Question

why is graphite a good conductor of electricity but diamond is non conductor of electricity​

Answer 1

Explanation:

Graphite can conduct electricity because of the delocalised (free) electrons in its structure. ... However, in diamond, all 4 outer electrons on each carbon atom are used in covalent bonding, so there are no delocalised electrons.

Answer 2

Graphite is a good conductor of heat and electricity because in graphite each carbon atom has a free electron in its valance shell, free electron are responsible for conductivity of electricity. Diamond is a giant covalent structure; each valence electron (outer shell electron) of every carbon atom forms a covalent bond, which means that there are no free electrons. Since electrical conductivity relies on the flow of free electrons, diamond is not a good conductor.

Explanation:

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