Which of the following will have the highest | vedclass

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(B) The bond energy of halogens is influenced by the small size of the fluorine atom,which leads to significant inter-electronic repulsion between the

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$Cl_2$

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(B) The bond energy of halogens is influenced by the small size of the fluorine atom,which leads to significant inter-electronic repulsion between the lone pairs of the two fluorine atoms. This makes the $F-F$ bond weaker than the $Cl-Cl$ bond. The general order of bond dissociation energy for halogens is $Cl_2 > Br_2 > F_2 > I_2$. Therefore,$Cl_2$ has the highest bond energy.

Which of the following will have the highest bond energy?

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The bond dissociation energy of $B-F$ in $BF_3$ is $646 \ kJ \ mol^{-1}$ whereas that of $C-F$ in $CF_4$ is $515 \ kJ \ mol^{-1}.$ The correct reason for higher $B-F$ bond dissociation energy as compared to that of $C-F$ is

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