International Scholarly Research Notices

Volume 2014 (2014), Article ID 123194, 6 pages

http://dx.doi.org/10.1155/2014/123194

Research Article

Electrochemical Synthesis of Magnesium Hexaboride by Molten Salt Technique

S. Angappan,¹ N. Kalaiselvi,² R. Sudha,¹ and A. Visuvasam¹

¹CSIR-Central Electrochemical Research Institute, Karaikudi 630006, India

²Department of Physics, Selvam Arts and Science College, Namakkal 637003, India

Received 24 March 2014; Revised 23 May 2014; Accepted 26 May 2014; Published 31 August 2014

Academic Editor: Sarkarainadar Balamurugan

Copyright © 2014 S. Angappan 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.

The present work reports electrochemical synthesis of MgB₆ from molten salts using the precursor consists of LiF–B₂O₃–MgCl₂. An attempt has been made to synthesize metastable phase MgB₆ crystal by electrolysis method. DTA/TGA studies were made to determine the eutectic point of the melt and it was found to be around 900°C. The electrolysis was performed at 900°C under argon atmosphere, at current density of 1.5 A/cm². The electrodeposited crystals were examined using XRD, SEM, and XPS. From the above studies, the electrochemical synthesis method for hypothetical MgB₆ from chloro-oxy-fluoride molten salt system is provided. Mechanism for the formation of magnesium hexaboride is discussed.

1. Introduction

Rare earth and alkaline earth metal borides belong to the group of nonoxide type metal-like compounds and have high melting point, high chemical stability, stable specific resistance, low expansion coefficient at certain temperature ranges, diverse magnetic orders, and high neutron absorbability [1, 2]. They have possessed excellent corrosion and wear resistance, chemical inertness, and thermal shock resistance more than that of oxide ceramics [3, 4]. The alkaline earth hexaborides were long thought to be simple polar semiconductors with single particle gap energy of several tenths of an eV and the energy gap is narrow as well as indirect band gap ( Ry).

Electrochemical synthesis of Mg–B system from molten salts is an economic feasible and environmental friendly way for the preparation of different binary phases [5]. Particularly, the Mg–B system was reported early [6, 7] to contain five phases, whereas Serebryakova [8] reported only four phases. Borides can exist as a wide range of compositions and display structural features, which depends strongly on the metal and boron ratio. Markowsky et al. proposed formation of three phases with higher B content as the result of thermal decomposition of MgB₂: (1) MgB₆, (2) unknown, and (3) MgB₁₂ [9]. However, Duhart reexamined these data and claimed that phase 1 corresponds to MgB₄ and phase 2 to MgB₆ and the formation of MgB₁₂ (phase 3) was not confirmed [10]. MgB₆ and MgB₄ do not exist as individual phases and obviously are metastable with rather long equilibration times. According to Somsonov et al. [11], Mg–B system has four stable borides: MgB₂, MgB₄, MgB₆, and MgB₁₂. Mg–B system contains the phases of MgB₂, MgB₄, MgB₆, MgB₁₂, and Mg₂B₁₄. So the Mg–B system is known as multiphase system. The aim of the present work is to study whether the thermodynamically unstable MgB₆ [12, 13] could be prepared as thermally stable compound by electrochemical synthesis method.

2. Experimental Procedure

The mixture of the salts LiF (12.95 mol%), B₂O₃ (22.27 mol%), and MgCl₂ (17.14 mol%) (analytical grade from Merck, India) was taken as an electrolyte in high-density graphite crucible and acts as an electrolyte cell as well as anode for the electrolytic process. The Molybdenum rod of 1 cm diameter fitted to a stainless steel rod is used as cathode. The crucible was filled with the stoichiometric quantities of electrolyte salts, which were dried at 500°C under argon atmosphere. The whole assembly was placed in an inconel reactor, which was kept in an electrical heating furnace with thermocouple. The experimental setup for the electrosynthesis of magnesium hexaboride is described elsewhere [14–17]. Then the salts were melted slowly under a continuous flow of argon gas. The melt was equilibrated at 900°C for one hour before proceeding electrolysis [15–17]. The bath was preelectrolyzed at 2.0 V for one hour to remove the impurities and moisture prior to electrolysis. The cathode was centrally positioned at the electrolytic cell. Experiment was carried out at current density of 1.5 A/cm² with the molar ratio of Mg : B as 1 : 6. After 5 hours of electrolysis the cathode was removed and the deposit was cooled in atmosphere. The deposit was then scraped off and the electrolyte adhering to it was leached with warm 5% HCl solution. Finally washing was done with distilled water for several times, the weight of the deposit was determined, and the nature of the powder was analyzed.

The phase formation and the structural details of the synthesized compound were characterized by X-ray powder diffraction (XRD) using CuKα ( Å) radiation with value range of 20 to 90 using PAnalytical X’pert powder diffractometer. Differential thermal analysis and thermogravimetric analysis (TGA/DTA) of the reaction mixture was done using Rigaku Thermal—Plus TG 8120 with heating speed 20°C/min in a flow of air. The Fourier transform infrared (FTIR) spectra were recorded in the range of 400 to 4000 cm⁻¹ using Perkin Elmer UK Paragon—500 spectrometer. Scanning electron microscopy (SEM) was employed for the morphological studies using JEOL JSM 3.5 CF Japan make model. UV Visible Spectrophotometer was employed for the absorbance study using JASCO Model 7800 UV Visible Spectrophotometer. Studying the binding energy of boron and magnesium was done using X-ray photoelectron spectroscopy Thermo Scientific UK Multilab 2000.

3. Results and Discussion

Figure 1 presents the powder XRD pattern of the MgB₆ synthesized by molten salt technique. The lattice constant value  Å is determined from the XRD data and is well matched with the reported value ( Å) [18–20] for MgB₆ (JCPDS data card number 08-0421) existing in body centered cubic crystal structure (the space group Pm3m) [20]. But indexing the plans for MgB₆ is difficult because the information on its lattice parameters and structure system is not available in 08-0421. The main building blocks of the MgB₆ structure are B₆ octahedra. Other than MgB₆ some additional traces of MgO are also present at and 62.5° due to the partial oxidation of Mg [21]. The crystalline size is found to be 42 nm calculated by using Debye-Scherrer equation as follows:

Figure 1: XRD pattern for MgB₆.

where is the Scherrer constant usually taken as 0.9, is the wavelength characteristics of the Cu-Kα radiation ( Å), is the full width at half-maximum (FWHM) in radiations, is the reflecting angle, and is the crystal size.

The TGA/DTA curve for the reaction mixture is shown in Figure 2. The figure showed that the eutectic point of the melt is found to be 820°C. The melt temperature is kept approximately 80°C higher than the eutectic point to reduce the melt viscosity. The LiF is used to increase the fluidity and electrical conductivity of the melt. Its decomposition potential is more cathodic than any other salts chosen. A gradual weight loss observed up to 497°C may be due to the removal of moisture and inbound water associated with the salts. The weight gain which is observed up to 761°C from 497°C, due to B₂O₃, begins to turn into liquid (melting point 450°C) in the heating process. These reactants whether in the liquid or gaseous state play a crucial role in determining the shape of the final product. Further, this weight gain is mainly due to the oxidation of the reactants (2) [22, 23]. MgCl₂ stretches excess Mg and also increases the electrical conductivity of the melt. This excess Mg combines with O forming MgO (from residual B₂O₃). The formation of 2MgCl₂·3B₂O₃ is due to the solid-state reaction between residual B₂O₃ and MgCl2, turn into molten state (melting point of MgCl₂: 708°C) is confirmed by an exothermic peak at 761°C. Finally, the reactants can be oxidized thoroughly at 761°C [24]. Further weight loss observed up to 1000°C is responsible for the transformation of the reactants into desired product. In the DTA curve, a sharp exothermic spike is observed at 742°C which may also be verified by confirming this process. This is gratuitous to the DSC curve (Figure 3) at 745°C; a sharp exothermic spine is observed that the heat of decomposition of salts is about 513.3 J/g.

Figure 2: TG/DTA curve for MgB₆.

Figure 3: DSC curve for MgB₆.

The reaction was carried out for MgB₆ in MgCl₂–B₂O₃–LiF system; the main chemical reactions are

The overall reaction is

Trace amount of the unreacted intermediate MgO was present in the synthesized compound as 0.6% and the remaining 99.4% was MgB₆ as depicted from XRD pattern.

The XPS spectrum for B 1s is shown in Figure 4(a). The higher binding energy value for B 1s exists at 198.6 eV. This reflects contributions from both trigonal BO₃ and tetrahedral BO₄ groups. The electron transfer would come from trigonal B 1s to B–O orbital and from the unfilled tetrahedral B 2p orbital to B–O [25, 26]. This B 1s → resonance as expected for sp²-bonded boron incorporated in the crystal [27]. Figure 4(b) shows the Mg 1s spectra for MgB₆ at 1314 eV revealed that the auger spectral distribution over an extruded energy range far from the threshold; there is an extra energy for Mg rich compound [28]. Figure 4(c) shows the O 1s spectrum for MgB₆ existing at 544 eV. This may be due to the core-hole Rydberg states containing O 1s → resonance [29, 30]. Figure 4(d) shows C 1s spectrum at 296 eV and reveals energy transitions between a carbon core level and an antibonding molecular orbital [31]. The surface is contaminated due to exposure to air during the processing of the sample.

(a)

(b)

(c)

(d)

Figure 4: XPS spectra for (a) B 1s, (b) Mg 1s, (c) O 1s, and (d) C 1s.

The Mg²⁺ cations in MgB₆ complex species have C6v pyramidal structures interacting with a planar hexagonal dianion. The bonding between these two may be due the electrostatic attraction [12].

The FTIR spectrum of MgB₆ is shown in Figure 5. The O–H stretching vibrations of water crystallization are represent at 3743 and 3413 cm⁻¹, respectively. The absorption at 2225 cm⁻¹ is assigned to O–H stretching vibration of cluster of water molecules of crystallization, respectively. The characteristic peak of Mg–B is observed at 1642 cm⁻¹ [32]. Longitudinal optic mode frequency of Mg–O is observed at 705 cm⁻¹; this MgO as impurity phases is also observed in the XRD pattern. The bending vibration for MgB₆ is observed at 437 cm⁻¹. The bending mode of Mg–B of BO₄ anion is assigned to 499 cm⁻¹. The asymmetric stretching vibration of Mg–B of BO₄ anion is observed at 1021 cm⁻¹. The asymmetric stretching vibration of B–O bond of trigonal BO₃ units is observed at 1367 cm⁻¹. The frequencies observed in the spectrum are in good agreement with the reported values [33, 34].

Figure 5: FTIR spectrum of MgB₆.

The SEM image of the sample is shown in Figure 6. The microstructure indicates that the particle diameters are in the range 4–8 μm. From the microstructure, the molten regions are clearly visible, which give the clear indication of MgB₆ formation. The white regions in SEM represent the impurity phase MgO present in the sample [35, 36]. The present study reveals the formation of MgB₆ phase as cubic crystal structure.

Figure 6: SEM image of MgB₆.

The mechanism of hexaboride formation was proposed by many authors [12, 14–17, 37–47]. According to Li and Jin, the negative charged boron atoms and the positive charged alkaline earth metal atoms form complexes of M²⁺ metal cation and dianion due to electrostatic attraction. They also suggested that the metal cations M²⁺ have definite role on stabilizing the dianion [12]. Kaptay and Kuznetsov reported that the boron components are dissolved in ionic form in the melt, to form boride phase on the cathode joint with metal cations [37]. Jose et al. reported the “unstable stoichiometric way” for the deposition of Barium hexaboride [14]. We reported earlier that the electrolytically dissociated metal and B ions deposit on the cathode as CeB₆ and SmB₆, respectively [15, 16]. We also reported in our earlier study on CaB₆ that the calcium and boron are reduced at the cathode to form submicron sized crystals [17]. As reported by Chen et al. [38], the formation of MgB₆ at 900°C as one of the secondary phases along with MgB₄ due the volatile nature of Mg at this temperature resulted in Mg deficiency on in situ Cu doping of MgB₂. The commonly accepted mechanism of boron deposition in molten salts is a single-step three-electron electrochemical reaction [39–43]. Gloor et al. investigated the multiexciton bound state of molecules in divalent hexaborides. They proposed that the larger energy gain per one electron-hole pair decreases the semiconducting gap and produced intermediate phase. This may be the reason for the formation of intermediate phase MgB₆ [44]. Li et al. described the diffusion of Mg vapour into boron creating a complex of Mg–B supersaturated solution, encompassing the formation of nonequilibrium MgB₆ [45]. Lee et al. and J. Q. Li also authenticated with S. Li [45] and postulated that the path of the reaction of supersaturated Mg–B cluster complex via spinodal decomposition leads to the formation of hypothetical phase MgB₆ [46, 47].

4. Conclusion

In summary, the electrochemical synthesis of hypothetical magnesium hexaboride by molten salt technology is presented. Various mechanisms for the formation of magnesium hexaboride are discussed. It is believed that the supersaturated MgB₆ cluster complex is postulated for the metastable magnesium hexaboride compound. Further experimental evidence is more needed to explore the thermodynamically unstable magnesium hexaboride.

Conflict of Interests

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

Acknowledgments

The authors would like to thank the Director of CSIR-CECRI for his keen interest and encouragement and staff of EMP Division for their support. S. Angappan acknowledges the Council of Scientific and Industrial Research (CSIR), India, for providing the financial assistant to the project EMPOWER (OLP 0060).

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