Why does sodium react more vigorously with water than Lithium?

The reactions of Sodium and Lithium with water

• $\underset{\left(\mathrm{Sodium}\right)}{2\mathrm{Na}\left(\mathrm{s}\right)}+\underset{\left(\mathrm{Water}\right)}{2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)}\to \underset{\left(\mathrm{Sodium}\mathrm{Hydraoxide}\right)}{2\mathrm{NaOH}\left(\mathrm{aq}\right)}+\underset{\left(\mathrm{Hydrogen}\mathrm{gas}\right)}{{\mathrm{H}}_2\left(\mathrm{g}\right)}$
• $\underset{\left(\mathrm{Lithium}\right)}{2\mathrm{Li}\left(\mathrm{s}\right)}+\underset{\left(\mathrm{Water}\right)}{2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)}\to \underset{\left(\mathrm{Lithium}\mathrm{Hydraoxide}\right)}{2\mathrm{LiOH}\left(\mathrm{aq}\right)}+\underset{\left(\mathrm{Hydrogen}\mathrm{gas}\right)}{{\mathrm{H}}_2\left(\mathrm{g}\right)}$

The explanation for sodium reacts more vigorously with water than Lithium

• Alkali metals include both sodium and lithium. They share several characteristics but some minor characteristics distinguish the two elements.
• To achieve a noble gas structure, alkali metals must give a single valence electron. As a result, they are all electropositive univalent metals.
• As one moves down the group, the electropositive nature rises. Therefore, sodium is more electropositive than lithium and its size is larger as well. As a result, Sodium reacts with water more violently than Lithium.