Vanadyl perchlorate
| Names | |
|---|---|
| Other names
tripercloratooxovanadium
| |
| Identifiers | |
| Properties | |
| VO(ClO4)3 | |
| Molar mass | 356.29 g/mol |
| Appearance | golden yellow liquid or crystals. |
| Melting point | 21-22 °C |
| Boiling point | 33.5 °C in vacuum |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards
|
oxidant |
| Related compounds | |
Related compounds
|
niobium perchlorate, vanadyl nitrate, chromyl perchlorate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
| |
Vanadyl perchlorate or vanadyl triperchlorate is a golden yellow coloured liquid or crystalline compound of vanadium, oxygen and perchlorate group. The substance consists of molecules covalently bound and is quite volatile.
Formation
Vanadyl perchlorate can be made by reacting vanadium pentoxide with dichlorine heptoxide at 5 °C. It is purified by distillation under a vacuum and recrystallisation at 21 °C.[1]
The reaction of barium perchlorate with vanadyl sulfate solution yields a vanadyl perchlorate solution.[2]
A solution of vanadium(V) perchlorate can be made by dissolving vanadium pentoxide in perchloric acid.[3] Pervanadyl perchlorate, also known as dioxovanadium perchlorate, contains VO2+ ions.[4]
Related
Other perchlorates include vanadyl diperchlorate, oxovanadium perchlorate or vanadium(IV) perchlorate, VO(ClO4)2, which dissolves in water.[5][6] Vanadic perchlorate, also known as vanadium(III) perchlorate solution in water, is a green-tinged blue colour, significantly different to most other V(III) solutions, which are complexed.[7]
References
- ^ Fedoroff, Basil T; Oliver E Sheffield. Encyclopedia of Explosives and Related Items Vol 10 of 10- U to Z. Vol. 10. p. V5.
- ^ Stritar, Jeffery Allan; Taube, Henry (November 1969). "Electron-transfer reactions of ruthenium(III) pentaammines with chromium(II), vanadium(II), europium(II)". Inorganic Chemistry. 8 (11): 2281–2292. doi:10.1021/ic50081a013.
- ^ Kustin, Kenneth; Toppen, David L. (June 1973). "Reduction of vanadium(V) by L-ascorbic acid". Inorganic Chemistry. 12 (6): 1404–1407. doi:10.1021/ic50124a038.
- ^ Ramsey, J. B.; Heldman, M. J. (July 1936). "Kinetics of the Trivalent Vanadium—Iodine Reaction". Journal of the American Chemical Society. 58 (7): 1153–1157. doi:10.1021/ja01298a026.
- ^ Iannuzzi, Melanie M.; Rieger, Philip H. (December 1975). "Nature of vanadium(IV) in basic aqueous solution". Inorganic Chemistry. 14 (12): 2895–2899. doi:10.1021/ic50154a006.
- ^ Wuethrich, K.; Connick, Robert E. (March 1967). "Nuclear magnetic resonance relaxation of oxygen-17 in aqueous solutions of vanadyl perchlorate and the rate of elimination of water molecules from the first coordination sphere". Inorganic Chemistry. 6 (3): 583–590. doi:10.1021/ic50049a035.
- ^ Furman, Sydney C.; Garner, Clifford S. (April 1950). "Absorption Spectra of Vanadium(III) and Vanadium(IV) Ions in Complexing and Non-complexing Media". Journal of the American Chemical Society. 72 (4): 1785–1789. doi:10.1021/ja01160a105.
