In graphite, the C-C bond length (141.5 , pm) | vedclass

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(A) In graphite, each carbon atom is $sp^2$ hybridised and forms three sigma bonds with other carbon atoms in a hexagonal planar network. The fourth v

Vedclass · Accepted Answer

There is $p\pi-p\pi$ bond delocalisation within the layer.

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(A) In graphite, each carbon atom is $sp^2$ hybridised and forms three sigma bonds with other carbon atoms in a hexagonal planar network. The fourth valence electron of each carbon atom remains in an unhybridised $p$-orbital, which overlaps laterally with the $p$-orbitals of adjacent carbon atoms to form a $p\pi-p\pi$ delocalised bond system across the entire layer. This partial double bond character reduces the $C-C$ bond length from the standard single bond value of $154 \, pm$ to $141.5 \, pm$.

In graphite, the $C-C$ bond length $(141.5 \, pm)$ is found to be shorter than the normal $C-C$ single bond length $(154 \, pm)$. This anomaly occurs due to:

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