In graphite,electrons are

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(D) In graphite,each carbon atom is $sp^2$ hybridized and uses $3$ of its $4$ valence electrons to form covalent bonds with $3$ other carbon atoms in

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Spread out between the structure

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(D) In graphite,each carbon atom is $sp^2$ hybridized and uses $3$ of its $4$ valence electrons to form covalent bonds with $3$ other carbon atoms in a hexagonal layer.The fourth electron remains in an unhybridized $p$-orbital,which overlaps with adjacent $p$-orbitals to form a delocalized $\pi$-electron cloud.Therefore,these electrons are spread out between the layers of the structure,allowing graphite to conduct electricity.

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