Arrange the following order of property indicated for each set :
$F_{2}, C l_{2}, B r_{2}, I_{2}$ (Increasing bond dissociation enthalpy).

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Solution

Bond dissociation energy usually decreases on moving down a group as the atomic size increases. However, the bond dissociation energy of $F_{2}$ is lower than that of $C l_{2}$ and $B r_{2}$ . This is due to the small atomic size of fluorine. Thus, the increasing order for bond dissociation energy among halogens is as follows :
$I_{2} < F_{2} < B r_{2} < C l_{2}$ .

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