Vanadium(V) fluoride is the inorganic compound with the chemical formula VF5. It is a colorless volatile liquid[1] that freezes near room temperature. It is a highly reactive compound, as indicated by its ability to fluorinateorganic substances.[2]
This conversion is conducted at 650 °C. It can also be synthesized by using elemental fluorine to fluorinate industrial concentrates and raw materials so as to produce VF5 on an industrial scale. VF5 can be synthesized from the reaction of raw materials such as metallic Vanadium, ferrovanadium, vanadium (V) oxide and vanadium tetrafluoride with elemental fluorine.[10]
VF5 ionises in the liquid state as reflected by the high values of Trouton's constant and electrical conductivities.[11]
Characteristics and reactivity
Interest in this highly corrosive compound began in the fifties when there were extensive studies of its physicochemical properties.[10] It is a powerful fluorinating and oxidizing agent. It oxidizes elemental sulfur to sulfur tetrafluoride:.
S + 4 VF5 → 4 VF4 + SF4
Like other electrophilic metal halides, it hydrolyzes, first to the oxyhalide:
VF5 + H2O → VOF3 + 2 HF
Then to the binary oxide:
2 VOF3 + 3 H2O → V2O5 + 6 HF
Hydrolysis is accelerated in the presence of base. Despite its tendency to hydrolyze, it can be dissolved in alcohols.
It is a Lewis acid, as illustrated by its formation of the hexafluorovanadate:[12][13][14]
VF5 + KF → KVF6
Vanadium pentafluoride is a weaker acid and mainly undergoes oxidative and fluorinating reactions.[15]
The compound fluorinates unsaturated polyfluoroolefins into polyfluoroalkanes.[10]
The compound dissolves without reaction in liquid Cl2 and Br2. VF5 is moderately soluble in HF.
^Canterford, J. H.; O'Donnell, Thomas A. (1967-03-01). "Reactivity of transition metal fluorides. IV. Oxidation-reduction reactions of vanadium pentafluoride". Inorganic Chemistry. 6 (3): 541–544. doi:10.1021/ic50049a025. ISSN0020-1669.
^Hagen, Kolbjoern.; Gilbert, Michael M.; Hedberg, Lise.; Hedberg, Kenneth. (1982-07-01). "Molecular structure of gaseous vanadium pentafluoride, VF5". Inorganic Chemistry. 21 (7): 2690–2693. doi:10.1021/ic00137a031. ISSN0020-1669.
^Brownstein, S. (1980-06-01). "The structure of VF5 in solution". Journal of Fluorine Chemistry. 15 (6): 539–540. doi:10.1016/S0022-1139(00)85231-8.
^Nikitin, M. I.; Zbezhneva, S. G. (2014-12-16). "Thermochemistry of vanadium fluorides: The formation enthalpies of vanadium fluorides". High Temperature. 52 (6): 809–813. doi:10.1134/S0018151X14060108. ISSN0018-151X. S2CID98343689.
^Trevorrow, L. E.; Fischer, J.; Steunenberg, R. K. (1957). "The Preparation and Properties of Vanadium Pentafluoride". Journal of the American Chemical Society. 79 (19): 5167–5168. doi:10.1021/ja01576a023.
^Cavell, R. G.; Clark, H. C. (1963). "Thermochemistry of vanadium fluorides". Transactions of the Faraday Society. 59: 2706. doi:10.1039/TF9635902706.
^ abcKrasil'nikov, V. A.; Andreev, G. G.; Karelin, A. I.; Guzeeva, T. I.; Furin, G. G.; Bardin, V. V.; Avramenko, A. A. (1995-10-17). "ChemInform Abstract: Synthesis and Use of Vanadium Pentafluoride". ChemInform. 26 (42): no. doi:10.1002/chin.199542022. ISSN1522-2667.
^Clark, H. C.; Emeléus, H. J. (January 1958). "40. Chemical reactions with vanadium, niobium, and tantalum pentafluorides". J. Chem. Soc.: 190–195. doi:10.1039/jr9580000190.
^Nikolsky, B. P. [Никольский, Б.П.] et al, eds. (1971). Справочник химика [The Chemist's Handbook] (in Russian). 3rd (corrected) ed. Leningrad: Khimiya.
^Knunyants, I. L. [Кнунянц, И.Л.] et al, eds. (1995). Химическая энциклопедия [A Chemical Encyclopedia] (in Russian). Moscow: Soviet Encyclopedias. ISBN978-5-85270-092-6
^Lidin, R. A. [Лидин Р.А.] et al (2000). Химические свойства неорганических веществ: Учеб. пособие для вузов [Chemical Properties of Inorganic Substances: A University Textbook] (in Russian). 3rd (corrected) ed. Мoscow: Khimiya. ISBN978-5-7245-1163-6
^Fowler, Brian R.; Moss, Kenneth C. (1979-12-01). "An N.M.R. study of the solution chemistry of vanadium pentafluoride". Journal of Fluorine Chemistry. 14 (6): 485–494. doi:10.1016/S0022-1139(00)82524-5.
Other reading
Arnold F. Holleman, Nils Wiberg: Lehrbuch der Anorganischen Chemie, 102. Auflage, de Gruyter, Berlin 2007, S. 1545, ISBN978-3-11-017770-1.
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