Which one of the following orders is correct for the bond dissociation enthalpy of halogen molecules

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

${Cl}_{2} > {Br}_{2} > F_{2} > I_{2}$

${Br}_{2} > I_{2} > F_{2} > {Cl}_{2}$

$F_{2} > {Cl}_{2} > {Br}_{2} > I_{2}$

answer is B.

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Detailed Solution

Bond dissociation energy of halogen family decreases down the group as the size of atom increases.

The decreasing order for the bond dissociation enthalpy of halogen molecules is

Cl₂ 57 kcal/mol>Br₂ 45.5 kcal/mol>F₂ 38 kcal/mol>I₂ 35.6 kcal/mol.

A halogen molecule having larger atoms should have low dissociation energy and vice versa. Fluorine is an exception because of interelectronic repulsion is present in small atom fluorine.

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