Compare the alkali metals and alkaline earth metals with respect to
(i) ionisation enthalpy
(ii) basically of oxides and
(iii) solubility of hydroxides

Explanation

(i) Ionization enthalpy `(DeltaH)`: Because of higher nuclear charge, the `DeltaA` Hof alkaline earth metals are higher than those of the corresponding alkali metals.
(ii) Basicity of oxide: The oxides of alkali and alkaline earth metals dissolve in water to form their respective hydroxides. These hydroxides are strong bases. However, since the ionization enthalpy of alkali metals is lower or the electropositive character of alkali metals is higher than that of the corresponding alkaline earth metal, therefore, the M-OH bond in alkali metals can more easily ionize `(MOHtoM^(+)OH)`, than in alkaline earth metals and hence alkali metal oxides are more basic than the corresponding alkaline earth metal oxides
(iii) Solubility of hydroxides: Because of smaller size and higher ionic charge, the lattice enthalpies of alkaline earth metals are much higher than that of the alkaline earth metal hydroxides. However the solubility of the hydroxides of both alkali and alkaline earth metals increase down the group due to larger decrease in their lattice enthalpies as compared to their hydration enthalpies