# Synthesis, Characterization, and Investigation of Visible Light Photocatalytic Activity of C Doped TiO2/CdS Core-Shell Nanocomposite

Authors: Atul B. Lavand; Yuvraj S. Malghe; Suraj H. Singh
Journal: Indian Journal of Materials Science
 (2015)

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## Abstract

Carbon (C) doped TiO2/CdS core-shell nanocomposite (C/TiO2/CdS) was synthesized using microemulsion method. Synthesized powder was characterized using X-ray diffraction (XRD), Fourier transform infrared spectroscopy (FTIR), energy dispersive X-ray spectroscopy (EDX), transmission electron microscopy (TEM), and UV-visible spectrophotometery. TEM images reveal that C/TiO2/CdS core-shell heterostructure is successfully prepared with CdS as a core and C doped TiO2 as a shell. UV-visible absorption spectra show that CdS nanoparticles act as a sensitizer and effectively enhance the photoabsorption capacity of C/TiO2/CdS nanocomposite in visible region. Visible light photocatalytic activity of synthesized nanocomposite was evaluated for the degradation of methylene blue. C/TiO2/CdS core-shell nanocomposite exhibits better photocatalytic activity as compared to bare TiO2, CdS, CdS/TiO2, and C doped TiO2.


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## Body

## 1.Introduction

Photocatalysis can be used as an abundant and clean energy source for different purposes like environmental remediation, clean energy production, and so forth [1–3]. Recent day’s lot of research is going on, to develop novel photocatalyst and improve its efficiency in visible/solar light [4–6]. In photocatalysis, light of energy greater than the semiconductor band gap which excites electron from valence band to conduction band is required. Among various photocatalysts reported TiO2 has attracted special attention due to its unique physical and chemical properties such as strong oxidizing and reducing ability, good permeability, better optical properties, chemical stability, low cost, and corrosion resistance [7–9]. Among the various forms of TiO2, anatase TiO2 exhibits better photocatalytic activity [10]. It has the band gap 3.2 eV and requires UV light (
λ
≤
387
nm
) to activate. Solar spectrum consists of 5% UV and ~45 to 50% visible light. To utilize visible light portion it is necessary to modify TiO2. One of the ways to modify TiO2 is to couple it with semiconductor with narrow band gap. CdS with band gap 2.4 eV is considered as one of the ideal sensitizers due to unique position of its conduction and valence band edges [11–14]. Unfortunately CdS/TiO2 composite suffers from major disadvantage that is quick recombination of photogenerated charge carriers which decreases the photocatalytic performance. To compensate this problem it is necessary to modify this composite by doping it with metals or nonmetals. Few reports are available in literature [13, 15, 16] regarding the preparation of hybrid materials in which Pt or C nanotubes are incorporated. These materials act as an excellent electron acceptor/transporter centre and effectively facilitate the migration of photoinduced electrons and suppress the charge combination in electron-transfer process due to electronic interaction between them and CdS/TiO2 composite. This effectively increases the photocatalytic activity. Carbonaceous materials are very popular in photocatalysis due to their wide range visible light absorption capacity and better adsorption power of organic pollutants [17, 18]. In such hybrid materials strong synergetic effect can be achieved. Therefore, in a present work we have synthesized C doped TiO2/CdS nanocomposite using microemulsion method and its visible light photocatalytic activity was investigated for the degradation of methylene blue dye.


## 2.Materials and Methods

### 2.1. Materials

Methylene blue (MB) practical grade was obtained from Hi Media Laboratories, Mumbai, and used without any further purification. Titanium isopropoxide Ti(iOPr)4 was purchased from Sigma Aldrich, Mumbai, and used as a source of titanium. All these chemicals, cyclohexane, n-butanol, N,N,N-cetyl trimethyl ammonium bromide (CTAB), acetone, cadmium nitrate (Cd(NO3)2·4H2O), sodium sulphide flakes (Na2S), sodium hydroxide (NaOH), and ethanol (99.7%), used for synthesis are of AR grade and are procured from SD Fine Chemicals, Mumbai, India, and are used without further purification.


### 2.2. Synthesis of Photocatalyst

#### 2.2.1. Synthesis of CdS Nanoparticles

50 mL 1 M cadmium nitrate, 25 mL double distilled water, 25 mL ethanol, and 0.01 M CTAB were mixed in a beaker and stirred for 30 min continuously. 50 mL 1 M Na2S, 25 mL ethanol, and 25 mL double distilled water were added to the above solution and stirred for 30 min. To this mixture 20 mL 2 M NaOH was added dropwise with continuous stirring. It gives light yellow precipitate. Mixture thus formed was transferred to autoclave (with Teflon-inner-liner) and kept in an oven at 100°C for 2 h. Later it was cooled to the room temperature and the residue obtained was separated using centrifugation, washed several times with distilled water followed by ethanol and finally with acetone, and dried at 40°C to get pure CdS.


#### 2.2.2. Synthesis of Pure and C Doped TiO2 Nanoparticles

Pure and C doped TiO2 nanoparticles were prepared using microemulsion method reported in our previous work [19]. 60 mL cyclohexane, 15 mL n-butanol, and 6 g CTAB were mixed together and mixture was stirred for 15 min. To this microemulsion solution containing 3 mL water and 9 mL 1 M titanium isopropoxide was added dropwise with constant stirring. This mixture was transferred to autoclave (with Teflon-inner-liner) and kept in an oven at 150°C for 2 h. Later it was cooled to the room temperature and the residue obtained was separated by centrifugation, washed several times with distilled water followed by ethanol and finally with acetone, and dried at 40°C. The product obtained was used as a precursor. This precursor was calcined in furnace at 300 and 500°C to get C doped and pure TiO2, respectively.


#### 2.2.3. Synthesis of C Doped TiO2/CdS Core-Shell Nanocomposite (C/TiO2/CdS)

80 mL cyclohexane, 20 mL butanol, 4.0 g CTAB, and 6 mL 1 M cadmium nitrate were mixed in a beaker and stirred for 30 min. To this microemulsion 6 mL 1 M Na2S was added and mixture was stirred for 30 min. Afterwards, 6 mL 1 M titanium isopropoxide was added dropwise with constant stirring. This mixture was transferred to autoclave (with Teflon-inner-liner) and kept in an oven at 150°C for 2 h. Later it was cooled to the room temperature and the residue obtained was separated using centrifugation, washed several times with distilled water followed by ethanol and finally with acetone, and dried at 40°C. Dried powder was calcined at 300 and 500°C for 2 h to get C doped and pure TiO2/CdS nanocomposite.


### 2.3. Characterizations

X-ray diffraction (XRD) patterns of all the calcined powders were recorded using Rigaku, (Model-Miniflex II) X-ray diffractometer with Cu Kα radiation (λ
=
0.15418
nm) at a scan rate 2° min−1. Average particle sizes were calculated using Debye-Scherrer equation t
=
n
λ
/
B
cos
⁡
θ
⁡, where t is average particle size, n
=
0.9, and B is full width of line at half of the maximum intensity (FWHM). FTIR spectra of samples were recorded with FTIR spectrophotometer (Bruker). Qualitative elemental analysis of the calcined powders was carried out using energy dispersive X-ray spectroscopy (EDX) using JEOL-JSM instruments. Particle size of the compounds prepared in this work was studied using transmission electron microscope (TEM) (FEI, USA, Model-Technai-G2). UV-visible spectrophotometer (Shimadzu, Model-1800) was used to study the band gap energy of synthesized nanopowders.


### 2.4. Photocatalytic Activity Study

Visible light photocatalytic activities of synthesized catalysts were evaluated for the degradation of methylene blue (MB) using 65 W compact fluorescent lamp (λ
>
420 nm, Philips, Mumbai). Photodegradation was carried out using a homemade photo reactor with water jacket to maintain temperature through experiment. Distance between the light and the reaction vessel is fixed at 10 cm. 0.05 g photocatalyst powder was dispersed in 50 mL 10 ppm MB solution. Prior to photocatalytic measurements, the aqueous suspension was stirred in the dark for 30 min to attain adsorption-desorption equilibrium. After reaction suspension was irradiated with visible light. At specific time intervals, 5 mL aliquot was taken out, catalyst was separated using centrifugation, and concentration of MB in the supernatant solution was estimated from UV-visible spectra recorded in the wavelength range 200–800 nm.


## 2.1. Materials

Methylene blue (MB) practical grade was obtained from Hi Media Laboratories, Mumbai, and used without any further purification. Titanium isopropoxide Ti(iOPr)4 was purchased from Sigma Aldrich, Mumbai, and used as a source of titanium. All these chemicals, cyclohexane, n-butanol, N,N,N-cetyl trimethyl ammonium bromide (CTAB), acetone, cadmium nitrate (Cd(NO3)2·4H2O), sodium sulphide flakes (Na2S), sodium hydroxide (NaOH), and ethanol (99.7%), used for synthesis are of AR grade and are procured from SD Fine Chemicals, Mumbai, India, and are used without further purification.


## 2.2. Synthesis of Photocatalyst

### 2.2.1. Synthesis of CdS Nanoparticles

50 mL 1 M cadmium nitrate, 25 mL double distilled water, 25 mL ethanol, and 0.01 M CTAB were mixed in a beaker and stirred for 30 min continuously. 50 mL 1 M Na2S, 25 mL ethanol, and 25 mL double distilled water were added to the above solution and stirred for 30 min. To this mixture 20 mL 2 M NaOH was added dropwise with continuous stirring. It gives light yellow precipitate. Mixture thus formed was transferred to autoclave (with Teflon-inner-liner) and kept in an oven at 100°C for 2 h. Later it was cooled to the room temperature and the residue obtained was separated using centrifugation, washed several times with distilled water followed by ethanol and finally with acetone, and dried at 40°C to get pure CdS.


### 2.2.2. Synthesis of Pure and C Doped TiO2 Nanoparticles

Pure and C doped TiO2 nanoparticles were prepared using microemulsion method reported in our previous work [19]. 60 mL cyclohexane, 15 mL n-butanol, and 6 g CTAB were mixed together and mixture was stirred for 15 min. To this microemulsion solution containing 3 mL water and 9 mL 1 M titanium isopropoxide was added dropwise with constant stirring. This mixture was transferred to autoclave (with Teflon-inner-liner) and kept in an oven at 150°C for 2 h. Later it was cooled to the room temperature and the residue obtained was separated by centrifugation, washed several times with distilled water followed by ethanol and finally with acetone, and dried at 40°C. The product obtained was used as a precursor. This precursor was calcined in furnace at 300 and 500°C to get C doped and pure TiO2, respectively.


### 2.2.3. Synthesis of C Doped TiO2/CdS Core-Shell Nanocomposite (C/TiO2/CdS)

80 mL cyclohexane, 20 mL butanol, 4.0 g CTAB, and 6 mL 1 M cadmium nitrate were mixed in a beaker and stirred for 30 min. To this microemulsion 6 mL 1 M Na2S was added and mixture was stirred for 30 min. Afterwards, 6 mL 1 M titanium isopropoxide was added dropwise with constant stirring. This mixture was transferred to autoclave (with Teflon-inner-liner) and kept in an oven at 150°C for 2 h. Later it was cooled to the room temperature and the residue obtained was separated using centrifugation, washed several times with distilled water followed by ethanol and finally with acetone, and dried at 40°C. Dried powder was calcined at 300 and 500°C for 2 h to get C doped and pure TiO2/CdS nanocomposite.


## 2.2.1. Synthesis of CdS Nanoparticles

50 mL 1 M cadmium nitrate, 25 mL double distilled water, 25 mL ethanol, and 0.01 M CTAB were mixed in a beaker and stirred for 30 min continuously. 50 mL 1 M Na2S, 25 mL ethanol, and 25 mL double distilled water were added to the above solution and stirred for 30 min. To this mixture 20 mL 2 M NaOH was added dropwise with continuous stirring. It gives light yellow precipitate. Mixture thus formed was transferred to autoclave (with Teflon-inner-liner) and kept in an oven at 100°C for 2 h. Later it was cooled to the room temperature and the residue obtained was separated using centrifugation, washed several times with distilled water followed by ethanol and finally with acetone, and dried at 40°C to get pure CdS.


## 2.2.2. Synthesis of Pure and C Doped TiO2 Nanoparticles

Pure and C doped TiO2 nanoparticles were prepared using microemulsion method reported in our previous work [19]. 60 mL cyclohexane, 15 mL n-butanol, and 6 g CTAB were mixed together and mixture was stirred for 15 min. To this microemulsion solution containing 3 mL water and 9 mL 1 M titanium isopropoxide was added dropwise with constant stirring. This mixture was transferred to autoclave (with Teflon-inner-liner) and kept in an oven at 150°C for 2 h. Later it was cooled to the room temperature and the residue obtained was separated by centrifugation, washed several times with distilled water followed by ethanol and finally with acetone, and dried at 40°C. The product obtained was used as a precursor. This precursor was calcined in furnace at 300 and 500°C to get C doped and pure TiO2, respectively.


## 2.2.3. Synthesis of C Doped TiO2/CdS Core-Shell Nanocomposite (C/TiO2/CdS)

80 mL cyclohexane, 20 mL butanol, 4.0 g CTAB, and 6 mL 1 M cadmium nitrate were mixed in a beaker and stirred for 30 min. To this microemulsion 6 mL 1 M Na2S was added and mixture was stirred for 30 min. Afterwards, 6 mL 1 M titanium isopropoxide was added dropwise with constant stirring. This mixture was transferred to autoclave (with Teflon-inner-liner) and kept in an oven at 150°C for 2 h. Later it was cooled to the room temperature and the residue obtained was separated using centrifugation, washed several times with distilled water followed by ethanol and finally with acetone, and dried at 40°C. Dried powder was calcined at 300 and 500°C for 2 h to get C doped and pure TiO2/CdS nanocomposite.


## 2.3. Characterizations

X-ray diffraction (XRD) patterns of all the calcined powders were recorded using Rigaku, (Model-Miniflex II) X-ray diffractometer with Cu Kα radiation (λ
=
0.15418
nm) at a scan rate 2° min−1. Average particle sizes were calculated using Debye-Scherrer equation t
=
n
λ
/
B
cos
⁡
θ
⁡, where t is average particle size, n
=
0.9, and B is full width of line at half of the maximum intensity (FWHM). FTIR spectra of samples were recorded with FTIR spectrophotometer (Bruker). Qualitative elemental analysis of the calcined powders was carried out using energy dispersive X-ray spectroscopy (EDX) using JEOL-JSM instruments. Particle size of the compounds prepared in this work was studied using transmission electron microscope (TEM) (FEI, USA, Model-Technai-G2). UV-visible spectrophotometer (Shimadzu, Model-1800) was used to study the band gap energy of synthesized nanopowders.


## 2.4. Photocatalytic Activity Study

Visible light photocatalytic activities of synthesized catalysts were evaluated for the degradation of methylene blue (MB) using 65 W compact fluorescent lamp (λ
>
420 nm, Philips, Mumbai). Photodegradation was carried out using a homemade photo reactor with water jacket to maintain temperature through experiment. Distance between the light and the reaction vessel is fixed at 10 cm. 0.05 g photocatalyst powder was dispersed in 50 mL 10 ppm MB solution. Prior to photocatalytic measurements, the aqueous suspension was stirred in the dark for 30 min to attain adsorption-desorption equilibrium. After reaction suspension was irradiated with visible light. At specific time intervals, 5 mL aliquot was taken out, catalyst was separated using centrifugation, and concentration of MB in the supernatant solution was estimated from UV-visible spectra recorded in the wavelength range 200–800 nm.


## 3.Results and Discussion

### 3.1. X-Ray Diffraction (XRD) Study

XRD patterns of C doped TiO2, CdS, and C doped TiO2/CdS core-shell nanoparticles were recorded and are presented in Figure 1. XRD pattern of CdS shows peaks which correspond to crystal planes (111), (200), (220), (311), (400), and (420) and are in good agreement with pure cubic CdS phase (JCPDS card number: 65-2887). Broadness of the peaks suggests that CdS particles are very small. XRD pattern of TiO2 precursor calcined at 300°C (C doped TiO2) suggests that at this temperature TiO2 formed is having anatase phase. Peaks at 2θ equal to 25.26, 38.16, 48.17, 54.03, 64.69, 68.16, 71.10, and 76.4° are assigned for (101), (004), (200), (105), (211), (204), (110), (220), and (215) h
k
l planes and are in good agreement with JCPD data file number 841285 (lattice planes of anatase TiO2 phase). XRD pattern of C/TiO2/CdS core-shell nanocomposite suggests that this composite formed is a mixture of cubic CdS and anatase TiO2 phase. Average crystallite sizes of all the compounds were calculated using Debye-Scherer equation and data is presented in Table 1.Table 1
Characteristic properties of photocatalyst.
Sample
Particle size/nma
C/at%b
Band gap (E
g)/eVc
Reaction parameters
Rate constant (k)/min−1
R
2
Pure TiO2
16.2
—
3.14
0.0045
0.949
C doped TiO2
11.3
13.41
2.86
0.0108
0.995
CdS
6.2
—
1.82
0.0053
0.952
C/TiO2/CdS core-shell
10.5
14.62
2.28
0.0326
0.958
a: particle sizes were obtained  from TEM images.
b: C content was obtained from  EDX  spectra.
c:λ values were obtained  from onset of light absorption edges and E
g values were calculated  using  Tauc plots.Figure 1
XRD patterns of CdS, C doped TiO2, and C/TiO2/CdS nanocomposite.


### 3.2. FTIR Study

FTIR spectra of CdS, C/TiO2/CdS precursor, C doped TiO2, and C/TiO2/CdS nanocomposite are shown in Figure 2. Precursor samples show bands at 3000–3500 cm−1 attributed to stretching vibration modes of OH group (TiO2-OH) (Figure 2(a)). It was believed that such TiO2-OH groups arise due to the hydrolysis reaction in the microemulsion process [20]. Peak at 1628 cm−1 is attributed to bending modes of –OH groups of water molecules adsorbed on the surface of catalyst [21]. Peak at 1389 cm−1 can be assigned to C-O stretching in carbonyl. Peak at 2920 cm−1 is assigned as characteristic peak of ammonium. Peak at 2851 cm−1 is due to symmetrical stretching vibration of methyl group. This information indicates that –OH and –C=O functional groups are present in precursor. Figure 2(b) shows that C doped TiO2 and C/TiO2/CdS samples show a band corresponding to Ti-O-Ti vibration at about 419 cm−1. Pure CdS shows a band at 605 cm−1 ascribed to Cd-S stretching [22, 23]. C/TiO2/CdS sample does not show peak which corresponds to Cd-S stretching at 605 cm−1 which might be due to formation of core-shell structure with CdS as core and C doped TiO2 as shell. FTIR spectra of product obtained after heating the precursor at 300°C for 2 h show no absorption peak in higher frequency region but give the sharp peak below 500 cm−1 which may be due to stretching frequency of Ti-O-Ti bond in titanium dioxide.Figure 2
FTIR spectra of CdS, C/TiO2/CdS precursor, C doped TiO2, and C/TiO2/CdS nanocomposite; (b) expanded view of FTIR spectra.
(a)
(b)


### 3.3. Energy Dispersive X-Ray Spectroscopy (EDX) Study

Figure3 represents EDX spectra of (a) C doped TiO2, (b) CdS, and (c) C/TiO2/CdS core-shell nanocomposite. EDX analysis shows that CdS nanoparticles contain only Cd and S elements with 60.83 and 39.17 at%, respectively. TiO2 precursor calcined at 300°C contains C, Ti, and O with 13.42, 18.72, and 67.86 at%, respectively. EDX analysis clearly showed the presence of Cd, S, C, Ti, and O elements in the composite sample with 4.42, 3.79, 14.64, 36.83, and 40.32 at%, respectively.Figure 3
EDX spectra of (a) C doped TiO2, (b) CdS, and (c) C/TiO2/CdS.
(a)
(b)
(c)


### 3.4. Transmission Electron Microscopy (TEM) Study

TEM image of C doped TiO2 is presented in Figure 4(a). This image shows that C doped TiO2 particles are spherical in shape and average particle size was found to be 10 to 12 nm. TEM image of CdS nanoparticle is shown in Figure 4(b). This image shows that CdS nanoparticles are spherical in shape and well dispersed. Average particle size is varying between 6 and 7 nm. Figure 4(c) represents the TEM image of C/TiO2/CdS core-shell nanocomposite. From this figure we can see that CdS particles act as a core and C doped TiO2 as a shell. A selected area electron diffraction (SAED) pattern of all the samples (inset) shows distinct rings indicating their crystalline nature.Figure 4
TEM images of (a) C doped TiO2, (b) CdS, and (c) C/TiO2/CdS core-shell nanocomposites.
(a)
(b)
(c)C/TiO2/CdS core-shell nanospheres were prepared by the microemulsion method. First Cd2+ ions from the aqueous Cd(NO3)2 solution form Cd(OH)2 microemulsion. Addition of sulfur in this solution gives CdS nanospheres by substituting OH− ions with S2− ions. After the addition of TTIP, Ti(OH)4 layer gets formed on CdS. This precursor was heated at 300°C for 2 h yielding C/TiO2/CdS core-shell nanocomposite. The possible mechanism of the formation of C/TiO2/CdS core-shell nanocomposite is described schematically in Figure 5.Figure 5
Schematic diagram showing the steps of formation of C/TiO2/CdS core/shell nanospheres by a microemulsion method.


### 3.5. UV-Visible Spectrophotometery Study

Photo response of pure CdS, C doped TiO2, and C/TiO2/CdS was studied from their UV-visible absorption spectra and presented in Figure 6. Pure TiO2 sample obtained at 500°C is white color and exhibits fundamental absorption edge at 387 nm. C doped TiO2 prepared at 300°C is blackish in color and shows absorption peak in visible region with band edge located at 433 nm. It indicates that C doping enhances absorption power and shifts absorption edge from UV to visible region. CdS nanopowder is yellow color and shows absorption edge around 680 nm. C/TiO2/CdS core-shell nanopowder obtained at 300°C is light grayish yellow color and shows absorption edge near 600 nm, indicating the effective enhancement in photoabsorption capacity in visible region. Optical band gap (E
g) was determined using Tauc equation, α
h
ν
=
A
(
h
ν
-
E
g
)
n
/
2, where α is absorption coefficient, ν is light frequency, A is proportionality constant, and E
g is band gap. Band gaps of CdS, C doped TiO2, and C/TiO2/CdS nanocomposite estimated from Tauc plots (Figure 6) are 1.82, 2.86, and 2.28 eV, respectively. This suggests that nanosized CdS works as a sensitizer and effectively increases the visible light absorption capacity of C doped TiO2.Figure 6
UV-visible absorption spectra and Tauc plots of pure CdS, C doped TiO2, and C/TiO2/CdS core-shell nanoparticles.


### 3.6. Visible-Light Photocatalytic Activity Study

UV-visible spectra of MB solution irradiated with visible light in presence of C/TiO2/CdS core-shell nanopowder at different time intervals were recorded and are presented in Figure 7. These spectra show that peak intensity at 688 nm decreases as the irradiation time increases. This is may be due to degradation of MB. Decrease in the concentration of MB was monitored by examining the variation in UV-visible spectra at 688 nm. Degradation of MB as a function of irradiation time in presence of different catalysts is presented in Figure 8(a). It shows that in absence of catalyst (i.e., photolysis process) MB dye is quite stable. In presence of C/TiO2/CdS core-shell nanocomposite ~97% of MB was degraded within 90 min. Kinetics of MB degradation in visible light was also studied. Graph of ln(C
0/C) against reaction time shows linear relationship, which indicates that photodegradation of MB follows first-order kinetics (Figure 8(b)). Rate constants (
K
) and R
2 values for corresponding reactions were calculated and are presented in Table 1. The order of rate constants in presence of different catalyst is C/TiO2/CdS > C doped TiO2 > CdS > pure TiO2. It is in good agreement with the results obtained from photocatalytic degradation curves. C/TiO2/CdS core-shell nanocomposite shows higher photocatalytic activity as compared to pure CdS, pure TiO2, and C doped TiO2. It may be attributed to small size of catalyst and increase in its photoabsorption strength by lowering the band gap energy. Reusability of C/TiO2/CdS core-shell nanocomposite was tested by reusing the recovered photocatalyst for multiple cycles and results obtained are presented in Figure 9. This figure shows that photocatalytic activity of catalyst does not change significantly up to third cycle indicating that the catalyst is quite stable and can be reused.Figure 7
UV-visible absorption spectra of MB aqueous solution irradiated with visible light at different time intervals in presence of C/TiO2/CdS nanocomposite.Figure 8
(a) Visible light photocatalytic degradation of MB in presence of pure TiO2, C doped TiO2, CdS, C/TiO2/CdS, and TiO2/CdS. (b) Plot of ln(C
0/C
t) against reaction time for different photocatalyst.
(a)
(b)Figure 9
Reuse of photocatalyst.


### 3.7. Degradation Mechanism

Photocatalytic degradation of MB dye can be attributed to the chemical reactions of active species likeO
H
∙ and O
2
∙
- with dye molecules on the surface of photocatalyst [24]. The enhancement of photocatalytic activity of C/TiO2/CdS core-shell nanocomposite heterostructure is due to effective coupling of CdS and C doped TiO2 as shown in Figure 10. Interstitial C doping can create intraband gap state close to the valence band edge of TiO2. Thus C doping leads to the narrowing of the band gap in TiO2 which increases its photoabsorption capacity in visible region. When C/TiO2/CdS nanocomposite is exposed to visible light, photogenerated electrons are injected from conduction band of CdS to the conduction band of TiO2, producing high concentration of electrons in the conduction band of TiO2. On the other hand, holes generated on CdS remain on the valence band of CdS which gives effective charge separation of electron and holes [25]. Meanwhile, the C species could trap the part of photogenerated holes, which potentially reacts with the water adsorbed on the surface of photocatalyst and forms reactive hydroxyl radicals (O
H
∙). Conduction band electrons accumulated on the surface of TiO2 react with dissolved oxygen in water and produce highly oxidative species such as superoxide radical (O
2
∙). These highly reactive radicals (O
H
∙ and O
2
∙) subsequently decompose organic substrate (MB) into CO2 and H2O.Figure 10
Photoinduced electron-hole pair formation mechanism at C/TiO2/CdS core-shell nanocomposite surface.


## 3.1. X-Ray Diffraction (XRD) Study

XRD patterns of C doped TiO2, CdS, and C doped TiO2/CdS core-shell nanoparticles were recorded and are presented in Figure 1. XRD pattern of CdS shows peaks which correspond to crystal planes (111), (200), (220), (311), (400), and (420) and are in good agreement with pure cubic CdS phase (JCPDS card number: 65-2887). Broadness of the peaks suggests that CdS particles are very small. XRD pattern of TiO2 precursor calcined at 300°C (C doped TiO2) suggests that at this temperature TiO2 formed is having anatase phase. Peaks at 2θ equal to 25.26, 38.16, 48.17, 54.03, 64.69, 68.16, 71.10, and 76.4° are assigned for (101), (004), (200), (105), (211), (204), (110), (220), and (215) h
k
l planes and are in good agreement with JCPD data file number 841285 (lattice planes of anatase TiO2 phase). XRD pattern of C/TiO2/CdS core-shell nanocomposite suggests that this composite formed is a mixture of cubic CdS and anatase TiO2 phase. Average crystallite sizes of all the compounds were calculated using Debye-Scherer equation and data is presented in Table 1.Table 1
Characteristic properties of photocatalyst.
Sample
Particle size/nma
C/at%b
Band gap (E
g)/eVc
Reaction parameters
Rate constant (k)/min−1
R
2
Pure TiO2
16.2
—
3.14
0.0045
0.949
C doped TiO2
11.3
13.41
2.86
0.0108
0.995
CdS
6.2
—
1.82
0.0053
0.952
C/TiO2/CdS core-shell
10.5
14.62
2.28
0.0326
0.958
a: particle sizes were obtained  from TEM images.
b: C content was obtained from  EDX  spectra.
c:λ values were obtained  from onset of light absorption edges and E
g values were calculated  using  Tauc plots.Figure 1
XRD patterns of CdS, C doped TiO2, and C/TiO2/CdS nanocomposite.


## 3.2. FTIR Study

FTIR spectra of CdS, C/TiO2/CdS precursor, C doped TiO2, and C/TiO2/CdS nanocomposite are shown in Figure 2. Precursor samples show bands at 3000–3500 cm−1 attributed to stretching vibration modes of OH group (TiO2-OH) (Figure 2(a)). It was believed that such TiO2-OH groups arise due to the hydrolysis reaction in the microemulsion process [20]. Peak at 1628 cm−1 is attributed to bending modes of –OH groups of water molecules adsorbed on the surface of catalyst [21]. Peak at 1389 cm−1 can be assigned to C-O stretching in carbonyl. Peak at 2920 cm−1 is assigned as characteristic peak of ammonium. Peak at 2851 cm−1 is due to symmetrical stretching vibration of methyl group. This information indicates that –OH and –C=O functional groups are present in precursor. Figure 2(b) shows that C doped TiO2 and C/TiO2/CdS samples show a band corresponding to Ti-O-Ti vibration at about 419 cm−1. Pure CdS shows a band at 605 cm−1 ascribed to Cd-S stretching [22, 23]. C/TiO2/CdS sample does not show peak which corresponds to Cd-S stretching at 605 cm−1 which might be due to formation of core-shell structure with CdS as core and C doped TiO2 as shell. FTIR spectra of product obtained after heating the precursor at 300°C for 2 h show no absorption peak in higher frequency region but give the sharp peak below 500 cm−1 which may be due to stretching frequency of Ti-O-Ti bond in titanium dioxide.Figure 2
FTIR spectra of CdS, C/TiO2/CdS precursor, C doped TiO2, and C/TiO2/CdS nanocomposite; (b) expanded view of FTIR spectra.
(a)
(b)


## 3.3. Energy Dispersive X-Ray Spectroscopy (EDX) Study

Figure3 represents EDX spectra of (a) C doped TiO2, (b) CdS, and (c) C/TiO2/CdS core-shell nanocomposite. EDX analysis shows that CdS nanoparticles contain only Cd and S elements with 60.83 and 39.17 at%, respectively. TiO2 precursor calcined at 300°C contains C, Ti, and O with 13.42, 18.72, and 67.86 at%, respectively. EDX analysis clearly showed the presence of Cd, S, C, Ti, and O elements in the composite sample with 4.42, 3.79, 14.64, 36.83, and 40.32 at%, respectively.Figure 3
EDX spectra of (a) C doped TiO2, (b) CdS, and (c) C/TiO2/CdS.
(a)
(b)
(c)


## 3.4. Transmission Electron Microscopy (TEM) Study

TEM image of C doped TiO2 is presented in Figure 4(a). This image shows that C doped TiO2 particles are spherical in shape and average particle size was found to be 10 to 12 nm. TEM image of CdS nanoparticle is shown in Figure 4(b). This image shows that CdS nanoparticles are spherical in shape and well dispersed. Average particle size is varying between 6 and 7 nm. Figure 4(c) represents the TEM image of C/TiO2/CdS core-shell nanocomposite. From this figure we can see that CdS particles act as a core and C doped TiO2 as a shell. A selected area electron diffraction (SAED) pattern of all the samples (inset) shows distinct rings indicating their crystalline nature.Figure 4
TEM images of (a) C doped TiO2, (b) CdS, and (c) C/TiO2/CdS core-shell nanocomposites.
(a)
(b)
(c)C/TiO2/CdS core-shell nanospheres were prepared by the microemulsion method. First Cd2+ ions from the aqueous Cd(NO3)2 solution form Cd(OH)2 microemulsion. Addition of sulfur in this solution gives CdS nanospheres by substituting OH− ions with S2− ions. After the addition of TTIP, Ti(OH)4 layer gets formed on CdS. This precursor was heated at 300°C for 2 h yielding C/TiO2/CdS core-shell nanocomposite. The possible mechanism of the formation of C/TiO2/CdS core-shell nanocomposite is described schematically in Figure 5.Figure 5
Schematic diagram showing the steps of formation of C/TiO2/CdS core/shell nanospheres by a microemulsion method.


## 3.5. UV-Visible Spectrophotometery Study

Photo response of pure CdS, C doped TiO2, and C/TiO2/CdS was studied from their UV-visible absorption spectra and presented in Figure 6. Pure TiO2 sample obtained at 500°C is white color and exhibits fundamental absorption edge at 387 nm. C doped TiO2 prepared at 300°C is blackish in color and shows absorption peak in visible region with band edge located at 433 nm. It indicates that C doping enhances absorption power and shifts absorption edge from UV to visible region. CdS nanopowder is yellow color and shows absorption edge around 680 nm. C/TiO2/CdS core-shell nanopowder obtained at 300°C is light grayish yellow color and shows absorption edge near 600 nm, indicating the effective enhancement in photoabsorption capacity in visible region. Optical band gap (E
g) was determined using Tauc equation, α
h
ν
=
A
(
h
ν
-
E
g
)
n
/
2, where α is absorption coefficient, ν is light frequency, A is proportionality constant, and E
g is band gap. Band gaps of CdS, C doped TiO2, and C/TiO2/CdS nanocomposite estimated from Tauc plots (Figure 6) are 1.82, 2.86, and 2.28 eV, respectively. This suggests that nanosized CdS works as a sensitizer and effectively increases the visible light absorption capacity of C doped TiO2.Figure 6
UV-visible absorption spectra and Tauc plots of pure CdS, C doped TiO2, and C/TiO2/CdS core-shell nanoparticles.


## 3.6. Visible-Light Photocatalytic Activity Study

UV-visible spectra of MB solution irradiated with visible light in presence of C/TiO2/CdS core-shell nanopowder at different time intervals were recorded and are presented in Figure 7. These spectra show that peak intensity at 688 nm decreases as the irradiation time increases. This is may be due to degradation of MB. Decrease in the concentration of MB was monitored by examining the variation in UV-visible spectra at 688 nm. Degradation of MB as a function of irradiation time in presence of different catalysts is presented in Figure 8(a). It shows that in absence of catalyst (i.e., photolysis process) MB dye is quite stable. In presence of C/TiO2/CdS core-shell nanocomposite ~97% of MB was degraded within 90 min. Kinetics of MB degradation in visible light was also studied. Graph of ln(C
0/C) against reaction time shows linear relationship, which indicates that photodegradation of MB follows first-order kinetics (Figure 8(b)). Rate constants (
K
) and R
2 values for corresponding reactions were calculated and are presented in Table 1. The order of rate constants in presence of different catalyst is C/TiO2/CdS > C doped TiO2 > CdS > pure TiO2. It is in good agreement with the results obtained from photocatalytic degradation curves. C/TiO2/CdS core-shell nanocomposite shows higher photocatalytic activity as compared to pure CdS, pure TiO2, and C doped TiO2. It may be attributed to small size of catalyst and increase in its photoabsorption strength by lowering the band gap energy. Reusability of C/TiO2/CdS core-shell nanocomposite was tested by reusing the recovered photocatalyst for multiple cycles and results obtained are presented in Figure 9. This figure shows that photocatalytic activity of catalyst does not change significantly up to third cycle indicating that the catalyst is quite stable and can be reused.Figure 7
UV-visible absorption spectra of MB aqueous solution irradiated with visible light at different time intervals in presence of C/TiO2/CdS nanocomposite.Figure 8
(a) Visible light photocatalytic degradation of MB in presence of pure TiO2, C doped TiO2, CdS, C/TiO2/CdS, and TiO2/CdS. (b) Plot of ln(C
0/C
t) against reaction time for different photocatalyst.
(a)
(b)Figure 9
Reuse of photocatalyst.


## 3.7. Degradation Mechanism

Photocatalytic degradation of MB dye can be attributed to the chemical reactions of active species likeO
H
∙ and O
2
∙
- with dye molecules on the surface of photocatalyst [24]. The enhancement of photocatalytic activity of C/TiO2/CdS core-shell nanocomposite heterostructure is due to effective coupling of CdS and C doped TiO2 as shown in Figure 10. Interstitial C doping can create intraband gap state close to the valence band edge of TiO2. Thus C doping leads to the narrowing of the band gap in TiO2 which increases its photoabsorption capacity in visible region. When C/TiO2/CdS nanocomposite is exposed to visible light, photogenerated electrons are injected from conduction band of CdS to the conduction band of TiO2, producing high concentration of electrons in the conduction band of TiO2. On the other hand, holes generated on CdS remain on the valence band of CdS which gives effective charge separation of electron and holes [25]. Meanwhile, the C species could trap the part of photogenerated holes, which potentially reacts with the water adsorbed on the surface of photocatalyst and forms reactive hydroxyl radicals (O
H
∙). Conduction band electrons accumulated on the surface of TiO2 react with dissolved oxygen in water and produce highly oxidative species such as superoxide radical (O
2
∙). These highly reactive radicals (O
H
∙ and O
2
∙) subsequently decompose organic substrate (MB) into CO2 and H2O.Figure 10
Photoinduced electron-hole pair formation mechanism at C/TiO2/CdS core-shell nanocomposite surface.


## 4. Conclusions

C/TiO2/CdS core-shell nanocomposites have been successfully synthesized using microemulsion method. C/TiO2/CdS nanocomposite shows red shift in the absorption spectra attributed to enhancement in the photoabsorption capacity. C/TiO2/CdS nanocomposite prepared in the present work exhibits better visible light photocatalytic activity compared to other photocatalysts for MB degradation. Photocatalyst prepared is stable and reusable.



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*Source: 690568-2015-10-05.xml*