The oxidation state and covalency of $\mathrm{Al}$ in $\left[\mathrm{AlCl}\left(\mathrm{H}_2…
The oxidation state and covalency of $\mathrm{Al}$ in $\left[\mathrm{AlCl}\left(\mathrm{H}_2 \mathrm{O}\right)_5\right]^{2+}$ respectively are
+3 and 6
+6 and 3
+1 and 2
-2 and 1
Solution
Oxidation state of $\mathrm{Al}$ in given compound
$
x+(-1)+5(0)=+2
$
Therefore, $(x)=+3$
In aqueous solution, the water molecules are just interacting electrostatically and not actually bonding. Their partially negative end is pulled by aluminium (+3) oxidation state in an ion-dipole interaction. $\mathrm{Cl}^{-}$is similarly pulled by $\mathrm{Al}(+3)$ oxidation state.
While covalency is 6 because 6 coordinate bonds are formed ( 5 by $\mathrm{H}_2 \mathrm{O}$ and 1 by $\mathrm{Cl}^{-}$).
Hence, the oxidation state and covalency of $\left[\mathrm{AlCl}\left(\mathrm{H}_2 \mathrm{O}\right)_5\right]^{2+}$ are +3 and 6 respectively