Chromium pentafluoride

Chromium pentafluoride
Names
	IUPAC name Chromium(V) fluoride
	Other names Chromium fluoride, Chromium(V) fluoride, Pentafluorochromium, Pentafluoridochromium
Identifiers
CAS Number	14884-42-5;
3D model (JSmol)	Interactive image;
ChemSpider	4574207;
PubChem CID	5460742;
CompTox Dashboard (EPA)	DTXSID601030434 ;
	InChI InChI=1S/Cr.5FH/h;5*1H/q+5;;;;;/p-5 Key: OMKYWARVLGERCK-UHFFFAOYSA-I;
	SMILES F[Cr](F)(F)(F)F;
Properties
Chemical formula	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
Crystal structure	orthorhombic
Space group	Pbcm, No. 57
Lattice constant	a = 782.9 pm, b = 753.4 pm, c = 551.8 pm
Formula units (Z)	4
Coordination geometry	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 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 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]

^ ^a ^b 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.
^ ^a ^b ^c 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.
^ Jacques Guertin; James A. Jacobs; Cynthia P. Avakian, eds. (2004). Chromium(VI) Handbook. CRC Press. p. 30. ISBN 9780203487969.
^ Riedel, Sebastian; Kaupp, Martin (2009). "The highest oxidation states of the transition metal elements". Coordination Chemistry Reviews. 253 (5–6): 606–624. doi:10.1016/j.ccr.2008.07.014.
^ A. G. Sharpe (2012). J.H. Simons (ed.). Fluorine Chemistry. Vol. 2. Elsevier. p. 24. ISBN 9780323145435.
^ A. G. Sharpe (1983). Advances in Inorganic Chemistry. Vol. 27. Academic Press. p. 103. ISBN 9780080578767.
^ Amit Aora (2005). Text Book Of Inorganic Chemistry. Discovery Publishing House. p. 649.

[Handbook-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.

[Shorafa-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". Coordination Chemistry Reviews. 253 (5–6): 606–624. doi:10.1016/j.ccr.2008.07.014.

[5] A. G. Sharpe (2012). J.H. Simons (ed.). Fluorine Chemistry. Vol. 2. Elsevier. p. 24. ISBN 9780323145435.

[6] A. G. Sharpe (1983). Advances in Inorganic Chemistry. Vol. 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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Chromium pentafluoride

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