Carbide

Calcium carbide
In chemistry, a carbide is a compound of carbon with a less electronegative element.[1] Many carbides are important industrially; for example, calcium carbide (CaC2) is a feedstock for the chemical industry and iron carbide (Fe3C, cementite) is formed in steels to improve their properties.
In general, carbides are classified according to the chemical bonding in the compounds, as follows:

salt-like ionic carbides;
covalent carbides;
interstitial carbides;
"intermediate" transition metal carbides. (In bonding terms, they sit between the salt-like and interstitial carbides.)
Contents

1 Ionic carbides

1.1 Acetylides
1.2 Methanides
1.3 Sesquicarbides


2 Covalent carbides
3 Interstitial carbides

3.1 Properties
3.2 Structure


4 Intermediate transition metal carbides
5 Some carbides and their uses
6 See also
7 Notes
8 References
9 Credits


Ionic carbides
Salt-like, ionic carbides are formed by the following metals:

group one metals (the alkali metals);
group two metals (the alkaline earths);
group three metals (scandium, yttrium, and lanthanum);
group 11 metals (copper, silver, and gold);
group 12 metals (zinc, cadmium, and mercury);
only aluminum from group 13, (gallium, indium and thallium do not appear to form carbides);
lanthanides, when forming MC2 and M2C3 carbides (where M is the metal);
actinides, when forming MC2 and M2C3 carbides.
Most commonly, they are salts of C22− and are called acetylides, ethynides, acetylenediides, or (rarely) percarbides. 

Some ionic carbides contain other anionic species, such as:

C4−, sometimes called methanides (or methides) because they hydrolyze to give methane gas;
C34− ion, sometimes called sesquicarbides, which hydrolyze to give methylacetylene.
The naming of ionic carbides is not consistent and can be quite confusing.

Acetylides
Acetylides contain the polyatomic ion C22−, in which there is a triple bond between the two carbon atoms (similar to acetylene). Examples are carbides of the alkali metals (such as Na2C2), some alkaline earths (such as CaC2) and lanthanoids (such as LaC2).
The C-C bond distance ranges from 109.2 picometers (pm) in CaC2 (similar to acetylene), to 130.3 pm in LaC2 and 134pm in UC2.

Methanides
Methanides contain the monatomic ion C4−. Examples of methanides are Be2C and Al4C3.
The C4− ion is a very strong base and will combine with four protons to form methane. The reaction may be written as follows:

C4− + 4H+ → CH4

Methanides commonly react with water to form methane, but reactions with other substances are also common.

Sesquicarbides
The polyatomic ion C34− is found in, for instance, Li4C3 and Mg2C3. The ion is linear and isoelectronic with CO2. The C-C distance in Mg2C3 is 133.2 pm.[2] Hydrolysis of Mg2C3 yields methylacetylene (CH3CCH), which was the first indication that it may contain C34−.

Covalent carbides
Silicon and boron form covalent carbides. Silicon carbide (SiC, or carborundum) has two similar crystalline forms, both of which are related to the structure of diamond. 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 and boron carbide are very hard, refractory (heat-resistant) materials. Both are important industrially. Boron also forms other covalent carbides, such as B25C.

Interstitial carbides
Properties
The carbides of transition metals of groups four, five, and six (with the exception of chromium) are often described as interstitial compounds. They are chemically quite inert, have metallic properties, and are refractory. Some exhibit a range of stoichiometries (that is, the metal and carbon atoms can be combined in different proportions). Titanium carbide and tungsten carbide are important industrially and are used to coat metals in cutting tools.

Structure
The carbon atoms are thought to fit into octahedral interstices in the metal lattice, when the metal atom radius is greater than 135 pm. If the metal atoms are cubic close packed (face-centered cubic), then eventually all the interstices could be filled to give a 1:1 stoichiometry, with the rock salt structure, as in the case of tungsten carbide (WC). When the metal atoms are hexagonal close packed, then only half the interstices are filled, giving a stoichiometry of 2:1, as in the case of divanadium carbide (V2C).
The following table shows actual structures of metals and their carbides. The notation "h/2" refers to the V2C-type structure mentioned above, which is an approximate description of the actual structures. The simple view that the lattice of the pure metal "absorbs" carbon atoms is true only for the monocarbides of vanadium (VC) and niobium (NbC).



Metal

Structure

Metallic radius (pm)

MC structure

M2C structure

Other carbides


titanium

hexagonal

147

rock salt






zirconium

hexagonal

160

rock salt






hafnium

hexagonal

159

rock salt






vanadium

cubic body centered

134

rock salt

h/2

V4C3


niobium

cubic body centered

146

rock salt

h/2

Nb4C3


tantalum

cubic body centered

146

rock salt

h/2

Ta4C3


chromium

cubic body centered

128





Cr23C6, Cr3C, Cr7C3, Cr3C2


molybdenum

cubic body centered

139

hexagonal

h/2

Mo3C2


tungsten

cubic body centered

139

hexagonal

h/2



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.[3]

Intermediate transition metal carbides
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 of these 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 are all hydrolyzed 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.

Some carbides and their uses
Calcium carbide (CaC2): It is used for the production of acetylene and calcium cyanamide (CaCN2), which is used in fertilizers. It is also important for the desulfurization of iron.
Silicon carbide (SiC), or carborundum: It is used as an abrasive and in ceramics.
Tungsten carbide (often called simply carbide): Being extremely hard, it is useful for the manufacture of cutting tools, abrasives, and bearings.
Cementite (iron carbide; Fe3C): It is an important constituent of steel.
Boron carbide: It is used in cutting tools, dies, and anti-ballistic armor plating. It is an effective absorbent of neutron radiation in nuclear power plants.
Tantalum carbide: It is an extremely hard, refractory, ceramic material, used in tool bits for cutting tools.
Titanium carbide: Similar to tantalum carbide, it is an extremely hard, refractory, ceramic material.
See also
Carbon
Chemical compound
Notes

↑ Some binary carbon compounds are not called carbides. They include: (a) graphite intercalation compounds; (b) alkali metal fullerides; (c) endohedral fullerenes, where the metal atom is encapsulated within a fullerene molecule; and (d) metallacarbohedrenes (met-cars), which are cluster compounds containing C2 units.

↑  Fjellvag H. and Pavel K. Crystal Structure of Magnesium Sesquicarbide. Chem. 1992, 31, 3260.

↑ de Novion, C.H., and J.P. Landesman. 1985. "Order and disorder in transition metal carbides and nitrides: experimental and theoretical aspects," Pure & Appl. Chem. 57 (10): 1391.


ReferencesISBN links support NWE through referral fees
Brown Jr., Theodore L., H. Eugene LeMay, Bruce Edward Bursten, and Julia R. Burdge. 2002. Chemistry: The Central Science. 9th ed. Upper Saddle River, NJ: Prentice Hall.
Chang, Raymond. 2006. Chemistry. 9th ed. New York, NY: McGraw-Hill Science/Engineering/Math.
Cotton, F. Albert, and Geoffrey Wilkinson. 1980. Advanced Inorganic Chemistry. 4th ed. New York, NY: Wiley. ISBN 0-471-02775-8.
Ettmayer, Peter, and Walter Lengauer. 1994. Carbides: transition metal solid state chemistry. In Encyclopedia of Inorganic Chemistry. Editor in chief R. Bruce King. Chichester, UK: Wiley. ISBN 0-471-93620-0.
Greenwood, N.N., and A. Earnshaw. 1998. Chemistry of the Elements. 2nd ed. Oxford, U.K.; Burlington, MA: Butterworth-Heinemann, Elsevier Science. ISBN 0750633654. Online version available here Retrieved January 4, 2008.
Inorganic compounds containing carbonCommon oxides:  CO2 · CO — Exotic oxides:  C3O2 · C2O · CO3
Compounds derived from oxides: Metal carbonyls · Carbonic acid · Bicarbonates · Carbonates 
Ionic compounds: Cyanides · Isocyanide · Cyanates · Thiocyanates · Carbides


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