Question

In graphite c-c bond length (141 pm) found to be shorter than normal c-c bond length (154 pm) this anomaly occurs due to

Answer 1

Answer:

There is pπ-pπ bond delocalised within the layer

Explanation:

Answer 2

Solution:

• In graphite, each carbon atom is $sp^2$ hybridized and is bonded to three other carbon atoms through a sigma bond while the fourth electron forms a $\pi -$bond.

• As the percentage s - character increases in the hybrid orbitals forming the bonds, the bond length decreases.
• The increasing order of percentage s - character is as follows:

          $sp^3 < sp^2 < sp$

• So, the decreasing order of bond length is as follows:

        $sp^3 - sp^3 > sp^3 - sp^2 > sp^2 - sp^2 > sp^3 - sp > sp^2 - sp > sp - sp$

Hence, in graphite, having $sp^2$ hybridization,  c-c bond length (141 pm) is found to be shorter than normal c-c bond length (154 pm)