Question

Hybridised states of carbon in Graphite and Diamond are respectively

• A. $sp^3,sp^3$
• B. $sp^3,sp^2$
• C. $sp^2,sp^2$
• D. $sp^2,sp^3$

Answer 1

Answer: (D)

$sp^2,sp^3$

Answer 2

In graphite, carbon is $s p^{2}$ hybridised. Each carbon is thus linked to three other carbon atoms forming hexagonal rings. On the other hand, in diamond carbon is $sp ^{3}$ hybridised. Each carbon is tetrahedrally linked to four strong $C - C$, $s p^{3}-s p^{3} \sigma$ -bonds.