In chemistry, a carbide is a compound composed of carbon and a less electronegative element. Carbides can be generally classified by chemical bonding type as follows: (i) salt-like, (ii) covalent compounds, (iii) interstitial compounds, and (iv) "intermediate" transition metal carbides. Examples include calcium carbide, silicon carbide, tungsten carbide (often called simply carbide), and cementite, each used in key industrial applications.
Salt-like carbides are composed of highly electropositive elements such as the alkali metals, alkaline earths, and group 3 metals including scandium, yttrium and lanthanum. Aluminium from group 13 forms carbides, but gallium, indium and thallium do not. In these materials feature isolated carbon centers, often described as "C4−"; two atom units, "C22−"" in the acetylides and three atom units "C34−" in the sesquicarbides. These formal anion C4−, sometimes called methanides (or methides) because they hydrolyse to give methane gas. The naming of ionic carbides is not consistent and can be quite confusing.
The monatomic ion C4− would be highly basic and is unknown except under extreme conditions (single atoms with negative charges greater than 1- are unknown, their description as anions represents a drastic simplification). Methanides in principle would react with water to form methane.
C4– + 4 H+ → CH4
Examples of compounds that are described as methanides include C4– are Be2C and Al4C3.
Several carbides are assumed to be salts of the acetylide anion C22−" , which has a triple bond between the two carbon atoms. Alkali metals, alkaline earth metals, and lanthanoid metals form acetylides, e.g., sodium carbide Na2C2, calcium carbide CaC2, and LaC2. Lanthanoids also form acetylides with formula M2C3. Metals from group 11 too tend to form acetylides, such as copper(I) acetylide and silver acetylide. Carbides of the actinide elements, which have stoichiometry MC2 and M2C3, are also described as salt-like derivatives of C22−".
The C-C triple bond length ranges from 109.2 pm in CaC2 (similar to ethyne), to 130.3 pm in LaC2 and 134 pm in UC2. The bonding in LaC2 has been described in terms of LaIII with the extra electron delocalised into the antibonding orbital on C22−, explaining the metallic conduction.
The polyatomic ion C34−, sometimes called sesquicarbide, is found in Li4C3, Mg2C3. The ion is linear and is isoelectronic with CO2. The C-C distance in Mg2C3 is 133.2 pm. Mg2C3 yields methylacetylene, CH3CCH, on hydrolysis which was the first indication that it may contain C34−.
The carbides of silicon and boron are described as "covalent carbides", although virtually all compounds of carbon exhibit some covalent character. Silicon carbide has two similar crystalline forms, which are both related to the diamond structure. Boron carbide, B4C, on the other hand has an unusual structure which includes icosahedral boron units linked by carbon atoms. In this respect boron carbide is similar to the boron rich borides. Both silicon carbide, SiC, (carborundum) and boron carbide, B4C are very hard materials and refractory. Both materials are important industrially. Boron also forms other covalent carbides, e.g. B25C.
The carbides of the group 4, 5 and 6 transition metals (with the exception of chromium) are often described as interstitial compounds. These carbides have metallic properties and are refractory. Some exhibit a range of stoichiometries, e.g. titanium carbide, TiC. Titanium carbide and tungsten carbide are important industrially and are used to coat metals in cutting tools.
The longheld view is that the carbon atoms fit into octahedral interstices in a close packed metal lattice when the metal atom radius is greater than approximately 135 pm:
* When the metal atoms are cubic close packed, (ccp), then filling all of the octahedral interstices with carbon achieves 1:1 stoichiometry with the rock salt structure, (note that in rock salt, NaCl, it is the chloride anions that are cubic close packed).
The following table shows actual structures of the metals and their carbides. (N.B. the body centred cubic structure adopted by vanadium, niobium, tantalum, chromium, molybdenum and tungsten is not a close packed lattice.) The notation "h/2" refers to the M2C type structure described above, which is only an approximate description of the actual structures. The simple view that the lattice of the pure metal "absorbs" carbon atoms can be seen to be untrue as the packing of the metal atom lattice in the carbides is different from the packing in the pure metal.
For a long time the non-stoichiometric phases were believed to be disordered with a random filling of the interstices, however short and longer range ordering has been detected.
In these carbides, the transition metal ion is smaller than the critical 135 pm, and the structures are not interstitial but are more complex. Multiple stoichiometries are common, for example iron forms a number of carbides, Fe3C, Fe7C3 and Fe2C. The best known is cementite, Fe3C, which is present in steels. These carbides are more reactive than the interstitial carbides, for example the carbides of Cr, Mn, Fe, Co and Ni all are hydrolysed by dilute acids and sometimes by water, to give a mixture of hydrogen and hydrocarbons. These compounds share features with both the inert interstitials and the more reactive salt-like carbides.
Metal complexes containing Cn fragments are well known. Most common are carbon-centered clusters, such as [Au6C(PPh3)6]2+. Similar species are known for the metal carbonyls and the early metal halides. Even terminal carbides have been crystallized, e.g., CRuCl2(P(C6H11)3)2.
Some metals, such as lead and tin, are believed not to form carbides under any circumstances. There exists however a mixed titanium-tin carbide, which is a two-dimensional conductor. (In 2007, there were two reports of a lead carbide PbC2, apparently of the acetylide type; but these claims have yet to be published in reviewed journals.)
In addition to the carbides, other groups of related carbon compounds exist:
* graphite intercalation compounds
1. ^ a b c d e f g h i j k l Greenwood, Norman N.; Earnshaw, A. (1984), Chemistry of the Elements, Oxford: Pergamon, pp. 318–22, ISBN 0-08-022057-6