Diamond is extremely hard whereas graphite is | vedclass

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(C) In $diamond$, each carbon atom is $sp^3$ hybridized and bonded to $4$ other carbon atoms in a rigid, three-dimensional tetrahedral network. This s

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each carbon atom in $diamond$ is chemically bonded to a greater number of neighbouring carbon atoms

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(C) In $diamond$, each carbon atom is $sp^3$ hybridized and bonded to $4$ other carbon atoms in a rigid, three-dimensional tetrahedral network. This structure prevents the movement of atoms, making it extremely hard.In $graphite$, each carbon atom is $sp^2$ hybridized, forming planar hexagonal layers. These layers are held together by weak $van \ der \ Waals$ forces, which allow the layers to slide over each other, making $graphite$ soft.

Diamond is extremely hard whereas graphite is soft. This is because

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