Which of the following has the maximum bond d | vedclass

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(B) The bond dissociation enthalpy depends on the size of the atoms and the lone pair-lone pair repulsion.For $O-O$,$N-N$,and $F-F$,the atoms are smal

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$C-C$

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(B) The bond dissociation enthalpy depends on the size of the atoms and the lone pair-lone pair repulsion.For $O-O$,$N-N$,and $F-F$,the atoms are small and have lone pairs that cause significant inter-electronic repulsion,weakening the bond.$C-C$ is a single covalent bond between carbon atoms which does not suffer from such lone pair repulsion.Therefore,the $C-C$ bond has a higher bond dissociation enthalpy compared to the others listed.

Which of the following has the maximum bond dissociation enthalpy?

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The electronic configuration of three elements $A$,$B$ and $C$ are given below. Stable form of $C$ may be represented by the formula
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$C : 1s^2, 2s^2, 2p^6, 3s^2, 3p^5$

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