Account of the following observations
(a) Ammonium salts are more soluble in water than the corresponding sodium salts
(b) `BeCI_(2)` is linear but `SnCI_(2)` is angular
(c ) `F_(2)` gas is more reactive than `CI_(2)` gas
(d) The bond lengths of both `O-O` bonds in ozone are equal .

Explanation

`overset(o+)NH_(4)(sp^(3)` hybridised, tetrahedral geometry) shows dipole moment and thus is polar So it bonds with water This gives an extra intermolecular attraction Whereas, `Na^(o+)` fails to from dipole moment bonds
(b) In `BeCI_(2)` Be is sp hybridised whereas in `SnCI_(2)` Sn is `sp^(2)` hybridised and has one lp over central metal This gives an angular shape to `SnCI_(2)` molecule
(c ) The bond energy of `F_(2)` is much lower than that of `CI_(2)` (Decreasing bond energies of halogens `CI_(2) gt Br_(2) gt F_(2) gt I_(2))`
In `F_(2)` molecule due to extremely small size of F-atom higher interelectronic repulsions dominate over nuclear-electrons attractive forces (bond formation) This results in very weak bond strength of `F-F` bond Hence, `F_(2)` gas is more reactive than `CI_(2)` gas
(d) `O_(3)` molecule shows resonance which results in equal bond lenghts

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