# Characterization and Catalytic Properties of Nano-Sized Au Metal Catalyst on Titanium Containing High Mesoporous Silica (Ti-HMS) Synthesized by Photo-Assisted Deposition and Impregnation Methods

Authors: R. M. Mohamed; Elham S. Aazam
Journal: International Journal of Photoenergy
 (2011)

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## Abstract

The photo-assisted deposition (PAD) and impregnation (img) synthesis of nano-sized Au metal on Ti-HMS are reported. The prepared catalysts were characterized by different techniques such as XRD, XAFS, TEM and nitrogen adsorption analysis. Photocatalytic reactivity using Au/Ti-HMS catalysts under visible-light condition on the oxidation of CO with O2 reaction was evaluated. The results have shown notable photocatalytic activity of PAD-Au/Ti-HMS which was 2.1 and 5.7 times higher than that of img-Au/Ti-HMS and Ti-HMS, respectively.


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## Body

## 1. Introduction

Titanium dioxide (TiO2) is one of the most intensively studied heterogeneous photocatalysis for the photodEgradation of toxic organic pollutants because it is nontoxic, relatively cheap, chemically stable within a wide pH range, and robust under UV light irradiation [1–7].Recently, the photodEgradation of some organic dyes using TiO2 under visible light irradiation has been reported. The studies were significant due to both fundamental and practical aspects exploiting unique mechanisms and perspectives rEgarding treatment of dye pollutants under sunlight. However, the application of TiO2 in photocatalytic reactions has been impeded as a result of the following obstacles. TiO2 photocatalysis can only absorb UV light due to their band structure, UV light component in sunlight is a relatively small part (ca. 3–5%) of the solar spectrum, and artificial UV light sources are expensive. Moreover, although fine TiO2 powders with large specific surface area exhibit high photocatalytic activity, an important issue rEgarding their recovery from aqueous suspensions has been taken into consideration [5–9].In the last few years, it has been pointed out that there is a strong interest in catalysis by gold due to the potential of highly dispersed gold on various supports to exhibit high catalytic activities for a number of reactions, including CO oxidation [10]; alcohol oxidation [11]; olefin epoxidation [12]; selective hydrogenation of unsaturated hydrocarbons, and so forth, In the past decade, supported gold particles have been applied to catalyze many different types of reactions. The literature reflects a consensus that the preparation method and choice of support significantly influence the size and activity of supported gold. Mesoporous silica, which possesses large pore size and high specific surface area, shows excellent performance for the conversion of bulky reactants and has been considered as notable support for gold loading.Various materials have been examined for supporting nano-gold. Of these, TiO2 is extremely active, and on this compound, nano-gold can catalyze CO oxidation at very low temperatures and can catalyze the preferential oxidation of CO in a hydrogen rich stream (PROX) at around room temperature [13]. However, it is well known that gold catalysts are sensitive to the preparation conditions, gold particle size, and the metal—support interaction. The gold particle size has a strong impact on the activity, because the reactivity of gold clusters depends largely on the type of uncoordinated sites exposed, ensemble effects and metal nanoparticles functionality, which can easily change during the reaction [14]. The influence of the catalyst’s preparation method, support type, pretreatment conditions, and Au particle size on the catalytic response of gold catalysts in CO oxidation was extensively reviewed by Bond and Bond and Thompson [15]. The gold-based catalysts also display variable catalytic activity, depending on the support [16]. This is because materials such as SiO2, Al2O3 or MgO are considered to be “inert” supports, which do not participate in the reaction mechanism, whereas transition metal oxides such as Fe2O3, CeO2 or TiO2 are “active” supports in reactions due to their high oxygen storage capacity and well known catalytic and redox properties. Indeed, most investigators agree that highly active gold catalysts can be supported on pure Fe2O3, CeO2 or TiO2 materials ([17] and references within). Unfortunately, those reducible oxides have low specific area. As a consequence, gold particles supported on pure Fe2O3, CeO2 or TiO2 are less stable than those supported on mixed oxide supports [18]. Thus, recently, attempts were conducted by supporting gold catalysts on high surface area (ca. 500–1000 m2 g−1) mesoporous silica materials such as MCM-48, HMS or SBA-15 [19–21]. In order to increase the oxygen mobility, those materials were modified with small amount of reducible metal oxide [22–24]. The chemical modification of mesoporous silica with transition metal oxides led to an increase of the activity of the total CO oxidation reaction, due to an enhancement of the catalyst thermal stability and minimization of Au particle sintering [25]. The positive effect of dispersing TiO2 over silica on the stability of Au particles was ascribed in the literature to the inhibition, by development of Si-O-Ti linkages, of the anatase formation upon calcination [26, 27]. Similar to the CO oxidation [22–24], the Au/Ti-SBA-15 systems showed an activity enhancement in the CO-PROX reaction compared to the Ti-free Au/SBA-15 [21].In the present study, we loaded gold onto Ti-HMS by two methods and applied the product Au/Ti-HMS as a photocatlyst to oxidize CO under visible light irradiation.


## 2. Experimental Section

### 2.1. Materials

Tetraethylorthosilicate (TEOS), dodecylamine (DDA), titanium isopropoxide, isopropyl alcohol (IPA) were purchased from Acros Organics Co.


### 2.2. Synthesis of Ti-HMS

Ti-HMS was synthesized as follows: The first solution (A) was prepared by slowly adding HCl to a mixture of DDA (3 g) and water (30 g) while stirring. The second solution (B) was prepared by adding TEOS (11.8 g) to a mixture of Titanium Isopropoxide (1 g) and IPA (18 g) while stirring. This was followed by adding solution (A) to solution (B) and the resulting solution was stirred for further 20 h, the resultant product was filtered. Finally calcination was carried out at 550°C for 5 h.


### 2.3. Catalyst Preparation

PAD-Au/Ti-HMS (1 wt% of Au metal) was synthesized using the photo-assisted deposition (PAD) route as follows: Au metal was deposited on Ti-HMS with aqueous solution of HAuCl4 under UV-light irradiation.Img-Au/Ti-HMS was synthesized by incipient wetness imprEgnation route, Au was loaded onto Ti-HMS with an aqueous solution of HAuCl4 (1 wt% of Au metal). The sample was dried at 378 K then followed by H2-reduction (20 mL min−1) at 673°C for 2 h.


### 2.4. Characterization Techniques

#### 2.4.1. X-Ray Diffraction (XRD)

To identify the crystallographic phases, the powders were characterized by X-ray diffraction (XRD) (Rigaku RINT, 2000, CuKα radiation, λ=0.15406 nm).


#### 2.4.2. UV-Vis Diffuse Reflectance Spectra (DRS UV-Vis)

Diffuse reflectance ultraviolet-visible absorption spectra (DRS UV-vis) were collected in the UV-vis range (200–800 nm) with BaSO4 as reference on a Shimadzu UV-2450 spectrophotometer at 295 K.


#### 2.4.3. EXAFS

The extended X-ray absorption fine structure (EXAFS) spectra were measured at the BL-7C facility of the Photon Factory at the National Laboratory for High-Energy Physics, Tsukuba. An Si (111) double crystal was used to monochromatize the X-rays from the 2.5 GeV electron storage ring. The Ni K-edge absorption spectrum was recorded in the fluorescence mode at 298 K. The normalized spectra were obtained by a known literature procedure [28], and Fourier transforms were performed on k3-weighted EXAFS oscillations in the range of 3–10 Å−1. The morphologies and particle sizes of the prepared samples were examined with a transmission electron microscope (Hitachi H-9500 operated at 300 kv).


#### 2.4.4. N2-Adsorption-Desorption Isotherms

The textural properties of the samples were evaluated from the adsorption-desorption isotherms of nitrogen at −196°C detected using a Nova2000 series apparatus (Chromatech). The specific surface areas of the materials were calculated using the BET method within a 0.005–0.30 range of relative pressure(P/P0). Prior to detection, the samples were dEgassed under vacuum at 270°C for 5 h.


### 2.5. Reactor Setup and PCO Experimental Procedure

The photocatalytic oxidations of carbon monoxide (PCO) experiments were carried out using a closed-circulation reactor at ambient temperature and pressure. A stainless steel cell (volume, 21 cm3) with a quartz window (diameter, 3 cm) for UV or visible transmission was connected to a magnetically driven circulation pump through an external Teflon-tubing. The total volume of the circulation reactor was 100 cm3. The gas circulation flow rate was about 100 cm3 min−1 and the residence time in the stainless steel reactor was 13 s per cycle. Gases used were CO (500 ppmv in Ar) and CO (500 ppmv in air) as a CO standard, dry air (99.9995%) and Ar (99.9999%) as a carrier gas. Each gas stream was dried by passing through a silica-gel moisture trap.PCO experiments were carried out with two different initial concentrations of CO; (30 and 500 ppmv). CO concentrations were adjusted by diluting the standard CO gas with the carrier gas using mass flow controllers. The reactor cell was placed in a wooden box that housed a 150-W mercury lamp. The sample was then irradiated with visible light, which was generated by a 150 W high-pressure mercury lamp and an appropriate cut off filter was placed in front of the reactor to remove part of UV radiation.The removal of CO and the production of CO2 were monitored using a gas chromatograph; Shimadzu GCMS-QP 5050A; and a gas-sampling valve. The removal efficiency of CO was calculated by applying the following equation:(1)%Removal efficiency=C°-CC°×100,
where C° is the original CO content and C is the retained CO.


## 2.1. Materials

Tetraethylorthosilicate (TEOS), dodecylamine (DDA), titanium isopropoxide, isopropyl alcohol (IPA) were purchased from Acros Organics Co.


## 2.2. Synthesis of Ti-HMS

Ti-HMS was synthesized as follows: The first solution (A) was prepared by slowly adding HCl to a mixture of DDA (3 g) and water (30 g) while stirring. The second solution (B) was prepared by adding TEOS (11.8 g) to a mixture of Titanium Isopropoxide (1 g) and IPA (18 g) while stirring. This was followed by adding solution (A) to solution (B) and the resulting solution was stirred for further 20 h, the resultant product was filtered. Finally calcination was carried out at 550°C for 5 h.


## 2.3. Catalyst Preparation

PAD-Au/Ti-HMS (1 wt% of Au metal) was synthesized using the photo-assisted deposition (PAD) route as follows: Au metal was deposited on Ti-HMS with aqueous solution of HAuCl4 under UV-light irradiation.Img-Au/Ti-HMS was synthesized by incipient wetness imprEgnation route, Au was loaded onto Ti-HMS with an aqueous solution of HAuCl4 (1 wt% of Au metal). The sample was dried at 378 K then followed by H2-reduction (20 mL min−1) at 673°C for 2 h.


## 2.4. Characterization Techniques

### 2.4.1. X-Ray Diffraction (XRD)

To identify the crystallographic phases, the powders were characterized by X-ray diffraction (XRD) (Rigaku RINT, 2000, CuKα radiation, λ=0.15406 nm).


### 2.4.2. UV-Vis Diffuse Reflectance Spectra (DRS UV-Vis)

Diffuse reflectance ultraviolet-visible absorption spectra (DRS UV-vis) were collected in the UV-vis range (200–800 nm) with BaSO4 as reference on a Shimadzu UV-2450 spectrophotometer at 295 K.


### 2.4.3. EXAFS

The extended X-ray absorption fine structure (EXAFS) spectra were measured at the BL-7C facility of the Photon Factory at the National Laboratory for High-Energy Physics, Tsukuba. An Si (111) double crystal was used to monochromatize the X-rays from the 2.5 GeV electron storage ring. The Ni K-edge absorption spectrum was recorded in the fluorescence mode at 298 K. The normalized spectra were obtained by a known literature procedure [28], and Fourier transforms were performed on k3-weighted EXAFS oscillations in the range of 3–10 Å−1. The morphologies and particle sizes of the prepared samples were examined with a transmission electron microscope (Hitachi H-9500 operated at 300 kv).


### 2.4.4. N2-Adsorption-Desorption Isotherms

The textural properties of the samples were evaluated from the adsorption-desorption isotherms of nitrogen at −196°C detected using a Nova2000 series apparatus (Chromatech). The specific surface areas of the materials were calculated using the BET method within a 0.005–0.30 range of relative pressure(P/P0). Prior to detection, the samples were dEgassed under vacuum at 270°C for 5 h.


## 2.4.1. X-Ray Diffraction (XRD)

To identify the crystallographic phases, the powders were characterized by X-ray diffraction (XRD) (Rigaku RINT, 2000, CuKα radiation, λ=0.15406 nm).


## 2.4.2. UV-Vis Diffuse Reflectance Spectra (DRS UV-Vis)

Diffuse reflectance ultraviolet-visible absorption spectra (DRS UV-vis) were collected in the UV-vis range (200–800 nm) with BaSO4 as reference on a Shimadzu UV-2450 spectrophotometer at 295 K.


## 2.4.3. EXAFS

The extended X-ray absorption fine structure (EXAFS) spectra were measured at the BL-7C facility of the Photon Factory at the National Laboratory for High-Energy Physics, Tsukuba. An Si (111) double crystal was used to monochromatize the X-rays from the 2.5 GeV electron storage ring. The Ni K-edge absorption spectrum was recorded in the fluorescence mode at 298 K. The normalized spectra were obtained by a known literature procedure [28], and Fourier transforms were performed on k3-weighted EXAFS oscillations in the range of 3–10 Å−1. The morphologies and particle sizes of the prepared samples were examined with a transmission electron microscope (Hitachi H-9500 operated at 300 kv).


## 2.4.4. N2-Adsorption-Desorption Isotherms

The textural properties of the samples were evaluated from the adsorption-desorption isotherms of nitrogen at −196°C detected using a Nova2000 series apparatus (Chromatech). The specific surface areas of the materials were calculated using the BET method within a 0.005–0.30 range of relative pressure(P/P0). Prior to detection, the samples were dEgassed under vacuum at 270°C for 5 h.


## 2.5. Reactor Setup and PCO Experimental Procedure

The photocatalytic oxidations of carbon monoxide (PCO) experiments were carried out using a closed-circulation reactor at ambient temperature and pressure. A stainless steel cell (volume, 21 cm3) with a quartz window (diameter, 3 cm) for UV or visible transmission was connected to a magnetically driven circulation pump through an external Teflon-tubing. The total volume of the circulation reactor was 100 cm3. The gas circulation flow rate was about 100 cm3 min−1 and the residence time in the stainless steel reactor was 13 s per cycle. Gases used were CO (500 ppmv in Ar) and CO (500 ppmv in air) as a CO standard, dry air (99.9995%) and Ar (99.9999%) as a carrier gas. Each gas stream was dried by passing through a silica-gel moisture trap.PCO experiments were carried out with two different initial concentrations of CO; (30 and 500 ppmv). CO concentrations were adjusted by diluting the standard CO gas with the carrier gas using mass flow controllers. The reactor cell was placed in a wooden box that housed a 150-W mercury lamp. The sample was then irradiated with visible light, which was generated by a 150 W high-pressure mercury lamp and an appropriate cut off filter was placed in front of the reactor to remove part of UV radiation.The removal of CO and the production of CO2 were monitored using a gas chromatograph; Shimadzu GCMS-QP 5050A; and a gas-sampling valve. The removal efficiency of CO was calculated by applying the following equation:(1)%Removal efficiency=C°-CC°×100,
where C° is the original CO content and C is the retained CO.


## 3. Results and Discussion

### 3.1. Characterization of the Fresh Catalysts

#### 3.1.1. X-Ray Diffraction

The hexagonal arrangements of mesoporous silica (HMS) in all synthesized catalysts were confirmed by the low-angle XRD patterns as shown in Figure1. The absence of diffraction peaks of either crystalline TiO2 or AuO are indicative of the retention of the mesoporous structure after the application of either photo-assisted deposition (PAD) or imprEgnation (img) method. Also, no diffraction peaks of Au in the patterns of Au-doped samples were observed. This is probably attributed to the low Au doping content (ca.1%). and may imply that Au particles are well dispersed within the Ti-HMS phase.Figure 1
XRD patterns of Ti-HMS (A), PAD-Au/Ti-HMS (B) and img-Au/Ti-HMS (C).


#### 3.1.2. Textural Properties

For all the catalysts, the surface parameters of surface area and the data calculated from thet-plot are compiled in Table 1. The N2 adsorption isotherms (not shown here) for the parent and the Au/Ti-HMS are typical of mesoporous solids (type IV), however, an increase in the adsorption capacity of the Ti-HMS was observed after introducing Au ions. From this table the SBET values follow the following order (parent Ti-HMS < img-Au/Ti-HMS < PAD-Au/Ti-HMS). Furthermore, the total pore volume of Au/Ti-HMS is higher than that of Ti-HMS.  The values of SBET and St are generally close in most samples indicating the presence of mesopores. The values of Smic are low compared to that of Smes implying that the main surface is mesoporous solid as represented by the isotherm. The surface texture data are correlated with the catalytic activity as will be mentioned later on.Table 1
Texture parameters of Ti-HM, img-Au/Ti-HMS and PAD-Au/Ti-HMS.
SampleSBET (m2/g)St (m2/g)Smeso (cm2/g)Smicro (cm2/g)Sext (cm2/g)Vp (cm3/g)Vmicro (cm3/g)Vmeso (cm3/g)r(Å)Ti-HMS6026104082004900.4000.0400.35421.59img-Au/Ti-HMS6436503002105200.4260.0520.36820.48PAD-Au/Ti-HMS7537503802126400.4810.0490.43618.38Note: (SBET) BET-surface area, (St) surface area derived from V1-t plots, (Smic) surface area of micropores, (Smes) surface area of mesopores, (Sext) external surface area, (Vp) total pore volume, (Vmic) pore volume of micropores, (Vmes) pore volume of mesopores, (r) mean pore radius.


#### 3.1.3. UV-Vis Spectroscopy

To gain insight into the effect of Ti/HMS doping with Au, UV-vis diffuse reflectance spectra were recorded at room temperature in the range of 200–900 nm (Figure2).  The Kubelka-Munk function, F(R), can be considered to be proportional to the absorption of radiation [29]. On this basis, the value of Eg, the band gap of the semiconductor, can be derived from the spectra by plotting (F(R)·hν)1/2 against hν as shown in Figure 3 [30]. The Eg values calculated for Ti-HMS, PAD-Au/Ti-HMS and img-Au/Ti-HMS are summarized in Table 2. The band-gap values usually reported for pure anatase and rutile phases are 3.2 and 3.03 eV, respectively [28]. However, these values are influenced by the method of synthesis, the existence of impurities doping the crystalline network and also the average crystal size of the semiconductor.Table 2
The calculated band gap energy of Ti-HMS, img-Au/Ti-HMS and PAD-Au/Ti-HMS.
SampleBaud gap energy (eV)Ti-HMS3.2img-Au/Ti-HMS3.0PAD-Au/Ti-HMS2.7Figure 2
Diffuse reflectance UV-vis absorption spectra of Ti-HMS (A), PAD-Au/Ti-HMS (B) and img-Au/Ti-HMS (C).Figure 3
Band-gap calculated from the DR-UV-vis spectra Ti-HMS, img-Au/Ti-HMS and PAD-Au/Ti-HMS.In a previous study, different methods for calculatingEg values from the UV-vis reflectance spectra were used. For example, some authors calculated the Eg values by a direct extrapolation of the F(R)spectrum whereas others reported the wavelength corresponding to the maximum absorption [31]. As a consequence, quite different Eg values for rutile and anatase samples are found in the literature. For instance, for anatase-based materials, the threshold wavelength values of 370 nm [32], 380 nm [33], 387 nm [34], 393 nm [35] and 403 nm [36] corresponding to a band gap range from 3.08 to 3.35 eV have been reported. In the case of rutile-based materials, an absorption wavelength as high as 437.4 nm (Eg=2.84eV) has been reported [36].In the present study, the band gap values calculated for Ti-HMS, img-Au/Ti-HMS and PAD-Au/Ti-HMS are 3.2, 3.0 and 2.7 eV respectively. These data clearly indicate that the study of UV-vis absorption constitutes an important tool for evaluating the changes produced in semiconductor materials by different preparation methods.


#### 3.1.4. EXAFS Measurements

The Fourier transforms of Pt LIII-edge EXAFS spectra of the Au-loaded catalysts are displayed in Figure4. The presence of the peak at 2.92 Å assigned to the Au-Au bond of Au metal, indicates the formation of nano-sized Au metal [37].Figure 4
Fourier transforms of the Pt LIII-edge EXAFS spectra for (A) img-Au/Ti-HMS              and (B) PAD-Au/Ti-HMS.The intensity of the Au-Au peak of the PAD-Au/Ti-HMS catalyst is smaller than the img-Au/Ti-HMS catalyst. This relationship clearly suggests that the size of the Au metal particles depends on the preparation method and show smaller particle size formed on the photo-deposited catalyst (PAD-Au/Ti-HMS) than on the img-Au/Ti-HMS catalyst.


#### 3.1.5. TEM Analysis

The TEM images of PAD-Au/Ti-HMS and img-Au/Ti-HMS catalysts are displayed in Figure5, and the particle distribution obtained from analysis of the TEM images is shown in Figure 6. These data are in strong agreement with the results obtained from EXAFS measurements. Nano-sized Au metal particles having a narrow size distribution (3–6 nm) were found on the PAD-Au/Ti-HMS catalyst, whereas aggrEgated Au metal particles of larger sizes (6–12 nm) were observed on img- Au/Ti-HMS catalyst. These data provide further evidence that the size of the Au metal particles depends on the preparation method.The TEM images of the PAD-Au/Ti-HMS (a) and img-Au/Ti-HMS (b) catalyst after H2 treatment at 473 K.
(a)(b)Size distribution diagrams of Au metal obtained from the TEM images of PAD-Au/Ti-HMS (a) and img-Au/Ti-HMS (b) catalyst after H2 treatment at 473 K.
(a)(b)


### 3.2. Catalyst Testing towards CO Photocatalytic Conversion

The photocatalytic conversion of CO is used as a probe reaction to test the catalytic activity of the prepared nanoparticles. The effect of Ti-HMS, img-Au/Ti-HMS and PAD-Au/Ti-HMS on photocatalytic oxidation of CO at room temperature after 1 h are shown in Figure7. The data demonstrate that the photocatalytic activities of the PAD-Au/Ti-HMS (97.8%) are higher than that of img-Au/Ti-HMS (47.9%) and the parent Ti-HMS (17.1%). Considering that, the pure Au oxides don not have photocatalytic oxidation properties, such variation in activity must be due to the differences in interaction between Au and Ti-HMS that led to several modifications in the physical properties such as band gap, particle size and surface texture.  Also, we can observe that, the catalytic activity of Ti-HMS generally increased with the addition of Au promoters. A maximum activity was obtained in the case of PAD-Au/Ti-HMS. The correlation between the photoactivity and the physical properties such as band gap, surface area and pore volume is depicted in Figure 8. It is clear that, the photocatalytic activity was at a maximum in the case of PAD-Au/Ti-HMS in which the surface area and pore volume were maximum but band gap was minimum.Figure 7
Photocatalytic conversion of CO (%) for Ti-HMS (a), img-Au/Ti-HMS (b) and PAD-Au/Ti-HMS (c).Figure 8
Effect of physical parameters of the materials on their photocatalytic activity for PAD-Au/Ti-HMS (A), img-Au/Ti-HMS (B) and Ti-HMS (C).In addition, Figure8 shows the good correlation between the band gap, surface area and pore volume with the catalytic activity where the activity is gradually increasing with the decrease of band gap and the increase of the surface area and pore volume.It is believed that the lack of electron scavengers (surface Ti4+) and hole traps (surface hydroxyl groups) is responsible for the rapid recombination rate of e-/h+, which leads to lower photocatalytic activity. The results show that the photocatalytic activities of the Au/Ti-HMS nanoparticles increased with decreasing the band gap. This is due to the low energy to exit electron from valance band to conduction band. Also, the PAD- Au/Ti-HMS has the best photoactivity, since it has the lowest band gap and particle size and the highest surface area and pore volume.


## 3.1. Characterization of the Fresh Catalysts

### 3.1.1. X-Ray Diffraction

The hexagonal arrangements of mesoporous silica (HMS) in all synthesized catalysts were confirmed by the low-angle XRD patterns as shown in Figure1. The absence of diffraction peaks of either crystalline TiO2 or AuO are indicative of the retention of the mesoporous structure after the application of either photo-assisted deposition (PAD) or imprEgnation (img) method. Also, no diffraction peaks of Au in the patterns of Au-doped samples were observed. This is probably attributed to the low Au doping content (ca.1%). and may imply that Au particles are well dispersed within the Ti-HMS phase.Figure 1
XRD patterns of Ti-HMS (A), PAD-Au/Ti-HMS (B) and img-Au/Ti-HMS (C).


### 3.1.2. Textural Properties

For all the catalysts, the surface parameters of surface area and the data calculated from thet-plot are compiled in Table 1. The N2 adsorption isotherms (not shown here) for the parent and the Au/Ti-HMS are typical of mesoporous solids (type IV), however, an increase in the adsorption capacity of the Ti-HMS was observed after introducing Au ions. From this table the SBET values follow the following order (parent Ti-HMS < img-Au/Ti-HMS < PAD-Au/Ti-HMS). Furthermore, the total pore volume of Au/Ti-HMS is higher than that of Ti-HMS.  The values of SBET and St are generally close in most samples indicating the presence of mesopores. The values of Smic are low compared to that of Smes implying that the main surface is mesoporous solid as represented by the isotherm. The surface texture data are correlated with the catalytic activity as will be mentioned later on.Table 1
Texture parameters of Ti-HM, img-Au/Ti-HMS and PAD-Au/Ti-HMS.
SampleSBET (m2/g)St (m2/g)Smeso (cm2/g)Smicro (cm2/g)Sext (cm2/g)Vp (cm3/g)Vmicro (cm3/g)Vmeso (cm3/g)r(Å)Ti-HMS6026104082004900.4000.0400.35421.59img-Au/Ti-HMS6436503002105200.4260.0520.36820.48PAD-Au/Ti-HMS7537503802126400.4810.0490.43618.38Note: (SBET) BET-surface area, (St) surface area derived from V1-t plots, (Smic) surface area of micropores, (Smes) surface area of mesopores, (Sext) external surface area, (Vp) total pore volume, (Vmic) pore volume of micropores, (Vmes) pore volume of mesopores, (r) mean pore radius.


### 3.1.3. UV-Vis Spectroscopy

To gain insight into the effect of Ti/HMS doping with Au, UV-vis diffuse reflectance spectra were recorded at room temperature in the range of 200–900 nm (Figure2).  The Kubelka-Munk function, F(R), can be considered to be proportional to the absorption of radiation [29]. On this basis, the value of Eg, the band gap of the semiconductor, can be derived from the spectra by plotting (F(R)·hν)1/2 against hν as shown in Figure 3 [30]. The Eg values calculated for Ti-HMS, PAD-Au/Ti-HMS and img-Au/Ti-HMS are summarized in Table 2. The band-gap values usually reported for pure anatase and rutile phases are 3.2 and 3.03 eV, respectively [28]. However, these values are influenced by the method of synthesis, the existence of impurities doping the crystalline network and also the average crystal size of the semiconductor.Table 2
The calculated band gap energy of Ti-HMS, img-Au/Ti-HMS and PAD-Au/Ti-HMS.
SampleBaud gap energy (eV)Ti-HMS3.2img-Au/Ti-HMS3.0PAD-Au/Ti-HMS2.7Figure 2
Diffuse reflectance UV-vis absorption spectra of Ti-HMS (A), PAD-Au/Ti-HMS (B) and img-Au/Ti-HMS (C).Figure 3
Band-gap calculated from the DR-UV-vis spectra Ti-HMS, img-Au/Ti-HMS and PAD-Au/Ti-HMS.In a previous study, different methods for calculatingEg values from the UV-vis reflectance spectra were used. For example, some authors calculated the Eg values by a direct extrapolation of the F(R)spectrum whereas others reported the wavelength corresponding to the maximum absorption [31]. As a consequence, quite different Eg values for rutile and anatase samples are found in the literature. For instance, for anatase-based materials, the threshold wavelength values of 370 nm [32], 380 nm [33], 387 nm [34], 393 nm [35] and 403 nm [36] corresponding to a band gap range from 3.08 to 3.35 eV have been reported. In the case of rutile-based materials, an absorption wavelength as high as 437.4 nm (Eg=2.84eV) has been reported [36].In the present study, the band gap values calculated for Ti-HMS, img-Au/Ti-HMS and PAD-Au/Ti-HMS are 3.2, 3.0 and 2.7 eV respectively. These data clearly indicate that the study of UV-vis absorption constitutes an important tool for evaluating the changes produced in semiconductor materials by different preparation methods.


### 3.1.4. EXAFS Measurements

The Fourier transforms of Pt LIII-edge EXAFS spectra of the Au-loaded catalysts are displayed in Figure4. The presence of the peak at 2.92 Å assigned to the Au-Au bond of Au metal, indicates the formation of nano-sized Au metal [37].Figure 4
Fourier transforms of the Pt LIII-edge EXAFS spectra for (A) img-Au/Ti-HMS              and (B) PAD-Au/Ti-HMS.The intensity of the Au-Au peak of the PAD-Au/Ti-HMS catalyst is smaller than the img-Au/Ti-HMS catalyst. This relationship clearly suggests that the size of the Au metal particles depends on the preparation method and show smaller particle size formed on the photo-deposited catalyst (PAD-Au/Ti-HMS) than on the img-Au/Ti-HMS catalyst.


### 3.1.5. TEM Analysis

The TEM images of PAD-Au/Ti-HMS and img-Au/Ti-HMS catalysts are displayed in Figure5, and the particle distribution obtained from analysis of the TEM images is shown in Figure 6. These data are in strong agreement with the results obtained from EXAFS measurements. Nano-sized Au metal particles having a narrow size distribution (3–6 nm) were found on the PAD-Au/Ti-HMS catalyst, whereas aggrEgated Au metal particles of larger sizes (6–12 nm) were observed on img- Au/Ti-HMS catalyst. These data provide further evidence that the size of the Au metal particles depends on the preparation method.The TEM images of the PAD-Au/Ti-HMS (a) and img-Au/Ti-HMS (b) catalyst after H2 treatment at 473 K.
(a)(b)Size distribution diagrams of Au metal obtained from the TEM images of PAD-Au/Ti-HMS (a) and img-Au/Ti-HMS (b) catalyst after H2 treatment at 473 K.
(a)(b)


## 3.1.1. X-Ray Diffraction

The hexagonal arrangements of mesoporous silica (HMS) in all synthesized catalysts were confirmed by the low-angle XRD patterns as shown in Figure1. The absence of diffraction peaks of either crystalline TiO2 or AuO are indicative of the retention of the mesoporous structure after the application of either photo-assisted deposition (PAD) or imprEgnation (img) method. Also, no diffraction peaks of Au in the patterns of Au-doped samples were observed. This is probably attributed to the low Au doping content (ca.1%). and may imply that Au particles are well dispersed within the Ti-HMS phase.Figure 1
XRD patterns of Ti-HMS (A), PAD-Au/Ti-HMS (B) and img-Au/Ti-HMS (C).


## 3.1.2. Textural Properties

For all the catalysts, the surface parameters of surface area and the data calculated from thet-plot are compiled in Table 1. The N2 adsorption isotherms (not shown here) for the parent and the Au/Ti-HMS are typical of mesoporous solids (type IV), however, an increase in the adsorption capacity of the Ti-HMS was observed after introducing Au ions. From this table the SBET values follow the following order (parent Ti-HMS < img-Au/Ti-HMS < PAD-Au/Ti-HMS). Furthermore, the total pore volume of Au/Ti-HMS is higher than that of Ti-HMS.  The values of SBET and St are generally close in most samples indicating the presence of mesopores. The values of Smic are low compared to that of Smes implying that the main surface is mesoporous solid as represented by the isotherm. The surface texture data are correlated with the catalytic activity as will be mentioned later on.Table 1
Texture parameters of Ti-HM, img-Au/Ti-HMS and PAD-Au/Ti-HMS.
SampleSBET (m2/g)St (m2/g)Smeso (cm2/g)Smicro (cm2/g)Sext (cm2/g)Vp (cm3/g)Vmicro (cm3/g)Vmeso (cm3/g)r(Å)Ti-HMS6026104082004900.4000.0400.35421.59img-Au/Ti-HMS6436503002105200.4260.0520.36820.48PAD-Au/Ti-HMS7537503802126400.4810.0490.43618.38Note: (SBET) BET-surface area, (St) surface area derived from V1-t plots, (Smic) surface area of micropores, (Smes) surface area of mesopores, (Sext) external surface area, (Vp) total pore volume, (Vmic) pore volume of micropores, (Vmes) pore volume of mesopores, (r) mean pore radius.


## 3.1.3. UV-Vis Spectroscopy

To gain insight into the effect of Ti/HMS doping with Au, UV-vis diffuse reflectance spectra were recorded at room temperature in the range of 200–900 nm (Figure2).  The Kubelka-Munk function, F(R), can be considered to be proportional to the absorption of radiation [29]. On this basis, the value of Eg, the band gap of the semiconductor, can be derived from the spectra by plotting (F(R)·hν)1/2 against hν as shown in Figure 3 [30]. The Eg values calculated for Ti-HMS, PAD-Au/Ti-HMS and img-Au/Ti-HMS are summarized in Table 2. The band-gap values usually reported for pure anatase and rutile phases are 3.2 and 3.03 eV, respectively [28]. However, these values are influenced by the method of synthesis, the existence of impurities doping the crystalline network and also the average crystal size of the semiconductor.Table 2
The calculated band gap energy of Ti-HMS, img-Au/Ti-HMS and PAD-Au/Ti-HMS.
SampleBaud gap energy (eV)Ti-HMS3.2img-Au/Ti-HMS3.0PAD-Au/Ti-HMS2.7Figure 2
Diffuse reflectance UV-vis absorption spectra of Ti-HMS (A), PAD-Au/Ti-HMS (B) and img-Au/Ti-HMS (C).Figure 3
Band-gap calculated from the DR-UV-vis spectra Ti-HMS, img-Au/Ti-HMS and PAD-Au/Ti-HMS.In a previous study, different methods for calculatingEg values from the UV-vis reflectance spectra were used. For example, some authors calculated the Eg values by a direct extrapolation of the F(R)spectrum whereas others reported the wavelength corresponding to the maximum absorption [31]. As a consequence, quite different Eg values for rutile and anatase samples are found in the literature. For instance, for anatase-based materials, the threshold wavelength values of 370 nm [32], 380 nm [33], 387 nm [34], 393 nm [35] and 403 nm [36] corresponding to a band gap range from 3.08 to 3.35 eV have been reported. In the case of rutile-based materials, an absorption wavelength as high as 437.4 nm (Eg=2.84eV) has been reported [36].In the present study, the band gap values calculated for Ti-HMS, img-Au/Ti-HMS and PAD-Au/Ti-HMS are 3.2, 3.0 and 2.7 eV respectively. These data clearly indicate that the study of UV-vis absorption constitutes an important tool for evaluating the changes produced in semiconductor materials by different preparation methods.


## 3.1.4. EXAFS Measurements

The Fourier transforms of Pt LIII-edge EXAFS spectra of the Au-loaded catalysts are displayed in Figure4. The presence of the peak at 2.92 Å assigned to the Au-Au bond of Au metal, indicates the formation of nano-sized Au metal [37].Figure 4
Fourier transforms of the Pt LIII-edge EXAFS spectra for (A) img-Au/Ti-HMS              and (B) PAD-Au/Ti-HMS.The intensity of the Au-Au peak of the PAD-Au/Ti-HMS catalyst is smaller than the img-Au/Ti-HMS catalyst. This relationship clearly suggests that the size of the Au metal particles depends on the preparation method and show smaller particle size formed on the photo-deposited catalyst (PAD-Au/Ti-HMS) than on the img-Au/Ti-HMS catalyst.


## 3.1.5. TEM Analysis

The TEM images of PAD-Au/Ti-HMS and img-Au/Ti-HMS catalysts are displayed in Figure5, and the particle distribution obtained from analysis of the TEM images is shown in Figure 6. These data are in strong agreement with the results obtained from EXAFS measurements. Nano-sized Au metal particles having a narrow size distribution (3–6 nm) were found on the PAD-Au/Ti-HMS catalyst, whereas aggrEgated Au metal particles of larger sizes (6–12 nm) were observed on img- Au/Ti-HMS catalyst. These data provide further evidence that the size of the Au metal particles depends on the preparation method.The TEM images of the PAD-Au/Ti-HMS (a) and img-Au/Ti-HMS (b) catalyst after H2 treatment at 473 K.
(a)(b)Size distribution diagrams of Au metal obtained from the TEM images of PAD-Au/Ti-HMS (a) and img-Au/Ti-HMS (b) catalyst after H2 treatment at 473 K.
(a)(b)


## 3.2. Catalyst Testing towards CO Photocatalytic Conversion

The photocatalytic conversion of CO is used as a probe reaction to test the catalytic activity of the prepared nanoparticles. The effect of Ti-HMS, img-Au/Ti-HMS and PAD-Au/Ti-HMS on photocatalytic oxidation of CO at room temperature after 1 h are shown in Figure7. The data demonstrate that the photocatalytic activities of the PAD-Au/Ti-HMS (97.8%) are higher than that of img-Au/Ti-HMS (47.9%) and the parent Ti-HMS (17.1%). Considering that, the pure Au oxides don not have photocatalytic oxidation properties, such variation in activity must be due to the differences in interaction between Au and Ti-HMS that led to several modifications in the physical properties such as band gap, particle size and surface texture.  Also, we can observe that, the catalytic activity of Ti-HMS generally increased with the addition of Au promoters. A maximum activity was obtained in the case of PAD-Au/Ti-HMS. The correlation between the photoactivity and the physical properties such as band gap, surface area and pore volume is depicted in Figure 8. It is clear that, the photocatalytic activity was at a maximum in the case of PAD-Au/Ti-HMS in which the surface area and pore volume were maximum but band gap was minimum.Figure 7
Photocatalytic conversion of CO (%) for Ti-HMS (a), img-Au/Ti-HMS (b) and PAD-Au/Ti-HMS (c).Figure 8
Effect of physical parameters of the materials on their photocatalytic activity for PAD-Au/Ti-HMS (A), img-Au/Ti-HMS (B) and Ti-HMS (C).In addition, Figure8 shows the good correlation between the band gap, surface area and pore volume with the catalytic activity where the activity is gradually increasing with the decrease of band gap and the increase of the surface area and pore volume.It is believed that the lack of electron scavengers (surface Ti4+) and hole traps (surface hydroxyl groups) is responsible for the rapid recombination rate of e-/h+, which leads to lower photocatalytic activity. The results show that the photocatalytic activities of the Au/Ti-HMS nanoparticles increased with decreasing the band gap. This is due to the low energy to exit electron from valance band to conduction band. Also, the PAD- Au/Ti-HMS has the best photoactivity, since it has the lowest band gap and particle size and the highest surface area and pore volume.


## 4. Conclusions

It can be concluded that the nano-sized particles of Au/Ti-HMS can be prepared via two methods:  photo-assisted deposition (PAD) and the conventional imprEgnation method (img). The characterization of such prepared catalysts by N2 adsorption, XRD, UV-vis and EXAFS techniques reveals the following remarks. (1)
The nano-sized Au  metal with  a mean diameter(d) of ca. 4 nm having a narrow size distribution was found on the PAD-Au/Ti-HMS catalyst, whereas the aggrEgated Au metal with various sizes are observed on img-Au/Ti-HMS catalyst (d~10nm).(2)
The calculated values of band gap for Ti-HMS, img-Au/Ti-HMS and PAD-Au/Ti-HMS are 3.2, 2.9 and 2.7 eV respectively.(3)
The N2 adsorption isotherms for the parent and the Au/Ti-HMS are typical of mesoporous solids, the surface area changed from 602 to 643 and 753 m2/g in case of img-Au/Ti-HMS and PAD-Au/Ti-HMS respectively.(4)
The intensity of the Au-Au peak of the PAD-Au/Ti-HMS catalyst is smaller than the img-Au/Ti-HMS catalyst. These findings suggest that the size of Au metal particles depends on the preparation method. Au metal particles formed on the photo-deposited catalyst (PAD-Au/Ti-HMS) show smaller particle sizes than those obtained from the imprEgnated catalyst (img-Au/Ti-HMS).



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*Source: 137328-2011-07-26.xml*