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Fast Synthesis of Fine Boron Carbide Powders using Electromagnetic Induction Synthesis Method

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01 December 2023

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04 December 2023

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Abstract
Boron carbide (B4C) powders with defined stoichiometry, high crystallinity, minimal impurity content, and a fine particle size are imperative for realizing the exceptional properties of this compound in advanced high-technology applications. Nevertheless, achieving the desired stoi-chiometry and particle size using traditional synthesis methods, which rely on prolonged, high-temperature processes, can be challenging. The primary objective of this study is to syn-thesize fine B4C powders characterized by high crystallinity and a sub-micron particle size, em-ploying a fast, and energy-efficient method. B4C powders are synthesized from elemental boron and carbon in a high-frequency induction heating furnace using the Electromagnetic Induction Synthesis (EMIS) method. The rapid heating rate achieved through contactless heating promotes the ignition and propagation of the exothermic chemical reaction between boron and carbon. Additionally, electromagnetic effects accelerate atomic diffusion, allowing the reaction to be completed in an exceptionally short timeframe. The grain size and crystallinity of B4C can be finely tuned by adjusting various process parameters, including the post-ignition holding temperature and the duration of heating. As a result, fine B4C powders can be synthesized in under 10 minutes. Moreover, these synthesized B4C powders exhibit high resistance to oxidation when exposed to air.
Keywords: 
Subject: Chemistry and Materials Science  -   Materials Science and Technology

1. Introduction

Boron carbide (B4C) has outstanding properties such as high hardness, low density, high melting point, high temperature stability, good thermoelectric characteristics, and high neutron absorption, making this material attractive for a wide range of applications especially in severe environments, including aerospace, nuclear reactors, and high-temperature thermoelectric conversion [1,2,3]. B4C is commonly used in nuclear applications as a neutron absorber [4]. The most recent applications of B4C include boron neutron capture therapy [5], microwave absorbers [6] and photocatalysts [7]. Boron carbide is known to exist as a single phase with carbon concentrations from 8.8 to 20 % [2]. Stoichiometry of boron carbide affects its mechanical, thermoelectric, optical and other properties [1].
B4C is commercially produced by carbo-thermic reduction of boric acid or magnesiothermy in the presence of carbon [3]. High temperatures and long time, which are necessary in carbo-thermic reduction or magnesiometry, result in a large grain size of the product, requiring time- and energy-consuming steps of crushing and grinding to obtain fine powders, necessary, for example, for fabrication of dense ceramics.
High-technology applications of B4C require powders with high purity, precise stoichiometry and fine particle size [4,5,6,7]. Direct synthesis of B4C from boron and carbon (Equation 1) can address issues of purity and stoichiometry.
4B + C = B4C, ΔH = -72.1 kJ mol-1
Boron and carbon are thoroughly mixed and compacted into pellets, which are then heated at temperatures >1500 °C [3]. Although this method is more expensive than carbothermal reduction one, it is preferable when boron to carbon ratio and high phase purity are important. Still, due to long time treatment at high temperatures the product is coarse and requires crushing, grinding, and ball-milling. While recent reports have introduced innovative synthesis methods for B4C particles with varying sizes and morphologies [6], there is no widely accepted approach for producing high-purity, fine B4C powders. Moreover, there is an increasing demand to promote environmentally friendly and energy-efficient methods for materials synthesis, propelled by efforts to mitigate the climate crisis.
Combustion synthesis, also known as self-propagating high-temperature synthesis (SHS), is a fast, low energy-consuming and low carbon-emission method for the synthesis of ceramic powders including carbides, nitrides, borides, oxides, and more [8,9]. Combustion synthesis exploits highly exothermic chemical reactions, where the heat generated during the reaction promotes and sustains the reaction itself. In a self-propagating mode, the reaction is initiated by a high-energy pulse, such as brief heating achieved by passing an electric current through a tungsten filament. Once ignited, the reaction propagates without the need for additional external energy input. An important parameter for assessing the feasibility of reaction propagation is the adiabatic temperature, which represents the maximum temperature attainable when all the heat generated during the reaction remains within the system. If the adiabatic temperature falls below a certain threshold, typically around 1800 K, the reaction cannot self-propagate. In such cases, alternative techniques like volume combustion (thermal explosion), chemical ovens, or combustion under elevated temperatures may be employed. The direct reaction between boron and carbon is exothermic (Equation 1), but enthalpy is low (-72.1 kJ mol-1) and the adiabatic temperature is only 955 K, therefore combustion synthesis from elements is not self-sustainable [10]; usually highly-exothermic magnesiothermic reaction is used for the combustion synthesis of B4C in SHS mode [11]. Evidence of an SHS reaction was observed during the field-activated reactive spark plasma sintering of B4C [10,12]. These findings suggest that, with the appropriate field assistance, combustion synthesis of B4C is achievable.
Recently, we introduced a novel synthesis technique, which we refer to as electromagnetic induction synthesis (EMIS), for producing various carbide materials [9,15]. EMIS combines combustion synthesis with the assistance of electromagnetic induction. Electromagnetic induction offers rapid, non-contact, and efficient heating of conductive materials, enabling precise power control and adjustable heating rates over a wide range [13,14]. Therefore, combustion synthesis reactions, even with a limited exothermicity, can be initiated and controlled [9]. Additionally, the electromagnetic field directly impacts the sample, accelerating atomic diffusion and enhancing chemical reactions [15]. By integrating combustion synthesis with electromagnetic induction assistance, it is possible to significantly reduce the time, temperature, and energy required for synthesis when compared to traditional synthesis techniques [9,15].
In this study, we demonstrate the efficient synthesis of fine B4C powders in a short timeframe using EMIS. The product properties are controlled by optimizing process parameters, including holding temperature and time. Furthermore, we show that the B4C powders synthesized through this method have high crystallinity which contributes to the improved resistance to oxidation when subjected to heating in air.

2. Materials and Methods

Amorphous boron (0.8 μm, Rare Metallic) and carbon black (80 nm, Asahi Thermal) powders were mixed in stoichiometric proportion with addition of ethanol using a SiC mortar with pestle. Then powders were dried in vacuum drying oven at 70 °C overnight. After drying mixtures were uniaxially pressed into pellets at 10 MPa pressure. A pellet was placed into a graphite crucible and covered with a graphite lid. The crucible was set in high-frequency induction heating (HF IH) apparatus (MU-αⅣ, SK Medical Electron, Japan) and heated under Ar flow. To measure temperature of the samples, an infrared optical pyrometer (working range 600~3000 °C) was used. Basic experimental set-up is shown in Figure 1 (a). The optical pyrometer was focused on the graphite lid as shown in Figure 1 (a). For recording an exothermic peak of the reaction, the graphite lid was taken off and temperature was measured on the top surface of the samples (Figure 1 (b)). The heating program consisted of three steps: preheating at a slow heating rate (300 °C·min-1), ignition at a high heating rate (1000 °C), and postheating (holding) at constant temperature (1900, 1950 and 1970 °C). Finally, the sample was cooled down naturally under Ar flow. The grey-colored lightly sintered product was obtained. The samples ID with the details of heating conditions are shown in Table 1.
Field-emission scanning electron microscopy (FE-SEM, Hitachi S-4800) was applied to characterize microstructure of the fracture surface, grain size and shape of as-synthesized samples. The mean particle size was calculated using ImageJ free software. The samples were lightly ground using a silicon carbide mortar and pestle for further analysis. Crystalline phases were determined using x-ray diffraction method (XRD, Aeris, Panalytical). The specific surface area was analyzed by static manometric nitrogen adsorption at cryogenic temperature (77 K) using a Belsorp 28SA apparatus. The samples were outgassed in vacuum at 300 °C for 2 hours directly prior to measurement. Calculation of the specific surface area (SSA, ABET) was done according to the Brunauer–Emmett–Teller (BET) theory in the range of 0.05~0.3 partial pressure. Average particle size d (nm) was calculated from ABET (m2·g-1) and density of B4C (ρ, 2.52 cm3·g-1) under assumption of spherical particles using Equation 2:
d = 6000/ABET×ρ
Non-isothermal oxidation tests were performed using a thermogravimetry differential thermal analyzer (TG-DTA, Bruker) in ambient air. Synthesized B4C powders were put into Pt pans and heated in air from room temperature to 700 °C under heating rate of 10 °C·min-1. Commercial B4C powder (H.C. Stark, Grade HS, 0.8 μm mean particle size) was measured using the same procedure for comparison. An oxidation onset temperature (OOT) was defined as the temperature at which weight of the sample starts to increase.

3. Results and Discussion

3.1. Ignition of the Reaction and Temperature-Time Profiles during Synthesis

Figure 2 (a) shows temperature vs time profile measured during heating without the graphite lid as shown in Figure 1 (b). It can be seen from Figure 2 (a) that after 60 s of slow heating the temperature of the pellet was about 600 °C. When the temperature achieved 800 °C, the heating rate was changed from 300 to 1000 °C·min-1. Then after 30 s of fast heating a sharp rise in temperature was observed, which started from 1303 °C. The sharp rise in temperature represents the exothermic peak appeared due to the exothermic reaction between boron and carbon leading to formation of B4C (Equation 1). The ignition temperature is close to the values observed in reactive spark-plasma sintering of B4C [12]. Maximum temperature of the exothermic peak was 1477 °C. It should be mentioned that the values of temperature measured without lid are always lower than measured on the graphite lid under the same IH power. Therefore actual values of the exothermic peak are expected to be higher, when the graphite lid covers the crucible, providing better thermal insulation. Direct visual observation of sample during heating confirmed sudden rise of light emission associated with a volume combustion reaction between boron and carbon. After sample reached temperature of 1700 °C, IH power was stopped and sample was allowed to cool down under Ar flow. It can be seen from the profile that temperature decreased from 1700 to less than 1000 °C in 2 minutes. One example of a typical temperature profile measured on the carbon lid is shown in Figure 2 (a). There is no temperature peak related to the exothermic reaction due to the low exothermic value of the reaction, which was not enough to affect the temperature of the crucible. Figure 2 (b) shows that temperature can be finely contolled during synthesis.

3.2. Characterization of the Synthesized B4C

3.2.1. Phase Composition

Figure 3 shows XRD patterns of the synthesized B4C samples. All major peaks were attributed to B4C. In case of sample 1 peaks of starting materials were observed as well, indicating that the reaction between boron and carbon was not completed at this stage. The exothermicity of the reaction between carbon and boron is not enough to complete the formation of B4C, therefore some unreacted elemental carbon and boron remained in the sample. Small peaks of boron trioxide (B2O3) were identified in sample 1. It is considered that B2O3 was present as an impurity in the starting boron powder. Boiling point of B2O3 is 1860 °C; and sublimation starts at 1500 °C. Sample 1 was heated up to 1700 °C, which is higher than sublimation temperature, but heating time was too short to eliminate all B2O3. When the additional post-heating step at temperatures higher than boiling point of boron dioxide was applied, the peaks of starting materials and B2O3 became negligible (samples 2-5). Significantly, with the rise in holding temperature from 1900 to 1950 °C, the previously observed broad halos between 22-24 degrees and 35-38 degrees vanished. This suggests an enhancement in phase purity and crystallinity as the temperature increased.
Heating at the rate as fast as 1000 °C·min-1 initiates the reaction between carbon and boron due to very high local temperature gradients induced in the sample. Then the reaction between boron and carbon proceeds via mutual diffusion of carbon and boron atoms. However, diffusion of boron and carbon atoms in B4C is a very slow process due to strong covalent bonds between the atoms and high activation barriers. Moreover, presence of boron dioxide can negatively affect diffusion process. Therefore, in case of sample 1 the reaction between boron and carbon was not completed. When postheating step at 1900~1970 °C was applied for a short time, the considerable improvement in the phase purity and crystallinity of the samples was observed, indicating acceleration of diffusion under high temperatures. Effective elimination of B2O3 could promote diffusion and B4C phase formation. Additionally, in our previous work [16] it was shown, that the induction (eddy) currents induced by high-frequency magnetic field of the coil penetrate through the carbon crucible walls and may affect diffusion processes via electromigration and related phenomena. Therefore, at temperatures beyond 1900 °C the reaction between boron and carbon was completed in a very short time compared to conventional synthesis [3].

3.2.2. Microstructure and Particle Size

Figure 4 shows SEM images of the fracture surface of the synthesized B4C. It can be confirmed that fine and uniform B4C grains were synthesized. There was no clear difference in grain shape and size between samples 2 and 3; the grain size is less than 1 μm. Samples 4 and 5 show larger grain size and better-defined grain shape than samples 2 and 3. Across all samples, the grain shape appeared oval with a low aspect ratio. As depicted in Figure 4 (c, d), heating at 1950 °C and 1970 °C (samples 4 and 5) resulted in the partial sintering of grains, a phenomenon not observed in samples 1 and 2. Previous studies have demonstrated that B4C particles can self-bond without the aid of low-melting additives films [17], and the assistance of IH promotes sintering of B4C [16]. Samples 4 and 5 exhibited a step-like relief on the surface of B4C particles, potentially linked to twinning within the grains [18]. In conclusion, it can be inferred that, when the maximum temperature during synthesis is 1950 °C and higher, the grain size and morphology develop very rapidly, therefore an optimal temperature is not higher than 1950 °C.

3.2.3. Specific Surface Area

Figure 5 shows adsorption and desorption isotherms of the samples 2 and 5. Other samples produced isotherms of similar shapes. The isotherms shown in Figure 5 belong to the type II of the IUPAC classification [19], thus showing that synthesized powders are non-porous or macroporous materials. Hysteresis between adsorption and desorption isotherms can be related to the presence of macropores. Table 2 shows BET specific surface area (SSA, SBET) and average particle size calculated from N2 gas adsorption data. The SSA of sample 2 is 17.2 m2·g-1 and an average calculated particle size is 138 nm. The calculated particle size is smaller than that observed by SEM (Figure 4 (a) and Table 2). This discrepancy can be related to the non-spherical irregular shape of the particles. Prolongation of heating at 1900 °C from 3 to 5 minutes leads to decrease of the SSA from 17.2 to 11.0 m2·g-1 and increase in the average calculated particle size from 138 to 216 nm. As can be seen from the Table 2, SEM grain size increased much less. When post-heating temperature was increased to 1950 °C, the SSA decreased to 2.3 m2·g-1, and average particle size increased to 1035 nm. At this temperature the gas-adsorption average particle size and SEM grain size show very close values. Heating to 1970 °C leads to further decrease in the SSA and increase of particle size. As was observed by SEM, heating at 1950 and 1970 °C leads to grain growth and partial sintering of B4C, thus decreasing SSA.

3.3. Non-Isothermal Oxidation of B4C Powders

Typical thermogravimetric (TG) curves plotted as weight gain (wt %) versus temperature of the synthesized B4C powders and commercial B4C powders are shown in Figure 6. The oxidation of B4C follows Equation 3 and accompanies a weight gain.
B4C(s) + 4O2(g) = 2B2O3(s,l) + CO2(g)
The TG curves clearly indicate that there was no measurable weight gain up to 480 °C. The small weight decrease observed in the commercial powder between 200 and 300 °C is related to the decomposition of boric acid formed on the surface of the powders in air. Beyond 480 °C weight of the commercial B4C powder starts to increase rapidly indicating oxidation of B4C according to Equation 3. The OOT of the commercial B4C powder, determined as the point on the TG curve where weight starts to increase, was 483 °C. The variation of OOT with the synthesized samples is shown in Table 2. The OOT of all synthesized B4C powders is higher than that of commercial powder and it increases with increasing post-heating holding temperature from 1900 to 1950 °C. Samples 2 and 3 have very close values of the oxidation temperature, indicating that their stability against oxidation is almost identical. Samples 2 and 3 differ in the postheating time, however, as was shown in the Section 3.2.1 and Section 3.2.2, their XRD patterns are almost identical and the grain size measured using SEM differs only by 30 nm. Post-heating at 1950 °C leads to improvement of crystallinity (Figure 3) and increases grain size (Figure 4). As a result, OOT of sample 4 is more than 60 °C higher than that of sample 3. OOT of sample 5, which was heated to 1970 °C, is lower than OOT of sample 4. Although both samples, 4 and 5, have similar SEM average grain size (Table 2), the grain size distribution is wider for sample 5, which affects OOT. The particle size has a great influence on oxidation behavior of B4C powders [20]. Theoretical calculations showed that powders with 1.52 μm particle size have OOT lower than 500 °C [20]. However, OOT of all samples synthesized in the present work exceeds that value. Therefore, it is concluded that OOT is affected by both the grain size and crystallinity of B4C powders.
As can be seen from Figure 6, beyond 600 °C oxidation proceeds very rapidly. The rate of oxidation of the synthesized powders is higher than that of commercial powder. This behavior can be explained by differences in the thickness of B2O3 thin film on the surface of B4C particles, which forms when the powders are exposed to air during handling. The thickness of the B2O3 layer influences the time required for oxygen to diffuse through the oxide layer, thus affecting the oxidation rate. The synthesized B4C powders were measured soon after the synthesis, therefore B2O3 layer was not formed yet on the surface. As can be seen from the XRD powders, no boron oxide phase was observed for the samples 2~5. The oxidation temperature was found to be independent of the time passed from the synthesis and handling conditions.

4. Conclusions

B4C powders were successfully synthesized through the high-heating rate, high-temperature, and short-time EMIS method. Phase purity and crystallinity were optimized by varying the conditions of a post-heating step. Powders synthesized with post-heating at 1950 °C for 3 minutes exhibited a graphite-free single-phase composition, a uniform particle size of approximately 1 μm, and a high oxidation onset temperature of 584 °C. This surpasses the oxidation onset temperature of commercial B4C powders by more than 100 °C. In summary, the EMIS method proves to be a promising approach for producing phase-pure, fine B4C powders, suitable as candidates for advanced technological applications.

Author Contributions

Conceptualization, A.G.; methodology, A.G.; validation, A.G., Y.K.; investigation, A.G.; resources, A.G., Y.K.; data curation, A.G.; writing—original draft preparation, A.G.; writing—review and editing, A.G., K.Y.; visualization, A.G.; supervision, A.G., Y.K.; project administration, A.G.; funding acquisition, A.G. All authors have read and agreed to the published version of the manuscript.

Funding

This research was supported by JSPS KAKENHI Grant Number 23K04432. 23K04432.

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

The data presented in this study are available on request from the corresponding author.

Acknowledgments

The authors acknowledge Mr. Masamitsu Imai (Tokyo Institute of Technology) for technical support.

Conflicts of Interest

The authors declare no conflict of interest. The funders had no role in the design of the study; in the collection, analyses, or interpretation of data; in the writing of the manuscript; or in the decision to publish the results.

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Figure 1. EMIS experimental set-up: (a) standard synthesis experiments, (b) recording the exothermic peak.
Figure 1. EMIS experimental set-up: (a) standard synthesis experiments, (b) recording the exothermic peak.
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Figure 2. Temperature-time profile during synthesis with temperature measured on: (a) the surface of the sample (Sample 1); (b) the graphite lid (Sample 3).
Figure 2. Temperature-time profile during synthesis with temperature measured on: (a) the surface of the sample (Sample 1); (b) the graphite lid (Sample 3).
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Figure 3. XRD patterns of synthesized B4C powders (sample ID numbers are indicated above the respective lines).
Figure 3. XRD patterns of synthesized B4C powders (sample ID numbers are indicated above the respective lines).
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Figure 4. SEM images of synthesized B4C powders: (a)sample 2; (b) sample 3; (c) sample 4; (d) sample 5.
Figure 4. SEM images of synthesized B4C powders: (a)sample 2; (b) sample 3; (c) sample 4; (d) sample 5.
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Figure 5. Adsorption/ desorption isotherms of the samples 2 and 5.
Figure 5. Adsorption/ desorption isotherms of the samples 2 and 5.
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Figure 6. TG curves of samples 2, 3, 5, and commercial B4C powder.
Figure 6. TG curves of samples 2, 3, 5, and commercial B4C powder.
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Table 1. Samples synthesized in the present work.
Table 1. Samples synthesized in the present work.
Tmax (°C) Point of T measurement Holding time at Tmax (min) Sample ID
1700 Sample 0 1
1900
1900		 Graphite lid 3 2
5 3
1950 3 4
1970 0 5
Table 2. Specific surface area, grain size and oxidation temperature of the B4C powders.
Table 2. Specific surface area, grain size and oxidation temperature of the B4C powders.
Sample ID SBET (m2·g-1) Average particle size (nm)1 SEM grain size (nm)2 OOT (°C)
2 17.2 138 450 521
3 11.0 216 480 521
4 2.3 1035 910 584
5 1.5 1550 1060 550
1 Calculated from N2 gas adsorption. 2 Calculated from SEM images using ImageJ software.
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