Carbon, a chemical element, has the symbol C with 6 as the atomic number. Carbon has a unique property to form bonds with other carbon atoms to form long chains, which may be straight, branched or even rings.
The carbon atoms may be linked by double or triple bond in addition to single bonds.
The carbon-carbon bond is very strong and hence stable. Carbon is also tetravalent. Because of these reasons, the number of carbon compounds is so large.

Let us study some more terms related to Carbon and the compounds formed by it.

Allotropes: The existence of elements in two or more different forms having different physical properties but with identical chemical properties.

Allotropism: The phenomenon of existence of an element in two or more physically different forms but with similar chemical properties.

Diamond: An allotrope of Carbon, in which each carbon atom lies at the centre of a regular tetrahedron and is covalently bonded with four carbon atoms located at the four corners of the regular tetrahedron.

Diamond

Graphite: An allotrope of Carbon, in which each carbon atom is covalent bonded with 3 neighboring carbon atoms forming layers of hexagonal networks separated by larger distance.

Graphite


Fullerene: An allotropic form of carbon in which 60 carbon atoms are arranged in the shape of a football.

Fullerene


Difference between Diamond and Graphite: Diamond is hard. It cannot conduct electricity. It is transparent.
On the other hand, Graphite is soft. Graphite can conduct electricity. It is greyish black in color.

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