The hybridizations of carbon in graphite,diam | vedclass

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Question

(B) Diamond,graphite,and $C_{60}$ are allotropes of carbon. In diamond,each carbon atom is bonded to four other carbon atoms in a tetrahedral geometry

Vedclass · Accepted Answer

$sp^2, sp^3, sp^2$

Vedclass · Answer

(B) Diamond,graphite,and $C_{60}$ are allotropes of carbon. In diamond,each carbon atom is bonded to four other carbon atoms in a tetrahedral geometry,resulting in $sp^3$ hybridization. In graphite,each carbon atom is bonded to three other carbon atoms in a planar hexagonal network,resulting in $sp^2$ hybridization. In $C_{60}$ (buckminsterfullerene),each carbon atom is also bonded to three other carbon atoms in a spherical structure,resulting in $sp^2$ hybridization. Therefore,the hybridizations are $sp^2, sp^3, sp^2$ respectively.

The hybridizations of carbon in graphite,diamond and $C_{60}$ are respectively

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