Reactions Between Ti2AlC, B4C, and Al and Phase Equilibria at 1000 °C in the Al-Ti-B-C Quaternary System
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As automotive, aerospace and the power industries increasingly look to carbide and boride based aluminum, Al, composites for their high specific strengths and increased thermal stability, it is important to characterize the equilibrium phase relations at temperatures common for processing these composites. Herein, two composites were fabricated starting with Al, Ti2AlC, and B4C. The Ti2AlC/B4C powders were mixed in both 50/50 and 75/25 vol.% ratios and cold pressed into 53% dense preforms. The preforms were pressureless melt infiltrated in the 900-1050 °C temperature range with Al. Ten hour equilibration experiments were also conducted at 1000 °C. X-ray diffraction and scanning electron microscopy confirmed that neither Ti2AlC nor B4C was an equilibrium phase. A number of reaction phases—AlB2, Al3BC, TiB2, TiC, TiAl3 and Al4C3—could be found in the non-equilibrated samples. However, the equilibrium phases were found to be Al, TiB2, Al3BC, and Al4C3 for the more B-rich composite and Al, TiB2, TiC, and Al4C3 for the Ti-rich composite. From these results, the 1000 °C quaternary phase diagram adjacent to the Al-TiB2-Al4C3 triangle and in the Al-rich corner was developed for the first time. This study is a requisite first step for the development and use of advanced composites in the Al-Ti-B-C system.
Keywordsaluminum equilibria MAX phase MMCs phase diagram
Metal matrix composites, MMCs, attempt to combine the advantageous properties of both metals and ceramics. Wear resistance, fatigue and fracture resistance, and reduced coefficient of thermal expansion (compared to the metal matrix) are attractive reasons to incorporate ceramic reinforcements into metal matrices, while retaining the good thermal and electrical conductivities, and machinability of metals. Mixing of a metal, or alloy, with a reinforcement phase may be achieved through a variety of processes such as stir casting, melt infiltration, powder metallurgy, among others. Common ceramic reinforcements include: Al2O3, SiC, B4C, TiC, and TiB2. A more thorough review of MMCs and their properties may be found elsewhere.[1,6]
Al-matrix composites reinforced with titanium carbide, TiC, and/or boron carbide, B4C, have been targeted as families of lightweight materials with the potential to operate at temperatures above those of Al and its alloys. The high hardness typical of boride and carbide-containing composites also makes them attractive for high wear applications. Their chemical stability and neutron absorption properties render them appealing in nuclear and other demanding industrial settings.[7,8]
Recently, magnesium, Mg, matrix composites reinforced with Ti2AlC—a member of the MAX phases—have been developed.[9, 10, 11] The MAX are a family of nanolayered, machinable, ternary carbides and nitrides, having the general formula Mn+1AXn—where n = 1, 2, 3; M is an early transition metal; A is an A-group element (mostly groups 13 and 14); and X is C and/or N. The MAX phases combine some of the best properties of metals and ceramics. Like metals they are machinable, electrically and thermally conductive,[13,14] damage tolerant and not susceptible to thermal shock. Like ceramics, some of them are lightweight (≈4 Mg/m3) and elastically rigid (Young’s moduli >300 GPa). Ti2AlC is also creep, fatigue and oxidation resistant.[12,16, 17, 18]
The aforementioned Mg and Mg alloys-MAX composites were manufactured by spontaneous melt infiltration, MI, at relatively low processing temperatures (750 °C) yielding composites with attractive mechanical properties. For example, the Young’s modulus and ultimate compressive strengths, UCSs, of a Mg alloy (AZ61) matrix composite reinforced with 50 vol.% Ti2AlC particles were measured to be 136 ± 6 GPa and 760 ± 9 MPa, respectively. In addition to the excellent mechanical properties, these composites can also dissipate almost 25% of the applied mechanical energy at high stresses.[11,19] Furthermore, the resulting composites were also most readily machinable, since both components are machinable. These promising results spurred interest in developing Al-MAX composites with comparable or better properties using MI.
Fabricating Al-matrix MAX reinforced composites is complicated by the fact that Al is not in equilibrium with most MAX phases. For example, Wang et al. attempted to fabricate Ti3AlC2 composites at elevated temperatures and found that above 950 °C, Ti3AlC2 reacted with Al to form TiC and TiAl3. To circumvent this problem Wang et al. hot pressed Al and Ti3AlC2 powders at a temperature (550 °C) at which the reaction kinetics were slow. More recently, Hu et al. used current-activated, pressure-assisted infiltration to fabricate Al-Ti2AlC composites. In this method, the processing and densification occur too rapidly for extensive reactions to occur. Their nearly full dense composites were lightweight with UCS’s of the order of 500 MPa. At 160 MPa cm3/g, their specific strengths were approximately 4 times higher than those of pure Al. These solutions to the problem, however, do not lend themselves to rapid, near-net shape, inexpensive manufacturing.
As noted above, the original goal of this work was to fabricate Al-Ti2AlC composites via MI. However, preliminary results obtained herein showed that porous Ti2AlC preforms were not easily wet by molten Al even at 1000 °C. At higher temperatures, the reaction was quite intense and did not result in a usable material. Poor wetting by Al is not unique to Ti2AlC, but is also encountered when fabricating MMCs with other carbides, such as TiC, B4C and SiC. Typically temperatures greater than 1000 °C are necessary for Al to wet TiC and/or B4C preforms in MI experiments.[3,4] However, it has been previously reported that Ti additions to B4C porous preforms enhance the infiltration kinetics of Al into the latter, which coincides with the finding that Ti-B interactions aid in the reactive wetting of Al on ceramic surfaces, though the reaction mechanisms and phase equilibria remain largely un-investigated. Nevertheless, this interest in manufacturing Al matrix composites with both borides and carbides would be greatly aided by an understanding of the reaction mechanisms and especially the equilibrium phase relations of these systems.
This work sought to enhance the infiltration kinetics of Al into Ti2AlC at lower temperatures by incorporating B4C in the preforms, in an attempt to reduce or eliminate the high temperature reactions observed between Ti2AlC and Al. However, when it was found that in all cases, a reaction occurred, the focus of the work shifted to understanding the equilibrium phase relations in the Al-Ti-B-C quaternary system. Before doing so, it is important to review the following phase diagrams.
Binary Phase Diagrams
Others reported that the transformation temperature may be as high as 972 ± 5 °C. AlB12 is stable to ≈2000 °C. The solubility of B in liquid Al at 1100 °C is about 7 at.%.
The only binary phase in the Al-C system is Al4C3. And while this phase has been reported to be stable to above 2100 °C, when in contact with TiAl3 it will react to form TiC and Al at ≈877 °C. The solubility of C in Al is negligible in the temperature range used herein.
A multitude of binary intermetallic phases exist between Al and Ti, that include Ti3Al, TiAl, Ti3Al5, TiAl2, Ti2Al5, Ti5Al11, and TiAl3. At 1000 °C, the stable phases are: α-Ti, β-Ti, TiAl3, TiAl, TiAl2, Ti2Al5, and TiAl3.[30,31]
Initial investigations of the Ti-B system suggested the existence of the binary phases Ti2B and Ti2B5, however the existence of these phases has since been refuted. The current Ti-B phase diagram, shows only the binary phases TiB, Ti3B4 and TiB2, all of which are stable to ≈2000 °C.
Non-stoichiometric TiCy (0.47 < y < 1.00) is the only Ti-C binary phase in the Ti-C system. The existence of various ordered phases such as Ti2C, Ti6C5, and Ti3C2 have sometimes been reported, however.
Within the B-C system, the only known binary phase is B4C, with B-rich (carbon deficient) variations of the form B4C1−z (0 < z < 0.55).[32,34] This phase is thermally stable to nearly 2500 °C. An extensive review of the history, processing, and properties of B4C can be found in the literature.
Ternary Phase Diagrams
More than forty phases are known to exist in the Al-B-C system. Isothermal experiments carried out at 900, 1000, and 1400 °C have been used to tentatively draw conclusions about equilibrium relations. The stable phases reported at 900 °C—including Al4C3, Al3BC, Al3BC3, Al3B48C2 and B4C—remain stable at 1000 °C (Fig. 1a). Since this work deals with the Al rich-corner of the quaternary phase diagram, the only relevant phase is Al3BC. The latter is reported to be stable to ≈1100 °C, after which it reacts with AlB12 to form Al3B48C2 and liquid Al.
Isothermal sections of the Al-Ti-C system have been extensively investigated over the 727 to 1300 °C temperature range, with reproducibility between studies. Of the three ternary phases known to exist, two—Ti3AlC2 and Ti2AlC—belong to the MAX phase family; the third, Ti3AlC, has a perovskite-type crystal structure.
Both Ti2AlC and Ti3AlC can be found in the ternary system at every temperature between 750 and 1300 °C. However, according to Pietzka and Schuster, Ti3AlC2 is not an equilibrium phase at, or below, 1000 °C. The equilibrium relations at 1000 °C (Fig. 1b) and 1300 °C have become the standard for this system. For simplicity, this study considers TiCy to be stoichiometric TiC (see below) and is represented as such in the ternary phase diagram.
There are no ternary compounds in this system. The phase relations between the binary phases have been well established.
No ternary phases exist in this system either. Isothermal sections at 800, 1000, 1350, and 1550 °C exist and show a dependence of the equilibrium phase relations on temperature. The most notable change in equilibrium relations is that TiB2 and AlB2 are in equilibrium at 800 °C, but not at, or above, 1000 °C. This is due to the thermodynamic instability of AlB2 due to the aforementioned decomposition reaction (Eq 1), though it should be noted that the transformation rate is slow.[26,40] The computationally determined Al-Ti-B isotherms generated by Witusiewicz et al. have been confirmed by experimental results and provide reliable equilibrium phase relations at 1000 °C (Fig. 1c). Again, non-stoichiometric phases are represented as point compounds.
The aim of this work was to investigate phase equilibria in the Al-Ti-B-C quaternary system at processing temperatures and compositions typical for the fabrication of Al matrix composites, i.e., near the Al corner and in the 900-1050 °C temperature range. To reach that goal, x-ray diffraction (XRD) and a scanning electron microscope (SEM) were used to characterize the reaction phases produced when Ti2AlC/B4C porous preforms were infiltrated by molten Al.
Pure Al (99+%, Alfa Aesar, Ward Hill, MA) bar stock and B4C powder (99+%, Alfa Aesar, Ward Hill, MA) with an average particle size <10 μm was used for this work. Commercial −325 mesh Ti2AlC powders were obtained (Kanthal, Sweden). It is worth noting here that Ti3AlC2 is an impurity phase found in these powders (≈17 wt.% from Rietveld analysis).
Two composites were fabricated starting with Al, Ti2AlC, and B4C. The first composite, henceforth referred to as BR, was more boron rich, having the Al:Ti:B:C molar ratio, calculated from Rietveld analysis of equilibrated microstructures (see below), of 3.3:1.1:2.5:0.5. The second composite, henceforth referred to as TiR, was more Ti-rich and the Al:Ti:B:C molar ratios in this case—again calculated from Rietveld analysis—were 3.4:1.1:1.3:0.7.
Preparation of Carbide Preforms
The Ti2AlC/B4C powders were mixed in the molar ratios of 4.5:5 and 7:4 for the BR and TiR composites, respectively. These ratios correspond to roughly 50/50 and 75/25 vol.% ratios of Ti2AlC/B4C for the BR and TiR composites, respectively. The mixed powders were ball milled for 24 h with yttria stabilized zirconia grinding media, cold pressed in a steel mold—to a load corresponding to a stress of 50 MPa—to form rectangular (BR = 6.1 × 12.7 × 69.4 mm3 and TiR = 8.1 × 12.8 × 69.3 mm3) ≈47 vol.% porous preforms. The preform densities were 1.76 and 1.98 g/cm3 for the BR and TiR preforms, respectively. Component densities were assumed to be 4.11 g/cm3 for Ti2AlC and 2.52 g/cm3 for B4C. No impurities or non-stoichiometry were considered.
Pressureless Melt Infiltration
The preforms were placed in alumina crucibles (AdValue Technology, Tucson, AZ), which were lined with graphite foil to avoid reactions with the crucible. Appropriately sized pieces of Al were placed on top of the preform and the assembly was placed in an alumina tube furnace and heated at a rate of 10 °C/min to 900, 950, 1000, or 1050 °C and allowed to soak for 0.5 h before furnace cooling to room temperature, RT. All experiments were carried out under flowing argon, Ar, gas at atmospheric pressure. The samples infiltrated at 1000 °C were cut in half and one half was further annealed at 1000 °C for 10 h, again under flowing Ar.
After cross-sectioning, mounting, and polishing (1200 grit) the microstructures were imaged using a SEM (Zeiss Supra 50VP, Germany) equipped with an energy-dispersive spectroscope (EDS) (Oxford Inca X-Sight, Oxfordshire, UK). Image analysis was undertaken using MATLAB (The MathWorks, Inc., Natick, MA) on select backscatter electron SEM micrographs to estimate the volume fractions of the various phases.
Powders for XRD were obtained by drilling the composites with a carbide drill bit and analyzed using a x-ray diffractometer (Rikagu Smartlab, Japan). The angular step was set to 0.02° over the 2θ = 5°-80° range, with a hold time of 0.5 and 2 s for 0.5 h infiltration and equilibration experiments, respectively. Scans were made through a 10 × 10 mm2 window slit using Cu Kα radiation (40 KV and 30 mA).
To verify the presence of Al4C3, additional careful powder XRD was conducted on the equilibrium samples of both compositions. Powder was prepared immediately prior to running the XRD patterns. An angular step of 0.02° was set over the range 2θ = 30°-33° and 39.5°-40.5°, with a hold time of 7 s. The slit and radiation conditions were the same as above. The hold time was extended here to enhance the intensity of the various peaks.
Rietveld refinements of the XRD patterns of the equilibrated samples were conducted using FullProf. Refined parameters were: six background parameters, lattice parameters of all phases, scale factors from which relative phase fractions are evaluated, and X profile parameters for peak width.
Observed phases from each experiment are reported with their relative increase or decrease in amount noted, if applicable, and calculated volume fractions, if available
(Relative increase ↑/Decrease ↓)
(Relative increase ↑/Decrease ↓)
Results from image analysis
B4C (5.4 vol.%)
B4C (5.1 vol.%)
B4C (2.1 vol.%)
B4C (9.6 vol.%)
Ti3AlC2 (5.3 vol.%)
B4C (4.7 vol.%)
B4C (<1 vol.%)
B4C (2.5 vol.%)
B4C (<1 vol.%)
B4C (<1 vol. %)
B4C (<1 vol.%)
Results from Rietveld analysis
The presence of Al4C3 was not apparent at first. The low intensity of its diffraction peaks were difficult to distinguish from background noise acquired with 0.5 s hold times. Further XRD patterns of the equilibration samples, using a 2 s hold time (Fig. 2), provided confidence that Al4C3 diffraction peaks were present. XRD patterns obtained with a hold time of 7 s, however, left no doubt as to the presence of this phase in the equilibrated samples (insets of Fig. 2).
Microstructures of Samples
(i) Al-containing phases, primarily Al3BC, replace B4C; (ii) the volume fraction of the Al/TiB2 regions (light grey contrast in Fig. 3a, c) increased at the expense of the Al/Al3BC regions (mid grey contrast) as the system tended towards equilibrium. The B4C volume fraction after the 10 h anneal was estimated to be <1 vol.%. Aside from the remaining B4C, no other non-equilibrium phases could be identified from microscopy (Fig. 3d); (iii) the TiB2 grains in the Al matrix were observed to notably coarsen with the prolonged annealing, growing from an estimated average diameter of <200 to >500 nm (Fig. 3b, d); (iv) TiB2 grains are found in the Al matrix, but not in the same regions as the Al4C3 or Al3BC phases (Fig. 3d).
The presence of Al4C3 was not directly observed in the SEM in any of the investigated samples. However, since Al4C3 is hygroscopic and dissolves in water at room temperature it is reasonable to assume that it dissolved during the water-based polishing procedure. Note that EDS analysis of cross-sectional SEM micrographs clearly show that some Al-rich regions were comprised of pure Al; others were found to contain substantial amounts of C with Al/C ratios that varied between 1.0 and 1.9. It is hereby acknowledged that there are several explanations for why C may be detected in some Al regions and not others, including, the presence of C-containing phases below the surface, but within the excitation volume of the EDS. Nevertheless, since Al4C3 peaks were observed—and twice confirmed—in the XRD patterns (insets in Fig. 2), there is no doubt that it exists in the microstructures. Another possibility is that the Al4C3 phase for some reason dissociated into C-rich Al regions. Therefore, the C-rich Al regions are tentatively labeled as Al4C3 in the micrographs. These comments notwithstanding, more work is needed to understand what happens to the Al4C3 phase.
Samples Melt Infiltrated for 0.5 h
XRD of Reaction Products
Additionally, the TiC peak intensities decreased with increasing infiltration temperatures (see peak at 2θ = 41.71° in Fig. 5). As AlB2 shares its dominant XRD peaks with other phases, its presence was better ascertained by microscopy. The shoulder in the TiB2 peak, at 2θ = 34.41°, may be the best diffraction evidence that the quantity of AlB2 decreases with MI temperature, as this shoulder is no longer observed after MI at 1050 °C (Fig. 5c).
Microstructures of Samples
Raising the infiltration temperature to 950 °C resulted in the disappearance of the Ti3AlC2 phase from both the XRD and SEM results (Fig. 6b, 7d). The microstructure at this temperature consisted of fine grains of TiB2 and TiC contained in an Al/TiAl3 matrix, with some unreacted B4C grains remaining (Fig. 7d). The latter were surrounded by Al3BC. The C-rich Al-containing regions were not found in regions of Ti-containing phases, but were only found in the vicinity of the Al and Al3BC phases (Fig. 9b). After the 1050 °C infiltration, there was no trace of TiAl3; the only phases remaining were TiC, TiB2, Al and C-rich Al-containing regions, with trace amounts of B4C (Fig. 7f).
In contrast to the microstructures seen after MI at 900 °C (Fig. 9a) and 950 °C (Fig. 9b), the ones MI at 1000 °C (Fig. 4b) and 1050 °C (Fig. 9c) showed regions with evenly dispersed grains of TiC and TiB2 in an Al matrix. The ternary Al3BC was not found above 950 °C and the large B4C grains were replaced by some C-containing Al matrix regions, surrounded by a ≈ 0.5 μm wide Ti-rich layer (Fig. 9c).
To examine the robustness of our conclusions, the position of the initial composition was re-calculated assuming that the stoichiometry of B4C to be B4C0.5, with all else remaining the same. When plotted, this composition point shifted by a negligible amount. We also carried out a calculation incorporating the presence of 20 wt.% Ti3AlC2 in the starting composition. In that case the initial Al:Ti:B:C molar ratio is 3.8:0.9:3.0:1.2. The resulting location point was nearly indiscernible from the location of the blue circle shown in Fig. 10(a).
Based on these findings, it can be concluded that neither the B4C stoichiometry nor the presence of ≈20 wt.% Ti3AlC2 in the initial powder affects the location of the initial composition in the conjectured equilibrium tetrahedron.
Based on the Rietveld refinements, the final Al:Ti:B:C molar ratio was calculated to be 3.8:1.3:2.9:0.6 (pink point in Fig. 10a) with corresponding high volume fractions of Al and TiB2 (Table 1). The discrepancy between the initial (3.8:0.9:3.0:1.2) and final molar compositions in this system is discussed below. However, as both compositions lie within the same equilibrium tetrahedron, this discrepancy in no way affects the conclusions of this study.
Based on the totality of our XRD and SEM results on the equilibrated TiR composition it is reasonable to conclude that the 4 apexes of this equilibrium tetrahedron are: Al, TiB2, Al4C3, and TiC (tan tetrahedron in Fig. 10b-c and Supplementary Information). The latter occupies a larger volume of the phase diagram (14.29 vol.%) than the B-rich composition and was also found to be unaffected by non-stoichiometries in the B4C and/or the presence of Ti3AlC2. In this case, the starting composition (blue circle in Fig. 10b) was in excellent agreement with the composition calculated from Rietveld refinement of the XRD results (pink point in Fig. 10b) after equilibration, with both compositions well within the boundaries of the equilibrium tetrahedron.
Constituent Phase Diagram at 1000 °C
An interactive quaternary phase diagram can be found in Supplementary Materials. Note that this phase diagram assumes all phases to be line compounds (Fig. 10c). That this is an oversimplification is obvious for the simple reason that TiC exists over a wide Ti:C molar ratio. However, since this is the first report of this quaternary phase diagram, and for the sake of simplicity, we chose to assume TiC and all other compounds to be line compounds. Understanding how the non-stoichiometry of TiC affects the diagram is important and should be mapped out, but is beyond the scope of this work.
Upon wetting of the preform by molten Al, the initial reactions would be between Al/B4C and Al/Ti2AlC according to Eq 2 and 3, respectively. AlB2 and Al3BC are in equilibrium below the peritectic transformation temperature of AlB2, and B4C has been reported to react with Al to form these products in various experiments.[40,44,45] Both of these phases were observed herein. The reaction of Ti2AlC with Al (Eq 3) at the investigated temperatures is in agreement with the surmised reaction path of Ti3AlC2 with Al above 900 °C.[12,20]
Reaction 3 is also to be expected from an inspection of the ternary phase diagram (Fig. 1b) as the TiC/TiAl3 equilibrium line must be crossed in reacting Al with the Ti2AlC (labeled ‘H’ in Fig. 1b). While TiAl3 was not observed in this system, its production by this reaction is presented clearly in the TiR composite fabricated at 900 °C (see below). Of the four phases produced by these two reactions (Eq 2 and 3) only Al3BC is an equilibrium phase, indicating that the transient phases—AlB2, TiAl3, and TiC—must at some point react to form equilibrium phases (Eq 4 and 5). The formation of TiB2 by the reaction of TiAl3 with AlB2 has been previously reported in Al matrix composites, though largely through aluminothermic reactions of KF based salts in an Al melt.[46,47] Additionally, thermodynamic calculations indicate that the reaction between TiC and AlB2 (Eq 6) is favorable in high temperature Al melts. Lastly, the reaction between TiC and Al3BC (Eq 5) was inferred by the necessity to balance the overall reaction (Eq 7) and has not been found in the literature. It is not unreasonable to speculate about the feasibility of this reaction as it keeps in line with the finding that TiC is not stable in some Al-B systems. The continual consumption of TiC in Eq 5 and 6 is in agreement with the decreasing TiC peak intensities in the XRD spectra acquired for each infiltration temperature (Fig. 5).
In general, the agreement between the surmised reaction (Eq 7) and reaction Eq 8 is excellent with the only difference being that the Rietveld calculations show less Al4C3 than surmised. The cause of this may be rationalized in two ways: (i) some amount of Al4C3 may have hydrolyzed and became amorphous prior to the collection of the XRD patterns, which would under represent the amount of Al4C3 in the Rietveld calculations; and/or (ii) non-stoichiometric B4C and/or impurities in the starting powders may be responsible for the production of less Al4C3. As noted above, however, since the molar compositions of both the left and right sides of Eq 8 clearly fall within the same equilibrium tetrahedron (black X and pink point in Fig. 10a, respectively) the unbalanced equation has no effect on the results of this study. It may be for similar reasons that there is a disagreement between molar compositions from Rietveld calculations and the starting powder weights; however, as all molar compositions fall within the same equilibrium tetrahedron the results of this study are sound.
Examination of the BR microstructures at each infiltration temperature coincides with the proposed reaction path. No MAX phase is observed in this system, indicating that Eq 3 must occur rapidly after wetting of the preform. The reaction with B4C (Eq 2), however, continues even after equilibration for 10 h (Fig. 3c). It has been suggested that Al3BC forms a diffusion barrier and limits the rate at which the B4C grains are consumed by Al and also the rate at which boron diffuses into the matrix. The results shown herein support this finding. As evidence for TiAl3 was also unobserved by our XRD or SEM investigations, and since more AlB2 is produced (Eq 2) than TiAl3 is consumed (Eq 4) it is probable that this reaction also occurs rapidly following the production of AlB2. This also explains why AlB2 could be found in some microstructures (Fig. 3b, 8), as the remaining AlB2 is proposed to be consumed by TiC (Eq 5), presumably by a slower reaction since both of these phases were observed.
The higher magnification SEM micrographs of the sample fabricated at 1050 °C (Fig. 8) sheds more light on the reaction path: the un-reacted B4C is surrounded by an Al3BC layer (expected from Eq 2), AlB2 is found in Ti-containing regions which is necessary if it is to react with TiC, and TiC was also found near the Al3BC phase, making it feasible that they could react to bring the system to equilibrium (Eq 6).
Since Eq 9-12 are identical to Eq 2-5, they will not be discussed further. However, in order to consume the remaining TiAl3 and bring the system to equilibrium, Eq 13 is proposed. This reaction is expected from analysis of the Al-Ti-C ternary diagram (Fig. 1b) and has been reported to occur at temperatures above the melting point of Al.
When the short time MI experiments for the TiR and BR compositions are compared, it becomes obvious that the sequence and rates of some of the reactions are notably different. For example, Ti2AlC was not observed in the TiR composition, but its reaction products (Eq 10) were seen in the XRD patterns (Fig. 6a) and SEM micrographs (Fig. 9a). In contrast, the reaction products of B4C with Al, Al3BC and AlB2 (Eq 9) phases were not observed after processing at 900 °C. This is clear evidence that Ti2AlC is less stable in excess Al than B4C. However, at 950 °C a notable shift in reaction products occurs. TiAl3 is consumed and Al3BC is produced (Eq 9 and 11), likely the result of increased reactivity of B4C with Al (Eq 9) at the higher temperature. As with the BR system, this indicates that TiAl3 is rapidly consumed upon the production of AlB2 (Eq 11), as AlB2 was not identified from XRD and the TiAl3 peaks almost disappear (Fig. 6b). Al3BC is clearly a primary phase at 950 °C, which argues in favor of a slower reaction between TiC and Al3BC (Eq 12) than the rate at which Al3BC is produced. It may also be that Eq 12 is responsible for the change in microstructure between 950 and 1050 °C (Fig. 9b and c, respectively). The consumption of Al3BC (Eq 12) and remnant TiAl3 (Eq 13) is necessary to bring the system to equilibrium.
Reaction with Ti3AlC2
Comparison with Literature Results
The reaction products after melt infiltration at 1000 °C established in this work agree with the products reported by other researchers using similar compositions, but different reaction methods. For example, Zou et al. produced TiC-TiB2-Al composites between 10 and 60 wt.% Al using self-propagating high-temperature synthesis. The maximum temperature of their reaction decreased from 2900 °C and approached the investigated temperature range of this work as the Al wt.% increased. Calculations show that their Al:Ti:B:C ratio ranges from 0.8:3.0:4.0:1.0 with 10 wt.% Al, to 11.1:3.0:4.0:1.0 with 60 wt.% Al. These compositions lie on the Al-TiB2-TiC face of the quaternary phase diagram (green points represent 10, 40, and 60 wt.% Al in Fig. 10c). In addition to these phases, they reported that Al4C3 and TiAl3 were also present in small amounts as a consequence of the fact that their system was not allowed to reach equilibrium.
Zhang et al. utilized quick spontaneous infiltration to make composites from Ti-B4C-Al powder preforms (55-60% dense) dipped in molten Al at 920 °C. The nominal composition of two of their composites, with Al:Ti:B:C molar ratios of 6:3:6:1.5 and 6:3:4:1, fall on the Al-Al4C3-TiB2 and Al-TiB2-TiC faces of the quaternary phase diagram, respectively (blue points in Fig. 10c). In both composites, Al, TiB2, and TiC were the primary phases found. In the B-rich composite, some TiAl3 was also detected. Neither Al4C3 nor Al3BC was observed by XRD after infiltration or differential thermal analysis (DTA) of both composites. Consequently, they computationally determined that the likely equilibrium products of the more B-rich composite were Al3BC, TiB2, and TiAl3. Our findings show that TiAl3 is not an equilibrium product of this composition.
However, the equilibrium phases present in the B-poor composition—Al, TiB2, and TiC—are in full agreement with our results. Their conclusion that B4C is also in equilibrium with TiB2 and TiC is at odds with our results. The most likely source of these discrepancies is the fact that Zhang et al. did not allow their samples to reach equilibrium.
The 1000 °C Al-Ti-B-C quaternary phase diagram in the Al-rich corner was determined. The final Al:Ti:B:C ratios in the equilibrated microstructures were 3.8:1.3:2.9:0.6 (B-rich) and 3.4:1.1:1.3:0.7 (Ti-rich).
And while both compositions were located near the center of quaternary phase diagram, they belonged to two separate equilibrium tetrahedra. For the B-rich composition the equilibrium phases were Al, Al3BC, TiB2 and Al4C3. In the Ti-rich case, the equilibrium phases were Al, TiC, TiB2 and Al4C3.
A reaction mechanism was proposed for both compositions to explain the observed reaction products after 0.5 h MI experiments and equilibrium conditions.
This work was supported by the Army Research Office (W911NF-11-1-0525). Additionally, the authors would like to acknowledge Grady Bentzel, Darin Tallman, and Prof. El’ad Caspi for their assistance with Rietveld refinements.
- 8.J. Salem and E. Fuller, Corrosion, Wear, Fatigue, and Reliability of Ceramics, Wiley, New York, 2009Google Scholar
- 10.B. Anasori, S. Amini, V. Presser, and M.W. Barsoum, Nanocrystalline Mg-Matrix Composites with Ultrahigh Damping Properties, Magnes. Technol., 2011, 2011, p 463-468Google Scholar
- 15.M.W. Barsoum, M.C. Flemings, E.J. Kramer, S. Mahajan, and P. Veyssiere, Physical Properties of the MAX Phases, Encyclopedia of Materials Science and Technology, K.H.J. Buschow, R.W. Cahn, and M.C. Flemings, Ed., Elsevier, Amsterdam, 2006, Google Scholar
- 18.M. Sundberg, G. Malmqvist, A. Magnusson and T. El-Raghy, Alumina Forming High Temperature Silicides and Carbides, 3rd Asian Meeting on Electroceramics (AMEC-3), Dec 7-11, 2003, Elsevier, UK, 2004, p. 1899-1904Google Scholar
- 25.H. Okamoto, Al-B (Aluminum-Boron), J. Phase Equilib. Diffus., 2006, 27, p 195-196Google Scholar