Question

graphite is a conductor but diamond is not why?​

Answer 1

$\huge\star{your{\mathfrak{\red{answer}}}}♬$

Graphite can conduct electricity because of the delocalised (free) electrons in its structure. These arise because each carbon atom is only bonded to 3 other carbon atoms. However, in diamond, all 4 outer electrons on each carbon atom are used in covalent bonding, so there are no delocalised electrons.

$\sf\green{hope \: it \: helps \: you.....∞}$

Answer 2

$\mathsf\red{The \: carbon \: atoms \: are \: bonded \: differently \: in \: each \: substance.}$

Explanation:

$\mathsf\red{☆}$ These substances are allotropes, which are substances that are made of the same elements but have different structures based on their bonding patterns.

$\mathsf\red{☆}$ Graphite consists of several 2D layers of covalently bonded atoms stacked together. Their configuration in this substance allows electrons to flow freely and thus conduct electricity, which is merely the flow of electrons from one place to another.

$\mathsf\red{☆}$ Diamond on the other hand consists of a 3D lattice structure with each carbon atom bonded to four other carbon atoms in a tetrahedral shape. This structure is extremely strong, but it keeps electrons in place, which is why diamond cannot conduct an electrical current.