# Enhanced Photocatalytic Property of Cu Doped Sodium Niobate

Authors: Jianbin Xu; Feng Zhang; Bingyang Sun; Yingge Du; Guoqiang Li; Weifeng Zhang
Journal: International Journal of Photoenergy
 (2015)

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## Abstract

We investigate the photocatalytic activity of Cu doped NaNbO3 powder sample prepared by the modified polymer complex method. The photocatalytic activity of hydrogen evolution from methanol aqueous solution was improved by Cu 2.6 at% doping. The photocatalytic degradation of rhodamine B (RhB) under visible light irradiation was enhanced in comparison with pristine NaNbO3. Cu introduction improved the adsorption property of NaNbO3, judging from the Fourier transform infrared spectra. Moreover, the ultraviolet light excitation in Cu doped sample would accelerate the mineralized process.


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## Body

## 1. Introduction

Semiconductor photocatalysis, including solar energy conversion and environmental remediation, has attracted much attention in the past four decades [1]. Besides the prototypical photocatalyst TiO2, various semiconductors have been examined for the photocatalytic activities, such as water splitting, dye degradation, CO2 reduction, and air purification [2–10]. Development of photocatalysts with higher efficiency remains as one of the key goals in order to better utilize the solar energy.Sodium niobate (NaNbO3), with a pseudoperovskite structure, has been studied as a photocatalyst with potential applications in solar fuel production and organic pollutants removal [11–18]. Many approaches have been applied to improve its photocatalytic activity [15, 18–22]. In particular, element doping was used to extend light absorption to visible region and to improve the photocatalytic efficiency [19, 22–24]. Nitrogen was first studied as the nonmetal dopant to achieve visible light activity for dye degradation and air purification [22, 23]. Recently, NaNbO3 samples with Ru doping were successfully prepared by hydrothermal method. Their photocatalytic activities could be improved only after loading the novel metal Pt, although the light absorption was extended to 600 nm [19]. La and Co codoping improved the light absorption property and enhanced the photocatalytic hydrogen evolution [24].It has been demonstrated that doping Cu in oxides and sulfides can modify their electronic structures [25–31]. For example, the replacement of Cu for Na in Na2Ta4O11 can create visible light absorption due to the introduction of Cu d10 orbital in the top of valence band [25]. Doping Cu also could enhance the photocatalytic activity of oxide photocatalysts [26, 30–33]. For instance, the Cu doping significantly increased the photocatalytic activity of K2Nb4O11 catalyst [26]. ZnO nanorods with increasing Cu doping also exhibited the enhanced photocatalytic activity [34]. The Cu(II) doped NaTaO3 sample loaded with 0.3 wt% NiO cocatalyst exhibited a dramatic increase of the activity in the hydrogen production reaction [27]. The AgNbO3 with trace of Cu modification showed an enhanced photocatalytic activity for oxygen evolution [35].In this study, we investigated the Cu doped NaNbO3 systematically. Cu doped NaNbO3 powder samples were prepared by the modified polymer complex method. The 2.6 at% doped sample shows the highest activity for hydrogen evolution from aqueous methanol solution. The Cu doping dramatically changes the mechanism of rhodamine B (RhB) degradation under visible light irradiation.


## 2. Experimental

The NaNbO3 powders were prepared by the modified polymer complex method [36]. The 10 mL NbCl5 ethanol solution (50 mg/mL) was diluted with 50 mL ethanol. Different amounts of sodium alginate and copper acetate were added to the above solution with stirring according to the formula of CuxNa1-2xNbO3. The nominal Cu molar amounts were 0, 0.026, 0.052, and 0.078. Then citric acid (10 g) and polyethylene glycol (10 g) were added. The mixtures were heated at 60°C until they turned into solid. The obtained solids were then heated at 390°C for 4 h and at 450°C for 3 h to form the original samples. To remove the Cu remains on the surface, we washed all original samples with diluted hydrochloric acid until the solution is colorless. The final samples were denoted as NN, A, B, and C, respectively.The crystal structures of samples were determined by an X-ray diffractometer (DX-2700 diffractometer, Fangyuan) with Cu Kα radiation (λ = 0.1542 nm). Fourier transform infrared (FTIR) spectra were measured by a spectrophotometer with KBr as the reference sample. Raman scattering spectra were obtained by a laser Raman spectrophotometer (RM-1000, Renishaw). The elements were analyzed by energy dispersive spectroscopy (EDS). The diffuse reflectance spectra were recorded using a UV–Uis spectrophotometer (UV-2550) and transformed to the absorption spectra automatically according to the Kubelka-Munk relationship.Photocatalytic activity was evaluated by the photocatalytic hydrogen evolution and degradation of RhB under light irradiation, which was emitted from a 300 W Xe lamp without filters. The sample (0.05 g) was added in 50 mL aqueous methanol solution (methanol: 20 vol%) in a glass reactor. Aqueous H2PtCl6 (10 g/L, 33.2 μL) solution was added to form a Pt cocatalyst. Before photocatalytic reaction, the reaction system was vacuumed and purged with N2 for 30 min to remove O2 that was dissolved in the aqueous solution. After being sealed by a quartz cover, the solution was irradiated from the topside by 300 W Xe lamp. The stirring was on during the reaction. The amount of H2 evolved was determined using gas chromatography (GC1690, Kexiao Ltd.).The photocatalytic degradation of RhB was carried out with 0.01 g powder sample suspended in a 100 mL RhB solution (2.5 mg/L) in a glass cell. The suspension was first allowed to reach adsorption–desorption equilibrium with continuous stirring for half an hour in the dark. The variation in RhB concentration was recorded using a UV-Vis spectrophotometer (UV-2550) by measuring the absorbance of the main peak.The amount ofO
∙
H radical, which is one of the important oxidization species, was measured by reported methods [37]. The reaction principle was that terephthalic acid (TA) readily reacted with O
∙
H radicals to produce highly fluorescent product, 2-hydroxyterephthalic acid (TAOH), which emitted photoluminescence at around 426 nm on the excitation of its own 312 nm absorption band. The intensity of the peak attributed to TAOH was known to be proportional to the amount of O
∙
H radicals formed. The experimental process was briefly described below. The 0.01 g powder sample was suspended in 100 mL solution (20 mM NaOH and 6 mM terephthalic acid). After 0.5 h of full arc Xe lamp irradiation, the solution was used for fluorescence spectrum measurements (Horiba, JY FluoroLog-3).


## 3. Results and Discussion

The XRD patterns of all samples are shown in Figure1(a). All of them could be indexed as the perovskite phase of sodium niobate according to PDF#19-1221. The crystalline quality is characterized by the full width at half maximum (FWHM) of the XRD curve. Compared with the NN sample, the FWHM of the peak located at 2
θ = 22.7° in the Cu doped samples decreases as shown on the right of Figure 1(a), indicating that the crystalline quality becomes better due to introducing Cu. The grain size could be estimated from the FWHM using Scherrer’s equation: d
X
R
D
=
0.9
λ
/
(
β
∗
cos
⁡
(
θ
)
), where λ is the X-ray wavelength; β is the FWHM (in radian); and θ is the half of diffraction peak angle (2
θ). The grain sizes were estimated to be 13 nm for NN and 22 nm for Cu doped samples, which was similar to the samples prepared by the polymer complex method [36]. When the Cu substituted for Na below 80% in Na2Nb4O11, the lattice constant would increase [25]. However, in our case, no peak shift was found due to the smaller concentration of Cu. The element analysis results for Cu/Nb ratios in the samples are in good agreement with the nominal values, as shown in Figure 1(b). Moreover, the main valence state of Cu is +1, judging from the result of X-ray photoelectron spectra (XPS), as shown in Figure 1(c). We, therefore, consider the Cu doped into the lattice as our expectation.Figure 1
(a) X-ray diffraction patterns of NN, A, B, and C (left). Enlarged view of the main peak at 22.7° (right). (b) Cu/Nb ratio obtained from EDS analysis (black squares). The dash line represents the theoretical value. (c) Cu 2p line obtained from B.
(a)
(b)
(c)To identify the change of structure due to Cu introduction, Raman and FTIR spectroscopy were measured, as shown in Figure2. The Raman spectra indicated that the Cu introduction did not change the NbO6 bonding length. As a comparison, when part of Na was replaced by Ag, the Raman band at ~600 cm−1 corresponding to the stretching model of NbO6 octahedron was shifted to higher wavenumber [38]. In FTIR spectra, the peak at 1063 cm−1 was associated with the bending modes of the adsorbed water [39]. Zhong et al. found that the C
u
-
O
a
d
s
-
(
C
O
)
a
d
s will generate a IR band above 1080 cm−1 [40]. Therefore, we assigned the peak at 1088 cm−1 as the result of Cu doping, representing the adsorption property of the surface. For easy comparison, we normalized the intensity of 1088 cm−1 to 1063 cm−1. The result indicated that the Cu doping changed the ratio of the intensity of peak at 1088 and 1063 cm−1, as shown in the inset of Figure 2(b). Sample A has the largest value, implying the best adsorption properties. For further increasing the Cu content, the ratio decreased, indicating that the Cu doping has an optimum amount. When the content of Cu is over the optimum amount, the Cu will aggregate on the surface and possibly screen the IR signal. Furthermore, it is known that the shape of the intense band at ~670 cm−1 corresponds to an asymmetric enlargement of the Nb-O bond of the octahedral NbO6 structures [22]. No change of that band among those samples revealed that the Nb-O band length did not change, which is consistent with the Raman results.Figure 2
(a) Raman and (b) FTIR spectra of NN, A, B, and C. The inset in (b) is the normalized intensity of peak at 1088 to 1632 cm−1 as a function of Cu content.
(a)
(b)Diffuse reflectance spectra of NN and A are shown in Figure3. The absorption edges are very similar, indicating that the Cu doping do not change the light absorption edge. Palasyuk et al. reported that 1% Cu doping would change the light absorption of Na2Ta4O11 significantly [25]. However, no obvious shift was observed in our case. Actually, the other Cu doped samples showed very similar absorption spectra with that of NN. The optical band gaps could be estimated from the absorption spectra using the following equation: (
α
h
υ
)
=
M
h
υ
-
E
g
n
/
2, where M, α, h
υ, and E
g are constant, absorption coefficient, the photon energy, and the optical band gap, respectively. In this equation, n is determined by the transition type and is equal to 1 for direct transition and 4 for indirect one. The values of n and E
g were estimated by the following steps: first, the plot of ln
⁡
(
α
h
υ
) versus ln
⁡
(
h
υ
-
E
g
) was drawn using an approximate value of E
g, and then the value of n was estimated from the slope of the straight line near the band edge; second, the plot of α
h
υ
2
/
n versus h
υ was drawn and then a tangential line was plotted near the band edge; the x-intercept of the tangential line corresponded to the optical band gap. The n for NN is equal to 4 because of the indirect transition. The band gaps of NN and A are the same and are estimated to be 3.3 eV, which is slightly smaller than 3.4 eV obtained from samples prepared by solid state reaction method and larger than 3.0 eV obtained from the plate like NaNbO3 [41, 42].Figure 3
Diffuse reflectance spectra of NN and A. The insets are the plots used to estimate the band gap.These samples were tested for H2 evolution from aqueous methanol solution, as displayed in Figure 4. H2 could be generated for all four samples. While sample A (2.6 at% Cu doping) shows the highest activity, the amount of H2 evolution increased in the order of C < B < NN < A. The H2 evolution rate was 112 μmol/h for C, 214 μmol/h for B, 228 μmol/h for NN, and 343 μmol/h for A. These results are larger than the samples prepared by solid state reaction under different atmospheres [43]. The suitable amount of Cu doping could enhance the photocatalytic H2 evolution. In previous report amorphous Cu(II) clusters modified α-Bi2O3 exhibited an enhanced photocatalytic activity [32]. Consequently, we consider the enhanced activity of H2 evolution originated from the better crystallinity and adsorption property.Figure 4
Amount of H2 evolution from aqueous methanol solution varied with irradiation time over NN, A, B, and C. The inset is the plot of rate of H2 evolution.Photocatalytic activity for the decomposition of RhB in an aqueous solution was evaluated in the presence of samples under visible light irradiation of Xe lamp. The variation in the concentration of RhB was recorded by measuring the UV-Vis spectrum. These temporal UV-visible spectral changes of RhB aqueous solution over NN and A during the photocatalytic degradation reactions are shown in Figure5(a). In the presence of A, RhB underwent pronounced photocatalytic degradation upon visible light irradiation. The wavelength corresponding to the maximal absorbance (λ
m
a
x) shifts gradually from the initial 554 nm towards shorter wavelength and finally reaches 498 nm, along with a gradual decrease in the maximal absorbance during photocatalytic reactions of the RhB solution, which are further quantitatively demonstrated in Figure 5(b). However, in case of NN, only a very small decrease in absorbance was observed and almost no shift of λ
m
a
x. Neither NN nor A can absorb the visible light. Therefore, the RhB decomposition over A is mainly considered as RhB sensitive self-degradation. From the FTIR we can find that the Cu doping improved the adsorption property. The RhB sensitive self-degradation is very close to the adsorption [44, 45]. Accordingly, we conclude that Cu doping enhanced the adsorption of RhB, leading to an improved photocatalytic activity.Figure 5
(a) Temporal changes of RhB absorption spectra in presence of NN and A under visible light irradiation (λ
>
420 nm). (b) Variation in C
/
C
0 (solid square and spot) and wavelength shift (empty square and cycle) over NN and A under visible light irradiation.
(a)
(b)We also carried out the experiment under full arc irradiation of Xe lamp. Both NN and A show the similar spectra profiles, as demonstrated in Figure6. Sample A exhibits similar activity under visible light and full arc irradiation. The blue shift of λ
m
a
x frequently observed in oxidizing RhB using oxides as photocatalyst is associated with the stepwise removal of the N-ethyl group during degradation of RhB (i.e., N, N, N′, N′-tetra-ethylated rhodamine) molecule [46, 47]. NN shows significantly different behaviors under full arc irradiation from that under visible light irradiation. NN could be excited by the UV light. Therefore, the removal of the N-ethyl group under full arc irradiation was thought to be caused by the light absorption.Figure 6
Variation inC
/
C
0 (b) and wavelength shift (a) over NN and A under full arc Xe lamp irradiation (solid square and cycle). Those under visible light (empty square and cycle) were also shown for comparison.
(a)
(b)We expected that the RhB degradation was related to theO
∙
H radical. To confirm that O
∙
H had effect on the dye degradation, we employed photoluminescence spectroscopy using terephthalic acid to test O
∙
H, as shown in Figure 7 [37, 46, 48]. We observed significant emission signal at 425 nm for NN and A sample after full arc irradiation for 0.5 h, confirming that significant O
∙
H radical was produced during the light irradiation and that it was involved in the photodegradation reaction. Moreover, when the isopropanol was added in the system, no degradation was found under full arc and visible light irradiation. These results indicated that the O
∙
H is mainly the oxidized species [49]. The very small emission signal under visible light irradiation could be caused by the leakage of UV light through the filter.Figure 7
Fluorescence spectra of 2-hydroxyterephthalic acid (TAOH) over NN and A after 1 h of full arc and visible light irradiation of Xe lamp.In the liquid phase,O
∙
H could be generated by the photogenerated electrons and holes [1, 50]. Methanol, which is usually used as sacrificing agent in the hydrogen evolution from water, could react with the photogenerated hole [2, 49, 51]. When the methanol was added in the solution, the processes of the N-ethyl group removal both under irradiation were delayed, as shown in Figure 8. This fact implied that the hole took part in the reaction. Moreover, when the system was irradiated by the full arc of Xe lamp, the process of mineralization will be speeded up in both reactions with and without methanol. These results indicated that the excitation of ultraviolet light in Cu doped sample only impacts the mineralized process.Figure 8
Variation inC
/
C
0 (b) and wavelength shift (a) over A with and without methanol under full arc and visible light irradiation of Xe lamp.
(a)
(b)


## 4. Conclusions

The nominal Cu atoms were doped into the sample. No changes of crystal structure and optical band gap were observed in Cu doped samples. Doping Cu improved the adsorption property. The photocatalytic activity of hydrogen evolution was improved by Cu 2.6 at% doping. The photocatalytic degradation of RhB under visible light was enhanced in comparison with the pristine NaNbO3. Moreover, the photoexcitation in Cu doped sample only impacts the process of mineralization.



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