Chromium pentafluoride

Chromium pentafluoride is the inorganic compound with the chemical formula CrF5.[3] It is a red volatile solid that melts at 34 °C.[1] It is the highest known chromium fluoride, since the hypothetical chromium hexafluoride has not yet been synthesized.[4]

Chromium pentafluoride
Names
IUPAC name
Chromium(V) fluoride
Other names
Chromium fluoride, Chromium(V) fluoride, Pentafluorochromium, Pentafluoridochromium
Identifiers
3D model (JSmol)
ChemSpider
Properties[1]
CrF5
Molar mass 146.988 g/mol
Appearance red crystals
Density 2.89 g/cm3
Melting point 34 °C (93 °F; 307 K)
Boiling point 117 °C (243 °F; 390 K)
Structure[2]
orthorhombic
Pbcm, No. 57
a = 782.9 pm, b = 753.4 pm, c = 551.8 pm
4
octahedral
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Chromium pentafluoride is one of the products of the action of fluorine on a mixture of potassium and chromic chlorides.[5]

In terms of its structure, the compound is a one-dimensional coordination polymer. Each Cr(V) center has octahedral molecular geometry.[2] It has the same crystal structure as vanadium pentafluoride.[6]

Chromium pentafluoride is strongly oxidizing, able to fluorinate the noble gas xenon and oxidize dioxygen to dioxygenyl.[2] Due to this property, it decomposes readily in the presence of reducing agents, and easily hydrolyses to chromium(III) and chromium(VI).[7]

See also
  • Chromium difluoride
  • Chromium trifluoride
  • Chromium tetrafluoride

References
  1. Perry, Dale L. (2011). Handbook of Inorganic Compounds, Second Edition. Boca Raton, Florida: CRC Press. p. 125. ISBN 978-1-43981462-8. Retrieved 2014-01-10.
  2. Shorafa, H.; Seppelt, K. (2009). "The structures of CrF5 and CrF5*SbF5". Zeitschrift für anorganische und allgemeine Chemie. 635 (1): 112–114. doi:10.1002/zaac.200800378.
  3. Jacques Guertin; James A. Jacobs; Cynthia P. Avakian, eds. (2004). Chromium(VI) Handbook. CRC Press. p. 30. ISBN 9780203487969.
  4. Riedel, Sebastian; Kaupp, Martin (2009). "The highest oxidation states of the transition metal elements" (PDF). Coordination Chemistry Reviews. 253 (5–6): 606–624. doi:10.1016/j.ccr.2008.07.014.
  5. A. G. Sharpe (December 2012). J.H. Simons (ed.). Fluorine Chemistry. 2. Elsevier. p. 24. ISBN 9780323145435.
  6. A. G. Sharpe (1983). Advances in Inorganic Chemistry. 27. Academic Press. p. 103. ISBN 9780080578767.
  7. Amit Aora (2005). Text Book Of Inorganic Chemistry. Discovery Publishing House. p. 649.


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