<Table> <Tr> <Td> </Td> <Td> This article needs additional citations for verification . Please help improve this article by adding citations to reliable sources . Unsourced material may be challenged and removed . (October 2013) (Learn how and when to remove this template message) </Td> </Tr> </Table> <Tr> <Td> </Td> <Td> This article needs additional citations for verification . Please help improve this article by adding citations to reliable sources . Unsourced material may be challenged and removed . (October 2013) (Learn how and when to remove this template message) </Td> </Tr> <P> A carbon--carbon bond is a covalent bond between two carbon atoms . The most common form is the single bond: a bond composed of two electrons, one from each of the two atoms . The carbon--carbon single bond is a sigma bond and is formed between one hybridized orbital from each of the carbon atoms . In ethane, the orbitals are sp - hybridized orbitals, but single bonds formed between carbon atoms with other hybridisations do occur (e.g. sp to sp). In fact, the carbon atoms in the single bond need not be of the same hybridisation . Carbon atoms can also form double bonds in compounds called alkenes or triple bonds in compounds called alkynes . A double bond is formed with an sp - hybridized orbital and a p - orbital that isn't involved in the hybridization . A triple bond is formed with an sp - hybridized orbital and two p - orbitals from each atom . The use of the p - orbitals forms a pi bond . </P> <P> Carbon is one of the few elements that can form long chains of its own atoms, a property called catenation . This coupled with the strength of the carbon--carbon bond gives rise to an enormous number of molecular forms, many of which are important structural elements of life, so carbon compounds have their own field of study: organic chemistry . </P>

What types of molecules can carbon bind to
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