Question

Diamond cannot conduct electricity but graphite can why ?

Answer 1

Answer:

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.

Explanation:

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Answer 2

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Conduction of electricity mainly depends upon presence of free electrons.

In graphite, each carbon atom is directly linked to only three carbon atoms through covalent bonds. Therefore, out of the four valence electrons in a carbon atom only three are used for bonding and the fourth is relatively free and can move from one carbon atom to other. This results in the conductivity of graphite.

In diamond, every carbon atom shares four of its available electrons with other carbon atoms, forming a tetrahedral network. Therefore diamond does not have any free electron to conduct electricity. So diamond is insulator.