The bond dissociation energies of F_2, Cl_2, | vedclass

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(C) Bond strength is directly proportional to bond dissociation energy. Since $Cl_2$ has the highest bond dissociation energy $(58 \ kcal/mol)$,it pos

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$Cl_2$

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(C) Bond strength is directly proportional to bond dissociation energy. Since $Cl_2$ has the highest bond dissociation energy $(58 \ kcal/mol)$,it possesses the strongest bond. Although $F_2$ is the smallest,the $F-F$ bond is weaker than the $Cl-Cl$ bond due to significant inter-electronic repulsion between the lone pairs of the small fluorine atoms.

The bond dissociation energies of $F_2, Cl_2, Br_2$ and $I_2$ are $37, 58, 46$ and $36 \ kcal/mol$ respectively. Which of these has the strongest bond?

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