Consider the following reaction.

$${\text{2Cr(OH}}{{\text{)}}_3}{\text{(s)}} + {\text{6Cl}}{{\text{O}}^ - }{\text{(aq)}} \to {\text{2CrO}}_4^{2 - }{\text{(aq)}} + {\text{3C}}{{\text{l}}_2}{\text{(g)}} + {\text{2O}}{{\text{H}}^ - }{\text{(aq)}} + {\text{2}}{{\text{H}}_2}{\text{O(l)}}$$

Which statement is correct?

A.     ${\text{Cr(OH}}{{\text{)}}_{\text{3}}}$ is the oxidizing agent and the oxidation number of chromium changes from +3 to +6.

B.     ${\text{Cr(OH}}{{\text{)}}_{\text{3}}}$ is the reducing agent and undergoes reduction.

C.     ${\text{Cl}}{{\text{O}}^ - }$ is the oxidizing agent and the oxidation number of chlorine changes from +1 to 0.

D.     ${\text{Cl}}{{\text{O}}^ - }$ is the reducing agent and the oxidation number of chlorine changes from –1 to 0.

C