### 2.3. Characterization of Samples

Powder X-rays diffraction (XRD) patterns were recorded with a PANalytical PW3040/60 X’Pert PRO MPD using a copperK
α radiation source (0.15418 nm). The intensities were obtained in the 2θ ranges between 20° and 70°. The X’Pert High-Score software was used for data handling. Rietveld refinement was performed on the diffraction patterns to determine the crystallite size and relative abundance of phases, using the MAUD 2.26 software and NIST Si powder to determine the instrumental function [38].The surface area measurements were carried out on a Micromeritics ASAP 2020/2010 apparatus using the Brunauer-Emmett-Teller (BET) model for N2 adsorption measurements. Prior to the adsorption run, all of the samples were outgassed at 473 K for 3 h.The UV-Vis absorption spectra were recorded using a Varian Cary 5 spectrometer, coupled with an integration sphere for diffuse reflectance studies, using a Carywin-UV/scan software. A sample of PTFE with 100% reflectance was used as reference.


### 2.4. Irradiation Procedures

Phenol and 2,4-dichlorophenol were used as model molecules to investigate the photocatalytic efficiency of zinc oxide based materials. Preliminary, we evaluate the stability of the materials at different pHs. pH was adjusted using HClO4 0.1 M or NaOH 0.1 M. The pH range of stability was established to be 5–8. The irradiation experiments were carried out in Pyrex glass cells filled with 5 mL of organic compound (20 mgL−1) and catalyst (1 gL−1). The irradiation was performed by using a TL K05 UV/A lamp 25 mW/m2 centered at 365 nm. Experiments using visible light only were performed in a devise equipped with a 1500 watt Xenon lamp (CO.FO.MEGRA, Milan, Italy) furnished with a 400 nm cut-off filter. The temperature reached during the irradiation was 30
±
2°C. In all cases, experiments were run without modifying the natural pH of the solution. The entire content of the cells was then filtered through 0.45 μm HA cellulose acetate membrane to remove ZnO particles and further analyzed by the appropriate analytical technique. Adsorption in the dark was assessed and was negligible for all materials. All experiments were performed in triplicate and the average results are plotted in the graphs. The stability of the material over prolonged irradiation time (24 and 48 h under UV-A lamp) was tested as well. The efficiency of preirradiated material is described in Section 3.2.


### 2.5. Analytical Determinations

The disappearance of the model molecule and the formation of transformation products as a function of the irradiation time were followed using an HPLC system (Merck-Hitachi L-6200 pumps), equipped with a Rheodyne injector, a RP C18 column (Lichrochart, Merck, 12.5 cm × 0.4 cm; 5μm packing), and a UV-Vis detector (Merck-Hitachi L-4200) set at 220 nm. Elution was carried out with acetonitrile and phosphate buffer (1
×
10
-
2 M) at pH 2.8 (40 : 60% v/v) at a flow rate of 1 mL/min.Chloride formation was evaluated by a Dionex ion chromatograph equipped with a conductometer detector, using a AS9HC anionic column and a buffer solution composed by NaHCO3 11 mM and K2CO3 4.5 mM as eluent at a flow rate of 1 mL/min. In these experimental conditions, the retention time for chloride ion was 5.30 min.


## 2.1. Materials and Reagents

Phenol, 2,4-dichlorophenol, catechol, 1,4-benzoquinone, resorcinol, hydroquinone, and all reactants employed in this work were purchased from Aldrich. Acetonitrile (AC0331 Supergradient HPLC grade eluent) was purchased from Scharlau. All aqueous solutions were prepared with ultrapure water Millipore Milli-Q™. All reactants employed in the synthesis processes, namely, ZnSO4·7H2O, ethylenediamine, ammonia, zinc acetate, and ethanol, were purchased from Aldrich and used without any further purification treatment.


## 2.2. Synthesis of ZnO and N-ZnO

Zinc oxide was synthesized following two different approaches. The first synthetic approach to produce bare ZnO involved a simple stirring process, adapted from [36]. Zinc acetate (2.2 g) and ethylenediamine (0.6 mL) were dissolved in 15 mL of ethanol. The solution was then stirred for 2 hours and dried at 50°C overnight and calcined at 500°C for two hours.Nitrogen-doped ZnO was synthesized by adding to the mother solution urea (0.6 g) and ethanol (15 mL) and the resulting mixture was kept under stirring until a stable sol was obtained. The sol was dried at 50°C overnight and calcined at 500°C for two hours. These samples will be hereafter labeled as ZnO_St and N-ZnO_St.The second method involved a microwave assisted precipitation process adapted from [37]: few drops of ammonia were added to a 0.25 M aqueous solution of ZnSO4·7H2O until the pH is 7 and a white precipitate appeared. The solution was stirred and heated in a domestic microwave oven (2.45 GHz and 800 W) for 1 min. N-ZnO sample was synthesized with the same procedure, adding 0.25 g of urea to the starting aqueous solution of ZnSO4·7H2O. Then, the product (for both samples) was centrifuged at 6000 rpm for 10 min and washed twice with deionized water. Both samples were dried at 50°C for 2 days and later calcined at 500°C for 2 hours. These samples will be hereafter labeled as ZnO_MW and N-ZnO_MW.


## 2.3. Characterization of Samples

Powder X-rays diffraction (XRD) patterns were recorded with a PANalytical PW3040/60 X’Pert PRO MPD using a copperK
α radiation source (0.15418 nm). The intensities were obtained in the 2θ ranges between 20° and 70°. The X’Pert High-Score software was used for data handling. Rietveld refinement was performed on the diffraction patterns to determine the crystallite size and relative abundance of phases, using the MAUD 2.26 software and NIST Si powder to determine the instrumental function [38].The surface area measurements were carried out on a Micromeritics ASAP 2020/2010 apparatus using the Brunauer-Emmett-Teller (BET) model for N2 adsorption measurements. Prior to the adsorption run, all of the samples were outgassed at 473 K for 3 h.The UV-Vis absorption spectra were recorded using a Varian Cary 5 spectrometer, coupled with an integration sphere for diffuse reflectance studies, using a Carywin-UV/scan software. A sample of PTFE with 100% reflectance was used as reference.


## 2.4. Irradiation Procedures

Phenol and 2,4-dichlorophenol were used as model molecules to investigate the photocatalytic efficiency of zinc oxide based materials. Preliminary, we evaluate the stability of the materials at different pHs. pH was adjusted using HClO4 0.1 M or NaOH 0.1 M. The pH range of stability was established to be 5–8. The irradiation experiments were carried out in Pyrex glass cells filled with 5 mL of organic compound (20 mgL−1) and catalyst (1 gL−1). The irradiation was performed by using a TL K05 UV/A lamp 25 mW/m2 centered at 365 nm. Experiments using visible light only were performed in a devise equipped with a 1500 watt Xenon lamp (CO.FO.MEGRA, Milan, Italy) furnished with a 400 nm cut-off filter. The temperature reached during the irradiation was 30
±
2°C. In all cases, experiments were run without modifying the natural pH of the solution. The entire content of the cells was then filtered through 0.45 μm HA cellulose acetate membrane to remove ZnO particles and further analyzed by the appropriate analytical technique. Adsorption in the dark was assessed and was negligible for all materials. All experiments were performed in triplicate and the average results are plotted in the graphs. The stability of the material over prolonged irradiation time (24 and 48 h under UV-A lamp) was tested as well. The efficiency of preirradiated material is described in Section 3.2.


## 2.5. Analytical Determinations

The disappearance of the model molecule and the formation of transformation products as a function of the irradiation time were followed using an HPLC system (Merck-Hitachi L-6200 pumps), equipped with a Rheodyne injector, a RP C18 column (Lichrochart, Merck, 12.5 cm × 0.4 cm; 5μm packing), and a UV-Vis detector (Merck-Hitachi L-4200) set at 220 nm. Elution was carried out with acetonitrile and phosphate buffer (1
×
10
-
2 M) at pH 2.8 (40 : 60% v/v) at a flow rate of 1 mL/min.Chloride formation was evaluated by a Dionex ion chromatograph equipped with a conductometer detector, using a AS9HC anionic column and a buffer solution composed by NaHCO3 11 mM and K2CO3 4.5 mM as eluent at a flow rate of 1 mL/min. In these experimental conditions, the retention time for chloride ion was 5.30 min.


## 3. Results and Discussion

### 3.1. Materials Characterization

XRD patterns for the synthetized samples are shown in Figure1. The diffraction peaks of bare (Figure 1 lines (a) and (c)) and doped (Figure 1 lines (b) and (d)) materials are attributable to the (1 0 0), (0 0 2), (1 0 1), (1 0 2), (1 1 0), (1 0 3), (2 0 0), (1 1 2), and (2 0 1) planes which are in accordance with the wurtzite hexagonal phase of ZnO [18]. These patterns are similar to all samples, assessing that neither the introduction of nitrogen nor the diverse synthesis changes the crystal structure of ZnO [36].Figure 1
XRD patterns for (a) ZnO_St, (b) N-ZnO_St, (c) ZnO_MW, and (d) N-ZnO_MW.The samples obtained using zinc sulphate as precursor (i.e., those obtained with the microwave assisted method) also show additional peaks attributable to zinc oxysulphate that did not evolve properly during the synthesis process. On the XRD patterns a Rietveld refinement was performed using the MAUD software that allowed estimating the average size of the crystallites. These values are about 70 and 40 nm for ZnO_MW and N-ZnO_MW nanostructures and 136 and 107 nm for ZnO_St and N-ZnO_St samples, respectively. Regardless of the synthetic method employed, the insertion of dopant caused a decrease in the crystallites size; this phenomenon was already observed and reported in the literature [39, 40].The specific surface area of the samples was measured applying the Brunauer-Emmett-Teller (BET) model on N2 adsorption measurement. Samples produced through the stirring method (ZnO_St and N-ZnO_St) exhibited a surface area of less than 10 m2/g, while those synthetized through microwave assisted method (ZnO_MW and N-ZnO_MW) have a slightly higher area (11.5
±
0.9 m2/g), underlining that the surface area is dependent on the synthetic method but is not affected by N-doping. The unexpected low surface area obtained with these synthetic processes was quite surprising, considering the quite high photoactivity of that samples, but higher than the commercial ZnO powder (4-5 m2/g) [41].Figure2 shows the absorption spectra (DRS UV-Vis) obtained for ZnO and N-doped ZnO samples. Two main issues arose from these spectra:(1)
the optical properties of the bare materials prepared from different synthetic methods (stirring and microwave assisted) are very similar;
(2)
the N-doping causes tiny modifications in the band gap (vide infra), but a high modification in the whole absorption spectra.In particular, the optical spectra of bare ZnO (Figure 2 line (A) and (B)) are dominated by the valence band (VB) to conduction band (CB) transition occurring at about 400 nm (ca. 3 eV) and the two spectra exhibit relatively small differences, in agreement with previous data reported in literature [36]. Figure 2 also compares the optical absorptions of N-doped zinc oxide (line (C) and (D)). A deep difference between doped and bare oxides spectra is evident. A large absorption in visible region of the optical spectra, together with a tiny red shift of the absorption edge (0.03 eV,vide infra), is observable. A small absorption shoulder centered at about 530 nm is more evident in Figure 2(b), where an enlargement of Figure 2(a) is provided. Doped samples show a pale grey-yellow color. The yellow is due to the presence of nitrogen into the structure (absorption band centered around 500–530 nm); the grey color is due to carbon impurities trapped into the structure during the calcination process (resulting in a tail in the absorption across the whole visible region).Figure 2
Kubelka-Munk transformed diffuse reflectance spectra of (a) (A) ZnO_St, (B) ZnO_MW, (C) N-ZnO_St, (D) N-ZnO_MW, and (b) their enlargement.
(a)
(b)The band gap of all the samples was calculated by linearization of the plot reportingα
h
ν
2 versus h
ν typical of direct band gap transitions for ZnO and Ce-ZnO through the Tauc plot from DRS measures [42]. Bare samples (namely, ZnO_St and ZnO_MW) show a band gap of 3.28 eV, while for N-doped ZnO (namely, N-ZnO_St and N-ZnO_MW) it is 3.25 eV, implying that the doping process does not induce a modification in the material band gap. This behavior is not surprising and was already reported in the literature [36].


### 3.2. Photocatalytic Tests

The photocatalytic activity of all synthetized materials was firstly investigated using phenol as model molecule. Phenol is known to be scarcely adsorbed at the catalyst surface and its degradation mainly proceeds through an initial oxidative attack, with the formation of hydroxylated derivatives [43, 44]. Preliminary tests showed that the direct photolysis process is very slow and can be considered negligible in the considered time window [45].The curves of phenol abatement as a function of irradiation time are plotted in Figure3 for ZnO_St and in Figure 4 for ZnO_MW. Under UV-A irradiation, the phenol disappearance similarly occurred with both bare and N-doped ZnO, irrespective of the synthetic method employed, and the complete disappearance is observed within 3 h of irradiation. Conversely, under Vis light irradiation, phenol degradation rate is higher with N-doped ZnO rather than with bare ZnO.Figure 3
Disappearance of phenol (20 mg L−1) in the presence of bare ZnO_St and N-doped zinc oxide N-ZnO_St (St method) (1 gL−1) under irradiation with UV-A or visible light.
(a)
(b)Figure 4
Disappearance of phenol (20 mg L−1) in the presence of bare (ZnO_MW) and N-doped zinc oxide (N-ZnO_MW) (MW method) (1 gL−1) under irradiation with a UV-A or visible light.
(a)
(b)Linear plots shown in left of Figures3(a) and 4(a) were obtained by fitting the degradation data with (1)-ln⁡CC0=kt,where C
0 is initial concentration and C is concentration measured after the irradiation time t; in all cases, a good linearity is observed. The calculated k values are summarized in Table 1.Table 1
Constant rate values calculated through (1).
K, min−1
ZnO_St
N-ZnO_St
ZnO_MW
N-ZnO_MW
UV-A
2.3 × 10−2
1.9 × 10−2
2.1 × 10−2
1.5 × 10−2
Vis
1.0 × 10−2
1.3 × 10−2
0.54 × 10−2
0.76 × 10−2Considering materials synthesized with MW method under Vis, the half-time life (t
1
/
2) was reduced from 130 min (ZnO) to 90 min (N-ZnO) and after 3 h of irradiation, almost 70% of phenol is abated, while with bare ZnO only 60% of phenol disappeared. Materials prepared through stirring method evidenced similar t
1
/
2 (almost 60 min) and under Vis after 3 h of irradiation the percentage of degraded phenol passes from 85% (bare ZnO) to 93% (N-doped ZnO). The experiment is repeated toward the abatement of phenol by using the materials preirradiated for 24 and 48 h under UV-A. Results show that the efficiency of the catalyst remains the same. As an example, the case of the phenol degradation with N-ZnO_St is reported in Figure 3(a).The photocatalytic increase observed with Vis light for N-doped systems cannot be ascribed to a variation in the materials band gap but could be attributed to the pronounced shoulder showing the presence of intraband gap states and not to a real shift of the band gap itself [19].The best performance was obtained with the materials preparedvia stirring synthetic method. A possible explanation of this behavior could be the fact that the materials preparedvia zinc acetate, as precursor, followed a better synthetic procedure and the final product was more clean and without defective compounds.The performance of zinc oxide based materials producedvia stirring method was also investigated toward the abatement of 2,4-dichlorophenol (2,4-DCP) under visible light. Once more, 2,4-DCP degradation faster occurred with N-doped material and the complete degradation was achieved within 2 h of irradiation (Figure 5(a)). Chloride ions were easier released in the case of N-doped material, too. The chloride evolution curve closely resembles the phenol disappearance curve. When employing N-doped material, the formation of chloride ions in stoichiometric amount was achieved within 2 h of irradiation, while with bare ZnO 3 h is required. Following 2,4-DCP degradation, the formation of some transformation products occurred, whose identity was confirmed by injection of authentic standard solution. Their concentration over time is reported in Figure 5(b) and showed the formation of hydroquinone (HQ) as main transformation product in both cases, at a slight higher amount in the presence of N-ZnO; 4-chlorophenol (4-CP) was also detected but was formed at higher concentration with bare material. These results are well matched with the chloride ions evolution.Figure 5
Disappearance of 2,4-dichlorophenol (20 mg L−1) and chloride evolution (a) and TPs formation (b) in the presence of bare and N-doped zinc oxide (St method) N-ZnO_St (1 gL−1) under visible light. Hydroquinone (HQ), resorcinol (Res), and 4-chlorophenol (4-CP) concentration over time are plotted.
(a)
(b)


## 3.1. Materials Characterization

XRD patterns for the synthetized samples are shown in Figure1. The diffraction peaks of bare (Figure 1 lines (a) and (c)) and doped (Figure 1 lines (b) and (d)) materials are attributable to the (1 0 0), (0 0 2), (1 0 1), (1 0 2), (1 1 0), (1 0 3), (2 0 0), (1 1 2), and (2 0 1) planes which are in accordance with the wurtzite hexagonal phase of ZnO [18]. These patterns are similar to all samples, assessing that neither the introduction of nitrogen nor the diverse synthesis changes the crystal structure of ZnO [36].Figure 1
XRD patterns for (a) ZnO_St, (b) N-ZnO_St, (c) ZnO_MW, and (d) N-ZnO_MW.The samples obtained using zinc sulphate as precursor (i.e., those obtained with the microwave assisted method) also show additional peaks attributable to zinc oxysulphate that did not evolve properly during the synthesis process. On the XRD patterns a Rietveld refinement was performed using the MAUD software that allowed estimating the average size of the crystallites. These values are about 70 and 40 nm for ZnO_MW and N-ZnO_MW nanostructures and 136 and 107 nm for ZnO_St and N-ZnO_St samples, respectively. Regardless of the synthetic method employed, the insertion of dopant caused a decrease in the crystallites size; this phenomenon was already observed and reported in the literature [39, 40].The specific surface area of the samples was measured applying the Brunauer-Emmett-Teller (BET) model on N2 adsorption measurement. Samples produced through the stirring method (ZnO_St and N-ZnO_St) exhibited a surface area of less than 10 m2/g, while those synthetized through microwave assisted method (ZnO_MW and N-ZnO_MW) have a slightly higher area (11.5
±
0.9 m2/g), underlining that the surface area is dependent on the synthetic method but is not affected by N-doping. The unexpected low surface area obtained with these synthetic processes was quite surprising, considering the quite high photoactivity of that samples, but higher than the commercial ZnO powder (4-5 m2/g) [41].Figure2 shows the absorption spectra (DRS UV-Vis) obtained for ZnO and N-doped ZnO samples. Two main issues arose from these spectra:(1)
the optical properties of the bare materials prepared from different synthetic methods (stirring and microwave assisted) are very similar;
(2)
the N-doping causes tiny modifications in the band gap (vide infra), but a high modification in the whole absorption spectra.In particular, the optical spectra of bare ZnO (Figure 2 line (A) and (B)) are dominated by the valence band (VB) to conduction band (CB) transition occurring at about 400 nm (ca. 3 eV) and the two spectra exhibit relatively small differences, in agreement with previous data reported in literature [36]. Figure 2 also compares the optical absorptions of N-doped zinc oxide (line (C) and (D)). A deep difference between doped and bare oxides spectra is evident. A large absorption in visible region of the optical spectra, together with a tiny red shift of the absorption edge (0.03 eV,vide infra), is observable. A small absorption shoulder centered at about 530 nm is more evident in Figure 2(b), where an enlargement of Figure 2(a) is provided. Doped samples show a pale grey-yellow color. The yellow is due to the presence of nitrogen into the structure (absorption band centered around 500–530 nm); the grey color is due to carbon impurities trapped into the structure during the calcination process (resulting in a tail in the absorption across the whole visible region).Figure 2
Kubelka-Munk transformed diffuse reflectance spectra of (a) (A) ZnO_St, (B) ZnO_MW, (C) N-ZnO_St, (D) N-ZnO_MW, and (b) their enlargement.
(a)
(b)The band gap of all the samples was calculated by linearization of the plot reportingα
h
ν
2 versus h
ν typical of direct band gap transitions for ZnO and Ce-ZnO through the Tauc plot from DRS measures [42]. Bare samples (namely, ZnO_St and ZnO_MW) show a band gap of 3.28 eV, while for N-doped ZnO (namely, N-ZnO_St and N-ZnO_MW) it is 3.25 eV, implying that the doping process does not induce a modification in the material band gap. This behavior is not surprising and was already reported in the literature [36].


## 3.2. Photocatalytic Tests

The photocatalytic activity of all synthetized materials was firstly investigated using phenol as model molecule. Phenol is known to be scarcely adsorbed at the catalyst surface and its degradation mainly proceeds through an initial oxidative attack, with the formation of hydroxylated derivatives [43, 44]. Preliminary tests showed that the direct photolysis process is very slow and can be considered negligible in the considered time window [45].The curves of phenol abatement as a function of irradiation time are plotted in Figure3 for ZnO_St and in Figure 4 for ZnO_MW. Under UV-A irradiation, the phenol disappearance similarly occurred with both bare and N-doped ZnO, irrespective of the synthetic method employed, and the complete disappearance is observed within 3 h of irradiation. Conversely, under Vis light irradiation, phenol degradation rate is higher with N-doped ZnO rather than with bare ZnO.Figure 3
Disappearance of phenol (20 mg L−1) in the presence of bare ZnO_St and N-doped zinc oxide N-ZnO_St (St method) (1 gL−1) under irradiation with UV-A or visible light.
(a)
(b)Figure 4
Disappearance of phenol (20 mg L−1) in the presence of bare (ZnO_MW) and N-doped zinc oxide (N-ZnO_MW) (MW method) (1 gL−1) under irradiation with a UV-A or visible light.
(a)
(b)Linear plots shown in left of Figures3(a) and 4(a) were obtained by fitting the degradation data with (1)-ln⁡CC0=kt,where C
0 is initial concentration and C is concentration measured after the irradiation time t; in all cases, a good linearity is observed. The calculated k values are summarized in Table 1.Table 1
Constant rate values calculated through (1).
K, min−1
ZnO_St
N-ZnO_St
ZnO_MW
N-ZnO_MW
UV-A
2.3 × 10−2
1.9 × 10−2
2.1 × 10−2
1.5 × 10−2
Vis
1.0 × 10−2
1.3 × 10−2
0.54 × 10−2
0.76 × 10−2Considering materials synthesized with MW method under Vis, the half-time life (t
1
/
2) was reduced from 130 min (ZnO) to 90 min (N-ZnO) and after 3 h of irradiation, almost 70% of phenol is abated, while with bare ZnO only 60% of phenol disappeared. Materials prepared through stirring method evidenced similar t
1
/
2 (almost 60 min) and under Vis after 3 h of irradiation the percentage of degraded phenol passes from 85% (bare ZnO) to 93% (N-doped ZnO). The experiment is repeated toward the abatement of phenol by using the materials preirradiated for 24 and 48 h under UV-A. Results show that the efficiency of the catalyst remains the same. As an example, the case of the phenol degradation with N-ZnO_St is reported in Figure 3(a).The photocatalytic increase observed with Vis light for N-doped systems cannot be ascribed to a variation in the materials band gap but could be attributed to the pronounced shoulder showing the presence of intraband gap states and not to a real shift of the band gap itself [19].The best performance was obtained with the materials preparedvia stirring synthetic method. A possible explanation of this behavior could be the fact that the materials preparedvia zinc acetate, as precursor, followed a better synthetic procedure and the final product was more clean and without defective compounds.The performance of zinc oxide based materials producedvia stirring method was also investigated toward the abatement of 2,4-dichlorophenol (2,4-DCP) under visible light. Once more, 2,4-DCP degradation faster occurred with N-doped material and the complete degradation was achieved within 2 h of irradiation (Figure 5(a)). Chloride ions were easier released in the case of N-doped material, too. The chloride evolution curve closely resembles the phenol disappearance curve. When employing N-doped material, the formation of chloride ions in stoichiometric amount was achieved within 2 h of irradiation, while with bare ZnO 3 h is required. Following 2,4-DCP degradation, the formation of some transformation products occurred, whose identity was confirmed by injection of authentic standard solution. Their concentration over time is reported in Figure 5(b) and showed the formation of hydroquinone (HQ) as main transformation product in both cases, at a slight higher amount in the presence of N-ZnO; 4-chlorophenol (4-CP) was also detected but was formed at higher concentration with bare material. These results are well matched with the chloride ions evolution.Figure 5
Disappearance of 2,4-dichlorophenol (20 mg L−1) and chloride evolution (a) and TPs formation (b) in the presence of bare and N-doped zinc oxide (St method) N-ZnO_St (1 gL−1) under visible light. Hydroquinone (HQ), resorcinol (Res), and 4-chlorophenol (4-CP) concentration over time are plotted.
(a)
(b)


## 4. Conclusions

Microwave assisted method and a more classic stirring process were applied for preparation of bare and N-doped nanostructured zinc oxide, as a potential highly efficient photocatalyst. The degradation of phenol on these sample was followed using both UV-A and visible light.UV light does not discriminate bare or doped materials but the irradiation with visible light evidenced the higher efficiency of doped materials compared to the bare oxides. This difference was also maintained in the chloride evolution, as with N-doped materials 2,4-dichlorophenol dechlorination was easily achieved. This aspect is interesting in order to obtain materials whose photocatalytic activity is promoted by solar light.



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*Source: 4129864-2016-06-19.xml*