Vanadium(V) oxide
Chemical compound
Vanadium(V) oxide, also known as vanadium pentoxide, is the inorganic compound with the formula V_O_. It is a brown/yellow solid, although when freshly precipitated, it appears orange. Because of its high oxidation state, it is both an amphoteric oxide and an oxidizing agent. It is the most stable compound of vanadium and is used as a catalyst in the production of sulfuric acid and maleic anhydride.
Structure
Vanadium(V) oxide adopts a layered structure consisting of distorted octahedra. Each vanadium center is surrounded by six oxygen atoms, forming a distorted octahedron. The V-O bonds are of different lengths, reflecting the different oxidation states of vanadium in the structure.
Production
Vanadium(V) oxide is produced by the calcination of ammonium metavanadate, NH_VO_. The process involves heating the compound in air, which results in the release of ammonia and water, leaving behind V_O_.
Applications
Vanadium(V) oxide is primarily used as a catalyst in the contact process for the production of sulfuric acid. It is also used in the production of maleic anhydride and as a precursor to other vanadium compounds. Additionally, it is used in ceramics and as a colorant for glass.
Reactions
Vanadium(V) oxide is an oxidizing agent and can be reduced to vanadium(IV) oxide, V_O_, and further to vanadium(III) oxide, V_O_. It reacts with alkalis to form vanadates and with acids to form vanadium oxytrichloride.
Safety
Vanadium(V) oxide is toxic and can cause irritation to the eyes, skin, and respiratory tract. It is important to handle it with care and use appropriate protective equipment.
Related pages
References
- Greenwood, N. N.; Earnshaw, A. (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9.
- Cotton, F. Albert; Wilkinson, Geoffrey (1988). Advanced Inorganic Chemistry (5th ed.). Wiley. ISBN 0-471-84997-9.
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