Copper(I) fluoride

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Copper(I) fluoride
Unit cell, ball and stick model of copper(I) fluoride
Names
IUPAC name
Copper(I) fluoride
Systematic IUPAC name
Fluorocopper[1]
Other names
Cuprous fluoride
Identifiers
3D model (JSmol)
ChemSpider
Properties
CuF
Molar mass 82.54 g·mol−1
Density 7.1 g cm−3
Structure
sphalerite
Hazards
Toxic TDangerous for the Environment (Nature) N
NFPA 704
Flammability code 0: Will not burn. E.g., waterHealth code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gasReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogenSpecial hazards (white): no codeNFPA 704 four-colored diamond
0
3
0
US health exposure limits (NIOSH):
PEL (Permissible)
TWA 1 mg/m3 (as Cu)[2]
REL (Recommended)
TWA 1 mg/m3 (as Cu)[2]
IDLH (Immediate danger)
TWA 100 mg/m3 (as Cu)[2]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

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]

References[edit]

  1. ^ "Copper Monofluoride - PubChem Public Chemical Database". The PubChem Project. USA: National Center for Biotechnology Information. 
  2. ^ a b c "NIOSH Pocket Guide to Chemical Hazards #0150". National Institute for Occupational Safety and Health (NIOSH). 
  3. ^ 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. 
  4. ^ Housecroft, C. E.; Sharpe, A. G. (2008). Inorganic Chemistry (3rd ed.). Prentice Hall. pp. 737–738. ISBN 978-0131755536. 
  5. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 1183–1185. ISBN 0-08-037941-9. 
  6. ^ 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. 
  7. ^ 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.