Microstructure, optical properties, and catalytic performance of Cu2O-modified ZnO nanorods prepared by electrodeposition.

Cu2O-modified ZnO nanorods are prepared by a two-step electrodeposition method on ITO substrates, and the deposition time of Cu2O is 0, 1, 5, and 10 min, respectively. Cu2O particles are embedded in the interspaces of the ZnO nanorods, and the amounts of the Cu2O particles increase obviously when the deposition time lasts longer. The peaks corresponding to ZnO nanorods and Cu2O particles are detected from scanning electron microscope (SEM) and X-ray diffraction (XRD) results. UV-vis absorption spectra measurements have shown the bandgaps of ZnO nanorods shift from 3.22 to 2.75 eV. The methyl orange (MO) concentration can be reduced to around 15% in 100 min with Cu2O electrodeposition time for 10 min.

Background

Zinc oxide (ZnO), a typical n-type semiconductor with a direct bandgap of 3.37 eV, is an attractive material that could be suitable for a window layer [1-4]. Low-dimensional nanostructural ZnO shows unique physical and chemical properties [5-8]. Up to now, great attention has been focused on the investigation of ZnO nanostructures including thin film, nanowires, nanorods, and nanoparticles [9-13]. Due to the high specific surface area and excellent optical and electrical properties, ZnO nanorods have attracted much attention for their applications in solar cells [14-18]. Unfortunately, the absorption of ZnO in the visible-light region is very low due to its wide bandgap [19,20]. To extend the absorption of ZnO into the visible region, narrow bandgap semiconductors, such as CdS, CdSe, and Cu2O, have been used to construct heterostructures with 1D ZnO [21-24]. Cuprous oxide (Cu2O), with a direct bandgap of 2.17 eV, is a natural p-type semiconductor owning good mobility and high minority carrier diffusion length [25,26]. Low-cost producibility, abundance, nontoxicity, and high absorption coefficient in the visible light region make Cu2O a promising material for photovoltaic application [27,28]. Cu2O is considered to be a promising partner with ZnO for p-n heterojunction due to its narrow energy band [29,30].

The Cu2O/ZnO heterojunction has always been synthesized by several methods, such as thermal oxidation, sputtering, pulsed laser deposition, chemical vapor deposition, and electrodeposition. To our knowledge, much attention is focused on the Cu2O/ZnO heterojunction for solar cells, and there are few reports involving Cu2O/ZnO nanorods for photocatalysis studies [31-33]. Jeong et al. [34] reported that interface recombination is the dominant carrier transport mechanism, and Cu2O/ZnO heterojunction solar cells have high potential as solar cells if the recombination and tunneling at the interface can be suppressed at room temperature. In the current work, we prepared Cu2O-modified ZnO nanorods by a two-step electrodeposition method. The amount of Cu2O is controlled by the deposition time. The effects of the deposition time on the morphological, microstructural, optical properties, and catalytic performance of the Cu2O-modified ZnO nanorods have been investigated in detail.

Methods

Preparation of Cu2O-modified ZnO nanorods

The Cu2O-modified ZnO nanorods were prepared by a two-step electrodeposition method on ITO substrates. Prior to the deposition, ITO substrates were ultrasonically cleaned in acetone, alcohol, and deionized water, sequentially. Firstly, an aqueous solution composed of 0.01 mol/L zinc nitrate (Zn(NO3)2) was used to prepare ZnO nanorods. The ITO substrates served as the working electrode, platinum worked as the counter electrode, and an Ag/AgCl electrode was the reference electrode. The electrodeposition procedure was conducted in a water bath for 1 h at a temperature of 70°C under the constant potential of −0.7 V vs the reference electrode. Consequently, the electrochemical deposition of Cu2O on the ZnO nanorods was performed in an aqueous solution composed of 0.05 mol/L copper acetate (Cu(CH3COO)2) and 0.1 mol/L sodium acetate (NaCH3COO). The ZnO/ITO films served as the working electrode, and the temperature of water bath was 40°C. The applied potential was controlled at −0.2 V vs the reference electrode and lasted for different times (1, 5, and 10 min) for each Cu2O-modified ZnO nanorods. The samples were labeled as Cu2O(1)-ZnO, Cu2O(5)-ZnO, and Cu2O(10)-ZnO, respectively. The pure Cu2O film was deposited at the same condition, and the deposition time is 30 min.

Characterization

The phase and crystalline structure of the as-deposited films were examined by X-ray diffraction (XRD; MAC Science, Yokohama, Japan) with an X-ray diffractometer employing Cu-Kα radiation. The surface morphology of the Cu2O-modified ZnO nanorod films was observed with a field-emission scanning electron microscope (FESEM; S4800, Hitachi, Ltd., Chiyoda, Tokyo, Japan). A UV-visible (UV-vis) spectrophotometer (UV-2550, Shimadzu, Tokyo, Japan) was used to measure the UV-vis absorption spectra of the as-deposited films. The surface composition was analyzed by X-ray photoelectron spectrometer (XPS; ESCALAB 250, Thermo Fisher Scientific, Waltham, MA, USA). The Raman spectra and photoluminescence (PL) spectra were recorded by micro-Raman spectroscope system. The photocatalytic activity of the as-prepared samples was evaluated by the photodegradation of methyl orange (MO) solution under visible light irradiation. The visible light source was obtained using a 420-nm cutoff filter. The samples (15 mm × 10 mm) were immersed in 10 mL 15 ppm MO solutions. The distance between the samples and the light source was fixed at 5 cm. After the given time interval, the UV-vis absorption spectra of MO were recorded by UV-vis spectrophotometer (Shimadzu, UV-2550).

Results and discussion

Surface morphology analysis

Figure 1 shows the scanning electron microscope (SEM) micrographs of the Cu2O-modified ZnO nanorods with different Cu2O deposition times. As shown in Figure 1a, each hexagonal nanorod has a diameter of about 200 nm and the length is about 1 μm. The nanorods are gradient and uniformly disperse on the ITO substrates. From Figure 1, it can be observed that cubic structure Cu2O particles embedded in the interspaces of the ZnO nanorods and the amounts of the Cu2O particles increase obviously when the deposition time increases [35]. It can also be found that as the Cu2O deposition time increases, the diameter and length of the nanorods decreased, which can be affected by electrolyte corrosion during the Cu2O deposition process.

Figure 1

SEM micrographs of the Cu O-modified ZnO nanorods. Cu2O-ZnO modified with different Cu2O deposition times of (a) 0 min, (b) 1 min, (c) 5 min, and (d) 10 min and (e) pure Cu2O, respectively.

Microstructure analysis

Figure 2 illustrates the XRD pattern of the Cu2O-modified ZnO nanorods with different deposition times of Cu2O particles. From Figure 2, the characteristic peaks of Cu and CuO are not observed for all the samples, suggesting that no metallic copper or CuO formed in the electrodeposition process. The single-phase polycrystalline Cu2O films have been obtained only with the applied potential below −0.3 V [36]. In Figure 2a, apart from the diffraction peaks corresponding to the ITO substrate, the peaks that corresponded to the reflections are 100, 002, 101, 102, 110, and 103 peaks of ZnO nanorods according to JCPDS: 89-1397. In Figure 2b,c,d, besides the peaks of ZnO nanorods and ITO substrate, the diffraction peaks of 111, 200, and 220 crystal planes of Cu2O appear (JCPDS: 05-0667). The Cu2O (111) peak (2θ = 36.50°) is very close to the ZnO (101) peak (2θ = 36.25°), and they are overlapped in the pattern. The intensities of the Cu2O characteristic peaks increase with the Cu2O electrodeposition time for increased amounts of the Cu2O nanoparticles. The characteristic peaks of Cu2O electrodeposited for 1 min (Figure 2b) can barely be detected, and this can be ascribed to an insufficient amount. In a word, the peaks of Cu2O particles are relatively weaker due to the shorter deposition time compared with ZnO nanorods.

Figure 2

XRD patterns of the Cu O-modified ZnO nanorods.

UV-vis absorbance and XPS analysis

Figure 3 shows the optical absorption spectra for the Cu2O-modified ZnO nanorods with different Cu2O deposition times from 0 to 10 min. An absorption edge at 390 nm for the ZnO nanorods was observed, as shown in Figure 3a. The absorption edges of the Cu2O-modified ZnO nanorods show an obvious redshift compared with pure ZnO nanorods and exhibit a broad absorption band in the UV region, which originates from the combinational effect of the narrow bandgap of Cu2O (approximately 2.17 eV) and wide bandgap of ZnO (approximately 3.37 eV) [37]. The absorbance in the visible light range increases with the increase of the deposition time of Cu2O. The introduction of Cu2O particles in ZnO nanorods extends the absorption edge to the visible light range, which is very important in making full use of sunlight.

Figure 3

UV-vis absorption spectra of the samples.

The optical bandgaps of ZnO and Cu2O can be determined based on the equation: (αhν)2 = A(hν − Eg) [38]. The energy bandgap (Eg) is measured by linear extrapolation to the hv-axis. The inset of Figure 4 shows (ahv)2 versus hv for the Cu2O films, and the estimated direct bandgaps are listed in Table 1. Due to variation in deposition time, the value of absorption spectra changed. For Cu2O-modified ZnO nanorods, when the Cu2O deposition time increases from 1 to 10 min, the corresponding bandgaps of Cu2O particles are 2.43, 2.38, and 2.30 eV, respectively. In addition, the bandgaps of ZnO nanorods shift from 3.22 to 2.75 eV, which is also consistent with previous SEM and XRD results.

Figure 4

Plot of ( ) vs photon energy for Cu O-modified ZnO nanorods.

Table 1

The estimated direct bandgaps of the Cu O-modified ZnO nanorods

	Cu 2 O deposition time (min)
	0	1	5	10
Cu2O bandgap (eV)	-	2.43	2.38	2.30
ZnO bandgap (eV)	3.22	3.11	3.00	2.75

XPS measurements were conducted for surface analysis of the Cu2O-modified ZnO nanorods with Cu2O deposition time for 5 min (Figure 5). As shown in Figure 5, the peaks of Zn2p and Cu2p are detected from the XPS spectrum. Two peaks of Zn2p located at 1,045.1 and 1,021.9 eV are assigned to Zn2p3/2 and Zn2p1/2, respectively, which can be assigned to Zn2+ in ZnO nanorods (Figure 5a) [39]. The typical XPS peaks of Cu (2p) at 952.2 and 932.4 eV for the Cu2O-modified ZnO nanorods indicate the existence of Cu+ during the deposition of Cu2O particles (Figure 5b). Furthermore, the characteristic peaks for Cu2+ at 953.6 (2p1/2) and 933.7 eV (2p3/2) were not observed [40]. This result confirms that the sample contains Cu+ rather than Cu2+ or Cu.

Figure 5

XPS spectra of the sample with Cu O deposition for 5 min (a, b).

Raman and PL spectra analysis

Figure 6 shows the Raman and PL spectra of Cu2O-modified ZnO nanorods with Cu2O deposition for 0 and 5 min. The peak at 437 cm−1 is due to the E2 high vibration mode of ZnO hexagonal crystal structure as shown in Figure 6a [41]. Figure 6a also shows that the stronger Raman peak of 218 cm−1, which corresponds to 2Γ12− vibration modes of Cu2O. Meanwhile, the relative weaker peaks of 146 and 626 cm−1 can be contributed to infrared vibration mode Γ15, which are excited from oxygen vacancy [42]. Figure 6b shows the PL spectra of Cu2O-modified ZnO nanorods. There appeared two component peaks of the UV emission in the PL spectra of Cu2O-modified ZnO nanorods. The predominant sharp peak appeared at about 380 nm could be assigned to the near band emission of the ZnO nanorods [43]. In addition, a wide emission with a peak at 600 nm was detected and regarded as defect-related emissions of ZnO nanorods. The existence of Cu2O particles has little impact on peak position of ZnO nanorods. The emissions at 380 and 600 nm were diminished when Cu2O particles were deposited on the ZnO nanorods, which may originate from the random multiple scattering in such structure.

Figure 6

Raman (a) and PL (b) spectra of the sample with Cu O deposition for 5 min.

Photocatalytic degradation of MO

The photocatalytic activities of the as-prepared samples were carried out by the degradation of MO solution under visible light irradiation, and the experimental results are shown in Figure 7. Here, C0 and C are the absorbance of the characteristic absorption peak (464 nm) of MO solution before and after irradiation. As indicated in Figure 7, the pure ZnO nanorods exhibit a weak ability for the degradation of MO. The poor degradation ability of the pure ZnO nanorods can be ascribed to the fact that the visible light cannot provide energy to excite electrons from the valance band to the conduction band. All the Cu2O-modified ZnO nanorods have strong degradation ability of MO than the pure ZnO nanorods [44]. With increasing Cu2O electrodeposition time, the degradation abilities of the Cu2O-modified ZnO nanorods enhanced. The reason is that Cu2O has higher degradation ability than ZnO. Meanwhile, the amount of Cu2O particles on the ZnO nanorods increases when increasing the Cu2O electrodeposition time. Furthermore, the Cu2O-modified ZnO nanorods have a large specific surface area than pure ZnO nanorods. It is worth mentioning that the MO concentration can be reduced to around 15% in 100 min with Cu2O electrodeposition time of 10 min. As a result, the photocatalytic activity of the Cu2O-modified ZnO nanorods depends on the Cu2O electrodeposition time.

Figure 7

The visible light photocatalytic degradation ratios to MO of the samples.

Conclusions

In summary, the Cu2O-modified ZnO nanorods are prepared by electrodeposition method on ITO substrates. XRD measurement shows the coexistence of Cu2O with cubic structure and ZnO with hexagonal structure. SEM images reveal that Cu2O particles embed in the interspaces of the ZnO nanorods and the amounts of the Cu2O particles increase obviously when the Cu2O deposition time lasts longer. The absorbance in visible light range increases with the increase of the deposition time of Cu2O. All the Cu2O-modified ZnO nanorods have strong degradation ability of MO than the pure ZnO nanorods under visible light irradiation. The nanorod's structure of the ZnO had been broken and resulted to a significant decrease of the special surface area associating with the increase of the Cu2O deposition time. The obtained films may be used in fabricating solar cell and treating dye wastewater.