Account for the following.
(i) Bi(V) is a stronger oxidising agent than Sb(V).
(i) Since, Bi in +5 oxidation state has a tendency to reduce into more stable +3 oxidation state by the acceptance of two electrons and hence acts as a strong oxidising agent.
${{Bi}^{5+}}$+ ${{2e}^{-}}$ -------->${{Bi}^{3+}}$
In contrast, Sb in +5 oxidation state is more stable than its +3 oxidation state. Therefore, Sb (V) has a less tendency to accept a pair of electrons than ${{Bi}^{5+}}$. Hence, Bi (V) is a stronger oxidising agent than Sb (V).