Consider the following reactions:
$$\begin{gathered} \mathrm{I} : {\mathrm{AlH}}_3+{\mathrm{H}}^{-}⟶{\mathrm{AlH}}_4^{-} \\ \mathrm{II} : {\mathrm{H}}_2\mathrm{O}+{\mathrm{H}}^{-}⟶{\mathrm{H}}_2+{\mathrm{OH}}^{-} \end{gathered}$$
Select the correct statements based on these reactions.

Lewis bases are those bases that can donate electron pairs to a Lewis acid (electron-deficient or electron-acceptor) whereas Bronsted base is that base that accepts a proton from Bronsted acid.

In the first reaction, AlH₃ is an electron-deficient specie because Al has an incomplete octet and has a vacant orbital. Hydride ion acts as a Lewis base which donates electron pair to the empty orbital of Al. In the second reaction, the hydride ion acts as a Bronsted base which can accept a proton from water and forms hydrogen gas.