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| 1. |
Arrange the following in the order of the property indicated for each set : F_(2), Cl_(2), Br_(2), I_(2) (Increasing bond dissocation energy) |
| Answer» Solution :`F_(2)` has exceptionally low bond dissociation ENTHALPY. Lone PAIRS in `F_(2)` molecule are much CLOSER to each other than in `Cl_(2)` molecule. Stronger electron-electron repulsions among the lone pairs in `F_(2)` molecule MAKE its bond dissociation enthalpy exceptionally low, `I_(2) < F_(2) < Br_(2) < Cl_(2)` | |