# Fabrication of CdS/H-TiO2 Nanotube Arrays and Their Application for the Degradation of Methyl Orange in Aqueous Solutions

Authors: Xiaosong Zhou; Fei Yang; Bei Jin; Liuyong Chen; Shanshan Li
Journal: Journal of Nanomaterials
 (2014)

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## Abstract

The fabrication and characterization of heterogeneous structures based on CdS and self-doped TiO2 nanotube arrays (H-TNTs) are reported for the first time. CdS was conformally deposited onto TiO2 nanotube arrays (TNTs) using a simple method of electrochemical atomic layer deposition. The as-prepared samples were characterized by scanning electron microscopy (SEM), X-ray photoelectron spectroscopy (XPS), UV-Vis diffusion reflection spectroscopy (UV-Vis DRS), and photoluminescence spectroscopy (PL) techniques. Compared with pure TNTs, CdS/H-TNTs exhibit enhanced photoelectrochemical properties and photocatalytic activity under visible light. Self-doping introduces oxygen vacancies and Ti3+ species, and the electrochemical deposition technique promotes the deposition of CdS onto TiO2 nanotube walls, forming a heterojunction compact structure and resulting in decrease in photocatalytic activity under visible light.


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## Body

## 1. Introduction

Since Fujishima and Honda first reported the use of a single-crystal TiO2 semiconductor photoanode for the photocatalytic decomposition of water [1], TiO2 photocatalysts have quickly attracted the worldwide attention of environmental and energy researchers. Because of its highly ordered structure, large surface area, high recovery and high recycle rate, capability for scale-up, and excellent controllability, TiO2 nanotube arrays are favorable structures for many applications. However, the large band gap of titania restricts its photocatalytic applications to the UV range. Efforts to shift the band gap of TiO2 while maintaining the material’s excellent charge-transfer properties and photocorrosion stability have primarily focused on metal/nonmetal ion doping to induce a red shift in the band gap [2]. However, the doping of foreign ions such as those of transition metals involves the drawbacks of thermal instability, a higher probability of forming charge carrier recombination centers, and expensive synthesis protocols [3]. Therefore, extending the photoresponse of TiO2 NTs to the visible-light range and increasing the material’s photocatalytic efficiency remain possible objectives of future research.Recently, appealing approaches based on dopant-free, pure TiO2 phase have been proposed to overcome the abovementioned shortcomings. Naldoni et al. prepared black, self-doped TiO2 nanoparticles with a band gap of 1.85 eV through the high-pressure hydrogenation of crystalline TiO2 [4]. Tao et al. reported the surface of self-doped Ti3+ rutile TiO2  {
011
} by the oxidation of bulk Ti interstitials, yielding a material with a band gap of only 2.1 eV [5]. Self-doping with Ti3+ bulk species has also been demonstrated [6]. In particular, Xing et al. developed “vacuum-activated TiO2” via annealing TiO2 in a vacuum drying oven to obtain a brownish powder with improved visible-light photocatalytic activities [7]. Zhang et al. reported that the Ti3+ ions exist on TiO2 nanotubes’ surfaces in the form of oxygen vacancy-Ti3+ pairs, leading to aggravated electron recombination in TiO2 nanotube-containing cells [8]. Samiee and Luo reported the annealing of TiO2 nanoparticles in various controlled atmospheres. The results suggest that the use of vacuum environments or the presence of hydrocarbon species during annealing is effective in enhancing the photocatalytic activity [9]. These pure TiO2 phase visible-light photocatalysts have shown band-gap narrowing mainly attributed to surface disorder [4] and point defects, such as oxygen vacancies [6] and Ti interstitials [10]. However, the fabrication of self-doped materials remains a challenge.Very recently, much active research has focused on the anchoring of narrow-band-gap semiconductor materials (such as CdS) to TNTs, rendering these oxides sensitive to visible light [11, 12]. In the CdS/TNTs integrated system, CdS has a relatively small band gap and is thus capable of harvesting photons in the visible and near-infrared regions [13]. The use of CdS is shown to enhance the charge carrier separation process and consequently is expected to enhance the inactivation efficiency. Zhu et al. reported on CdS/TNTs coaxial heterogeneous structures. These coaxial heterogeneous structures show a fivefold enhancement in photoactivity relative to the photoactivity of pure TiO2 NTs [14].In this paper, we report the study of CdS-sensitized H-TNTs photoelectrodes and their photocatalytic performance. It is shown that the CdS/H-TNTs heterojunction structures exhibit enhanced photoelectrochemical properties and photocatalytic activities.


## 2. Experimental

### 2.1. Synthesis of H-TNTs

TNTs were fabricated by a method described in our previous report [15]. In a typical procedure, a 2 × 3 cm2 cleaned Ti sheet (99%) with a thickness of 0.1 mm was used as an anode and Ir/Ta alloy as a cathode. The electrolyte was an aqueous solution composed of 1,2,3-propanetriol, NH4F (1.0 wt.%), and H2O (15 vol.%). The anodizing voltage was varied from 0 to 25 V at a rate of 100 mV·S−1 and was held at 25 V for 2 h. The prepared TNTs were then annealed in a hydrogen atmosphere at 500°C for 4 h and quickly cooled to obtain H-TNTs. For comparison, TNTs were also annealed at 500°C in air for 4 h.


### 2.2. Synthesis of CdS/H-TNTs

CdS deposition was carried out from a solution containing 0.005 M Na2S (Na2S·9H2O), 0.01 M CdSO4 (CdSO4
·8/3H2O), and 0.15 M EDTA2− (C10H14O8N2Na2
·2H2O) at a pH level of 8.5, which was adjusted with perchloric acid and ammonia. A Pt foil counter electrode and an Ag/AgCl were used in the three-electrode system. Initial cyclic voltammetry experiments were carried out at a deposition potential of −0.75 V (versus Ag/AgCl). The deposition time for CdS electrodeposition was 5 h.


### 2.3. Characterization of As-Prepared Samples

X-ray diffraction (XRD) patterns were recorded on an X-ray diffractometer (D/max-IIIA, Japan) using Cu Ka radiation and operating at 30 kV/30 mA over an angle range of 10 to 80°. The surface morphology was examined using a scanning electron microscope (SEM) (LEO1530VP, LEO Company) operated at an acceleration voltage of 15 kV. UV-Vis light absorption spectra were obtained on a Hitachi UV-3010 spectrophotometer equipped with an integrating sphere assembly and using the diffuse reflection method and BaSO4 as a reference. Electron paramagnetic resonance spectroscopy (EPR) was performed on a Bruker A300 spectrometer instrument. The instrument settings were as follows: microwave frequency of 9.51 GHz; microwave power of 3.16 mW; and modulation amplitude of 1 G at 100 kHz.


### 2.4. Photoelectrochemical and Photocatalytic Tests of As-Prepared Samples

Photocurrent measurements were carried out in a standard electrode photoelectrochemical cell using an electrochemical workstation (CV-27, BAS). The as-prepared samples, platinum gauze, and Ag/AgCl were used as working, counter, and reference electrodes, respectively. A sodium sulfate solution (0.5 M) was used as the electrolyte. Photocurrent was generated using filtered light (λ
>
40
0 nm, 150 mW/cm2) from a PLS-SXE300UV Xe lamp. The light/dark short-circuit photocurrent response under zero bias was recorded with an Agilent digital multimeter.The photocatalytic activity was measured in a XPAII reactor. The samples (8 × 20 mm2) were immersed in 10 mL quartz test tubes containing 4 mL of methyl orange (MO) (10 mg/L) in the dark for 1 h to achieve adsorption equilibrium before irradiation. Visible-light (λ
>
40
0 nm) photocatalytic experiments were then conducted for 120 min. The remaining dye concentrations in the reaction solution were determined using the U3010 spectrophotometer. The entire decomposition process was conducted by sparging air at a flow rate of 10 mL/min.The existence ofOH
∙ can be tested by the terephthalic acid (C8H6O4, TA) fluorescent method. It has been demonstrated that OH
∙ can react with TA and generate luminescent TAOH according to the equation [16] OH
∙ + TA →TAOH.An 8 × 20 mm2 sheet of as-prepared photocatalyst was added to 4 mL of a solution containing 10 mM NaOH and 3 mM TA in a quartz reactor. Prior to photoreaction, the suspension was magnetically stirred in the dark for 1 h to ensure the establishment of an adsorption/desorption equilibrium. The photoreaction was carried out as the foregoing photocatalytic reaction under visible light without oxygen bubbled into the suspension. After 150 min of photoreaction, the fluorescence spectra of the resultant solution were measured on an Edinburgh F-900 fluorescence spectrophotometer using an excitation wavelength of 320 nm.


## 2.1. Synthesis of H-TNTs

TNTs were fabricated by a method described in our previous report [15]. In a typical procedure, a 2 × 3 cm2 cleaned Ti sheet (99%) with a thickness of 0.1 mm was used as an anode and Ir/Ta alloy as a cathode. The electrolyte was an aqueous solution composed of 1,2,3-propanetriol, NH4F (1.0 wt.%), and H2O (15 vol.%). The anodizing voltage was varied from 0 to 25 V at a rate of 100 mV·S−1 and was held at 25 V for 2 h. The prepared TNTs were then annealed in a hydrogen atmosphere at 500°C for 4 h and quickly cooled to obtain H-TNTs. For comparison, TNTs were also annealed at 500°C in air for 4 h.


## 2.2. Synthesis of CdS/H-TNTs

CdS deposition was carried out from a solution containing 0.005 M Na2S (Na2S·9H2O), 0.01 M CdSO4 (CdSO4
·8/3H2O), and 0.15 M EDTA2− (C10H14O8N2Na2
·2H2O) at a pH level of 8.5, which was adjusted with perchloric acid and ammonia. A Pt foil counter electrode and an Ag/AgCl were used in the three-electrode system. Initial cyclic voltammetry experiments were carried out at a deposition potential of −0.75 V (versus Ag/AgCl). The deposition time for CdS electrodeposition was 5 h.


## 2.3. Characterization of As-Prepared Samples

X-ray diffraction (XRD) patterns were recorded on an X-ray diffractometer (D/max-IIIA, Japan) using Cu Ka radiation and operating at 30 kV/30 mA over an angle range of 10 to 80°. The surface morphology was examined using a scanning electron microscope (SEM) (LEO1530VP, LEO Company) operated at an acceleration voltage of 15 kV. UV-Vis light absorption spectra were obtained on a Hitachi UV-3010 spectrophotometer equipped with an integrating sphere assembly and using the diffuse reflection method and BaSO4 as a reference. Electron paramagnetic resonance spectroscopy (EPR) was performed on a Bruker A300 spectrometer instrument. The instrument settings were as follows: microwave frequency of 9.51 GHz; microwave power of 3.16 mW; and modulation amplitude of 1 G at 100 kHz.


## 2.4. Photoelectrochemical and Photocatalytic Tests of As-Prepared Samples

Photocurrent measurements were carried out in a standard electrode photoelectrochemical cell using an electrochemical workstation (CV-27, BAS). The as-prepared samples, platinum gauze, and Ag/AgCl were used as working, counter, and reference electrodes, respectively. A sodium sulfate solution (0.5 M) was used as the electrolyte. Photocurrent was generated using filtered light (λ
>
40
0 nm, 150 mW/cm2) from a PLS-SXE300UV Xe lamp. The light/dark short-circuit photocurrent response under zero bias was recorded with an Agilent digital multimeter.The photocatalytic activity was measured in a XPAII reactor. The samples (8 × 20 mm2) were immersed in 10 mL quartz test tubes containing 4 mL of methyl orange (MO) (10 mg/L) in the dark for 1 h to achieve adsorption equilibrium before irradiation. Visible-light (λ
>
40
0 nm) photocatalytic experiments were then conducted for 120 min. The remaining dye concentrations in the reaction solution were determined using the U3010 spectrophotometer. The entire decomposition process was conducted by sparging air at a flow rate of 10 mL/min.The existence ofOH
∙ can be tested by the terephthalic acid (C8H6O4, TA) fluorescent method. It has been demonstrated that OH
∙ can react with TA and generate luminescent TAOH according to the equation [16] OH
∙ + TA →TAOH.An 8 × 20 mm2 sheet of as-prepared photocatalyst was added to 4 mL of a solution containing 10 mM NaOH and 3 mM TA in a quartz reactor. Prior to photoreaction, the suspension was magnetically stirred in the dark for 1 h to ensure the establishment of an adsorption/desorption equilibrium. The photoreaction was carried out as the foregoing photocatalytic reaction under visible light without oxygen bubbled into the suspension. After 150 min of photoreaction, the fluorescence spectra of the resultant solution were measured on an Edinburgh F-900 fluorescence spectrophotometer using an excitation wavelength of 320 nm.


## 3. Results and Discussion

### 3.1. SEM and XRD Analysis of CdS/H-TNTs

Figure1 shows SEM images of the as-prepared samples. A top-view SEM image of pure TNTs is shown in Figure 1(a); it can be observed that the as-prepared samples are uniform and well-aligned nanotubes with an outer average diameter of 100 nm and a tube-wall thickness of approximately 15 nm. Figure 1(d) show a side-view of pure TNT layers, which indicates that the layer thickness is approximately 800 nm. Figures 1(b) and 1(e) show face- and side-view SEM images of the H-TNTs, respectively. The size and length of nanotubes were not significantly altered, which indicates that the hydrogen doped into the structures did not modify the morphology of the TNTs. However, many small particles on the face or inside of the nanotubes after CdS electrodeposition can be distinguished (shown in Figures 1(c) and 1(f)). The SEM images clearly show that CdS was successfully deposited onto the TiO2 nanotubes.Morphologies of as-obtained samples: top-view SEM images of (a) pure TNTs, (b) H-TNTs, and (c) CdS/H-TNTs; side-view SEM images (d) TNTs, (e) H-TNTs, and (f) CdS/H-TNTs.
(a)
(b)
(c)
(d)
(e)
(f)The XRD pattern of the as-prepared sample is shown in Figure2. It is clear that the nanotubes consist of pure anatase TiO2 (JPCDS No. 21-1272) [17], and the peaks of Ti are derived from the Ti substrate. The peaks of the H-TNTs are the same as those of pure TNTs. These results suggest that the hydrogen doped into the TNTs has no effect on the nanotubes’ crystal structure. Only the diffraction peaks of single-phase CdS and the TiO2 substrate, without the superfluous peaks of elemental Cd or S, were observed for the CdS/H-TNTs. The characteristic peaks of CdS are attributed to the cubic phase of CdS (JPCDS 80-0019) [12].Figure 2
XRD patterns of as-synthesized samples: (a) TNTs, (b) H-TNTs, and (c) CdS/H-TNTs.


### 3.2. EPR and DRS Analysis of CdS/H-TNTs

The EPR spectra corresponding to the pure TNTs and H-TNTs at 77 K are shown in Figure3; the species most likely responsible for these signals were assigned based only on reported g-tensor values. For pure TNTs, the values of g
1, g
2, and g
3 are 2.006, 2.005, and 2.004, respectively, indicating the presence of a single adsorption site for the anion on the TiO2 surface after thermal treatment. The g-values of H-TNTs can be observed to fall between 1.985 and 1.999, which is attributed to the Ti3+ species [18]. The results indicate a composite resonance arising from both the surface and bulk Ti3+ centers after hydrogen reduction treatment.Figure 3
EPR spectra of as-prepared samples: (a) TNTs and (b) CdS/H-TNTs.Figure4 presents the UV-visible diffuse reflectance spectra of the as-prepared samples. Compared with the spectra of the pure TNTs, the H-TNT spectra show strong visible-light absorption from 400 nm to 700 nm. However, there are two strong visible-light absorption peaks at 460 and 720 nm, and significantly enhanced visible-light absorption by the CdS/H-TNTs can be inferred. These results suggest that hydrogen doping and CdS deposition can affect the UV-visible absorption of the samples.Figure 4
UV-vis absorption spectra of as-obtained samples: (a) TNTs, (b) H-TNTs, and (c) CdS/H-TNTs.


### 3.3. Photocatalytic Activity

Figure5 shows the photocatalytic activity exhibited by the as-obtained samples toward the decomposition of the organic pollutant MO under visible-light irradiation. It is evident that the CdS/H-TNTs exhibited much higher efficiency than the H-TNTs and pure TNTs. In particular, the decolorizing rate of the CdS/H-TNTs (88.7%) was approximately 14 times that of the pure TNTs (6.4%) and 4 times that of the H-TNTs (20.1%) under visible-light irradiation.Figure 5
Photocatalytic activity of as-prepared samples: (a) TNTs, (b) H-TNTs, and (c) CdS/H-TNTs.The photocurrent responses of the as-prepared samples at a bias of 0 V versus Ag/AgCl are shown in Figure6. The CdS/H-TNTs exhibited superior performance with greater photocurrent generation efficiency compared to other samples. The photocurrent density of the CdS/H-TNTs (310 μA·cm−2) was 15 times that of the pure TNTs (20 μA·cm−2). The higher photocurrent indicates that more photoinduced electrons could be transferred efficiently from the CdS/H-TNTs to the counter electrode via the external circuit under visible-light illumination. The photocatalytic activity of the catalyst greatly depended on the charge transfer of electron-holes, which is in good agreement with the higher photocatalytic activity observed for the CdS/H-TNTs compared with that of the pure TNTs.Figure 6
Photocurrent response of as-synthesized samples: (a) TNTs, (b) H-TNTs, and (c) CdS/H-TNTs.It is well known that in the photooxidation reactions of organic molecules, the VB holes generated, or the main active species generated (such asOH
∙ radicals) from the reaction of holes with surface-adsorbed water or hydroxyl groups can be directly utilized [16]. To qualitatively distinguish the involvement of holes and/or OH
∙ radicals in the oxidation of MO, the prepared samples’ capabilities for generating OH
∙ radicals were compared by detecting the amount of 2-hydroxy terephthalic acid from the reaction of OH
∙ radicals with terephthalic acid [19]. The CdS/H-TNTs showed approximately 13 times higher efficiency compared with the pure TNTs under visible-light irradiation (shown in Figure 7). This result indicates that the excellent capability of the CdS/H-TNTs for decomposing MO is probably caused by the direct involvement of photogenerated holes and electrons under visible-light illumination.Figure 7
Fluorescence spectra recorded during visible-light illumination on samples in 10 mM NaOH and 3 mM terephthalic acid solution (excitation at 320 nm): (a) TNTs, (b) H-TNTs, and (c) CdS/H-TNTs.


### 3.4. Photocatalytic Mechanism

The high efficiency achieved by the prepared samples may be attributed to two major improvements. First, oxygen vacancies and Ti3+ species created by self-doping cause the band gap of TiO2 to narrow (shown in Figure 8). Second, the electrochemical deposition technique promotes the deposition of CdS onto the TiO2 nanotube walls, forming a heterojunction compact structure that allows for the rapid and efficient transfer of photogenerated electrons from CdS to the Ti substrate; this charge transfer compares favorably with that of traditional mesoporous film electrodes, leading to greatly reduced electron-hole recombination and much improved photocurrent and efficiency.Figure 8
Schematic illustration of charge transfer and separation in CdS and H-TNTs under visible-light irradiation.


## 3.1. SEM and XRD Analysis of CdS/H-TNTs

Figure1 shows SEM images of the as-prepared samples. A top-view SEM image of pure TNTs is shown in Figure 1(a); it can be observed that the as-prepared samples are uniform and well-aligned nanotubes with an outer average diameter of 100 nm and a tube-wall thickness of approximately 15 nm. Figure 1(d) show a side-view of pure TNT layers, which indicates that the layer thickness is approximately 800 nm. Figures 1(b) and 1(e) show face- and side-view SEM images of the H-TNTs, respectively. The size and length of nanotubes were not significantly altered, which indicates that the hydrogen doped into the structures did not modify the morphology of the TNTs. However, many small particles on the face or inside of the nanotubes after CdS electrodeposition can be distinguished (shown in Figures 1(c) and 1(f)). The SEM images clearly show that CdS was successfully deposited onto the TiO2 nanotubes.Morphologies of as-obtained samples: top-view SEM images of (a) pure TNTs, (b) H-TNTs, and (c) CdS/H-TNTs; side-view SEM images (d) TNTs, (e) H-TNTs, and (f) CdS/H-TNTs.
(a)
(b)
(c)
(d)
(e)
(f)The XRD pattern of the as-prepared sample is shown in Figure2. It is clear that the nanotubes consist of pure anatase TiO2 (JPCDS No. 21-1272) [17], and the peaks of Ti are derived from the Ti substrate. The peaks of the H-TNTs are the same as those of pure TNTs. These results suggest that the hydrogen doped into the TNTs has no effect on the nanotubes’ crystal structure. Only the diffraction peaks of single-phase CdS and the TiO2 substrate, without the superfluous peaks of elemental Cd or S, were observed for the CdS/H-TNTs. The characteristic peaks of CdS are attributed to the cubic phase of CdS (JPCDS 80-0019) [12].Figure 2
XRD patterns of as-synthesized samples: (a) TNTs, (b) H-TNTs, and (c) CdS/H-TNTs.


## 3.2. EPR and DRS Analysis of CdS/H-TNTs

The EPR spectra corresponding to the pure TNTs and H-TNTs at 77 K are shown in Figure3; the species most likely responsible for these signals were assigned based only on reported g-tensor values. For pure TNTs, the values of g
1, g
2, and g
3 are 2.006, 2.005, and 2.004, respectively, indicating the presence of a single adsorption site for the anion on the TiO2 surface after thermal treatment. The g-values of H-TNTs can be observed to fall between 1.985 and 1.999, which is attributed to the Ti3+ species [18]. The results indicate a composite resonance arising from both the surface and bulk Ti3+ centers after hydrogen reduction treatment.Figure 3
EPR spectra of as-prepared samples: (a) TNTs and (b) CdS/H-TNTs.Figure4 presents the UV-visible diffuse reflectance spectra of the as-prepared samples. Compared with the spectra of the pure TNTs, the H-TNT spectra show strong visible-light absorption from 400 nm to 700 nm. However, there are two strong visible-light absorption peaks at 460 and 720 nm, and significantly enhanced visible-light absorption by the CdS/H-TNTs can be inferred. These results suggest that hydrogen doping and CdS deposition can affect the UV-visible absorption of the samples.Figure 4
UV-vis absorption spectra of as-obtained samples: (a) TNTs, (b) H-TNTs, and (c) CdS/H-TNTs.


## 3.3. Photocatalytic Activity

Figure5 shows the photocatalytic activity exhibited by the as-obtained samples toward the decomposition of the organic pollutant MO under visible-light irradiation. It is evident that the CdS/H-TNTs exhibited much higher efficiency than the H-TNTs and pure TNTs. In particular, the decolorizing rate of the CdS/H-TNTs (88.7%) was approximately 14 times that of the pure TNTs (6.4%) and 4 times that of the H-TNTs (20.1%) under visible-light irradiation.Figure 5
Photocatalytic activity of as-prepared samples: (a) TNTs, (b) H-TNTs, and (c) CdS/H-TNTs.The photocurrent responses of the as-prepared samples at a bias of 0 V versus Ag/AgCl are shown in Figure6. The CdS/H-TNTs exhibited superior performance with greater photocurrent generation efficiency compared to other samples. The photocurrent density of the CdS/H-TNTs (310 μA·cm−2) was 15 times that of the pure TNTs (20 μA·cm−2). The higher photocurrent indicates that more photoinduced electrons could be transferred efficiently from the CdS/H-TNTs to the counter electrode via the external circuit under visible-light illumination. The photocatalytic activity of the catalyst greatly depended on the charge transfer of electron-holes, which is in good agreement with the higher photocatalytic activity observed for the CdS/H-TNTs compared with that of the pure TNTs.Figure 6
Photocurrent response of as-synthesized samples: (a) TNTs, (b) H-TNTs, and (c) CdS/H-TNTs.It is well known that in the photooxidation reactions of organic molecules, the VB holes generated, or the main active species generated (such asOH
∙ radicals) from the reaction of holes with surface-adsorbed water or hydroxyl groups can be directly utilized [16]. To qualitatively distinguish the involvement of holes and/or OH
∙ radicals in the oxidation of MO, the prepared samples’ capabilities for generating OH
∙ radicals were compared by detecting the amount of 2-hydroxy terephthalic acid from the reaction of OH
∙ radicals with terephthalic acid [19]. The CdS/H-TNTs showed approximately 13 times higher efficiency compared with the pure TNTs under visible-light irradiation (shown in Figure 7). This result indicates that the excellent capability of the CdS/H-TNTs for decomposing MO is probably caused by the direct involvement of photogenerated holes and electrons under visible-light illumination.Figure 7
Fluorescence spectra recorded during visible-light illumination on samples in 10 mM NaOH and 3 mM terephthalic acid solution (excitation at 320 nm): (a) TNTs, (b) H-TNTs, and (c) CdS/H-TNTs.


## 3.4. Photocatalytic Mechanism

The high efficiency achieved by the prepared samples may be attributed to two major improvements. First, oxygen vacancies and Ti3+ species created by self-doping cause the band gap of TiO2 to narrow (shown in Figure 8). Second, the electrochemical deposition technique promotes the deposition of CdS onto the TiO2 nanotube walls, forming a heterojunction compact structure that allows for the rapid and efficient transfer of photogenerated electrons from CdS to the Ti substrate; this charge transfer compares favorably with that of traditional mesoporous film electrodes, leading to greatly reduced electron-hole recombination and much improved photocurrent and efficiency.Figure 8
Schematic illustration of charge transfer and separation in CdS and H-TNTs under visible-light irradiation.


## 4. Conclusion

We have reported on the conceptual design and suitable architecture of a composite material formed from H-TNTs and the narrow-band-gap compound semiconductor CdS. The photocatalytic activity and photoelectrochemical performance of the CdS/H-TNTs were investigated. The CdS/H-TNTs exhibited higher photocatalytic activity and photoelectrochemical performance than pure TNTs under visible light. This novel heterostructure architecture provides a promising way to develop effective devices for light energy conversion and wastewater treatment.



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*Source: 678505-2014-05-14.xml*