Answer:
(i) Due to small size of Beryllium ion,\[BeO\]is
covalent and polymeric in nature and hence, is insoluble in water.
The hydration energy
of\[BeS{{O}_{4}}\] is higher than its lattice energy and hence it is soluble in
water.
(ii) Both \[BaO\]
and \[BaS{{O}_{4}}\] are ionic compounds. The size of \[{{O}^{2-}}\]ion is very
small in size in comparison to size of \[SO_{4}^{2-}\]ion while \[B{{a}^{2+}}\]
ion is comparatively a large ion. Since, bigger anion stabilizes a bigger
cation,\[BaS{{O}_{4}}\] is more stable than\[BaO\]. Hence,\[BaO\] is soluble
due to small size of \[{{O}^{2-}}\]ion and high hydration energy while\[BaS{{O}_{4}}\]
is insoluble due to low hydration energy.
(iii) Covalent character of \[LiI\] is greater than that of \[KI\]
hence \[LiI\] is more soluble in ethanol (non-polar solvent) than \[KI\].
You need to login to perform this action.
You will be redirected in
3 sec