Why $S m^{+ 2}$ ions in solution are good reducing agent but an aqueous solution of $C e^{+ 4}$ is a good oxidising agent?

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Solution

Both $S m^{2 +}$ and $C e^{4 +}$ are belonging to landanold series in which
the $+ 3$ oxidation state is the must stable. Thus, both the ions
tend to acquire $+ 3$ oxidation state. $C e^{+}$ does so by
undergoing reduction and thus, a good oxidising agent $S m^{2 +}$ ions
undergo oxidation to acquire stable state and thus acts
as a reducing agent.

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