Which of the followin option is correct for the bond dissociation ethalpy of halogen molecules?

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

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

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

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

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Solution

The correct option is B $C l_{2} > B r_{2} > F_{2} > I_{2}$
The order of bond dissociation enthalpy is:
$C l_{2} > B r_{2} > F_{2} > I_{2}$
A reason for this anomaly is the relatively large electron-electron repulsion among the lone pairs in $F_{2}$ molecule where they are much closer to each other than in case of $C l_{2}$ .
$∴$ Option b is correct.

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