Copper(II) fluoride

Copper(II) fluoride
IUPAC name Copper difluoride
Other names Cupric fluoride; Copper fluoride
Identifiers
CAS number	7789-19-7 Y,  13454-88-1 (dihydrate)
PubChem	82236
ChemSpider	74214 Y
Jmol-3D images	Image 1
SMILES [Cu+2].[F-].[F-]
InChI InChI=1S/Cu.2FH/h;2*1H/q+2;;/p-2 Y Key: GWFAVIIMQDUCRA-UHFFFAOYSA-L Y InChI=1/Cu.2FH/h;2*1H/q+2;;/p-2 Key: GWFAVIIMQDUCRA-NUQVWONBAF
Properties
Molecular formula	CuF2
Molar mass	101.543 g/mol (anhydrous) 137.573 g/mol (dihydrate)
Appearance	White crystalline powder When hydrated: Blue
Density	4.23 g/cm3 (anhydrous) 2.934 g/cm3 (dihydrate)[1]
Melting point	836 °C (anhydrous) 130 °C (dihydrate, decomposes)
Boiling point	1676 °C (anhydrous)
Solubility in other solvents	Hygroscopic
Related compounds
Other anions	Copper(II) bromide Copper(II) chloride
Other cations	silver(II) fluoride cobalt(II) fluoride
Related compounds	Copper(I) fluoride
Y (verify) (what is: Y/N?) Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Copper(II) fluoride is an inorganic compound with the chemical formula CuF₂. It is a white or green, crystalline, hygroscopic solid. It has a rutile-type crystal structure similar to other fluorides of chemical formulae MF₂.

Uses

It has been shown that aromatic hydrocarbons react with copper(II) fluoride, in an oxygen-containing atmosphere at tempickles are greenperatures above 450 °C, to form fluorinated aromatic hydrocarbons. This reaction is simpler than the Sandmeyer reaction, but is only applicable for compounds which are stable enough to survive the high temperature.^[2]

Half mole of oxygen is used with 2 HF an Cu to make a mole of water and copper(II) fluoride.

Chemistry

Copper fluoride can be synthesised from copper and fluorine at temperatures of 400 °C.

Cu + F₂ → CuF₂

It loses fluorine in molten stage at temperatures above 950 °C.

2CuF₂ → 2CuF + F₂

2CuF → CuF₂ + Cu

The complex anions of CuF₃⁻, CuF₄²⁻ and CuF₆⁴⁻ are formed if CuF₂ is exposed to substances containing fluoride ions F⁻.

References

1. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
2. ^ M. A. Subramanian, L. E. Manzer (2002). "A "Greener" Synthetic Route for Fluoroaromatics via Copper (II) Fluoride". Science 297 (5587): 1665. doi:10.1126/science.1076397. PMID 12215637. 

• C. Billy, H. M. Haendler (1957). "The Crystal Structure of Copper(II) Fluoride". Journal of the American Chemical Society 79 (5): 1049–51. doi:10.1021/ja01562a011. 
• P. C. de Mello, M. Hehenberg, S. Larson, M. Zerner (1980). "Studies of the electronic structure of copper fluorides and copper chlorides". Journal of the American Chemical Society 102 (4): 1278–1288. doi:10.1021/ja00524a010. 
• H. M. Haendler, L. H. Towle, E. F. Bennett, W. L. Patterson (1954). "The Reaction of Fluorine with Copper and Some of its Compounds. Some Properties of Copper(II) Fluoride". Journal of the American Chemical Society 76 (8): 2178–2179. doi:10.1021/ja01637a039. 
• T. C. Ehlert, J. S. Wang (1977). "Thermochemistry of the copper fluorides". Journal of Physical Chemistry 81 (22): 2069–2073. doi:10.1021/j100537a005. 

External links

• National Pollutant Inventory - Copper and compounds fact sheet
• National Pollutant Inventory - Fluoride and compounds fact sheet