Cadmium fluoride

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Cadmium fluoride
CAS number 7790-79-6 YesY
ChemSpider 23036 YesY
EC number 232-222-0
Jmol-3D images Image 1
Molecular formula CdF2
Molar mass 150.41 g/mol
Appearance grey or white-grey crystals
Density 6.33 g/cm3, solid
Melting point 1110 °C
Boiling point 1748 °C
Solubility in water 4.35 g/100 mL
Solubility soluble in acid
insoluble in ethanol alcohol and liquid ammonia
Crystal structure Fluorite (cubic), cF12
Space group Fm3m, No. 225
EU Index 048-006-00-2
EU classification Carc. Cat. 2
Muta. Cat. 2
Repr. Cat. 2
Highly toxic (T+)
Dangerous for the environment (N)
R-phrases R45, R46, R60, R61, R25, R26, R48/23/25, R50/53
S-phrases S53, S45, S60, S61
Related compounds
Other anions Cadmium chloride,
Cadmium bromide
Cadmium iodide
Other cations Zinc fluoride,
Mercury(II) fluoride,
Copper(II) fluoride,
Silver(II) fluoride,
Calcium fluoride,
Magnesium fluoride
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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Infobox references

Cadmium fluoride (CdF2) is a mostly water-insoluble source of cadmium used in oxygen-sensitive applications, such as the production of metallic alloys. In extremely low concentrations (ppm), this and other fluoride compounds are used in limited medical treatment protocols. Fluoride compounds also have significant uses in synthetic organic chemistry.[1]


Cadmium fluoride is prepared by the reaction of gaseous fluorine or hydrogen fluoride with cadmium metal or its salts, such as the chloride, oxide, or sulfate.

It may also be obtained by dissolving cadmium carbonate in 40% hydrofluoric acid solution, evaporating the solution and drying in a vacuum at 150 °C.

Another method of preparing it is to mix cadmium chloride and ammonium fluoride solutions, followed by crystallization. The insoluble cadmium fluoride is filtered from solution.[2]


Cadmium fluoride, like all cadmium compounds, is toxic and should be used with care. Fluoride is mildly toxic by comparison.

See also[edit]


  1. ^ "Cadmium Fluoride". Retrieved 2009-06-06. 
  2. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8

External links[edit]