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

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(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.

Vedclass · Answer

(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:

Similar Questions

Which of the following compounds does not show resonance?

All bond lengths are identical in :-

Give rules for writing resonance structures.

During the formation of the dimer $N_2O_4$ from two molecules of $NO_2$,what happens to the unpaired electron on the nitrogen atom of each $NO_2$ molecule?

$(i)$ Draw the resonance structures of $N_2O_3$ and state its shape.
$(ii)$ Indicate the bond angles and bond lengths in it.

Vedclass Test Series

Exam Paper Generator

Online Exam Module