Why `Cr^(2+)` is strongly reducing while `Mn^(3+)` is strongly oxidising ?

How would you account for the following : Of the d^4 species, Cr^(2+) is strongly reducing while Mn(III) is strongly oxidising.

Give an explanation for the following observation : With the same d-orbital configuration (d^4) , Cr^(2+) ion is a reducing agent but Mn^(3+) ion is an oxidising agent.

In aqueous solution, Cr^(2+) is stronger reducing agent than Fe^(2+) . This is because

Give reason for the following : Mn^(3+) is a good oxidising agent.

H_2O_2 is acting as a reducing agent as well as oxidising agent

Which is stronger reducing agent Cr^(2+) or Fe^(2+) and why ?

Which is a stronger reducing agent, SbH_(3) or BiH_(3) , and why ?