Question
Graphite is a covalent solid yet soft and good conductor of electricity.
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Answer
- Each carbon atom in graphite is $sp^2$ hybridised and covalently bonded to other three $sp2$ hybridised carbon atoms forming σ bonds and the fourth electron in $2p_z$ orbital of each carbon atom is used in the formation of a π bond. This results in the formation of hexagonal rings in two dimensions.
- In graphite, the layers consisting of hexagonal carbon network are held together by weak van der Waal’s forces imparting softness.
- The electrons in π bonds in the ring are delocalised and free to move in the delocalised molecular orbitals giving good electrical conductance.
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