Journal of Chemistry

Volume 2014 (2014), Article ID 713573, 7 pages

http://dx.doi.org/10.1155/2014/713573

Research Article

Preparation of Mesoporous SnO₂ by Electrostatic Self-Assembly

Yang Jing, Wang Yan, and Xu Xiaowen

School of Chemistry and Biology Engineering, Jiangsu Key Laboratory for Environment Functional Materials, University of Science and Technology of Suzhou, Suzhou 215009, China

Received 12 June 2014; Revised 7 August 2014; Accepted 7 August 2014; Published 21 August 2014

Academic Editor: Fan Dong

Copyright © 2014 Yang Jing 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.

We report a simple and scalable strategy to synthesize mesoporous SnO₂ with tin dioxide nanoparticles of 5-6 nm crystalline walls and 3-4 nm pore diameter with the assistance of as templating agent at room temperature. The samples were characterized by XRD, TEM, UV-DRS, XPS, and BET. The product has a moderately high surface area of 132 m² g⁻¹ and a narrow mesoporous structure with an average pore diameter of 3.5 nm. The photocatalytic activities of the mesoporous SnO₂ were evaluated by the degradation of methyl orange (MO) in aqueous solution under UV light irradiation.

1. Introduction

Porous has received great attention because of its wide-ranging applications, in areas such as in lithium-ion batteries [1], gas sensors [2], catalysis [3–5], solar cells [6, 7], and supercapacitor electrodes [8] due to its abundance, low cost, and high surface area. Recently, the extensions of soft or/and hard templating procedures to prepare porous SnO₂ with huge specific surface areas have been reported [3]. In order to obtain mesoporous SnO₂, the reported general approach is to use a templating agent, usually a surfactant, which is removed by calcination or chemical extraction after the SnO₂ network is formed. However, the posttreatment, such as high-temperature calcination, may affect the properties of the SnO₂ particles and may reduce the surface areas and pore volume. Therefore, avoiding the use of surfactants is highly desirable and would be beneficial in terms of cost, environmental impact, and scale-up potential. For instance, Mancin and coworkers constructed mesoporous silica through a surfactant-free approach. The templating agent that they used is a hydrolytically unstable inorganic phase and the template could be removed by solvent exchange with water at room temperature [9], but the surface area and pore structure of mesoporous silica had remained unclear.

In this work, we developed a novel, facile, and controllable technique to synthesize mesoporous SnO₂. The technique of electrostatic self-assembly of charged colloidal particles was exploited to prepare mesoporous SnO₂. In our previous works, mesoporous NiO has been fabricated with the assistance of [10]. Our concept is that two kinds of soluble salt in acidic solution do not hydrolyze. The formation of the homogeneous assemblies is initiated with the generation of a large number of nucleuses after the mixing of the acidic precursor with basic solutions. It is well known that the solubility of Sn(OH)₄ in aqueous solution is determined by the pH and the Sn⁴⁺ concentration. When the pH was adjusted to around 4, the Sn⁴⁺ ions are almost transformed to colloidal Sn(OH)₄

However, the isoelectric point of colloidal Sn(OH)₄ solutions is 4.5 [11]. The pH value that we used (4) was below the isoelectric point of Sn(OH)₄; hence the surfaces of Sn(OH)₄ colloid are positively charged because of the presence of abundant protonated hydroxyl groups. ions could be condensed in acid solution, and the extent of condensation depended on the pH level. The dominant species are ions in pH range of 7–12, and the protonated species were those of ions and of ions in pH ranges 3–5 and at pH below 2, respectively [12]. Therefore, the positively charged Sn(OH)₄ and the negatively charged ions began to coprecipitate (2) when ions were added to colloidal solutions of Sn(OH)₄ at a pH value of 4

Systems of nanoparticles (NPs) interacting through electrostatic forces have been reported. For example, Grzybowski and coworkers reported that large 3D crystals could be prepared by the electrostatic self-assembly of oppositely charged metallic nanoparticles [13]. Crystal growth requires advancing of grain boundaries. Grain boundaries can be “pinned” and hence their motion is restricted by introducing tiny secondary-phase particles along the grain boundaries. The growth of NPs is generally inhibited by surface modification with organic molecules, such as surfactants and ligands [14]. In our system, ions play the role of traditional organic passivating ligands that anchor onto the surface of colloidal Sn(OH)₄ particles and form the “pins” at grain boundaries, inhibiting the growth of the particles. Then SnO₂/MoO₃ is formed following the process of separation and calcination. Mesoporous SnO₂ was prepared by dissolving SnO₂/MoO₃ with NaOH solution. Figure 1 illustrates the preparation procedure of mesoporous SnO₂.

Figure 1: Schematic illustration of the preparation of mesoporous SnO₂.

2. Experimental Section

2.1. Synthesis

Chemicals: all of the chemicals (analytic reagent, AR) were used as received without further purification.

In a typical experiment, SnCl₄5H₂O (0.02 M) was dissolved in deionized water (50 mL) and produced a clear precursor solution after stirring for 1 h. (NH₄)₆Mo₇O₂₄4H₂O (0.0029 M) was dissolved in deionized water (50 mL) to obtain the solution of (NH₄)₆Mo₇O₂₄, which was added to the solution of SnCl₄ dropwise. After stirring for 30 min, the pH of the solution was adjusted to 4 by dropwise addition of NH₃·H₂O solution (2 M). The resulting mixture was stirred for an additional 3 h. Then the precipitate was centrifuged and thoroughly washed with deionized water to remove remaining Cl⁻ and to obtain the precursor. The precursor was calcined at 400°C in an oven for 3 h with a heating rate of 10°C min⁻¹ and then cooled to ambient temperature to obtain SnO₂@MoO₃. The SnO₂/MoO₃ was dissolved in NaOH solution (2 M) for 2 days under magnetic stirring, was collected by filtration with a membrane filter, and was dried at 110°C to obtain mesoporous SnO₂.

2.2. Characterizations

The phase structures of as-prepared products were characterized by X-ray diffraction (XRD) (Bruker D8 advance) with Cu-Kα radiation (λ = 1.5418 Å) over a 2θ range between 5° and 70° and the scanning speed of 4° min⁻¹ with a step of 0.02°. The sample morphology was examined by transmission electron microscope (TEM) with the accelerating voltage of the electron beam of 200 kV (JEOL JEM-3930EX). Diffuse reflectance spectra (DRS) were obtained for the dry-pressed disk samples using a scan UV-vis spectrophotometer (Hitachi U-3010) equipped with an integrating sphere assembly, using BaSO₄ as reflectance sample. The spectra were recorded at room temperature in air, in the range of 200–800 nm. Specific surface area and pore diameter of samples were measured by the BET method using N₂ adsorption measurement (ASAP 2020 V3.01H) on nitrogen adsorption at 77 K after the pretreatment at 393 K for 2 h. The specific surface area was calculated by the Brunauer-Emmett-Teller (BET) method, and pore size distribution was obtained from desorption plots by a Barrett-Joyner-Halenda (BJH) analysis. X-ray photoelectron spectroscopy (XPS) spectra were acquired with a Kratos Axis Ultra DLD spectrometer (Kratos Analytical-A Shimadzu group company) using a monochromatic Al Kα source (1486.6 eV). The analyzer uses hybrid magnification mode (both electrostatic and magnetic) and take-off angle is 90°. Under slot mode, the analysis area is 700 × 300 μm. Analysis chamber pressure is less than 5 × 10⁻⁹ Torr. Pass energy of 160 eV and 40 eV is normally used for survey spectra and narrow scan spectra, respectively. The BE scale was calibrated according to the C 1s peak (284.8 eV) of adventitious carbon on the analyzed sample surface.

2.3. Measurements of Photocatalytic Activity

The photocatalytic activity of samples was evaluated in terms of the degradation of methyl orange (MO, 10 mg/L). The photocatalyst (0.05 g) was added into a 100 ml quartz photoreactor containing 50 ml of a MO solution. The mixture was stirred for 0.5 h in the dark in order to reach the adsorption-desorption equilibrium. Ultraviolet light was obtained by a 200 W high-pressure mercury lamp with main emission wavelength 313 nm as light source and the distance between the light and the reaction tube is 20 cm. After a given irradiation time, the samples were withdrawn for subsequent analysis with a UV-vis spectrophotometer (Shanghai 760).

3. Results and Discussion

The XRD pattern of the mesoporous SnO₂ is illustrated in Figure 2 to confirm the constitution of the product. It shows eight characteristic diffraction peaks at 26.6°, 33.9°, 37.9°, 51.8°, 54.8°, 61.9°, 64.7°, and 65.9°, corresponding to the (110), (101), (200), (211), (220), (310), (112), and (301) crystalline planes of SnO₂ (JCPDS card number 41-1445). No diffraction peaks of other impurities were detected, indicating that MoO₃ exists in the product in amorphous form. The crystallite size calculated from the widened (110) diffraction peak at 2θ = 26.6° according to the Scherrer equation is 5.1 nm, which is in good accord with the thickness observed on HRTEM (Figure 3).

Figure 2: XRD patterns of SnO₂@MoO₃ and mesoporous SnO₂.

Figure 3: (a) TEM image of SnO₂@MoO₃; (b) HRTEM image of SnO₂@MoO₃; (c) TEM image of mesoporous SnO₂; (d) HRTEM images of image of mesoporous SnO₂. Inset shows the corresponding SAED patterns.

The morphology and microstructure of the prepared SnO₂@MoO₃ and mesoporous SnO₂ were examined by TEM measurements. Figures 3(a) and 3(b) show representative SnO₂@MoO₃ samples and Figures 3(c) and 3(d) show representative mesoporous SnO₂, which aggregated from ultrafine nanoparticles with a typical diameter of 6 nm. It can be clearly seen that amorphous MoO₃ layer was coated onto SnO₂ nanoparticles in SnO₂@MoO₃ in Figure 3(b), confirming that the formation mechanism of SnO₂/MoO₃ is exactly as described in Figure 1. The SnO₂ nanoparticles with a size of about 5-6 nm can be identified. The SAED (inset of Figure 3(b)) image presents the polycrystalline behavior of the materials due to the spot and ring patterns. The spacing between two adjacent lattice fringes are 0.24 nm and 0.17 nm, corresponding well to the spacing of the (200) and (220) plane of SnO₂ (Figure 3(d)), respectively. This is perfectly in agreement with the XRD analytical results. Since SnO₂ is insoluble and MoO₃ is highly soluble in NaOH solution, the content of Mo atoms in SnO₂@MoO₃ is reduced from 16.6% before dissolution to 6.9% after dissolution in NaOH solution (Figure 4), which suggests that plays the role of the protective and stabilizing agent coated onto SnO₂ to inhibit the growth of the particles during calcination.

(a)

(b)

Figure 4: The EDX patterns of the content of Mo atoms in SnO₂@MoO₃ (a) and mesoporous SnO₂ (b).

The nitrogen adsorption-desorption isotherm (a) and BJH-derived pore size distributions (b) of the sample are shown in Figure 5. Its micro/mesoporous properties are indicated by the hybrid isotherm (I + IV) type in Figure 5(a). The sample has a BET surface area of 132 m² g⁻¹, a narrow mesoporous structure with an average pore diameter (Figure 3(b)) of 3.5 nm, and a pore volume of 0.12 cm³ g⁻¹. The BET surface area of samples increased to 132 m² g⁻¹ from 21 m² g⁻¹, and the average pore diameter reduced from 4.2 nm to 3.5 nm after dissolution with NaOH, which suggests that MoO₃ plays the role of the protective and stabilizing agent coated onto SnO₂ to inhibit the growth of the particles during calcinations.

(a)

(b)

Figure 5: Nitrogen adsorption-desorption isotherm (a) and pore size distribution (b).

The diffuse reflectance spectra of the samples show photoresponse in visible light region (Figure 6). The absorption edge of mesoporous SnO₂ is estimated to be 420 nm with a band gap of 3.0 eV, which is less than the bulk band gap (3.6 eV). Meanwhile, it can be clearly observed that SnO₂@MoO₃ exhibits a higher absorbance in the visible light range than mesoporous SnO₂. This may be caused by the fact that MoO₃ shell can serve as a component in the composites and the interfacial coupling effect between MoO₃ and SnO₂ particles is possibly for the red-shift of the band gap. Such an enhancement in the visible light harvesting, including absorbance and scattering, can increase the number of photogenerated electrons and holes to participate in the photocatalytic reaction and enhance the photocatalytic performance [15].

Figure 6: Diffuse reflectance spectra of SnO₂/MoO₃ and mesoporous SnO₂.

The surface chemical composition and chemical states of mesoporous SnO₂ were further confirmed by X-ray photoelectron spectroscopy (XPS). Only Sn, Mo, C, and O species were detected (Figure 7(a)). In Figure 7(b), the Sn3d5 binding energy peaks are observed at ~486.7 and ~495.1 eV, corresponding to the spin orbit of Sn3d5/2 and Sn3d3/2, which suggests that Sn in the samples exists in a tetravalent-oxidation state [16]. The Mo 3d core level spectrum of the MoO₃ consists of a spin orbit doublet with peaks at 232.6 and 235.8 eV, associated with Mo cations in the higher oxidation state (Mo⁶⁺) (Figure 7(c)) [17]. Additionally, the peak with an O1s binding energy around 530.8 eV is attributed to oxygen in the SnO₂ crystal lattice, which corresponds to the Sn–O–Sn bonds [18], while the other peak positioned at 530.4 eV should be ascribed to the typical Mo−O bond [19].

(a)

(b)

(c)

(d)

Figure 7: (a) XPS survey spectra of mesoporous SnO₂. High-resolution XPS of (b) Sn3d, (c) Mo3d, and (d) O1s spectra.

The photocatalytic activities of the investigated samples were evaluated by measuring the time-dependent degradation of MO in an aqueous catalyst suspension. Figure 8 illustrates the relative concentration C/C ₀ of MO as a function of time under ultraviolet light irradiation in the presence of the catalysts. Prior to irradiation, the suspension of the catalyst and dye solution was stirred in the dark for 0.5 hours to reach the equilibrium adsorption. It was noteworthy that the adsorption of MO was found to gradually increase with the increase of Mo content and MO could be completely decolorized after 2.5 hours.

Figure 8: Photodegradation of MO under ultraviolet light irradiation by SnO₂@MoO₃ and mesoporous SnO₂.

In order to evaluate the photocatalytic activity of the synthesized mesoporous SnO₂, photocatalytic degradation of methylene blue (MB) was also studied under ultraviolet light irradiation. Mesoporous SnO₂ also performed on photocatalytic activity of degradation of MO. The effect of the pH value of the MO solution on the photocatalytic activity of mesoporous SnO₂ was tested. It can be observed that the pH value can significantly affect the photocatalytic activity. The degradation rates are 60% and 100% under the conditions of pH = 4 and pH = 7, respectively, while it is only 10% when the pH value is further increased to 9.

4. Conclusion

In summary, we have synthesized SnO₂ nanoparticles 5-6 nm in size with the assistance of in aqueous solution at room temperature and assembled them into mesoporous materials. Mesoporous SnO₂ shows photocatalytic activities by the degradation of MO in aqueous solution under UV light irradiation.

Conflict of Interests

The authors declare that there is no conflict of interests regarding the publication of this paper.

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