Vanadium is a transition metal that can be found in the four consecutive oxidation states +2 to +5. In aqueous solution, it forms different colored water complexes as shown in the figure above. [V(H 2 O) 6 ] 2+ is lilac, [V(H2O) 6 ] 3+ is green, [VO(H 2 O) 5 ] 2+ is blue, and [VO(H 2 O) 5 ] 3+ is yellow. Which compound do you expect to act as a reducing agent and which as an oxidant? Solution As vanadium has electronic configuration 3d 3 4s 2 .In [VO(H2O)5]3+ vanadium is in +5 oxidation state which is maximum oxidation state possessed by vanadium so it will try to accept the electron or it will reduce itself and oxidize other. So [VO(H2O)5]3+ will act as oxidizing agent. While in [V(H2O)6]2+ vanadium is present in +2 oxidation state so it will try to oxidize itself into +3 or +5 state. So it will act as reducing agent. and  [V(H2O)6]3+ in this vanadium(V)is present in +3 state so it can either reduce itself to +2 or oxidize itself to +5 state so it can act both as an oxidizing (oxidant) or reducing agent (reductant). .