The correct order of bond dissociation enthalpy of halogens is

C l_{2} > B r_{2} > F_{2} > I_{2}

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F_{2} > C l_{2} > B r_{2} > I_{2}

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$C l_{2} > F_{2} > B r_{2} > I_{2}$

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$I_{2} > B r_{2} > C l_{2} > F_{2}$

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Solution

The correct option is A $C l_{2} > B r_{2} > F_{2} > I_{2}$
Answer (1)

Bond dissociation energy of halogen family decreases down the group as the size of atom increases. But $F_{2}$ has $F — F$ , $F_{2}$ involves repulsion of non-bonding electrons and more over its size is small. So, due to repulsions its bond becomes weak and hence bond dissociation energy is very low.

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