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ISRN Chemical Engineering
Volume 2012 (2012), Article ID 954869, 7 pages
http://dx.doi.org/10.5402/2012/954869
Research Article

Effect of Sintering Temperatures on the Synthesis of SnO𝟐 Nanospheres

1Material Science and Electrochemistry Research Laboratory, Department of Chemistry, Shivaji University, Kolhapur 416004, India
2Chemical Engineering Division, Institute of Chemical Technology, Matunga, Mumbai 400019, India
3Inorganic Nano-Material Laboratory, Department of Chemistry, Hanyang University, Seoul 133-791, Republic of Korea

Received 17 February 2012; Accepted 6 March 2012

Academic Editors: R. M. Leblanc, L. Liotta, and I. Poulios

Copyright © 2012 Bharat G. Pawar 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

In this communication we report the rapid nanostructure of SnO2 with a spherical morphology which has been prepared in large scale via sol-gel method. The products were characterized with scanning electron microscopy, X-ray powder diffraction, transmission electron microscopy, FTIR, and photoluminescence spectroscopy. The strong photoluminescence of the nanosphere in visible region suggested possible application in nanoscaled optoelectronic devices. A possible growth mechanism for the SnO2 nanosphere in terms of solvation, hydrolysis, and polymerization was proposed.

1. Introduction

Nanometer-sized materials have recently attracted a considerable amount of attention due to their unique electrical, physical, chemical, and magnetic properties as well as their potential for technological applications [1]. Semiconductor nanoparticles have been extensively studied from both experimental and theoretical views—points owing to their potential application in solar energy conversion, photocatalysis, and optoelectronic industry [2]. Tin oxide (SnO2), a n-type semiconductor with a wide band gap (3.6 eV, at 300 K), is well known for its potential applications in gas sensors, dye sensitized solar cells, and transparent conducting electrodes and as a catalyst support [3, 4]. Therefore, many processes have been proposed to synthesize SnO2 nanostructures; some involve dry processes such as sputtering from tin oxide target [5] or from metallic target followed by oxidation [6] and chemical vapour deposition (CVD) [7], while others are based on wet processes, including spray pyrolysis [8] and sol-gel-related methods which have been used to prepare tin oxide coating, particles, and precipitates [915].

One of the most widely used, solution-based nanoparticle synthesis methods is the sol-gel process which involves the evolution of an inorganic network, known as sol, from certain precursor material and consequent gelation of this inorganic network to form ordered three-dimensional gel structure. The next step in the process is the destruction of the evolved gel, thus, resulting in the formation of nanocrystalline material [16]. The sol-gel process is widely used for manufacturing nanoparticles of different metal oxide materials like SnO2 [17, 18], TiO2 [19], ZnO [20, 21], and SiO2 [22]. Amongst various methods, sol-gel process is a relatively novel process for the preparation of functional material that needs precise microstructural control in order to satisfy desired properties [23]. Sol-gel method has advantage of low cost and does not need complicated equipments and could be carried out at more or less ambient conditions, so this method is adopted and applied to synthesize tin oxide nanocrystalline powder.

In the presented work, nanocrystalline SnO2 powder was synthesized using sol-gel route and possible sol-gel growth mechanism was proposed. The cost of the starting precursor used to synthesize nanomaterial decides the cost of the final product. Tin chloride was used as precursor which is cheap as compared to the granulated tin and tin alkoxide. It offers the synthesis of nanocrystalline SnO2-monodispersed particles of nanometer sizes with very large surface area. To the best of the author knowledge this is the first report on calculating percent crystallinity and crystalline size of the sol-gel-synthesized nanocrystalline SnO2 powder, against sintering temperature.

2. Experimental

2.1. Preparation of Powder

The SnO2 sol was prepared by dissolving 1.5 g tin chloride dihydrate (95% SnCl2· 2H2O, Merck, India) and 5 g citric acid (99.5% C6H8O7·H2O, Merck, India) in 8 M HNO3 in a conical flask until a clear solution was obtained. Aqueous ammonia (25%, s d fine-chem Ltd., Mumbai, India) was added dropwise into the solution with stirring, until a pH of 9 was reached. The sol thus prepared was found to be transparent and stable with no precipitation or turbidity. The obtained sol was refluxed at 373 K for 2 h upon which it slowly turned into a turbid colloidal solution. After 5-6 h, the gel was separated via decantation, washed several times with double distilled water and ethanol to remove impurities. After drying at 373 K for 5 h in a hot air oven, the dried gel powder was ground in a mortar and finally sintered in muffle furnace at 373, 473, 573, 673, 773, 873, 973, 1073 K for 2 h.

2.2. Characterization of Powder

A detailed elucidation of the structure and composition was carried out by various characterization techniques. The structural elucidations of SnO2 nanoparticle were carried out using X-ray diffractometer (XRD) (Rigaku MiniFlex at angle between 2 and 80° with scan rate of 2°/min, using Cu Kα1 radiation = 1.5418 Å). The crystallite size was determined based on XRD peak broadening, was confirmed by transmission electron microscope (TEM) (Omega EM 912, operated at 200 kV), and was used for grain size confirmation. Sample for TEM investigation was prepared by putting an aliquote of dichloromethane solution of SnO2 nanoparticles onto an amorphous carbon substrate supported on a copper grid. Surface area, pore volume, and pore diameter were obtained from BET (Micrometer ASAP 2010 Instrument, USA) examination. The surface morphology and size of SnO2 particle were analyzed by using the scanning electron microscope (SEM) (JOEL JSM 680 LA15 KV). The elemental stoichiometry for the quantitative elemental analysis was obtained from the energy dispersive X-ray analyzer.

3. Result and Discussion

The XRD patterns of all the samples of SnO2 nanoparticles at different sintering temperatures from 373 K–1073 K are shown in Figure 1. The samples, namely, a, b, c, d, e, f, g, and h, are referred with respect to their sintering temperatures of 373–1073 K, respectively. The formation of tetragonal rutile structural phase is confirmed and the peaks obtained are well matched with the JCPDS card no. 14-1445. The XRD plot of the powder samples sintered at different temperature shows increase in the peak intensity values with respect to temperature of sintering thereby showing an increasing crystallinity of the samples with an increasing sintering temperature. Further, it is observed that at lower temperature the peaks are not well resolved indicating the presence of amorphous phase, and secondly the sintering temperature increased indicating the removal of impurities and the formation of crystalline phase. The peak orientations in the planes (110), (101), (200), (211), (220), (002), (310), (112), (301), and (321) clearly indicate the effective growth of the nanostructure in the X-direction. The peak with orientation (301) starts to split at the temperature of 873 K, indicating that higher crystallinity of the material is obtained at high temperature. The width of reflection is considerably broadened, indicating a small crystalline domain size. The broadening decreases with an increase of heat treatment temperature in the range of 373−1073 K.

954869.fig.001
Figure 1: XRD pattern of the nanosized SnO2 nanoparticles synthesized by sol-gel method, sintering at temperature step at 373–1073 K.

Crystalline size “D” was obtained by the measurement of the broadening of diffraction lines and applying the Debye- Scherrer formula [24]:𝐷=0.94𝜆,𝛽cos𝜃(1)

where 𝜆 is the wavelength of Cu Kα1 radiations (1.5418 Å), 𝛽 the full-width at half-maximum of the peaks corresponding to the plane, and θ the angle obtained from 2𝜃 value corresponding to a maximum intensity peak in XRD pattern. The crystalline size of obtained SnO2 particles was varying from 3 to 17 nm, as shown in Figure 2.

954869.fig.002
Figure 2: Variation of the crystalline size of the SnO2 nanoparticles with sintering temperature step, 373–1073 K.

The % of crystallinity of specimen is an indication of the uniformality of lattice structure in the specimen. A sample with higher crystallinity would show improved properties such as packing density and stability, than one with relatively lower crystallinity. The amorphous content of the sample may be determined by taking the ratio of the amorphous area of the X-ray diffractogram to the total area. By amorphous area we mean that area of diffractogram is not contained by any specific diffraction peak. In the past, we have successfully used this method for determining the % crystallinity of metal oxide [25, 26]. The process involves the following:(i)smoothing the diffraction graph by a suitable smoothening method (Savitzky-Golay method is preferred);(ii)creating a baseline for the diffractogram whereby all the peaks shall be essentially starting at a common base. This is done by making use of the Sonnefield- Visser method obtained as part of the software;(iii)computing integral area which is nothing but the crystalline area of the material;(iv)now the total area of the diffractogram is computed by carrying out this entire operation except that baseline is not created;(v)now 100 times the ratio of crystalline area to the total area is the % crystallinity;(vi)100 minus the % crystallinity is indicated as the amorphous content;

The phase transformation is a temperature-dependant process. We observed that as sintering temperature increases, % of crystallinity increases and it ranges in between 16–54%. The sample sintering at 1073 K shows highest crystallinity, that is, 54.84%, while sample sintered at 373 K shows lowest crystallinity percentage, that is, 16.33%. Figure 3 shows the % increase in crystallinity with an increase in the sintering temperature.

954869.fig.003
Figure 3: Variation of the crystallinity of the SnO2 nanoparticles with sintering temperature step, 373–1073 K.

Figure 4(a) exhibits an intense, very broad IR peak ranging from 3600–2500 cm−1 with maxima at 3126 cm−1 which may be due to absorbed water and ammonia. As heat treatment increases above 873 K, peak at 3126 cm−1, due to ammonia completely disappears after calcination (Figure 4(b)). The peak at 1383 cm−1 can be ascribed to the bending vibration of NO3 ions occluded into the gel [2, 27]. The peaks are reduced as the calcination temperatures are increased. The next peak obtained between (1232–900 cm−1) is attributed to the hydroxyl-tin vibrations [28]. The peak at 625 cm−1 and 519 cm−1 are attributed to Sn-O stretching modes of Sn-Sn-O and Sn-OH, respectively.

fig4
Figure 4: FT-IR spectrum of SnO2 nanoparticle prepared by sol-gel method (a) as prepared and (b) sintered at 873 K.

The scanning electron microscopy images of the SnO2 nanoparticle prepared by sol-gel method and the effect of sintering temperatures on the same are studied. Figures 5(a), 5(b), 5(c), 5(d) show microstructural homogeneities and remarkably different morphology for SnO2 powder with different sintering temperatures. To avoid the confusion and get the clear idea of the crystal growth, only few SEM images are given, namely, of samples a, b, c, and d. It is clearly seen that the crystal size of the nanoparticles goes on increasing as the sintering temperature increases. At the initial stages seen in samples a and b, the crystalline size is of only few nanometers, whereas at higher temperatures the size of nanoparticles increases to around 17 nm. The uniformity in the crystal size of the samples prepared in all the calcinated samples is observed and hence the practical production of uniformed size nanoparticles of SnO2 can be developed, for an industrial application. The grain size of the nanoparticles varied within a few nanometer ranges and is totally depending on the sintering temperatures with linearity.

fig5
Figure 5: SEM image of SnO2 nanoparticles synthesized by sol-gel method (a) as prepared, (b) sintered at 573 K, (c) sintered at 873 K (d), and sintered at 1073 K.

Figure 6(a) shows a low resolution TEM image whose inset is the magnified image. In Figure 6(b) the high resolution TEM image of SnO2 is shown. One micron square area was considered for obtaining the reflection fringes. Presence of spotted-lines instead of regular points or continuous lines have proven the nanostructure of SnO2. The calculated interplanar 0.41 and 0.39 nm spacings were close to that of interplanar spacing of (110) and (101) reflection planes (0.411 and 0.391 nm), respectively, of SnO2. Unclear but uniform reflection circle was due to nanocrystalline form of SnO2; as for amorphous metal oxide, fuzzy pattern is dominant whereas distinct regular spot is commonly seen in crystalline oxides. The EDAX pattern in Figure 6(d) is recorded while TEM analysis has confirmed an existence of Sn and O element in 57 and 33 wt % ratio.

fig6
Figure 6: (a) TEM, (b) HR-TEM, (c) SAED, (d) EDAX measurements of SnO2 nanoparticles synthesized by sol-gel method.

Figure 7 shows room temperature photoluminescence spectrum of SnO2 nanopowders in the range of 290–550 nm. Strong peak at 413 and weak peak at 446 and 474 nm are nearly equal to earlier report [29]. It is clear that the two strong peaks at 446 and 474 nm may be due to luminescence centers, such as the presence of nanocrystal or defects in SnO2 nanogranules and are important in application of this powder in optoelectronic devices, but that is not yet clear.

954869.fig.007
Figure 7: Room temperature photoluminescence spectrum of SnO2 nanoparticles synthesized by sol-gel method.

We propose the possible mechanism of formation of the SnO2 nanoparticles as discussed below. The growth of SnO2 from tin chloride dihydrate precursor using sol-gel process generally undergoes four stages, such as solvation, hydrolysis, polymerization, and transformation into SnO2. The tin chloride dihydrate precursor was first solvated into HNO3 along with citric acid dihydrate to form tin citrate complex. From (2), the addition of ammonium hydroxide neutralizes the excess acid that remains in solution. After refluxing, the tin citrate complex breaks down and tin hydroxide is formed (3). Thus formed tin hydroxide after calcination forms tin oxide with removal of water as shown in (4):SnCl2SnCl4Sn-Citrate(2)Sn-CitrateSn(OH)4+H2O(3)Sn(OH)4SnO2+2H2O(4)

The hydrolysis and condensation generally occur fast and need to be inhibited for avoiding precipitation and allowing the sol-gel formation. The gel is based on polymeric formation with Sn-Sn-O bond which appears as a result of oleation of the hydroxyl complex, Sn(OH)n with subsequent polymerization with the splitting of water molecule. The increase in the number of bridge bonds, occurring in the gelation stage, is also continued under the action of temperature in the course of thermal treatment. The dehydration process can be described by the following scheme [30]:2(Sn-OH)𝑛=(Sn-Sn-O)𝑛+𝑛H2O.(5)

The inorganic network of freshly prepared gels retains considerable amount of liquid of the liquid-phase, composed of water; hence, the gel is dried at 373 K for 5 hours. Citric acid is widely used as complexing agent. Citric acid (H3L) is a weak triprotic acid and dissociates in a stepwise manner in a solution depending upon the pH of the solution. Only when the pH value of the solution is above 6.4, species L becomes a dominant one [31]. The complexation reactions between the metal ion and citric acid are also highly dependent upon pH and cannot occur at very strong acidic conditions. Thus, we adjusted the pH value of the solution to ~9. Another advantage of this basic condition is that the isoelectric point of the SnO2 powder lies at a pH of 2.5–3.7 [27, 32, 33]. The strong acidic condition enhances the hydrogen bonding among the protonated nanocrystallites leading to a high degree of agglomeration among freshly prepared nanocrystallites. The chelated tin has six-fold coordination available for reacting while 4 fold is available in an inorganic starting material so its reactivity is greatly lowered [34, 35].

The general formula is M(OOR)n (M-refers to Sn), and when sol was refluxed at 373 K, the solution changed slowly into gel; the controlled sol-gel process can be described as follows [36]:

hydrolysis:M(OOR)𝑛+𝑥H2OM(OOR)𝑛-𝑥(OH)𝑥+𝑥RCOOH(6)

condensation:2M(OOR)𝑛-𝑥(OH)𝑥(OH)𝑥1(OOR)𝑛-𝑥MO+H2O.(7) When the dried gels were heat-treated at different calcinating temperatures, nanocrystalline SnO2 having very small size and very high surface areas was obtained. Upon heating at higher temperature, the specific surface area of the sol-gel-obtained nanocrystalline SnO2 decreased, especially at above 773 K which can be explained as follows. In citric acid-based sol-gel method, the complexing ligand may also act as a surface protecting agent, protecting the newly transformed nanocrystalline SnO2 from agglomeration at lower temperature, but when heated to high temperature, the citric acid is destroyed, its protecting property is lost, and the SnO2 nanocrystals starts agglomerating resulting into an increase in its size.

4. Conclusion

Using sol-gel method nanocrystalline SnO2 powder has been successfully synthesized. The synthesized SnO2 nano-powder was analyzed at 373–1073 K calcining temperature. Oxide phase formation has been confirmed from FT-IR studies. Particle size was confirmed through TEM. X-ray diffraction pattern confirms the tetragonal structure of SnO2. Thus, this synthesis method is fast, simple, convenient and is feasible on industrial scale to synthesize SnO2 nanomaterial. The possible applications of SnO2 nanoparticles are in gas sensor, solar cells, optoelectronic devices, paint industry, and surface coating industry.

Acknowledgments

One of the authors (B. G. Pawar) acknowledges the Department of Atomic Energy, Board of Atomic Research in Nuclear Science (Grant Sanction no. 2008/36/83/-BRNS/4009), Government of India. The authors are also grateful to University Grants Commission, New Delhi, and Department of Science and Technology, Government of India, for SAP and DST-FIST programme facilities.

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