The C-C bond length is maximum in | vedclass

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(C) In $diamond$, each carbon atom is $sp^3$ hybridized and forms four single $C-C$ sigma bonds. The bond length of a pure $C-C$ single bond is $154 \

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diamond

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(C) In $diamond$, each carbon atom is $sp^3$ hybridized and forms four single $C-C$ sigma bonds. The bond length of a pure $C-C$ single bond is $154 \ pm$. In $graphite$ and fullerenes ($C_{60}$, $C_{70}$), the carbon atoms are $sp^2$ hybridized, resulting in resonance and partial double bond character. Partial double bond character leads to a shorter bond length (approximately $141.5 \ pm$ in graphite). Therefore, the $C-C$ bond length is maximum in diamond.

Column-$I$	Column-$II$
$A$. $BF_4^-$	$1$. Oxidation state of central atom is $+4$
$B$. $AlCl_3$	$2$. Strong oxidizing agent
$C$. $SnO$	$3$. Lewis acid
$D$. $PbO_2$	$4$. Can be further oxidized
	$5$. Tetrahedral shape

The $C-C$ bond length is maximum in

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