The chemistry of vanadium is noteworthy for the accessibility of the four adjacent oxidation states 2–5.
In aqueous solution, vanadium forms metal aquo complexes of which the colours are lilac [V(H₂O)₆]²⁺, green [V(H₂O)₆]³⁺, blue [VO(H₂O)₅]²⁺, yellow-orange oxides, the formula for which depends on pH .
Vanadium(II) compounds are reducing agents, and vanadium(V) compounds are oxidizing agents.
Vanadium(IV) compounds often exist as vanadyl derivatives, which contain the VO²⁺ center.

Ammonium vanadate(V) (NH₄VO₃) can be successively reduced with elemental zinc to obtain the different colors of vanadium in these four oxidation states.
Lower oxidation states occur in compounds such as V(CO)₆, [V(CO)
₆]⁻
 and substituted derivatives.

Vanadium pentoxide is a commercially important catalyst for the production of sulfuric acid, a reaction that exploits the ability of vanadium oxides to undergo redox reactions.

The vanadium redox battery utilizes all four oxidation states: one electrode uses the +5/+4 couple and the other uses the +3/+2 couple.
Conversion of these oxidation states is illustrated by the reduction of a strongly acidic solution of a vanadium(V) compound with zinc dust or amalgam.
The initial yellow color characteristic of the pervanadyl ion [VO₂(H₂O)₄]⁺ is replaced by the blue color of [VO(H₂O)₅]²⁺, followed by the green color of [V(H₂O)₆]³⁺ and then the violet color of [V(H₂O)₆]²⁺.
The chemistry of vanadium is noteworthy for the accessibility of the four adjacent oxidation states 2–5. In aqueous solution, vanadium forms metal aquo complexes of which the colours are lilac [V(H₂O)₆]²⁺, green [V(H₂O)₆]³⁺, blue [VO(H₂O)₅]²⁺, yellow-orange oxides, the formula for which depends on pH . Vanadium(II) compounds are reducing agents, and vanadium(V) compounds are oxidizing agents. Vanadium(IV) compounds often exist as vanadyl derivatives, which contain the VO²⁺ center.
Ammonium vanadate(V) (NH₄VO₃) can be successively reduced with elemental zinc to obtain the different colors of vanadium in these four oxidation states. Lower oxidation states occur in compounds such as V(CO)₆, [V(CO)
₆]⁻
 and substituted derivatives.
Vanadium pentoxide is a commercially important catalyst for the production of sulfuric acid, a reaction that exploits the ability of vanadium oxides to undergo redox reactions.
The vanadium redox battery utilizes all four oxidation states: one electrode uses the +5/+4 couple and the other uses the +3/+2 couple. Conversion of these oxidation states is illustrated by the reduction of a strongly acidic solution of a vanadium(V) compound with zinc dust or amalgam. The initial yellow color characteristic of the pervanadyl ion [VO₂(H₂O)₄]⁺ is replaced by the blue color of [VO(H₂O)₅]²⁺, followed by the green color of [V(H₂O)₆]³⁺ and then the violet color of [V(H₂O)₆]²⁺.
Vanadium