The correct statement(s) about Cr2+ and Mn3+ is(are): [Atomic numbers of Cr=24 and Mn=25] Cr2+ is a reducing agent, Mn3+ is an oxidizing agent, Both Cr2+ and Mn3+ exhibit d4 electronic configuration, When Cr2+ is used as a reducing agent, the chromium ion attains d5 electronic configuration.

(A) Cr2+ is a reducing agent. It itself loses electrons (and hence acts as a reducing agent) and forms higher oxidation states. In fact, +6 oxidation state of Cr is very stable. Hence, the option (A) is correct (B) Mn3+ is an oxidizing agent. It itself gains electrons (and hence acts as an oxidizing agent) to form Mn2+ with 3d5 electronic configuration which is stable as it is half-filled. Hence, the option (B) is correct (C) Cr and Mn have outer ionic configurations of 3d54s1 and 3d54s2 respectively. Hence, both Cr2+ and Mn3+ exhibit d4 electronic configuration. Hence, the option (C) is correct (D) When Cr2+ is used as a reducing agent, the chromium ion attains d3 (as in Cr3+) electronic configuration. Hence, the option (D) is incorrect.