Journal of Nanomaterials

Journal of Nanomaterials / 2010 / Article

Research Article | Open Access

Volume 2010 |Article ID 589372 |

Amartya Chakrabarti, Tao Xu, Laura K. Paulson, Kate J. Krise, John A. Maguire, Narayan S. Hosmane, "Synthesis of Boron Nanorods by Smelting Non-Toxic Boron Oxide in Liquid Lithium", Journal of Nanomaterials, vol. 2010, Article ID 589372, 5 pages, 2010.

Synthesis of Boron Nanorods by Smelting Non-Toxic Boron Oxide in Liquid Lithium

Academic Editor: Zhi-Li Xiao
Received25 Nov 2009
Accepted16 Feb 2010
Published15 Apr 2010


In contrast to the conventional bottom-up syntheses of boron nanostructures, a unique top-down and greener synthetic strategy is presented for boron nanorods involving nontoxic boron oxide powders ultrasonically smelted in liquid lithium under milder conditions. The product was thoroughly characterized by energy dispersive X-ray analysis, atomic emission spectroscopy, thermogravimetric analysis and, UV-Vis spectroscopy, including structural characterization by transmission electron microscopy (TEM).

1. Introduction

Elemental boron, by virtue of its unique electron-deficient nature, superhardness (Knoop: 2160–2900), and high melting point ( 2200°C), has been found to be very useful in a diverse range of industrial applications including semiconductors, wear-resistant additives and protective coatings, as well as high-temperature devices [1]. Boron-based nanomaterials have attracted a wide range of interests in a number of applications [2]. For example, boron-doped diamond nanopowder has been synthesized and its electrochemical behavior studied; it is proved to be an excellent electrocatalyst support material [3] and also an electrode material [4]. Boron-based nanoparticles are now being extensively investigated as a boron source in boron neutron capture therapy [58]. The high surface-to-volume ratio of boron nanoparticles coupled with boron’s high energy content makes such nanoparticles attractive as fuel additives in conventional hydrocarbon fuels for airbreathing propulsion systems [9, 10]. Their robust thermal and electrical stability, compared to metal nanowires, should make 1-dimentional boron nanostructures such as nanowires, nanorods, nanobelts, or nanotubes, as promising materials for nanoscale electrically conducting interconnects in nanoelectronic devices [11, 12].

Despite the rapid growth of their applications, limited progress has been made in the synthesis of boron nanomaterials. Nearly all synthetic methods for boron nanomaterials are based on the bottom-up strategy that inevitably involves the usage of gas phase decomposition of the highly toxic and flammable precursory gases under drastic reaction conditions. For example, synthesis of amorphous boron nanoparticles from furnace heating of diborane at 700°C was reported in early 1950s [13]. The product had a large size distribution. Later, laser heating and arc discharge was employed to narrow down the size distribution of the boron nanoparticles [14, 15]. On the other hand, synthesis of boron nanowires was first reported by Ruoff and coworkers through the decomposition of diborane on NiB powder as a catalyst at 1100°C [16]. In a similar fashion, boron nanorods were fabricated by reduction of diborane on a thin film of Al catalyst over silicon substrates at the temperature range of 750–900°C [17]. While boron nanoribbons were prepared recently through catalyst-free pyrolysis of diborane at 630–750°C [18], crystalline boron nanobelts were formed via laser ablation techniques at temperatures from 700 to 1000°C [19]. Alternatively, BCl3 was used as a boron precursor to synthesize boron nanotubes at 870°C with hydrogen gas as reducing agent [20]. To date, some progress has been made in moderating the reaction conditions including a room temperature solution-based synthesis of boron nanoparticles through reduction of boron tribromide utilizing sodium naphthalenide [21]. Nonetheless, the boron precursors in all of the reported syntheses are highly toxic. Therefore, a greener and energy-efficient synthetic strategy is warranted for the synthesis of boron nanostructures.

In this context, it is important to note that a top-down method was reported for nanoporous platinum from its oxide [22]. In this method, lithium was used to intercalate through the matrix of PtO2 microparticles electrochemically via the reductive smelting process: . The by-product Li2O could be removed by extraction in acidic aqueous solution or water in order to isolate nanoporous platinum. We also demonstrated a bottom-up strategy for the synthesis of Pt nanoparticles directly from bulk Pt using Li as a solvent [23]. These results posed a question whether this methodology could be extended to produce boron nanostructures as well. Although the magnesium metal has been known to be a good reducing agent in the production of bulk boron from boron oxide [24], in the production of boron nanostructures we chose to utilize the lithium metal due to the fact that Li (reduction potential 3.07 V) is a much stronger reducing agent than Mg (reduction potential 2.37 V) and assures the feasibility of the reaction. In addition, the corrosive intercalation of liquid Li into other materials is a notorious flaw when it is used as a coolant in nuclear reactors [25, 26], but is taken here as an advantage to produce nanostructured boron from boron oxide, which is a nontoxic starting material that is conveniently available from the major natural sources of boron, for example, borax. Figure 1 illustrates the synthetic strategy of the top-down methodology.

2. Experimental Section

2.1. Synthesis of Boron Nanorods

500 mg of B2O3, previously dried overnight at 110°C under vacuum, was thoroughly ground inside an argon glove-box using a mortar and pestle. Subsequently, metallic lithium was weighed in a 6-fold molar ratio to B2O3, in a nickel crucible and melted at 200°C. In the Ar glovebox, B2O3 powders were added under sonication into the molten Li and temperature of the mixture was increased up to 250°C and maintained at that temperature under a tip-sonication for 2 hours. The mixture was cooled down to room temperature and taken out of the glovebox. Methanol was added to this mixture in order to remove any unreacted lithium. The resulting solution was filtered, washed thoroughly with hot water, dilute potassium hydroxide solution, dilute hydrochloric acid solution followed by repeated washing with cold water. The brownish product was then dried under vacuum at 70°C for 24 hours before characterization. Approximately 150 mg of product was collected after complete drying in vacuo.

The solid product was subjected to all available characterization techniques. Transmission electron microscopy (TEM) imaging of the purified product was done by a Hitachi H-600 (75 kV) instrument and elemental analysis of the samples was done through energy dispersive X-ray (EDX) studies using a field emission scanning electron microscope (Hitachi S-4700-II), and identified the product to be the boron nanorods.

Since the EDX spectrum has not been able to determine any lithium traces present in the boron nanorods sample, we ran an atmoic emission studies using the atomic absorption spectrometer (AAS, Perkin Elmer 3110). About 20 mg of boron nanorods sample was dispersed in 50 mL of deionized water. The atomic emmision was measured for the sample at the characteristic emission wavelength of lithium of 670.8 nm. To get the lithium concentration in the sample, a calibration plot was generated by running several samples of lithium solutions with known concentrations. Four different solutions of known lithium nitrate (1 ppm, 5 ppm, 10 ppm, and 15 pmm) were prepared by diluting the stock custom-grade standard lithium solution ( g/mL) from Inorganic Ventures Inc. in deionized water.

Thermogravimetric analysis (TGA, Perkin-Elmer Pyris 1) was performed on the boron nanorods samples. A known amount of sample (perivously vacuum dried at 70°C for 48 hours) was subjected to a temperature scan from 25°C to 700°C and the corresponding weight losses were recorded.

UV-Vis scpectroscopy (Perkin Elmer Lambda 19) was also carried out on the boron nanorod sample. Boron nanorod sample solution was prepared as a deionized water dispersion using a quartz cell. Deionized water was used as blank reference in the experiment. The solution was subjected to a wavelength scan from 700 nm to 190 nm.

3. Results and Discussion

In the preparatory process of the boron nanorod, the purification part was the key to the synthetic success. Apparently, it was crucial to avoid any formation of lithium borides in the synthesis or at least destroy such a contaminant in the product with proper treatment and washing sequences. According to some earlier work by Serebryakova et al. lithium diboride is not very stable and is easily soluble in methanol; it also decomposes in weak mineral acid solutions [27]. On the other hand, lithium tetraboride is not stable in potassium hydroxide solution. Thus, these observations guided the purification protocol applied in the synthesis of boron nanorods described above. To avoid the vigorous reaction of water with lithium, methanol was first added after completion of the reaction. One of the reasons for not washing the product immediately with water is to avoid the formation of lithium hydroxide which is capable of etching the nickel crucible. The B2O3, being soluble in hot water, was easily removed by washing with hot water. While potassium hydroxide solution was used to remove any lithium tetraboride, dilute HCl solution was used to take away the lithium diborides, if any, as well as to neutralize the basic condition of the solution. Washings were repeated until the product was free of any residual acid.

Figure 2 is the TEM images of the resulting boron materials. Apparently, the dominant feature is the rod-like structures (Figure 2(a)). The preferential formation of boron nanorods over nanoparticles must be associated with the streaming-like ultrasonic propagation [28, 29], which can transfer acoustic momentum efficiently to the liquid lithium [30], leading to a sort of directed lithiation in a B2O3 powder. While in a random insertion of lithum, the dominant resulting structure of boron is believed to be nanoparticles. The TEM images also suggest that the diameters of most of the nanorods exhibit a fairly narrow distribution, ranging between 20 and 40 nm. The length of the rods varies and most of the length of the nanorods fall in the region between 80 and 200 nm, but there are some longer nanorods of more than 500 nm (Figure 2(b)). Some spherical boron nanoparticles embedded in the boron nanorods (Figure 2(c)) were also observed. Nonetheless, we were able to produce boron nanorods in good yields (85%) from B2O3 by this ultrasonic smelting method. This simple and greener process neither involves any harmful and toxic boron precursors nor does it require any severe reaction conditions.

Figure 3 shows the EDX spectrum of the specimen which clearly bears no evidence of containing any elements other than boron (95 at.%) and oxygen (5 at.%). The very trace amount of oxygen found is due to the presence of the inevitable water moisture and oxygen absorbed on the boron nanorods or perhaps trace amount of unreacted B2O3.

The concentration versus signal intensity plot is depicted in Figure 4. When the signal intensity for the boron nanorods sample was fed into the calibration, bearing the trendline of = 0.12x, the lithium concentration for the sample came out to be 1.83 ppm. The atomic ratio of lithium to boron in the sample thus calculated to be less than 0.95%.

Figure 5 exhibits the TGA thermogram of boron nanorod sample. Under inert atmosphere (argon), the boron nanorods sample was thermally stable and did not show any significant weight loss within the experimental temperature range, which demonstrates the absence of any other vulnerable impurities in the prepared sample. However, when heated in air, the sample started to gain weight at temperature above 550°C due to the inevitable oxidation.

There are several reports on the theoretical calculation for the crystal structure and optical properties of boron crystals [31, 32]. The UV-Vis spectra of boron nanorod sample is demonstrated in Figure 6. The peak observed at 198 nm (6.26 eV) closely matches with the values reported by Yang et al. [17]. The peak threshold was observed around 225 nm (corresponding to 5.5 eV) which obtained its maximum at 198 nm (6.26 eV ). Since quartz is transparent in the UV region, the peak is believed to be due to the boron sample.

4. Conclusion

We report here the first top-down synthesis of boron nanorods at low temperature and without usage of any catalysts or flammable and toxic gaseous precursors. Nontoxic boron oxide was reduced by lithum in this ultrasonication assisted synthesis. The purity of the product was confirmed by EDX spectroscopy, atomic absorption spectroscopy, and thermogravimteric analysis; whereas the structural confirmation has been derived from transmission electron microscopy. Bundles of nanorods of a narrow range of diameters, along with some spherical particles, were observed under the microscope. Thus, this work demonstrates an alternative route for low temperature, nonhazardous large-scale synthesis of boron nanomaterials.


T.Xu acknowledges the support of the American Chemical Society Petroleum Research Fund (Type G 46374-G10). The sixth of author thanks the support of the National Science Fundation (CHE-0601023 and CHE-0906179) and the fifth of author thanks the Robert A. Welch Foundation (N-1322). The authors thank Ms. Lori Bross for help with the TEM. The sixth author gratefully acknowledges the second-time Humboldt Research Prize for US Senior Scientists from the Alexander von Humboldt Stiftung and the Inaugural Board of Trustees Professorship Award from Northern Illinois University.


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Copyright © 2010 Amartya Chakrabarti 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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