When zeolite, which is hydrated sodium aluminium silicate is treated with hard water, the sodium ions are exchanged with which of the following ion(s)?
Identify the correct formula of halides of alkaline earth metals from the following.
Choose the correct statements from the following.
Which of the following are the correct reasons for anomalous behaviour of lithium?
How do you account for the strong reducing power of lithium in aqueous solution?
Strong reducing power of lithium in aqueous solution can be understood in terms of electrode potential. Electrode potential is a measure of the tendency of an element to lose electrons in the aqueous solution. It mainly depends upon the following three factors i.e.,
(i) $\mathrm{Li}(\mathrm{s}) \xrightarrow[\text { Enthalpy }]{\text { Sublimation }} \mathrm{Li}(g)$
(ii) $\mathrm{Li}(g) \xrightarrow[\text { Enthalpy }]{\text { Ionisation }} \mathrm{Li}^{+}(g)+\mathrm{e}^{-}$
(iii) $\mathrm{Li}^{+}(g)+a q \longrightarrow \mathrm{Li}^{+}(a q)+$ enthalpy of hydration
With the small size of its ion, lithium has the highest hydration enthalpy. However, ionisation enthalpy of Li is highest among alkali metals but hydration enthalpy predominates over ionisation enthalpy.
Therefore, lithium is the strongest reducing agent in aqueous solution mainly because of its high enthalpy of hydration.