Cadmium(II) fluoride
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| Names | |
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IUPAC name
Cadmium fluoride
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| Other names
Cadmium(II) fluoride, Cadmium difluoride
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| Identifiers | |
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3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.029.293 |
| EC Number | 232-222-0 |
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PubChem CID
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| Properties | |
| CdF2 | |
| Molar mass | 150.41 g/mol |
| Appearance | grey or white-grey crystals |
| Density | 6.33 g/cm3, solid |
| Melting point | 1,110 °C (2,030 °F; 1,380 K) |
| Boiling point | 1,748 °C (3,178 °F; 2,021 K) |
| 4.35 g/100 mL | |
| Solubility | soluble in acid insoluble in ethanol alcohol and liquid ammonia |
| -40.6·10−6 cm3/mol | |
| Structure | |
| Fluorite (cubic), cF12 | |
| Fm3m, No. 225 | |
| Thermochemistry | |
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Std enthalpy of
formation (ΔfH |
-167.39 ± 0.23 kcal. mole-1 at 298.15 (K, C?) |
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Gibbs free energy (ΔfG˚)
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-155.4 ± 0.3 kcal. mole-1 at 298.15 (K, C?) |
| Hazards | |
| GHS pictograms |
  
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| GHS signal word | Danger |
| H301, H330, H340, H350, H360, H372, H400, H410 | |
| P201, P202, P260, P264, P270, P271, P273, P281, P284, P301+310, P304+340, P308+313, P310, P314 | |
| US health exposure limits (NIOSH): | |
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PEL (Permissible)
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[1910.1027] TWA 0.005 mg/m3 (as Cd) |
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REL (Recommended)
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Ca |
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IDLH (Immediate danger)
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Ca [9 mg/m3 (as Cd)] |
| Related compounds | |
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Other anions
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Cadmium chloride, Cadmium bromide Cadmium iodide |
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Other cations
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Zinc fluoride, Mercury(II) fluoride, Copper(II) fluoride, Silver(II) fluoride, Calcium fluoride, Magnesium fluoride |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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 (what is   ?) |
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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. The standard enthalpy has been found to be -167.39 kcal. mole−1 and the Gibbs energy of formation has been found to be -155.4 kcal. mole−1, and the heat of sublimation was determined to be 76 kcal. mole−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.
Cadmium fluoride has also been prepared by reacting fluorine with cadmium sulfide. This reaction happens very quickly and forms nearly pure fluoride at much lower temperatures than other reactions used.
CdF2 can be transformed into an electronic conductor when doped with certain rare earth elements or yttrium and treated with cadmium vapor under high temperature conditions. This process creates blue crystals with varying absorption coefficients depending on the concentrations of the dopant. A proposed mechanism explains that the conductivity of these crystals can be explained by a reaction of Cd atoms with interstitial F− ions. This creates more CdF2 molecules and releases electrons which are weakly bonded to trivalent dopant ions resulting in n-type conductivity and a hydrogenic donor level.
Cadmium fluoride, like all cadmium compounds, is toxic and should be used with care. Fluoride is mildly toxic by comparison.
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Wikipedia