Which among the following molecules has the l | vedclass

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(D) The bond dissociation enthalpy of halogens generally decreases down the group due to an increase in atomic size. However,$F_2$ is an exception bec

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$I_2$

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(D) The bond dissociation enthalpy of halogens generally decreases down the group due to an increase in atomic size. However,$F_2$ is an exception because of the small size of the fluorine atom. In $F_2$,the lone pairs on the fluorine atoms experience significant inter-electronic repulsion,which weakens the $F-F$ bond. Therefore,$F_2$ has a lower bond dissociation enthalpy than $Cl_2$ and $Br_2$,but $I_2$ has the lowest bond dissociation enthalpy due to the largest atomic size and longest bond length.

Which among the following molecules has the lowest bond dissociation enthalpy?

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