# Photocatalytic Degradation ofNOx Using Ni-Containing TiO2

Authors: Yao-Hsuan Tseng; Bo-Kai Huang
Journal: International Journal of Photoenergy
 (2012)

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## Abstract

The nickel-containing titania was synthesized and employed in the photomineralization ofNOx. A nickel-modified titania photocatalyst was prepared by photodeposition method with using Degussa-P25 TiO2 particle and nickel chloride as raw materials, respectively. The physical analyses were carried out using X-ray photoelectron spectroscopy (XPS), X-ray diffraction (XRD), transmittance electron microscope (TEM), and photoluminescence spectroscopy (PL), to observe changes in particles following nickel modification. The results showed that Ni does not enter into the TiO2 crystal lattice and is dispersed onto the TiO2 surface uniformly. Ni improved the intensity of PL spectra with an appropriate Ni content on the TiO2 surface. The modified titanium dioxide with 0.1 mol% of nickel exhibited two times the NOx-removal activity of bare TiO2 under ultraviolet illumination. The nickel content in this photodeposition process plays an important role in affinity to NOx molecules, recombination rate of electron-hole pair, and content of active site on the TiO2 surface and therefore affects the optical and photocatalytic properties.


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## Body

## 1. Introduction

Since the discovery of the photoelectrochemical splitting of water using titanium dioxide electrodes [1–3], researchers have extensively studied semiconductor-based photocatalysis. Today, titanium dioxide is a representative photocatalyst material, due to its powerful redox properties and wide range of applications, such as air purification, water purification, deodorization, self-cleaning surfaces, antibacterial coating, and so forth [1, 4–7].The photocatalytic capacity of TiO2 powder heavily depends on its microstructure and physical properties, which are in turn determined by the preparation conditions [8–10]. Several attempts have been made to increase the photodegradation efficiency of TiO2, by either noble metal deposition or ion doping [11–14]. For example, Pt-doped, N-doped, C-doped, and S-doped TiO2 are applied as visible-light-responsive photocatalysts [1, 12–14], and cocatalysts and co-adsorbents, such as Ag, Au, activated carbon, and carbon nanotubes (CNTs) [10, 15–17], are used for the improvement of photocatalytic activity under UV illumination. However, in developing their widespread use for any practical application, the cost and stability of the material must be considered first. The anion and noble metal dopants do not have much practicability due to their insufficient stability, complicated preparation process, and expensive raw material. In contrast, transition metal cations have been found to be applied dopants and cocatalysts for the improvement of photocatalytic activity [18–24]. Some researchers report that the Ni2+ ion dopant improves the photocatalytic activity of certain semiconductor photocatalyst because the existence of Ni2+ suppresses recombination of electron-hole pair on the TiO2 surface [18–20]. However, the raw material and processes of these previous works, such as organic precursors, sol-gel, and ion-implantation methods [18–22], are not inexpensive enough for mass production. Herein, we present a facile and cost-effective method for the preparation of highly active nickel-containing TiO2 developed using TiO2 particle and nickel chloride.


## 2. Experimental Details

### 2.1. Preparation of Ni-TiO2 Particle

The nickel-containing, nanostructured TiO2 particles were prepared by the photoreduction process by using nickel chloride and Degussa P25 as a nickel precursor and a pristine photocatalyst, respectively. Ni-TiO2 was prepared by mixing 3 g of nonporous TiO2 (Degussa P25), 50 mL of ethanol, and certain amount of NiCl2·6H2O in 200 mL of double-distilled water. The solution was well mixed by ultrasonic treatment for 1 h. The initial pH value was adjusted to 8 with 0.1 M of NaOH solution [23]. A nitrogen stream at the rate of 30 mL/min was continuously introduced into the reaction chamber to remove oxygen in the solution. The solution was then irradiated with four UVC lamps (Philips TUV 10 W/G10 T8) with an intensity of 2 mW/cm2 for 3 h. Ni ions were reduced to nickel metallic nanoparticles by the photo-generated electrons of TiO2, then deposited on the surface of TiO2. The Ni-TiO2 particles were obtained by centrifugation at 10000 rpm, washing with DI water, and drying at 373 K for 12 h. Sample nomenclature was defined as follows: x% Ni/TiO2 photocatalyst prepared by the photodeposition process with nickel content x mol%. The Ni/TiO2 molar ratios were controlled at 0, 0.05, 0.1, 0.2, 0.5, 1, 2, and 4%.


### 2.2. Characterization

The photocatalyst crystal phase was identified using X-ray diffraction with Cu Kα (λ = 0.154 nm) radiation (Shimadzu Rigaku D/Max RCXRD 6000). Average particle size and morphology was obtained by transmission electron microscopy (TEM, Hitachi S600-100 KV). The photoluminescence spectroscopy (PL) data were obtained on a luminescence spectrometer (Jasco FP-6500LE) under excitation with 325 nm irradiation. Material compositions were determined by X-ray photoelectron spectroscopy (Perkin Elmer SSI-M probe XPS system and S4800) and energy dispersion spectroscopy (Horiba, EX-210).


### 2.3. Photocatalytic Activity

Figure1 depicted the continuous flow system used for NOx degradation over TiO2. A round-shaped Pyrex glass vessel (ϕ× H, 10 cm × 4 cm) was used as the photoreactor to conduct the degradation of NOx, and a sample dish (ϕ, 7 cm) was located inside the vessel containing the TiO2 powder. A black lamp provided a UV light source with an intensity of 1 mW/cm2 (Sankyo Denki FL 20SBLB, main peak located at 352 nm). The NOx degradation was carried out at room temperature using an air stream containing 1.0 ppm NO as feedstock. Two mass flow controllers (MFCs) (Brooks 5850E) manipulated relative humidity (RH = 50%) in the feeding stream. The reaction gas in the feeding stream passed through the vessel containing TiO2 powder (0.2 g) at a flow rate of 1 L/min. An on-line chemiluminescent NOx analyzer (Eco Physics, CLD 700 AL) continuously monitored NO and NO2 concentrations for gas analysis in the outlet.Figure 1
Schematic continuous flow reaction system for photocatalytic degradation of NO.


## 2.1. Preparation of Ni-TiO2 Particle

The nickel-containing, nanostructured TiO2 particles were prepared by the photoreduction process by using nickel chloride and Degussa P25 as a nickel precursor and a pristine photocatalyst, respectively. Ni-TiO2 was prepared by mixing 3 g of nonporous TiO2 (Degussa P25), 50 mL of ethanol, and certain amount of NiCl2·6H2O in 200 mL of double-distilled water. The solution was well mixed by ultrasonic treatment for 1 h. The initial pH value was adjusted to 8 with 0.1 M of NaOH solution [23]. A nitrogen stream at the rate of 30 mL/min was continuously introduced into the reaction chamber to remove oxygen in the solution. The solution was then irradiated with four UVC lamps (Philips TUV 10 W/G10 T8) with an intensity of 2 mW/cm2 for 3 h. Ni ions were reduced to nickel metallic nanoparticles by the photo-generated electrons of TiO2, then deposited on the surface of TiO2. The Ni-TiO2 particles were obtained by centrifugation at 10000 rpm, washing with DI water, and drying at 373 K for 12 h. Sample nomenclature was defined as follows: x% Ni/TiO2 photocatalyst prepared by the photodeposition process with nickel content x mol%. The Ni/TiO2 molar ratios were controlled at 0, 0.05, 0.1, 0.2, 0.5, 1, 2, and 4%.


## 2.2. Characterization

The photocatalyst crystal phase was identified using X-ray diffraction with Cu Kα (λ = 0.154 nm) radiation (Shimadzu Rigaku D/Max RCXRD 6000). Average particle size and morphology was obtained by transmission electron microscopy (TEM, Hitachi S600-100 KV). The photoluminescence spectroscopy (PL) data were obtained on a luminescence spectrometer (Jasco FP-6500LE) under excitation with 325 nm irradiation. Material compositions were determined by X-ray photoelectron spectroscopy (Perkin Elmer SSI-M probe XPS system and S4800) and energy dispersion spectroscopy (Horiba, EX-210).


## 2.3. Photocatalytic Activity

Figure1 depicted the continuous flow system used for NOx degradation over TiO2. A round-shaped Pyrex glass vessel (ϕ× H, 10 cm × 4 cm) was used as the photoreactor to conduct the degradation of NOx, and a sample dish (ϕ, 7 cm) was located inside the vessel containing the TiO2 powder. A black lamp provided a UV light source with an intensity of 1 mW/cm2 (Sankyo Denki FL 20SBLB, main peak located at 352 nm). The NOx degradation was carried out at room temperature using an air stream containing 1.0 ppm NO as feedstock. Two mass flow controllers (MFCs) (Brooks 5850E) manipulated relative humidity (RH = 50%) in the feeding stream. The reaction gas in the feeding stream passed through the vessel containing TiO2 powder (0.2 g) at a flow rate of 1 L/min. An on-line chemiluminescent NOx analyzer (Eco Physics, CLD 700 AL) continuously monitored NO and NO2 concentrations for gas analysis in the outlet.Figure 1
Schematic continuous flow reaction system for photocatalytic degradation of NO.


## 3. Results and Discussion

### 3.1. PhotocatalyticNOx Degradation over Ni-TiO2

Many researchers use NO oxidation to determine photocatalytic reactivity in various TiO2 photocatalytic applications [11–13, 15, 25]. The electron-hole pair (e−-h+) generated upon light excitation is trapped at the TiO2 surface as spatially separated redox-active sites. The general mechanism of NOx oxidation by photocatalyst is as follows. Hydrogen ions and hydroxide ions are dissociated from water. The active oxygen species are produced on the TiO2 surface. The nitric monoxide is oxidized to nitric acid or nitrous acid by active oxygen species. Based on the gas-phase chemistry of NOx [25, 26], NO is converted to HNO3 as a consecutive photooxidation via a NO2 intermediate:(1)O2+e-⟶O2-(2)OH-+h+⟶OH∙(3)H+O2-⟶HO2∙(4)NO+HO2∙⟶NO2+OH∙(5)NO2+OH∙⟶HNO3(6)NO+OH∙⟶HNO2.
Finally, the nitric acid forms on the catalyst. Photocatalyst activity will lessen as acid accumulates. To illustrate the reaction behavior of NO photocatalytic oxidation, 0.2 g of 0.1% Ni-TiO2 and 1 mW/cm2 of light intensity were used to conduct the experiment. At first, a 1 ppm NO gas stream was introduced into the photoreactor under dark conditions. As shown in the Figure 2, in the beginning, the NO concentration in the gas phase dropped rapidly without generation of NO2 due to NO adsorption on the TiO2. A few minutes later (2–4 min), the NO was saturated on the TiO2 and in the photoreactor, and the NO concentration was thus returned to 1 ppm. The UV lamps were turned on to start this photocatalytic reaction. The steady state of this photocatalytic reaction was achieved as soon as the photocatalyst was illuminated. The NO concentration decreased from 1 to 0.57 ppm, and the NO2 concentration increased to 0.1 ppm. The NOx concentration, which represents the accumulated mixture of NO and NO2, was maintained at 0.67 ppm under UV illumination. The activities of these TiO2 samples do not obviously decrease during 30 mins of operation, due to the short reaction time.Figure 2
Time-course of the changes in concentration of NO, NO2, and NOx in the presence of 0.1% Ni-TiO2 under UV light, reaction conditions as given in Table 1.Figure3 shows the NOx removal and NO2 generation rates obtained using various Ni-containing TiO2 particles under UV irradiation. The NOx removal activity for these samples with different Ni content decreased in the order: 0.1% Ni-TiO2 > 0.2% Ni-TiO2 > 0.05% Ni-TiO2 > 0.5% Ni-TiO2 > 1% Ni-TiO2 > P25 > 4% Ni-TiO2, indicating the optimal Ni content is 0.1 mol%. The 0.1% Ni-TiO2 has two times the NOx-removal activity of P25 particle. Under UV illumination, these Ni-containing photocatalysts exhibit better activities in NOx mineralization than pristine TiO2, except for 4% Ni-TiO2. The apparent quantum efficiency (Φ) and selectivity of NO2 (Sel.NO2) further computed based on the following equations [12, 13, 27] are listed in Table 1:(7)φ=moleof(NO+NO2)degradedEinsteinofincidentphotons(8)Sel.NO2=[NO2]generated[NO]converted.Table 1
The apparent quantum yields and selectivities of NO2 of various catalysts: catalyst loading: 0.2 g, intensity of irradiation: 1 mW/cm2, inlet concentration of NO, 1 ppm, inlet flow rate, 1 L/min, relative humidity: 55%, reaction temperature, 26°C.
CatalystP250.05% Ni0.1% Ni0.2% Ni0.5% Ni1% Ni4% NiΦ(%)2.132.632.852.582.071.801.30Sel.NO2 (%)62.830.724.429.536.948.556.0Figure 3
Effect of Ni content and regeneration time on the removal rate ofNOx.The order of apparent quantum efficiency (0.1% Ni-TiO2 > 0.05% Ni-TiO2 > 0.2% Ni-TiO2 > P25 > 0.5% Ni-TiO2 > 1% Ni-TiO2 > 4% Ni-TiO2) is not consistent with the NOx removal activity. It indicates that the nickel content over 0.5% is excess to reduce the active area of TiO2, resulting in the small quantum efficiency. When comparing the reaction behaviours over P25 and 0.05–0.2% Ni-TiO2 samples, no significant difference in the NO conversion was observed, and the NO2 generation rates over these Ni-TiO2 samples were much less than that over P25, resulting in the better photocatalytic activity of the Ni-TiO2. The selectivity of NO2 of the photocatalyst has a great effect on the NOx-removal activity, as shown in Table 1 and Figure 3. For example, the NOx removal activity of 1% Ni-TiO2 is better than P25 even if the quantum efficiency of P25 is larger than 1% Ni-TiO2. It might be the Ni particle has a good affinity to NO2. The platinum-modified TiO2 also has this property [16], and Ni is much cheaper than Pt. It is a worthy property for NO removal photocatalysis because NO2 is an undesired intermediate in the consecutive oxidation of NO, where the threshold concentrations of NO2 and NO are 3 and 25 ppm, respectively, [12].According to the reaction scheme of the photooxidation of NO, the photocatalyst would be deactivated after long-term operation due to the coverage of active sites by adsorbedNO3- ions at the catalyst surface. However, the adsorbed NO3- ions could be easily rinsed out with DI water, enabling regeneration of the catalyst. Figure 3 also indicates the removal rates of NOx over 1st-, 3rd-, and 5th-regenerated 0.1% Ni-TiO2 samples. The experimental results indicate the photocatalytic activity will be gradually decreased with the increase in operation and regeneration times. The photocatalytic activity of 0.1% Ni-TiO2 sample becomes stable after four reaction and regeneration cycles. It showed that over 93% of the photocatalytic activity could be recovered after multi-reaction-regeneration cycles. The reason for the slight decrease of photocatalytic activity is that the unstable nickel particles peel off from the TiO2 surface in the regeneration procedure. It can be confirmed by checking the nickel contents with using energy dispersive X-ray analysis after the regeneration procedure. It indicates most nickel particles on the TiO2 surface are quite stable. This means that the prepared Ni-TiO2 could provide very good stability for NOx degradation. As a result, good stability, easy regeneration, and high reactivity will provide a great opportunity for the application in air purification with using nickel-modified photocatalysts.


### 3.2. Characterization of Ni-TiO2

Figure4 illustrates the X-ray diffraction patterns of the samples before and after photodeposition treatment. The XRD pattern of the prepared TiO2 powder in Figure 4 reveals the peaks of anatase (101) and rutile (110) at 2θ = 25.4° and 27.5°, respectively, indicating that the bulk P25 TiO2 composition is a mixture of rutile and anatase. Since all samples were dried at the relatively low temperature of 373 K and only a small amount of Ni salt was added, there were no significant differences between the samples. No peaks corresponding to crystalline phase of Ni metal and NiO were found due to small crystallite size and low nickel content. According to Scherrer’s equation, by using the full width at half maximum height of the main peaks at 2θ = 25.4° and 27.5°, respectively, for anatase and rutile phases, the TiO2 anatase and rutile grain sizes of all prepared samples were around 21 and 15 nm. The results indicate that the addition of Ni salt produced insignificant changes in the primary TiO2 particle size.Figure 4
XRD patterns of prepared TiO2 samples.Figure5 shows the morphology of the Ni-deposited titanium oxide as captured by TEM. The deposited Ni particles measuring approximately 1–3 nm were dispersed on the surface of the P25. The pH value of the slurry influences the morphology of deposited metal particles on the TiO2 surface [28]. This study finds that the reduction rate increases as the pH value increases. However, Ni particles cannot adhere well on TiO2 when the pH value is higher than 10. The optimal pH value for the photodeposition of Ni in our study was found to be 8 [23]. The stability of Ni-TiO2 was confirmed by checking their TEM images after the photocatalytic reaction and regeneration procedure.TEM morphology of (a) P25 and (b) 1% Ni-TiO2.
(a)(b)Element composition and chemical states on the surface of prepared samples were determined by XPS high-resolution scans over the Ti 2p and Ni 2p spectra regions. Figure6(a) shows the Ni 2p spectra of Ni-TiO2 samples. For 0.1–1% Ni-TiO2 samples, their spectra exhibit broad peaks due to the small amount of Ni, and indicate the existence of Ni(II) and Ni(III) in these TiO2 particles. However, the plenty amount of Ni(0) is found on the surface of 4% Ni-TiO2 particle. In the preparation of Ni-TiO2 via the photodeposition process, the valence state of nickel on the TiO2 surface should be zero because nickel ions are reduced by the photo-produced electrons from the TiO2. The Ni 2p3/2 peaks of the samples assigned for Ni(0), Ni(II), and Ni(III) of binding energy are 852.9, 854.3, and 855.9 eV, respectively, [18–20, 23]. The compounds regarding Ni(II) and Ni(III) are major in the forms of NiO and Ni2O3 because the existence of Cl on the TiO2 surface is not observed. The metal oxides could be resulted from the oxidation of small nickel particles by heating in air [23, 29]. The Ni content of 4% Ni-TiO2 should be much more than those of other samples, and therefore partial nickel on the 4% Ni-TiO2 are not oxidized. The relatively atomic ratios of Ni(0), Ni(II), and Ni(III) species on the 4% Ni-TiO2 are 55 : 26 : 19, as estimated from XPS results. In Figure 6(b), Ti (2p3/2,1/2) core level spectra confirm that the Ti(IV) is indeed present in the pristine TiO2 sample. However, the Ti 2p3/2 peak becomes broad and asymmetric with increasing Ni content. We interpreted the Ti 2p3/2 peak for the Ni-TiO2 sample as a combination of the Ti(IV) (peak at 458.7 eV) and a Ti(III) (peak at 457.2 eV). The appearance of Ti(III) is probably due to the loss of oxygen atoms from TiO2 during the oxidation of metallic nickel particles. Moreover, following the Ar+ ion etching process of 4% Ni-TiO2, the peak intensities associated with the Ti(III) species decreased; after 90 s of etching (etching depth = 5 nm), the Ti(III) species could not be observed on the TiO2. This shows that the Ti(III) species exists predominantly on the surface, as shown in Figure 6(b). It indicates the partial Ti(IV) species on the surface is reduced to Ti(III) as the metallic nickel is oxidized to nickel oxide.(a) XPS spectra over Ni 2p (b) Ti 2p of prepared samples.
(a)(b)The photoluminescence emission spectra were detected for various photocatalysts, as presented in Figure7, to elucidate the fate of e–/h+ pairs in the semiconductor particles (TiO2). As anticipated, the pristine TiO2 photocatalyst (P25) shows a broad PL emission band, which is similar to the results of the literature [30]. The P25 and Ni-TiO2 samples exhibit similar excitonic PL emission band, demonstrating that the nickel species does not cause the new PL phenomena. The spectrum exhibits a broad emission region from 350 to 450 nm wavelengths with an excitation wavelength of 325 nm. The PL intensities of Ni-TiO2 particles lessen with the increase in the Ni content. A small amount of Ni gives a higher PL intensity of the Ni-TiO2 particle than P25, but the PL intensity of the Ni-TiO2 is smaller than that of pristine TiO2 as the Ni content is more than 1%. It indicates that Ni species in the higher concentration condition do not act as a trapping site to capture photogenerated electron from TiO2 conduction band, but it becomes the recombination centre of electron-hole as its concentration is less than 0.5%. The excitonic PL intensity of TiO2 decreases as the increase in particle size, which is ascribed to the decrease in the content of surface oxygen vacancy and defect with increasing particle size [11, 30]. In this work, the TiO2 size effect on PL intensity should be not significant here due to the small difference in crystallite size between these samples (see Figure 4). Therefore, the loss in PL intensities of 4% and 1% Ni-TiO2 results from the active sites on the TiO2 surface are covered by the Ni species. The metal particles on the TiO2 surface, such as Ag, Au, Pt, act as trapping sites to capture photogenerated electron from TiO2 conduction band, separating the photogenerated electron-hole pairs [14, 16]. The Ni species on the as-synthesized Ni-TiO2 particles seems to be the recombination sites of the photogenerated electron-hole pairs. It is probably as the metallic Ni and Ni ions could capture photogenerated holes and electrons, respectively. Thus, the recombination rate of photogenerated electrons and holes increased, leading to an increase in the PL signal. Some literatures report that the Ni dopant suppresses recombination of electron-hole pair on the TiO2 surface [18–20]. The different phenomena observed in the former reports and this work are reasonably due to the different preparation process and Ni content. The Ni content used in the former works is 2–10 mol%, so the PL intensity of TiO2 decreased obviously in the existence of large Ni content [18, 19]. For the above reasons, the results indicate the 0.1% Ni-TiO2 should exhibit the smallest photocatalytic activity. However, the 0.1% Ni-TiO2 exhibits the highest removal rate of NO under UV illumination than other samples. It reveals there should be another factors influencing its activity. The light absorbance is not the reason for good photoactivity of Ni-TiO2 because the UV-vis diffuse reflectance spectra of P25 and 0.1% Ni-TiO2 are the same (not shown here). Thus, the nickel species exhibits a good affinity to NO and NO2 molecules, so the photogenerated active oxygen species on TiO2 particles could contact NOx molecules rapidly, resulting in the enhancement of PL intensity and NOx removal rate on the 0.1% Ni-TiO2.Figure 7
Photoluminescence spectra of prepared TiO2 samples.


## 3.1. PhotocatalyticNOx Degradation over Ni-TiO2

Many researchers use NO oxidation to determine photocatalytic reactivity in various TiO2 photocatalytic applications [11–13, 15, 25]. The electron-hole pair (e−-h+) generated upon light excitation is trapped at the TiO2 surface as spatially separated redox-active sites. The general mechanism of NOx oxidation by photocatalyst is as follows. Hydrogen ions and hydroxide ions are dissociated from water. The active oxygen species are produced on the TiO2 surface. The nitric monoxide is oxidized to nitric acid or nitrous acid by active oxygen species. Based on the gas-phase chemistry of NOx [25, 26], NO is converted to HNO3 as a consecutive photooxidation via a NO2 intermediate:(1)O2+e-⟶O2-(2)OH-+h+⟶OH∙(3)H+O2-⟶HO2∙(4)NO+HO2∙⟶NO2+OH∙(5)NO2+OH∙⟶HNO3(6)NO+OH∙⟶HNO2.
Finally, the nitric acid forms on the catalyst. Photocatalyst activity will lessen as acid accumulates. To illustrate the reaction behavior of NO photocatalytic oxidation, 0.2 g of 0.1% Ni-TiO2 and 1 mW/cm2 of light intensity were used to conduct the experiment. At first, a 1 ppm NO gas stream was introduced into the photoreactor under dark conditions. As shown in the Figure 2, in the beginning, the NO concentration in the gas phase dropped rapidly without generation of NO2 due to NO adsorption on the TiO2. A few minutes later (2–4 min), the NO was saturated on the TiO2 and in the photoreactor, and the NO concentration was thus returned to 1 ppm. The UV lamps were turned on to start this photocatalytic reaction. The steady state of this photocatalytic reaction was achieved as soon as the photocatalyst was illuminated. The NO concentration decreased from 1 to 0.57 ppm, and the NO2 concentration increased to 0.1 ppm. The NOx concentration, which represents the accumulated mixture of NO and NO2, was maintained at 0.67 ppm under UV illumination. The activities of these TiO2 samples do not obviously decrease during 30 mins of operation, due to the short reaction time.Figure 2
Time-course of the changes in concentration of NO, NO2, and NOx in the presence of 0.1% Ni-TiO2 under UV light, reaction conditions as given in Table 1.Figure3 shows the NOx removal and NO2 generation rates obtained using various Ni-containing TiO2 particles under UV irradiation. The NOx removal activity for these samples with different Ni content decreased in the order: 0.1% Ni-TiO2 > 0.2% Ni-TiO2 > 0.05% Ni-TiO2 > 0.5% Ni-TiO2 > 1% Ni-TiO2 > P25 > 4% Ni-TiO2, indicating the optimal Ni content is 0.1 mol%. The 0.1% Ni-TiO2 has two times the NOx-removal activity of P25 particle. Under UV illumination, these Ni-containing photocatalysts exhibit better activities in NOx mineralization than pristine TiO2, except for 4% Ni-TiO2. The apparent quantum efficiency (Φ) and selectivity of NO2 (Sel.NO2) further computed based on the following equations [12, 13, 27] are listed in Table 1:(7)φ=moleof(NO+NO2)degradedEinsteinofincidentphotons(8)Sel.NO2=[NO2]generated[NO]converted.Table 1
The apparent quantum yields and selectivities of NO2 of various catalysts: catalyst loading: 0.2 g, intensity of irradiation: 1 mW/cm2, inlet concentration of NO, 1 ppm, inlet flow rate, 1 L/min, relative humidity: 55%, reaction temperature, 26°C.
CatalystP250.05% Ni0.1% Ni0.2% Ni0.5% Ni1% Ni4% NiΦ(%)2.132.632.852.582.071.801.30Sel.NO2 (%)62.830.724.429.536.948.556.0Figure 3
Effect of Ni content and regeneration time on the removal rate ofNOx.The order of apparent quantum efficiency (0.1% Ni-TiO2 > 0.05% Ni-TiO2 > 0.2% Ni-TiO2 > P25 > 0.5% Ni-TiO2 > 1% Ni-TiO2 > 4% Ni-TiO2) is not consistent with the NOx removal activity. It indicates that the nickel content over 0.5% is excess to reduce the active area of TiO2, resulting in the small quantum efficiency. When comparing the reaction behaviours over P25 and 0.05–0.2% Ni-TiO2 samples, no significant difference in the NO conversion was observed, and the NO2 generation rates over these Ni-TiO2 samples were much less than that over P25, resulting in the better photocatalytic activity of the Ni-TiO2. The selectivity of NO2 of the photocatalyst has a great effect on the NOx-removal activity, as shown in Table 1 and Figure 3. For example, the NOx removal activity of 1% Ni-TiO2 is better than P25 even if the quantum efficiency of P25 is larger than 1% Ni-TiO2. It might be the Ni particle has a good affinity to NO2. The platinum-modified TiO2 also has this property [16], and Ni is much cheaper than Pt. It is a worthy property for NO removal photocatalysis because NO2 is an undesired intermediate in the consecutive oxidation of NO, where the threshold concentrations of NO2 and NO are 3 and 25 ppm, respectively, [12].According to the reaction scheme of the photooxidation of NO, the photocatalyst would be deactivated after long-term operation due to the coverage of active sites by adsorbedNO3- ions at the catalyst surface. However, the adsorbed NO3- ions could be easily rinsed out with DI water, enabling regeneration of the catalyst. Figure 3 also indicates the removal rates of NOx over 1st-, 3rd-, and 5th-regenerated 0.1% Ni-TiO2 samples. The experimental results indicate the photocatalytic activity will be gradually decreased with the increase in operation and regeneration times. The photocatalytic activity of 0.1% Ni-TiO2 sample becomes stable after four reaction and regeneration cycles. It showed that over 93% of the photocatalytic activity could be recovered after multi-reaction-regeneration cycles. The reason for the slight decrease of photocatalytic activity is that the unstable nickel particles peel off from the TiO2 surface in the regeneration procedure. It can be confirmed by checking the nickel contents with using energy dispersive X-ray analysis after the regeneration procedure. It indicates most nickel particles on the TiO2 surface are quite stable. This means that the prepared Ni-TiO2 could provide very good stability for NOx degradation. As a result, good stability, easy regeneration, and high reactivity will provide a great opportunity for the application in air purification with using nickel-modified photocatalysts.


## 3.2. Characterization of Ni-TiO2

Figure4 illustrates the X-ray diffraction patterns of the samples before and after photodeposition treatment. The XRD pattern of the prepared TiO2 powder in Figure 4 reveals the peaks of anatase (101) and rutile (110) at 2θ = 25.4° and 27.5°, respectively, indicating that the bulk P25 TiO2 composition is a mixture of rutile and anatase. Since all samples were dried at the relatively low temperature of 373 K and only a small amount of Ni salt was added, there were no significant differences between the samples. No peaks corresponding to crystalline phase of Ni metal and NiO were found due to small crystallite size and low nickel content. According to Scherrer’s equation, by using the full width at half maximum height of the main peaks at 2θ = 25.4° and 27.5°, respectively, for anatase and rutile phases, the TiO2 anatase and rutile grain sizes of all prepared samples were around 21 and 15 nm. The results indicate that the addition of Ni salt produced insignificant changes in the primary TiO2 particle size.Figure 4
XRD patterns of prepared TiO2 samples.Figure5 shows the morphology of the Ni-deposited titanium oxide as captured by TEM. The deposited Ni particles measuring approximately 1–3 nm were dispersed on the surface of the P25. The pH value of the slurry influences the morphology of deposited metal particles on the TiO2 surface [28]. This study finds that the reduction rate increases as the pH value increases. However, Ni particles cannot adhere well on TiO2 when the pH value is higher than 10. The optimal pH value for the photodeposition of Ni in our study was found to be 8 [23]. The stability of Ni-TiO2 was confirmed by checking their TEM images after the photocatalytic reaction and regeneration procedure.TEM morphology of (a) P25 and (b) 1% Ni-TiO2.
(a)(b)Element composition and chemical states on the surface of prepared samples were determined by XPS high-resolution scans over the Ti 2p and Ni 2p spectra regions. Figure6(a) shows the Ni 2p spectra of Ni-TiO2 samples. For 0.1–1% Ni-TiO2 samples, their spectra exhibit broad peaks due to the small amount of Ni, and indicate the existence of Ni(II) and Ni(III) in these TiO2 particles. However, the plenty amount of Ni(0) is found on the surface of 4% Ni-TiO2 particle. In the preparation of Ni-TiO2 via the photodeposition process, the valence state of nickel on the TiO2 surface should be zero because nickel ions are reduced by the photo-produced electrons from the TiO2. The Ni 2p3/2 peaks of the samples assigned for Ni(0), Ni(II), and Ni(III) of binding energy are 852.9, 854.3, and 855.9 eV, respectively, [18–20, 23]. The compounds regarding Ni(II) and Ni(III) are major in the forms of NiO and Ni2O3 because the existence of Cl on the TiO2 surface is not observed. The metal oxides could be resulted from the oxidation of small nickel particles by heating in air [23, 29]. The Ni content of 4% Ni-TiO2 should be much more than those of other samples, and therefore partial nickel on the 4% Ni-TiO2 are not oxidized. The relatively atomic ratios of Ni(0), Ni(II), and Ni(III) species on the 4% Ni-TiO2 are 55 : 26 : 19, as estimated from XPS results. In Figure 6(b), Ti (2p3/2,1/2) core level spectra confirm that the Ti(IV) is indeed present in the pristine TiO2 sample. However, the Ti 2p3/2 peak becomes broad and asymmetric with increasing Ni content. We interpreted the Ti 2p3/2 peak for the Ni-TiO2 sample as a combination of the Ti(IV) (peak at 458.7 eV) and a Ti(III) (peak at 457.2 eV). The appearance of Ti(III) is probably due to the loss of oxygen atoms from TiO2 during the oxidation of metallic nickel particles. Moreover, following the Ar+ ion etching process of 4% Ni-TiO2, the peak intensities associated with the Ti(III) species decreased; after 90 s of etching (etching depth = 5 nm), the Ti(III) species could not be observed on the TiO2. This shows that the Ti(III) species exists predominantly on the surface, as shown in Figure 6(b). It indicates the partial Ti(IV) species on the surface is reduced to Ti(III) as the metallic nickel is oxidized to nickel oxide.(a) XPS spectra over Ni 2p (b) Ti 2p of prepared samples.
(a)(b)The photoluminescence emission spectra were detected for various photocatalysts, as presented in Figure7, to elucidate the fate of e–/h+ pairs in the semiconductor particles (TiO2). As anticipated, the pristine TiO2 photocatalyst (P25) shows a broad PL emission band, which is similar to the results of the literature [30]. The P25 and Ni-TiO2 samples exhibit similar excitonic PL emission band, demonstrating that the nickel species does not cause the new PL phenomena. The spectrum exhibits a broad emission region from 350 to 450 nm wavelengths with an excitation wavelength of 325 nm. The PL intensities of Ni-TiO2 particles lessen with the increase in the Ni content. A small amount of Ni gives a higher PL intensity of the Ni-TiO2 particle than P25, but the PL intensity of the Ni-TiO2 is smaller than that of pristine TiO2 as the Ni content is more than 1%. It indicates that Ni species in the higher concentration condition do not act as a trapping site to capture photogenerated electron from TiO2 conduction band, but it becomes the recombination centre of electron-hole as its concentration is less than 0.5%. The excitonic PL intensity of TiO2 decreases as the increase in particle size, which is ascribed to the decrease in the content of surface oxygen vacancy and defect with increasing particle size [11, 30]. In this work, the TiO2 size effect on PL intensity should be not significant here due to the small difference in crystallite size between these samples (see Figure 4). Therefore, the loss in PL intensities of 4% and 1% Ni-TiO2 results from the active sites on the TiO2 surface are covered by the Ni species. The metal particles on the TiO2 surface, such as Ag, Au, Pt, act as trapping sites to capture photogenerated electron from TiO2 conduction band, separating the photogenerated electron-hole pairs [14, 16]. The Ni species on the as-synthesized Ni-TiO2 particles seems to be the recombination sites of the photogenerated electron-hole pairs. It is probably as the metallic Ni and Ni ions could capture photogenerated holes and electrons, respectively. Thus, the recombination rate of photogenerated electrons and holes increased, leading to an increase in the PL signal. Some literatures report that the Ni dopant suppresses recombination of electron-hole pair on the TiO2 surface [18–20]. The different phenomena observed in the former reports and this work are reasonably due to the different preparation process and Ni content. The Ni content used in the former works is 2–10 mol%, so the PL intensity of TiO2 decreased obviously in the existence of large Ni content [18, 19]. For the above reasons, the results indicate the 0.1% Ni-TiO2 should exhibit the smallest photocatalytic activity. However, the 0.1% Ni-TiO2 exhibits the highest removal rate of NO under UV illumination than other samples. It reveals there should be another factors influencing its activity. The light absorbance is not the reason for good photoactivity of Ni-TiO2 because the UV-vis diffuse reflectance spectra of P25 and 0.1% Ni-TiO2 are the same (not shown here). Thus, the nickel species exhibits a good affinity to NO and NO2 molecules, so the photogenerated active oxygen species on TiO2 particles could contact NOx molecules rapidly, resulting in the enhancement of PL intensity and NOx removal rate on the 0.1% Ni-TiO2.Figure 7
Photoluminescence spectra of prepared TiO2 samples.


## 4. Conclusions

In this study, the Ni-containing TiO2 particle was successfully prepared via a photodeposition process. Characterization results revealed that the particle size, crystal structure, and light absorption were unchanged after modification with Ni salt. PL spectra identified that the small amount of Ni on TiO2 enhances the recombination of photogenerated electrons and holes. The nickel species exhibits a good affinity to NOx molecules, resulting in the increase in NOx removal rate and the decrease in selectivity of NO2 over the TiO2. The excess Ni content on TiO2 hinders reaction rate, due to coverage effect of nickel species on the active site on TiO2 surface. Thus, 0.1 mol% Ni content is the proper content to prepare the highly photocatalytic material for removal of NOx. In conclusion, this simple and energy-saving process for the production of Ni-containing photocatalysts can be applied practically for removal of NOx.



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*Source: 832180-2012-02-08.xml*