In which allotrope of carbon does each carbon | vedclass

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(C) Carbon has an electronic configuration of $2, 4$. In diamond, each carbon atom is $sp^3$ hybridized and forms four strong covalent bonds with four

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Diamond

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(C) Carbon has an electronic configuration of $2, 4$. In diamond, each carbon atom is $sp^3$ hybridized and forms four strong covalent bonds with four other carbon atoms in a tetrahedral arrangement. In graphite, each carbon atom is $sp^2$ hybridized and forms three covalent bonds with other carbon atoms, leaving one electron delocalized. In $C_{60}$ (fullerene), each carbon atom is also $sp^2$ hybridized and forms three bonds.

In which allotrope of carbon does each carbon atom form four bonds with other carbon atoms?

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