The hybridisation of C in diamond,graphite an | vedclass

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(B) The hybridization of carbon in the given compounds is determined by the number of sigma bonds and lone pairs attached to the carbon atom.$1$. In d

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$sp^3, sp^2, sp$

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(B) The hybridization of carbon in the given compounds is determined by the number of sigma bonds and lone pairs attached to the carbon atom.$1$. In diamond,each carbon atom is bonded to four other carbon atoms via single bonds,resulting in $sp^3$ hybridization.$2$. In graphite,each carbon atom is bonded to three other carbon atoms in a planar hexagonal structure,resulting in $sp^2$ hybridization.$3$. In ethyne $(C_2H_2)$,each carbon atom is bonded to one hydrogen atom and one other carbon atom via a triple bond,resulting in $sp$ hybridization.Therefore,the order is $sp^3, sp^2, sp$.

The hybridisation of $C$ in diamond,graphite and ethyne is in the order

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