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Journal of Chemistry
Volume 2013, Article ID 585920, 7 pages
http://dx.doi.org/10.1155/2013/585920
Research Article

Photosensitization of Colloidal SnO2 Semiconductor Nanoparticles with Xanthene Dyes

School of Chemistry, Bharathidasan University, Tiruchirappalli, Tamil Nadu 620 024, India

Received 2 May 2013; Revised 18 September 2013; Accepted 19 September 2013

Academic Editor: Veysel T. Yilmaz

Copyright © 2013 N. Nagarajan et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Abstract

The photochemical behavior of xanthene dyes (fluorescein, erythrosine, and eosin) with colloidal SnO2 nanoparticles was probed by UV-visible, steady state, and time resolved fluorescence measurements. The prepared SnO2 nanoparticles were characterized by using UV-visible and powder XRD measurements. The xanthene dyes were adsorbed on the surface of colloidal SnO2 nanoparticles through electrostatic interaction. Apparent association constant () was calculated from the relevant fluorescence data. The larger value of apparent association constant indicates a strong association between xanthene dyes and SnO2 nanoparticles. The fluorescence quenching is mainly attributed to electron transfer from the excited state xanthenes to the conduction band of colloidal SnO2. The electron transfer mechanism was explained based on the Rehm-Weller equation as well as the energy level diagram.

1. Introduction

The photosensitization of electron transfer across the semiconductor solution interface plays a vital role in light energy conversion in photoelectrochemical cells, wastewater treatment, nanoelectric devices, silver halide photography, and electrophotography. Effort in this area has concentrated on improving the visible light response of wide-band semiconductors such as SnO2, ZnO, and TiO2. Sensitization is achieved by adsorption of dye molecules at the semiconductor surface which, upon excitation, inject an electron into its conduction band [1, 2]. The first successful experiment of this type was described by Putseiko and Terenin [3] who found that the Dember effect of ZnO powder in visible light was sensitized by xanthene and cyanine dyes.

The investigation and development of the dye-semiconductor systems are essential for various fields of applications. Recently Ferrere et al. and Tian et al. used perylene-SnO2 systems for dye sensitized solar cells [46]. The SnO2 is a stable n-type semiconductor with a wide-band gap ( eV) being used for various applications, including solid-state gas sensor, photovoltaic devices, dye-based solar cells, transparent conductive films for display and solar cells, catalysis, and anode materials of secondary lithium ion battery [79].

Xanthenes belong to the most widely used organic dyes, serving as luminophores [10], molecular probes, bioconjugates, stains, and biologically active substances [11, 12]. These dyes are utilized for photosensitization of redox processes [13, 14] in energy transfer and light sensitization studies [15]. They are also used in light-harvesting dendrimers [16], in biochemistry and medicine as reactants for determination of Zn2+, NO [17], and H2O2 [18], in sensor devices for H2S [19], in studying carbon nanotubes [20], for creation of water-soluble fluorescent polymers [21] and new ionic liquids [2225], and many other fields. Previously we have reported photosensitization of various dyes with semiconductor nanoparticles [26, 27]. The structures of xanthene dyes studied in the present work are shown in Scheme 1.

585920.sch.001
Scheme 1

In the present work, we have studied the interaction between xanthene dyes, namely, fluorescein (FN), eosin (EN), and erythrosine (ERN) with colloidal SnO2 nanoparticles by using steady state and life time measurements. The electron transfer mechanism is proved by Rehm-Weller equation.

2. Experimental Methods

2.1. Materials

The xanthene dyes were obtained from Aldrich and used without further purification. Dihydrate tin (II) chloride (SnCl2·2H2O) and ethylene glycol (EG) were purchased from Loba, and they were used as such. Double distilled water was used for preparing the solutions throughout. All measurements were performed at ambient temperature.

3. Instrumentation

3.1. Steady-State Measurements

The fluorescence quenching measurements were carried out with JASCO FP-6500 spectrofluorimeter. The slit widths 5 nm and scan rate (500 nm/min) for both excitation and emission were maintained constant for all the measurements. Quartz cells ( cm) with high vacuum Teflon stopcocks were used for measurements. Absorption spectral measurements were recorded using JASCO V630 UV-visible spectrophotometer.

3.2. Time Resolved Fluorescence Measurements

Fluorescence lifetime measurements were carried out in a picosecond time correlated single photon counting (TCSPC) spectrometer. The excitation source was the tunable Ti-sapphire laser (Tsunami, Spectra Physics, USA). The fluorescence decay was analyzed by using the software provided by IBH (DAS-6).

3.3. Powder X-Ray Diffraction Measurements

X-ray diffraction was recorded with a PAN analytical X’ Pert Pro MPD X-ray diffractometer using Cu Kα radiation ( nm) with a Ni filter. The tube current was 30 mA with a tube voltage of 40 kV. The 2θ angular regions between 20 and 80 were explored at a scan rate of 5° min−1.

4. Preparation of Colloidal SnO2 Nanoparticles

Colloidal SnO2 nanoparticles were prepared according to the literature method [28]. In a typical procedure, 0.2 g of SnCl2·2H2O (dissolved in 10 mL of EG) was added to 40 mL of EG that was hosted in a round-bottom flask. After the pH of the solution was kept at 3-4, the solution had been refluxed at 190°C for 2 hours with constant stirring under atmospheric pressure; the clear solution turned into a slight yellow colloid with the reaction time increasing. The resulting SnO2 colloid was used for the further studies.

5. Results and Discussion

5.1. Determination of Particle Size of Colloidal SnO2 Nanoparticles

The relationship between band gap shift () and radius () of the particles is used to determine the particle size by using Brus equation: where is the reduced Planck’s constant, is the radius of the particle, is the effective reduced masses of the and in the semiconductor, is the electron charge, and is the relative permittivity of the semiconductor.

Reduced effective mass of the exciton () [29] was used for the calculation. A columbic and polarization term in the equation was neglected. The calculated particle size of the prepared colloidal SnO2 is 1.84 nm.

5.2. XRD Characterization of SnO2 Nanoparticles

To clarify the crystalline structure, an XRD pattern of the SnO2 powder is collected and shown in Figure 1. The diffraction peaks at around 27, 34, 52, and 66° are assigned to SnO2 (110), (101), (211), and (301) (PDF no. 411445), respectively. No diffraction peaks due to metallic Sn or other tin oxides were discerned. The diffraction peaks in the XRD pattern broadened because the particles in the sample are too small. The primary particle size calculated by Scherrer formula is about 1.65 nm.

585920.fig.001
Figure 1: X-ray diffraction (XRD) spectrum of SnO2 nanoparticles.
5.3. Absorption Studies

In an aqueous suspension, the polar surface of metal oxide semiconductor nanoparticles assists adsorption of polar species in solution, and such interactions can lead to absorption spectra changes of these molecules [30, 31]. To find out whether there is any ground state interaction between the sensitizer, that is, xanthene dyes and colloidal SnO2 nanoparticles, ground state absorption measurements of Xanthene in the presence and absence of colloidal SnO2 nanoparticles have been carried out. Figure 2 shows the absorption spectra of FN ( M) in water with different concentrations of SnO2 nanoparticles ( M). Upon increasing the concentration of SnO2 nanoparticles, the absorption decreases gradually [32]. But EN and ERN show red shift with decrease in absorbance (Figures 3 and 4). The presence of an isosbestic point at 531 nm for EN and 543 nm for ERN in these absorptions shows the existence of dye in the adsorbed and unadsorbed state. Such a red shift of 14 nm and 17 nm in the absorption peak indicates a strong interaction of the dye with SnO2 surface. Similar spectral changes have been observed for several organic dyes on metal oxide surfaces [33].

585920.fig.002
Figure 2: Absorption spectrum of FN ( M; red color) in the presence of colloidal SnO2 ( M; blue color) in water. The arrow indicates the absorbance decreases on increasing concentration of colloidal SnO2.
585920.fig.003
Figure 3: Absorption spectrum of EN ( M; red color) in the presence of colloidal SnO2 ( M; blue color) in water. The arrow indicates the absorbance decreases with red shift on increasing concentration of colloidal SnO2.
585920.fig.004
Figure 4: Absorption spectrum of ERN ( M; red color) in the presence of colloidal SnO2 ( M; blue color) in water.The arrow indicates the absorbance decreases with red shift on increasing concentration of colloidal SnO2.
5.4. Fluorescence Quenching Studies

The excited state interaction between xanthene dyes and SnO2 colloid is observed by spectrofluorimetric measurements. Figure 5 shows the emission spectrum of FN in absence and presence of SnO2 colloid. The fluorescence emission of FN ( M) was quenched upon successive addition of SnO2 colloid (0– M). Other two dyes also show similar type of spectral behavior (spectra are not shown here). The quenching of FN fluorescence by SnO2 colloid can be described by Stern-Volmer: where and are the fluorescence intensities of xanthene dyes in the absence and presence of SnO2 colloid, respectively. is Stern-Volmer constant and [] is the concentration of respective quencher. The ratios were calculated and plotted against quencher concentration according to (2).

585920.fig.005
Figure 5: Fluorescence quenching of FN ( M; red color) with colloidal SnO2 ( M; blue color) in water.

The Stern-Volmer plot (Figure 6) for EN and ERN is obtained as upward curvature. These types of upward curvature suggest that it may follow static type of mechanism [34]. But, in the case of FN, it gives linear plot. The linear plot mostly results in dynamic quenching. But its value exceeds () the limited values of dynamic quenching (), so it also may follow the static quenching.

585920.fig.006
Figure 6: Stern-Volmer plot versus [SnO2] of FN, EN, and ERN dyes.
5.5. Fluorescence Lifetime Measurements

In general, time resolved measurement is the most definitive method for differentiating static and dynamic quenching process. Figure 7 presents a representative plot of the logarithm of the relative fluorescence intensity versus time of EN in absence and presence of SnO2 colloid, from which the lifetimes () of the excited singlet states were obtained by iterative reconvolution of the measured instrument response function. Fluorescence lifetime observed for EN is unchanged with addition of colloidal SnO2. The other two dyes also follow the same trend (spectra are not shown here). This observation shows that quenching follows static mechanism. Static quenching does not decrease the lifetime because only the fluorescent molecules are observed, and the uncomplexed fluorophores have the unquenched lifetime [35]. Static quenching arises due to the formation of complex between fluorophore and the quencher. Hence the association constant () was calculated by the method given below.

585920.fig.007
Figure 7: Fluorescence decay curve of (i) instrument response curve (Brown color decay), (ii) EN ( M; red color), and (iii) EN in the presence of colloidal SnO2 ( M; blue color).

The equilibrium between the adsorbed and unadsorbed dye molecules is expressed by using (3); in this equation is the apparent association constant which can be calculated from the fluorescence data by using the reported method [31]: where is the apparent association constant, is the initial fluorescence intensity of dye molecules, is the fluorescence intensity of SnO2 adsorbed dyes, and is the observed fluorescence intensity at its maximum. Figure 8 shows the linear straight line dependence of on the reciprocal concentration of colloidal SnO2. The values are listed in Table 1.

tab1
Table 1: Excitation () and emission () wavelengths of the xanthene dyes and apparent association constant () from fluorescence data for dyes with colloidal SnO2.
585920.fig.008
Figure 8: Linear straight line dependence of on the reciprocal concentration of colloidal SnO2.

The values decrease in the following order:FN > EN > ERN.

This trend is observed due to the absence of bulkier electronegative group in FN. So the electrostatic interaction between the dye molecule and SnO2 will be more. So it has higher values. But in the case of EN and ERN, it has four bulkier electronegative bromine and iodine atoms. So it has lower values.

5.6. Mechanism of Quenching

The fluorescence quenching of dyes by SnO2 colloid may occur through two possible mechanisms such as energy or electron transfer. There is no overlap between the emission spectra of dyes with the absorption spectrum of SnO2 colloid (Figure 9), and also the band-gap energy of SnO2 ( eV) [36] is greater than the excited state energy of dyes () shown in Table 2. Thus, energy transfer from excited dyes to SnO2 colloid is not possible. It can therefore be concluded that the fluorescence quenching shown in Figure 5 should not be caused by energy transfer.

tab2
Table 2: Photophysical properties of xanthene dyes.
585920.fig.009
Figure 9: Combined absorption spectrum of colloidal SnO2 (black) and emission spectra of dyes (green: FN, red: EN, and blue: ERN).

The possible way of quenching is through electron transfer from excited state dye molecules to the conduction band of SnO2 colloid as shown in Scheme 2.

585920.sch.002
Scheme 2: Schematic diagram describing the conduction and valence band potentials of SnO2 and the electron-donating energy levels of dyes.

The feasibility of electron transfer from dyes to SnO2 can be explained on the basis of energy level diagram based on the excited state oxidation potential of dyes obtained from the oxidation potential of dyes and their singlet state energy according to the equation, , in Table 2, and the conduction band potential of SnO2 lies around 0.0 eV as shown in Scheme 3. From the scheme we observed that the electron transfer process is feasible.

585920.sch.003
Scheme 3: Proposed electron transfer mechanism.
5.7. Calculation of Free Energy Changes () for the Electron Transfer Reactions

To have a better understanding of electron transfer, we have estimated free-energy change () for each dye-SnO2 systems following Rehm-Weller equation [37]: where is the oxidation potential of the donor, is the reduction potential of the acceptor, is the excitation energy of the fluorescent state, and is the columbic term. Since one of the species is neutral and the solvent used is polar in nature, the columbic term in the above expression is neglected [38]. The values thus calculated for the electron transfer processes in the systems studied in water are all negative (Table 2). Hence, the ET processes were thermodynamically feasible [39].

6. Conclusion

The effect of colloidal SnO2 nanoparticles on the absorption and fluorescence spectra of dyes such as eosin, erythrosine, and fluorescein has been studied. The result in perturbation of the absorption spectrum shows the surface complex formation through adsorption of dyes on the surface of colloidal SnO2. Static nature of quenching has been confirmed by unaltered fluorescence lifetime from time resolved measurements. Based on the energetic calculations the mechanism of electron transfer from excited state dyes to the conduction band of colloidal SnO2 was suggested.

Conflict of Interests

The authors declare that they have no conflict of interests.

Acknowledgments

N. Nagarajan thanks DST INSPIRE for the fellowship (IF 10495). R. Renganathan and N. Nagarajan thank DST, India, for their financial support in the form of a Research Grant (Ref. no. SR/S1/PC-12/2011, dt. 20/09/2011). Authors also thank UGC/DST-FIST for UV-VIS and Fluorescence facilities in the School of Chemistry, Bharathidasan University. They are thankful to Professor P. Ramamurthy, NCUFP, University of Madras, Chennai for time resolved measurements.

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