Ionic mobility of `Li^(+)` is less than `Na^(+) and K^(+)` because

Alkali metal salts ionic and soluble in water. The solubility of an ionic compound depends on (i) lattic ethalpy and (ii) hydration enthalpy. These two factor oppose each other. If hydration ethalpy is high, the ions will have greater tendency to be hydrated and therefore the solubility will be high. The smaller the cation, the greater is the degree of hydration. The reducing behaviour of alkali metals in solution is also dependent on the hydration enthalpy besides other factors. The ionic mobility of Li^(o+) is less than of the Na^(o+) ion in solution because

Alkali metal salts ionic and soluble in water. The solubility of an ionic compound depends on (i) lattic ethalpy and (ii) hydration enthalpy. These two factor oppose each other. If hydration ethalpy is high, the ions will have greater tendency to be hydrated and therefore the solubility will be high. The smaller the cation, the greater is the degree of hydration. The reducing behaviour of alkali metals in solution is also dependent on the hydration enthalpy besides other factors. The ionic mobility of Li^(o+) is less than of the Na^(o+) ion in solution because

The ionic mobility of Li^(+) is less than that of the Na+ ion in solution because

IE of Li^(-) will be more than Na^(-) ?

Assertion (A): The mobility of Na^(o+) is lower than that of K^(o+) ion. Reason (R): The ionic mobility depends upon the effective radius of the ion.

Assertion (A): The mobility of Na^(o+) is lower than that of K^(o+) ion. Reason (R): The ionic mobility depends upon the effective radius of the ion.

Assertion: Na^(+) and Al^(3+) are isoelectronic but the magnitude of the ionic radius of Al^(3+) is less than that of Na^(+) Reason: The magnitude of effective nuclear charge of the outer shell electrons in Al^(3+) is greater than in Na^(+)