International Scholarly Research Notices

International Scholarly Research Notices / 2011 / Article

Research Article | Open Access

Volume 2011 |Article ID 692594 | 5 pages | https://doi.org/10.5402/2011/692594

Process for Producing Nano-Alpha-Alumina Powder

Academic Editor: C. Malagú
Received21 Mar 2011
Accepted18 Apr 2011
Published06 Jul 2011

Abstract

This paper is trying to explore the effect of stirring time on the synthesis of nano-α-Alumina particles. In this study, alumina nanoparticles were synthesized through alkoxide route using sol-gel method, where aqueous solutions of aluminum isopropoxide and 0.5 M aluminum nitrate nanohydrate were used for preparing alumina sol. Sodium dodecylbenzen sulfonate (SDBS) was used as the surfactant stabilizing agent. The prepared solution was stirred at different times (24, 36, 48, and 60 hours) at 60°C. The Samples were, then, characterized by X-ray diffraction, thermogravimetry analysis (TGA), differential scanning calorimetry (DSC), scanning electron microscopy (SEM) and Transmission Electron Microscopy(TEM) . The introduction of different stirring times affected the particle size and shape and the degree of aggregation. By increasing the stirring time, (starting from 24 to 48 hours) the particle size decreased, but agglomeration became hard for 60 hours of stirring time. The finest particle size (20–30 nm) was obtained at 48-hour stirring time.

1. Introduction

Alumina is one of the most widely used ceramic materials as catalysts, catalyst supports and absorbents, and also wear resistant coating [1]. It can be prepared through methods such as sol-gel [2, 3], hydrothermal [4], coprecipitation, mechanical milling, vapor-phase reaction and combustion methods [5, 6]. However, nanoscale alpha-alumina (α-Al2O3) powder is difficult to obtain. It is due to two reasons first, α-Al2O3 is in a stable phase after calcining at high temperature, which easily prompts the grain growth of powder and makes it difficult to get nanoscale particles; secondly, α-Al2O3 particles tend to aggregate during dehydration process in wet chemistry method. Therefore, it is necessary to develop a new method to overcome this problem [7, 8]. Sol-gel synthesis offers relatively inexpensive scale processing of mixed oxide materials with a good control over the stoichiometry and morphology which helps to tailor the required materials on atomic scale to suit specific applications [5].

This study tends to synthesize nanosized α-Al2O3 by controlling the particle size, distribution, and shape.

2. Material and Method

Aluminum isopropoxide Al (OC3H7)3 (Merck, German), aluminum nitrate nonahydrate Al (NO3)3·9H2O (Merck, German), and Sodium dodecylbenzen sulfonate (SDBS) (Merck, German) were used as raw materials to prepare nano-α-Al2O3. The starting solution was prepared through using aluminum isopropoxide and 0.5 M aluminum nitrate aqueous solution as a solvent with the water purity of 99% and aluminum isopropoxide in the powder form gradually added to it.

The molar ratio of alumina sol (ALP/ALN) was 3 so that the raw materials can be completely dissolved and provide clear solutions. The solutions were continuously stirred for 24, 36, 48, and 60 hours. Later, Sodium dodecylbenzen sulfonate (SDBS) was added by adjusting the molar ratio between alkoxide and surfactants to 0.1 and stirred for one hour. It is expected that the optimal time for the addition of surfactant is prior to the onset of the nucleation and growth step. The solutions were heated up to 60°C and stirred constantly for evaporation process. Viscosity and color changed as the sol turned into a transparent stick gel. The gels were, then, heat-treated at 90°C for 8 hours. Dried gels were calcined at temperature between 1000 and 1200°C. Finally, the calcined powders crushed by using mortar and pestle.

Phase identifications were performed by X-ray Diffraction (XRD) using nickel-filtered Cu Kα radiation in the range of 2𝜃=1080 with a scanning speed of 5° per minute. The ultrasonic bath was applied to suspend calcined powder in ethanol, and subsequently, few droplets of it were used for microstructure evaluation by Phillips CM12 transmission electron microscopy (TEM) and Cambridge Stereoscan 200 and Leica Cambridge S-360 scanning electron microscopy (SEM). The process steps are illustrated in Figure 1.

3. Results and Discussion

The synthesis of nano-α-Al2O3 was achieved through increasing the stirring time so that the excessive grain growth and aggregation of nanoparticles could be prevented. The XRD analysis (Figure 2) showed the most stable phase, α-Al2O3 occured dominantly at 1200°C.

The observation reported by Hyuk-Joon et al. [9] indicated that completion of the most stable phase of α-alumina occurs at this temperature. During thermal treatment, stable α-Al2O3 phase can be obtained through the following series of phase transformation before conversion to α-Al2O3: hydrousaluminabohemite𝛾𝛿𝜃𝛼(1)(see [12]).

Figure 3 illustrates the TGA curve, at heating rate of 10°C/min in air. There is a sharp decrease observed in specimen weight (~6%) at temperature of <400°C; seemingly, this decrease is due to the elimination of the residual water content which is absorbed on the surface of nanocrystalline bohemite particles [10].

From 400–750°, weight loss of the mat is less than 1%, and also there is less decrease in temperature. So, the volatilization does not happen obviously [11]. From 750 to 1200°C, weight loss is observed again, and the temperature oscillates obviously, and it shows an exothermic reaction.

The DSC curve of the precursor is illustrated in Figure 4. In the temperature region of 25–270°C, a broadened endothermic peak as well as a slight endothermic peak around 279.83°C emerges which is associated with the vaporization of physically bound absorbed water [2] and [12].

Three small exothermal peaks at 420, 456, and 479°C are attributed to the pseudomophic phase transformation of bohemite to γ-Al2O3. [2, 12, 13]. The endothermic peaks at 882 and 953°C are attributed to the phase transformation of γ-Al2O3 to δ-Al2O3 and θ-Al2O3. Also, α-Al2O3 phase formation occurred at around 1035 and 1130 with two exothermic peaks [13]. This is in consistence with the XRD results which indicate that α-Al2O3 phase occurred at 1100–1200°C.

Figure 5 shows SEM micrographs that by increasing the stirring time, the particle become finer and less agglomerated until 48 hour stirring.The particle started to agglomerate and to be more dense in structure at 60 h.

Novakovic and Korthaus [7] and Hasmaliza et al. [5] had reported that drying of the sol invariably leads to agglomeration because the residual salts present in the sol as the water evaporates forms solid bridges between particles. Besides that, the particle size and shape of the α-alumina is determined by the crystal structure of the original hydroxide and the series of phase transformations which occur during calcinations.

The TEM micrographs Figures (6(a), 6(b), 6(c), and 6(d)) of the α-Al2O3 particles show that the Particles, after 24, 36, and 60 hours of stirring, predominantly were in irregular angular shapes. As for the sample with stirring time of 48 hours, the particle shapes were mainly spherical Figure 6(c). The size of particles, after 24 hours of stirring, is in the range of 270–320 nm and had a lot of agglomeration, and the size of particles, after 36 hours of stirring, fell in the range of 250–300 nm, and had a lot of agglomeration, but after 48 hours, the particle sizes were in the range of 20–30 nm and had a good quality of dispersion. After 60 hours of stirring, the sizes of particles were in the range of 150–200 nm and a lot of agglomeration and only little dispersion were observed.

Takhashi et al. [8] found that during stirring of the solution, the viscosity increased; therefore, the particle size improved but, due to the spinner revolution, the particle size decreased. As it proceeded, after 48 hours, more water evaporated from the sol, the supersaturated solution, thus, supplied the material necessary to bond colliding particles and form agglomerates. According to Lin et al. [14], agglomeration of solid products from two liquid ionic solutions A and B is as follows:An++BnC(2) This reaction involves the instantaneous (mixing-controlled) chemical reaction, subsequent crystallization of the product (i.e., nucleation and growth of crystals), and its agglomeration.

At low supersaturation, there are usually negligible effects of agglomeration, and the crystals’ size distribution is mainly affected by the competition between the nucleation and the growth of the crystal. However, at high supersaturation, the process is dominated by agglomeration.

As it proceeds, more water evaporates from sol, the supersaturated solution, thus, supplies the material necessary to bond colliding particles and form the agglomerates. Local concentrations, also, determine the electrical interaction between the small colloidal particles because most particles in aqueous media are charged and the resulting repulsion force depends on the solution composition.

Hence, due to these reasons, the agglomeration process enhances after 60 hours of stirring time, and there was strong agglomeration observed in the samples. This is in agreement with the observation of this study as shown in Figure 6(d).

Consequently, despite the high temperature (1200°C), the obtained particle size ranged between 20 and 30 nm after 48 hours of stirring time. Furthermore, Wright and Sommerdijk [15] explained that the colloidal particles tend to obtain surface charge by ionization or adsorption of ions or polar molecules from the solution in stable sols. The charged surface layer, in turn, attracts a second more diffuse layer of ions of opposite charge in the neighboring solution. The van der waals attractive forces which potentially lead to aggregation fall as 𝑟6. On the other hand, the electrostatic repulsions vary as 𝑟1, between the link-charged ions of the diffuse layers around the nearest charged colloid particles.

Therefore, the repulsions dominate the vanderwaals attractions, and the particles are stable in opposition to the aggregation unless the thickness of the diffuse layer can be significantly decreased.

The main way in which the diffuse layer thickness can be decreased is raising the ionic strength of the solution, and in particular, increasing the charge on the counterion. Hence, the stirring time was effective in controlling the size of the particles and their degree of aggregation.

4. Conclusions

In this research, the sol-gel method for the synthesis of aluminum oxide from aluminum alkoxide complexes was explained. However, selecting and controlling the exact stirring time for controlling the size of particles and the degree of aggregation are important. The evolution in the alumina precursor involved the decomposition which was followed by amorphous-to-γ-Al2O3 and γ-to-α-Al2O3 phase transformation. Nano-α-Al2O3 was observed at 1200°C, when the transformation had just completed. The microstructural observation showed nanoscale α-Al2O3 powder with 48 hours of stirring time were obtained in the range of 20–30 nm. Moreover, the particle size after 48 hours, in comparison with 24, 36, and 60 hours, generated a better dispersion as well as finer particles.

Acknowledgment

The authors would like to thank the Ministry of Science, Technology, and Innovation, Malaysia, University Putra Malaysia, and University Sains Malaysia in providing fund and support for this work.

References

  1. R. Aghababazadeh, A. R. Mirhabibi, J. Pourasad, A. Brown, A. Brydson, and N. Ameri Mahabad, “Economical synthesis of nanocrystalline alumina using an environmentally low-cost binder,” Journal of Surface Science, vol. 601, no. 13, pp. 2864–2867, 2007. View at: Publisher Site | Google Scholar
  2. L. Jiang, P. Yubai, X. Changshu, G. Qiming, and J. Jingkun, “Low temperature synthesis of ultrafine α-Al2O3 powder by a simple aqueous sol–gel process,” Ceramics International, vol. 32, no. 5, pp. 587–591, 2005. View at: Publisher Site | Google Scholar
  3. G. M. Ming, J. Z. Ying, and L. X. Zi, “A new route to synthesis of γ-alumina nanorods,” Materials Letters, vol. 61, no. 8-9, pp. 1812–1815, 2007. View at: Publisher Site | Google Scholar
  4. D. G. Wang, F. Guo, J. F. Chen, H. Liu, and Z. Zhang, “Preparation of nano aluminium trihydroxide by high gravity reactive precipitation,” Chemical Engineering Journal, vol. 121, no. 2-3, pp. 109–114, 2006. View at: Publisher Site | Google Scholar
  5. M. Hasmaliza, S. S. How, and S. Rahayu, “α-Alumina nanoparticle synthesize through sol-gel isopropoxide system,” in Proceedings of the International Conference on Applied Production Technology (APT '07), Beijing, China, 2007. View at: Google Scholar
  6. L. T. Geik, Y. L. Kong, and A. K. M. Wan, “Synthesis and characterization of sol-gel alumina nanofibers,” Journal of Sol-Gel Science and Technology, pp. 1–17, 2007. View at: Publisher Site | Google Scholar
  7. R. Novakovic and B. Korthaus, Advanced Ceramics for Use in Highly Oxidizing / Corrosive Environment, Trans Tech Publications, Switzerland.
  8. N. Takahashi, N. Kakuta, A. Ueno, K. Yamaguchi, and T. Fujil, “Characterization of iron oxide thin film prepared by the sol-gel method,” Journal of Materials Science, vol. 26, no. 2, pp. 497–504, 1991. View at: Publisher Site | Google Scholar
  9. Y. Hyuk-Joon, W. J. Jin, T. K. Iu, and S. H. Kug, “Temperature formation of α-alumina by doping of an alumina sol,” Journal of Colloid and Interface Science, vol. 211, no. 1, pp. 110–113, 1999. View at: Publisher Site | Google Scholar
  10. C. C. Yong and J. Wang, “Mechanical—activation—triggered Gibbsite—to–Bohmite Transition and Activation—derived Alumina powders,” Journal of the American Ceramic Society, vol. 84, no. 6, pp. 1225–1230, 2001. View at: Google Scholar
  11. A. Sedaghat, E. Taheri-Nassaj, and R. Naghizadeh, “An alumina mat with a nano microstructure prepared by centrifugal spinning method,” Journal of Non-Crystalline Solids, vol. 352, no. 26-27, pp. 2818–2828, 2006. View at: Publisher Site | Google Scholar
  12. H. Arami, M. Mazloumi, K. Khalifehzadeh, and S. K. Sadrnezhaad, “Bundles of self-assembled boehmite nanostrips from a surfactant free hydrothermal route,” Journal of Alloys and Compounds, vol. 461, no. 1-2, pp. 551–554, 2008. View at: Publisher Site | Google Scholar
  13. Y. K. Park, E. H. Tadd, M. Zubris, and R. Tannenbaum, “Size-controlled synthesis of alumina nanoparticles from aluminum alkoxides,” Materials Research Bulletin, vol. 40, no. 9, pp. 1506–1512, 2005. View at: Publisher Site | Google Scholar
  14. L. L. Sather, C. J. Lin, K. J. Lee, and N. J. Sather, “Slow motion of two spheres in a shear field,” The Journal of Fluid Mechanics, vol. 43, pp. 45–47, 1970. View at: Publisher Site | Google Scholar
  15. J. D. Wright and N. A. J. M. Sommerdijk, Sol-gel Materials Chemistry and Applications, vol. 33431, Boca Raton, Fla, USA, 2001.

Copyright © 2011 Fatemeh Mirjalili 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.


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