ORI GIN AL PA PER
Synthesis and Characterization PbS and Bi2S3
Nanostructures via Microwave Approachand Investigation of Their Behaviors in Solar Cell
Mohammad Yousefi • Mohammad Sabet •
Masoud Salavati-Niasari • Hamid Emadi
Received: 6 February 2012 / Published online: 25 April 2012
� Springer Science+Business Media, LLC 2012
Abstract PbS and Bi2S3 nanostructures were synthesized successfully via a
microwave approach. For synthesis of PbS nanoparticles, a new precursor,
[bis(salisylate) lead (II)]; [Pb(Hsal)2] was used. The products were characterized by
X-ray diffraction, scanning electron microscopy, and photoluminescence spectros-
copy. Thin film of Bi2S3 was prepared by doctor’s blade technique and solar cell
made from ITO/Bi2S3/PbS/Pt layers. I–V characterization was investigated for this
cell and fill factor, open circuit voltage and short circuit current values were
obtained.
Keywords PbS � Bi2S3 � Nanostructures � Microwave � Solar cells
Introduction
In recent years, semiconductor nanomaterials have received considerable attention
due to their wide applications in the fabrication of optical and electronic devices
[1–3]. Bi2S3 is a kind of semiconductors with an Eg of 1.3 eV [4]. Bi2S3 has potential
applications including photovoltaics [5], IR spectroscopy [6] and thermoelectrics
[7, 8]. Many techniques including hydrothermal [9, 10] solvothermal [11–13]
biomolecule assisted method [14] thermal decomposition, ionic liquid-assisted
M. Yousefi
Islamic Azad University, Shahre Rey Branch, P.O. Box 18155-144, Tehran, Islamic Republic of Iran
M. Sabet � M. Salavati-Niasari (&)
Institute of Nano Science and Nano Technology, University of Kashan, P.O. Box 87317-51167,
Kashan, Islamic Republic of Iran
e-mail: [email protected]
H. Emadi
School of Chemistry, College of Science, University of Tehran, Tehran, Islamic Republic of Iran
123
J Clust Sci (2012) 23:511–525
DOI 10.1007/s10876-012-0463-1
templating route [15], photochemical synthesis method [16], sonochemical [17],
template-synthesis methods [18] and microwave [19] have been applied to prepare
Bi2S3 nanoparticles or superstructures. Bi2S3 nanostructures with different morphol-
ogies, such as nanorods [20] nanotubes [21], flower-like structures [22], nanoribbions
[23] and nanowire [24], have been synthesized.
As an important IV–VI group semiconductor, lead sulfide (PbS) has attracted
considerable attention owing to its especially small direct band gap (0.41 eV) and
larger excitation Bohr radius (18 nm) [25–27], and has been widely used in many
fields such as Pb2? ion-selective sensor [28], photography [29], IR detector [30] and
solar absorber. Moreover, an exceptional third-order nonlinear optical property of
PbS nanoparticles has been found, which makes PbS nanocrystals a promising
candidate for photonic and optical switching device applications [31]. The
absorption edge of PbS exhibits a large blue shift [32] when one shrinks the
crystallite size to the nanometer size regime. Recently, various methods have been
developed to synthesize PbS submicro-/nano-crystals, including solvothermal
method [33], chemical vapor deposition (CVD) method [34], ultrasonic method
[35], and electrodeposited route [36]. Microwave-assisted synthesis [37] is a very
attractive process for producing a variety of materials. In this work two types of
nanostructured semiconductors with different features were synthesized via facile
microwave approach. The effects of several parameter on product size and
morphology such as sulfur sources, sulfur concentration, microwave irradiation time
and power were investigated. The optical properties were studied by PL
spectroscopy. Bi2S3 Thin film was fabricated by Doctor’s blade technique.
Subsequently PbS thin film was covered on Bi2S3 film via Doctor’s blade method
and their features were obtained from I–V curve.
Experimental
Materials
All the chemical reagents used in experiments were of analytical grade and used as
received without further purification. [Pb(Hsal)2] precursor was synthesized as
follow: Pb(NO3)2 was dissolved in 50 mL of distilled water to form a homogeneous
solution. The stoichiometric amount of sodium salicylate dissolved in an equal
volume of distilled water, and then was added dropwise into the above solution
under magnetic stirring. The solution was stirred for about 30 min and refluxed for
3 h. The obtained precipitate was isolated, washed several times with distilled water
and ethanol and dried at 60 �C for 2 h. The achieved product was characterized by
X-ray diffraction (XRD). Anal. calcd for C14H10O6Pb: C, 34.93; H, 2.09; Pb, 43.04.
Found: C, 34.76; H, 1.97; Pb, 42.11 %. The molecular formulae of the complex has
been assigned on the basis of the results of their elemental analyses. The lead(II)
complexes are extremely stable in the solid state and in solution and are relatively
stable against ligand dissociation even in highly acidic solutions. The molar
conductance values of the complexes measured in DMF corresponds to
nonelectrolytes.
512 M. Yousefi et al.
123
Characterization
X-ray diffraction patterns were recorded by a Rigaku D-max C III, X-ray
diffractometer using Ni-filtered Cu Ka radiation. Scanning electron microscopy
(SEM) images were obtained on LEO-1455VP equipped with an energy dispersive
X-ray spectroscopy. FE-SEM images were obtained on HITACHI S-4160. Room
temperature photoluminescence (PL) was studied on an F-4500 fluorescence
spectrophotometer. Elemental analysis was obtained from Carlo ERBA Model EA
1108 analyzer. The metal contents of the samples were measured by atomic
absorption spectrophotometer (AAS-Perkin-Elmer 4100–1319) using a flame
approach.
Preparation of PbS and Bi2S3 Nanostructures
In a typical experimental process, the stochiometric amount of Pb(Hsal)2 and
different sulfur sources were dissolved in 30 ml ethylene glycol separately and
stirred for 20 min. Then these solutions mixed together and stirred for 30 min.
Finally solution was transferred to 100 ml beaker and the contents were exposed to
microwave irradiation in a domestic microwave oven, operating at 2,450 MHz, for
different output power and time. The obtained black powder was washed several
times with distilled water and ethanol to remove any unreacted reactants and
impurity and dried in vacuum. Experimental conditions for preparation of PbS are
shown at Table 1.
Table 1 Experimental condition for the preparation of PbS nanoparticles
Sample
no.
Figure
no.
Sulfur source Microwave
time (min)
Microwave
power (W)
Pb:S mole
ratio
1 2a Thioacetamide 2 750 1:1
2 2b Thiourea 2 750 1:1
3 2c L-cysteine 2 750 1:1
4 2d Carbon disulfide 2 750 1:1
5 2e Thiosemicarbazide 2 750 1:1
6 2f Ammonium sulfide 2 750 1:1
7 2g Sodium sulfite 2 750 1:1
8 2h Thiosemicarbazide ?
Thioacetamide
2 750 1:1
9 3a Thioacetamide 2 750 1:2
10 (optimized
sample)
3b Thioacetamide 2 750 1:3
11 4a Thioacetamide 2 600 1:3
12 4b Thioacetamide 2 900 1:3
13 5a Thioacetamide 3 750 1:3
14 5b Thioacetamide 5 750 1:3
Synthesis and Characterization PbS and Bi2S3 Nanostructures 513
123
The reaction for preparation of Bi2S3 was similar to PbS synthesis. In a typical
synthesis 1.00 g (0.002 mol) of Bi(NO3)3�5H2O powder and 0.14 ml (0.002 mol)
thioglycolic acid (TGA) as sulfur source were dissolved in 30 ml ethylene glycol,
separately. Then the solutions were mixed together and stirred for 30 min. Finally
solution was exposed to microwave irradiation for different time and powers. The
obtained black powders were washed several times with water and ethanol and dried
at 60 �C for 2 h. Experimental conditions for preparation of Bi2S3 are shown at
Table 2.
Manufacturing
Bi2S3 film as absorber layer was prepared by doctor’s blade coating using slurry of
0.05 g Bi2S3 powder dispersed in 5 ml ethanol, 0.05 g ethyl cellulose and 0.05 ml
Triton X-100 mixture on Indium Tin Oxide (ITO)-coated glass substrate. Then, the
glass substrate was maintained at 200 �C for 30 min to remove the organic
compounds. Subsequently, other similar paste from PbS nanoparticles was prepared
and technique was deposited on Bi2S3 layer by doctor’s blade. In current
investigation, PbS was selected as n-layer. The counter-electrode was prepared by
chemical deposition of a platinum solution above an ITO electrode. This electrode
was placed over the PbS/Bi2S3 electrode. The redox electrolyte consisted of 0.05 M
LiI, 0.05 M I2 and 0.5 M 4-tert-butylpyridine at acetonitrile as a solvent. The
photocurrent–voltage (I–V) curves were used to calculate short-circuit current (Isc),
open-circuit voltage (Voc) and fill factor (FF). I–V measurement was made under
simulated Air Mass 1.5 global illumination. Also, the active cell area was 1 cm2.
The image of the fabricated cell process is depicted at Scheme 1.
Table 2 Experimental condition for the preparation of Bi2S3 nanostructures
Sample no. Figure
no.
Microwave
time (min)
Microwave
power (W)
Bi:S mole
ratio
Morphology
15 6a 2 750 3:1 Aggregated nanoparticles
16 6b 2 750 2:1 Aggregated nanoparticles
17 6c 2 750 1:1 Petal-like structures
18 6d 2 750 1:2 Flower-like nanostructures
19 6e 2 750 1:3 Nanorods
20 6f 2 750 1:4 Aggregated nanorods
21 (optimized
sample)
6g 2 750 1:5 Urchin-like nanostructures
22 7a 2 600 1:5 Aggregated nanorods
23 7b 2 900 1:5 Aggregated nanorods
24 8a 5 750 1:5 Aggregated
nanorods ? irregular
masses
25 8b 7 750 1:5 Aggregated nanorods
514 M. Yousefi et al.
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Results and Discussion
X-ray Diffraction Pattern
Figure 1 shows the XRD pattern of Pb precursor (Fig. 1a), PbS (Fig. 1b) and Bi2S3
(Fig. 1c) nanostructures. As shown in Fig. 1b, the main diffraction peaks were
observed at 26.134�, 30.238�, 43.234�, 51.133�, 53.590�, 62.69�, 69.043�, 71.041�,
and 79.049� in the XRD pattern of the PbS which confirm the formation of PbS with
tetragonal structure. (JCPDS No. 78-1897, a = 5.9143A). The crystal size of the
PbS nanoparticles was estimated by Debye–Scherrer equation [38] (d = 0.9 k/bcosh) and it was about 29.2 nm. In Fig. 1c all the peaks reflected from (3 1 0),
(2 1 1), (2 2 1), (3 0 1), (3 1 1), (4 2 0), (4 3 0), (2 5 0), (4 4 0), (5 0 1), (3 1 2),
(2 4 2), (1 7 1), (7 2 1), (6 5 1) and (8 1 1) planes matched well with the standard
JCPDS-17-0320 pattern of Orthorhombic Bi2S3. The crystal size of the Bi2S3
nanostructures was calculated about 14.6 nm. No impurity peaks was observed for
PbS and Bi2S3 which indicate the products have high purity.
SEM Images
Figure 2a–h shows the SEM images of PbS nanostructures that prepared from
several sulfur sources. Based on modern complex theory, the sulfide source
molecules, some of which dissociate and release S2-, also behave as potential
ligands [39]. Therefore by using different sulfur sources different morphologies
were obtained (Fig. 2). Table 3 described the morphology of PbS nanostructure
prepared with eight different sulfur sources. Figure 4 exhibits the effect of sulfur
concentration on morphology of PbS nanostructures. By increasing the mole ratio of
S:Pb to 2:1 (Fig. 4a), the size of particles becomes smaller and further increase (3:1)
will cause to the formation of small and separated particles (Fig. 4b).
Figure 5 shows the effect of microwave power on shape of the PbS
nanostructures. At 600 W microwave irradiation due to little energy of microwave,
the product was mainly composed from agglomerated particles (Fig. 5a). By
increasing the power to 750 W the sufficient energy for preparation of PbS
nanoparticles has been created and hence PbS nanoparticles formed which were
Scheme 1 Schematic diagram illustrating the image of solar cell fabrication process
Synthesis and Characterization PbS and Bi2S3 Nanostructures 515
123
consisted of separated particles with smaller diameter (Fig. 4b). By further increase
of microwave power, due to high energy of microwave irradiation, the active
surface of nanoparticles [40] adhere together and bigger particles have been
achieved (Fig. 5b). In fact, due to diffusion process of the reactants to the surface of
the growing crystallite led to growth proceeds through the new nucleations and
increasing the number of particles [41]. Therefore, the optimum power for PbS
nanoparticles formation is 750 W.
Fig. 1 X-ray diffraction pattern of a Pb precursor, b sample no. 10 and c sample no. 21
516 M. Yousefi et al.
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Figure 6 shows the SEM images of PbS nanostructures that prepared at 3
(Fig. 6a) and 5 (Fig. 6b) min. The influence of microwave time on morphology is
Fig. 2 Scanning electron microscopy images of a–h sample no. 1–8 respectively
Synthesis and Characterization PbS and Bi2S3 Nanostructures 517
123
similar to the power effect. By increasing time the energy of microwave has been
increased and aggregated particles were obtained.
Figure 7 shows the SEM image of Bi2S3 nanostructured synthesized from
Bi(NO3)3�5H2O and TGA at different mole ratio of Bi:S. When the Bi:S mole ratio
was 3:1, irregular masses were obtained (Fig. 7a). By increasing the sulfur source to
2:1 (Fig. 7b) the product shape was similar to 3:1 mol ratio. The increase of sulfur
concentration to 1:1 (Fig. 7c), leads to significant difference from particles to flower
Fig. 3 Scanning electron microscopy images of a sample no. 9 and b sample no. 10
Table 3 The morphology of PbS nanostructure prepared with eight different sulfur sources
Figure no. Sulfur source Morphology
2a Thioacetamide Nanoparticles
2b Thiourea Nanocubics
2c L-cysteine Nanocubics ? nanoparticles
2d Carbon disulfide Nanocubics ? nanoparticles
2e Thiosemicarbazide Star-like nanostructures
2f Ammonium sulfide Aggregated nanocubics
2g Sodium sulfite Sphere-like structures
2h Thiosemicarbazide ? Thioacetamide Aggregated nanoparticles
Fig. 4 Scanning electron microscopy images of a sample no. 11 and b sample no. 12
518 M. Yousefi et al.
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like morphology. As shown in this figure concentricity plates were created petal-like
structure. By further increase in sulfur concentration (1:2), the flower structure
becomes perfect (Fig. 7d). When the Bi:S mole ratio was changed to 1:3 besides the
flower-like structure, rod-like structure obtained (Fig. 7e). When the Bi:S mole ratio
was changed to 1:4 (Fig. 7f) another significant variation in morphology was
observed. In other words, in this concentration, the flower-like structure replaced
with the aggregated rods. Finally, at 1:5 mol ratio the product was mainly composed
of urchin-like and rod-like structures (Fig. 7g). Hence the best mole ratio for
preparation of Bi2S3 nanostructures was 1:5. Actually, the trick in microwave
synthesis of urchin-like Bi2S3 nanocrystal presented here is the usage of TGA as a
sulfur source and stability agents, which was previously used as the stability agent
to prevent the chalcogenide nanocrystals from aggregating [42].
Figures 8 and 9 show the effect of microwave power and time on Bi2S3
morphology. The best power for Bi2S3 nanostructured formation was 750 W
(Fig. 7g) which is similar to the PbS results. At 600 W (Fig. 8a) and 900 W
(Fig. 8b) the products haven’t specified morphology. Also the best time for creation
proper morphology was 2 min (Fig. 7g) and in the other time such as 3 (Fig. 9a) and
5 min (Fig. 9b) the obtained products do not have good structures.
Figure 10 shows the SEM of Bi2S3 thin film. The fabricated thin film has non-
uniform surface and several lumps are located at thin film surface that may be a
strong factor for electron trap and weak operation of solar cell.
Photoluminescence spectrum
Figures 11 and 12 show the room temperature PL spectroscopy of PbS and Bi2S3
nanostructures, separately. As shown in this figures, The calculated band gaps from
PL were 2.9 and 2.24 eV for PbS and Bi2S3 respectively that show a large blue shift
in comparison with their bulk samples with 0.41 eV (PbS) [43] and 1.3 eV (Bi2S3)
[4]. These different values are due to quantum size effect. In other words, by
decreasing the particle size, the PL band shifts to lower wavelength. Therefore the
bandgap becomes higher.
Fig. 5 Scanning electron microscopy images of a sample no. 13 and b sample no. 14
Synthesis and Characterization PbS and Bi2S3 Nanostructures 519
123
Fig. 6 Scanning electron microscopy images of a–g sample no. 15–21 respectively
520 M. Yousefi et al.
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I–V Characterization
The current–voltage measurement for PbS/Bi2S3 solar cell is shown in Scheme 1. It
was found that the fabricated device has solar cell behavior. The FF, Voc and Isc
Fig. 7 Scanning electron microscopy images of a sample no. 22 and b sample no. 23
Fig. 8 Scanning electron microscopy images of a sample no. 24 and b sample no. 25
Fig. 9 Scanning electronmicroscopy image of Bi2S3 thinfilm
Synthesis and Characterization PbS and Bi2S3 Nanostructures 521
123
were 25 %, 40 and 0.004 mA respectively. The main reasons for these low values
are mentioned below:
1. Due to high bandgap of Bi2S3 the generation of electron–hole becomes low and
hence the Voc value decreased.
2. The urchin-like morphology of Bi2S3 leads to the caption of the generated
electrons in Bi2S3 structure and therefore they can’t transfer to n-layer and so
the Isc becomes low.
3. Another factor that restricts the Isc is presence of many small particles in PbS
nanostructures. By decreasing the particle size the grain boundaries that located
Fig. 10 Room temperaturephotoluminescence of sampleno. 10
Fig. 11 Room temperaturephotoluminescence of sampleno. 21
522 M. Yousefi et al.
123
between the particles have been increased and subsequently, electron trap states
become high.
4. The Bi2S3 and PbS have orthorhombic and tetragonal structures, respectively.
These phase difference is an important factor that restrict the cell operation and
therefore FF has been decreased.
5. The presence of several lumps at thin film surface and non-uniform structure of
film are two strong parameters that restrict the solar cell operation.
A characterization comparison for solar cell with other similar works is shown in
Table 4.
Conclusion
In this study, two nanostructured semiconductors were synthesized via microwave
approach. Several effects on product morphology and size such as sulfur
Fig. 12 I–V characterization of solar cell
Table 4 The characterization comparison for solar cell with other similar works
Structure Voc (mV) Jsc(mA/cm2) FF Ref.
Glass/ITO/CdS/PbS/conductive graphite 290 14 0.36 [44]
TCO/window (CdS-ZnS)/Bi2S3/PbS/graphite
electrode/Ag
130–310 0.5–5 0.25–0.42 [45]
ITO/ZnO/PbS/CdS/Pt 281.3 1.48 57 [46]
ITO/ZnO/CdS/PbS/Pt 311.4 2.20 55 [46]
ITO/ZnO/CdS/Pt 292.2 1.69 59 [46]
ITO/ZnO/PbS/Pt 272.9 1.27 55 [46]
TCO/Bi2S3/PbS/graphite electrode/Ag 220–280 1.1–2.1 0.26–0.34 [47]
TCO/CdS/Sb2S3/PbS/graphite electrode/Ag 620–660 2.95–3.73 0.29–0.031 [48]
Synthesis and Characterization PbS and Bi2S3 Nanostructures 523
123
concentration, microwave power and time and sulfur sources have been investi-
gated. Best structures were selected for studying their behavior in solar cell.
Because of the Bi2S3 had smaller bandgap from PbS nanoparticles, it used to as
p-layer. Optical properties of products were studied by PL spectroscopy and it was
found that due to quantum size effect, the bandgap of two semiconductors were
shifted to lower wavelength. Thin film of Bi2S3 and PbS were prepared by doctor’s
blade technique and solar cell was made from ITO/Bi2S3/PbS/Pt-ITO layers. I–V
characterization was obtained from this cell. Calculated FF, Voc and Isc were
obtained from I–V curve showing very low values. Several parameters such as
morphology of products, high band gap of p-layer, non-uniform thin film and
difference of products structure are responsible to weak operation of solar cell.
Acknowledgments Authors are grateful to Council of Islamic Azad University, Shahr-e Rey Branch,
Tehran and University of Kashan for providing financial support to undertake this work.
References
1. B. O. Dabbousi, M. G. Bawendi, O. Onitsuka, and M. F. Rubner (1995). Appl. Phys. Lett. 66, 1316.
2. V. L. Colvin, M. C. Schlamp, and A. P. Alivisatos (1994). Nature 370, 354.
3. D. L. Klein, R. Roth, A. K. L. Lim, A. P. Alivisatos, and P. L. McEuen (1997). Nature 389, 699.
4. J. Black, E. M. Conwell, L. Seigle, and C. W. Spencer (1957). J. Phys. Chem. Solids 2, 240.
5. C. Y. Wu, S. H. Yu, S. F. Chen, G. N. Liu, and B. H. Liu (2006). J. Mater. Chem. 16, 3326.
6. J. Grigas, E. Talik, and V. Lazauskas (2002). Phys. Status Solidi B 232, 220.
7. P. Boudjouk, M. P. Remington, D. G. Grier, B. R. Jarabek, and G. McCarthy (1998). J. Inorg. Chem.37, 3538.
8. L. D. Zhao, B. P. Zhang, W. S. Liu, H. L. Zhang, and J. F. Li (2008). J. Solid State Chem. 181, 3278.
9. Y. Yu and W.-T. Sun (2009). Mater. Lett. 63, 1917.
10. A. Phuruangrat, T. Thongtem, and S. Thongtem (2009). Mater. Lett. 63, 1496.
11. G. Zhu, P. Liu, J. Zhou, X. Bian, X. Wang, J. Li, and B. Chen (2008). Mater. Lett. 62, 2335.
12. W. J. Lou, M. Chen, X. B. Wang, and W. M. Liu (2007). Chem. Mater. 19, 872.
13. X. Yang, X. Wang, and Z. Zhang (2006). Mater. Chem. Phys. 95, 154.
14. Q. Lu, F. Gao, and S. Komarneni (2004). J. Am. Chem. Soc. 126, 54.
15. J. Jiang, S. H. Yu, W. T. Yao, H. Ge, and G. Z. Zhang (2005). Chem. Mater. 17, 6094.
16. W. B. Zhao, J. J. Zhu, Y. Zhao, and H. Y. Chen (2004). Mater. Sci. Eng. B 110, 307.
17. H. Wang, J. J. Zhu, J. M. Zhu, and H. Y. Chen (2002). J. Phys. Chem. B. 106, 3848.
18. L. S. Li, N. J. Sun, Y. Y. Huang, Y. Qin, N. N. Zhao, G. N. Gao, M. X. Li, H. H. Zhou, and L. M. Qi
(2008). Adv. Funct. Mater. 18, 1194.
19. J. Lu, Q. F. Han, X. J. Yang, L. D. Lu, and X. Wang (2007). Mater. Lett. 61, 2883.
20. G. Xie, Z. P. Qiao, M. H. Zeng, X. M. Chen, and S. L. Gao (2004). Crys. Growth Des. 4, 513.
21. C. H. Ye, G. W. Meng, Z. Jiang, Y. W. Wang, G. Z. Wang, and L. D. Zhang (2002). J. Am. Chem.Soc. 124, 15180.
22. B. Zhang, X. C. Ye, W. Y. Hou, Y. Zhao, and Y. Xie (2006). J. Phys. Chem. B. 110, 8978.
23. Z. P. Liu, J. B. Liang, S. Li, S. Peng, and Y. T. Qian (2004). Chem. Eur. J. 10, 634.
24. Y. W. Koh, C. S. Lai, A. Y. Du, E. P. T. Tiekink, and K. P. Loh (2003). Chem. Mater. 15, 4544.
25. J. L. Machol, F. W. Wise, R. C. Patel, and D. B. Tanner (1993). Phys. Rev. B. 48, 2819.
26. S. Wang, A. Pan, H. Yin, Y. He, Y. Lei, Z. Xu, and B. Zou (2006). Mater. Lett. 60, 1242.
27. L. Xu, W. Zhang, Y. Ding, W. Yu, J. Xing, F. Li, and Y. J. Qian (2004). Cryst. Growth. 273, 213.
28. H. Hirata and K. Higashiyama (1971). Bull. Chem. Soc. Jpn. 44, 2420.
29. P. K. Nair, O. Gomezdaza, and M. T. S. Nair (1992). Adv. Mater. Opt. Electron. 1, 139.
30. P. Gadenne, Y. Yagil, and G. Deutscher (1989). J. Appl. Phys. 66, 3019.
31. D. J. Asunskis, I. L. Bolotin, and L. Hanley (2008). J. Phys. Chem. C 112, 9555.
32. Z. Zeng and S. Wang (1999). J. Chem. Mater. 11, 3365.
524 M. Yousefi et al.
123
33. C. Zhang, Z. Kang, E. Shen, E. Wang, L. Gao, F. Luo, C. Tian, C. Wang, and Y. Lan (2006). J. Phys.Chem. B. 110, 184.
34. J. P. Ge, J. Wang, H. X. Zhang, X. Wang, Q. Peng, and Y. D. Li (2005). Chem. Eur. J. 11, 1889.
35. P. T. Zhao, G. Chen, Y. Hu, X. L. He, K. Wu, Y. Cheng, and K. X. Huang (2007). J. Cryst. Growth.303, 632.
36. K. K. Nanda and S. N. Sahu (2001). Adv. Mater. 13, 280.
37. C. Gabriel, S. Gabriel, E. H. Grant, B. S. J. Halstead, and D. M. P. Mingos (1998). Chem. Soc. Rev.27, 213.
38. R. Jenkins, and R. L. Snyder (1996). Introduction to X-ray Powder Diffractometry (Wiley, New
York, p. 90).
39. S. Peng, J. Liang, L. Zhang, Y. Shi, and J. Chen (2007). J. Cryst. Growth. 305, 99.
40. L. Yan, Y. Si-rong, L. Jin-dan, H. Zhi-wu, and Y. Dong-sheng (2011). Trans. Nonferrous Met. Soc.China 21, s483.
41. A. R. Abbasi and A. Morsali (2010). Ultrason. Sonochem. 17, 572.
42. A. M. Qin, Y. P. Fang, W. X. Zhao, H. Q. Liu, and C. Y. Su (2005). J. Cryst. Growth 283, 230.
43. K. Inuk and W. W. Frank (1997). J. Opt. Soc. Am. B. 14, 1632.
44. J. Hernandez-Borja, Y. V. Vorobiev, and R. Ramı0rez-Bon (2011). Sol. Energy Mater. Sol. Cells 95,
1882.
45. H. Moreno-Garcıa, M. T. S. Nair, and P. K. Nair (2011). Thin Solid Films 519, 7364.
46. C. Liu, Z. Liu, Y. Li, J. Ya, L. E and L. An (2011). Appl. Surf. Sci., 257, 7041.
47. H. Moreno-Garcıa, M. T. S. Nair, and P. K. Nair (2011). Thin Solid Films 519, 2287.
48. S. Messina, M. T. S. Nair, and P. K. Nair (2009). Thin Solid Films 517, 2503.
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123