Chemistry - Complete d-block Question with Solution | TestHub

Cr²⁺ is reducing in nature because it readily loses an electron to act as a reducing agent and form Cr³⁺. Chromium in the +2 state has a $d^4$ electronic configuration ($[Ar]3d^4$). Upon losing an electron (oxidation), it changes from a $d^4$ to a $d^3$ configuration ($[Ar]3d^3$). In an aqueous medium, the $d^3$ configuration provides a highly stable, half-filled $t_{2g}$ subshell ($t_{2g}{}^3{e}_g{}^0$). This extra stability drives the oxidation process, making option (A) the correct answer.