Copper(I) fluoride
(Redirected from Copper monofluoride)
-fluoride-unit-cell-3D-balls.png)
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| Names | |
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| IUPAC name
Copper(I) fluoride
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| Systematic IUPAC name
Fluorocopper[1] | |
| Other names
Cuprous fluoride
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| CuF | |
| Molar mass | 82.544 g·mol−1 |
| Density | 7.1 g cm−3 |
| Structure | |
| sphalerite | |
| Hazards | |
| GHS labelling: | |
 
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| Warning | |
| NFPA 704 (fire diamond) | |
| NIOSH (US health exposure limits): | |
PEL (Permissible)
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TWA 1 mg/m3 (as Cu)[2] |
REL (Recommended)
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TWA 1 mg/m3 (as Cu)[2] |
IDLH (Immediate danger)
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TWA 100 mg/m3 (as Cu)[2] |
| Related compounds | |
Other anions
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Copper(I) chloride Copper(I) bromide Copper(I) iodide |
Other cations
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Silver(I) fluoride Gold(I) fluoride |
Related compounds
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Copper(II) fluoride |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Copper(I) fluoride or cuprous fluoride is an inorganic compound with the chemical formula CuF. Its existence is uncertain. It was reported in 1933 to have a sphalerite-type crystal structure.[3] Modern textbooks state that CuF is not known,[4] since fluorine is so electronegative that it will always oxidise copper to its +2 oxidation state.[5] Complexes of CuF such as [(Ph3P)3CuF] are, however, known and well characterised.[6]
Synthesis and reactivity
[edit]Unlike other copper(I) halides like copper(I) chloride, copper(I) fluoride tends to disproportionate into copper(II) fluoride and copper in a one-to-one ratio at ambient conditions, unless it is stabilised through complexation as in the example of [Cu(N2)F].[7]
- 2CuF → Cu + CuF2
See also
[edit]- Copper(II) fluoride, the other simple fluoride of copper
References
[edit]- ^ "Copper Monofluoride - PubChem Public Chemical Database". The PubChem Project. USA: National Center for Biotechnology Information.
- ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0150". National Institute for Occupational Safety and Health (NIOSH).
- ^ Ebert, F.; Woitinek, H. (1933). "Kristallstrukturen von Fluoriden. II. HgF, HgF2, CuF und CuF2". Z. anorg. allg. Chem. 210 (3): 269–272. doi:10.1002/zaac.19332100307.
- ^ Housecroft, C. E.; Sharpe, A. G. (2008). Inorganic Chemistry (3rd ed.). Prentice Hall. pp. 737–738. ISBN 978-0-13-175553-6.
- ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 1183–1185. ISBN 978-0-08-037941-8.
- ^ Gulliver, D. J.; Levason, W.; Webster, M. (1981). "Coordination Stabilised Copper(I) Fluoride. Crystal and Molecular Structure of Fluorotris(triphenylphosphine)copper(I)·Ethanol (1/2), Cu(PPh3)3F·2EtOH". Inorg. Chim. Acta. 52: 153–159. doi:10.1016/S0020-1693(00)88590-4.
- ^ Francis, Simon G.; Matthews, Steven L.; Poleshchuk, Oleg Kh; Walker, Nicholas R.; Legon, Anthony C. (2006-09-25). "N2-Cu-F: A Complex of Dinitrogen and Cuprous Fluoride Characterized by Rotational Spectroscopy". Angewandte Chemie. 118 (38): 6489–6491. doi:10.1002/ange.200601988. PMID 16937427.