Cr2+ is a stronger reducing agent because it can lose one of its electron to become Cr3+ in which the t2g level of d-orbital is half filled and eg level is empty.

Which is a stronger oxidizing agent Mn3+ and Cr2+?

Out of Cr3+ and Mn3+, Mn3+ is a stronger oxidising agent because it has 4 electrons in its valence shell and when it gains one electron to form Mn2+, it results in the half-filled (d5) configuration that has extra stability.

Cr^2 + is reducing in nature while the same d – orbital configuration (d^4) Mn^+3 is an oxidising agent.

Is Cr2+ a strong reducing agent?

Cr2+ has d4 configuration while Cr3+ has more stable d5 configuration. Thus Cr has a tendency to acquire Cr3+ due to greater stability of +3 oxidation state. Cr2+ acts as a reducing agent.

Answer: Cr2+ is a stronger reducing agent than Fe2+. This can be explained on the basis of the standard electrode potential values E°(Cr3+/Cr2+ = –0.41 V) and E° (Fe3+/Fe2+ = + 0.77 V). Thus Cr2+ is easily oxidised to Cr3+ but Fe2+ cannot be as readily oxidised to Fe3+.