Answer:
(i) Ionisation enthalpy: On
account of higher nuclear charge and smaller radii, the first ionization enthalpies
of alkaline earth metals are higher than those of corresponding alkali metals.
However, second ionisation enthalpies of alkaline earth metals are lower than
those of corresponding alkali metals as alkali metals ions \[({{M}^{+}})\] have
inert gas configurations.
(ii) Basicity of
oxides: The oxides of both alkali and alkaline earth metals are basic in
nature. They combine with water and form strong bases. However, the hydroxides
of alkali metals easily ionise to furnish \[O{{H}^{-}}\]ions as their ionization
enthalpies are lower than alkaline earth metals. Hence, the oxides of alkali
metals are more basic than the corresponding alkaline earth metal oxides.
(iii) Solubility
of hydroxides: On account of smaller size and higher charge on the ions of
alkaline earth metals, the lattice energies of the hydroxides of alkaline earth
metals are much higher than those of the alkali metal hydroxides. Hence, the solubility
of hydroxides of alkaline earth metals is lower than corresponding hydroxides
of alkali metals. However, solubility increases in both the groups from top to
bottom.
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