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Cadmium fluoride - Wikipedia

From Wikipedia, the free encyclopedia

Cadmium fluoride
Names

IUPAC name Cadmium fluoride
Other names Cadmium(II) fluoride, Cadmium difluoride
Identifiers
CAS Number	7790-79-6^Y
3D model (JSmol)	Interactive image
ChemSpider	23036^Y
ECHA InfoCard	100.029.293
EC Number	232-222-0
PubChem CID	24634 71356118 dihydrate
UNII	M0975E7Z8Z^Y
CompTox Dashboard (EPA)	DTXSID6064878
InChI InChI=1S/Cd.2FH/h;21H/q+2;;/p-2^Y Key: LVEULQCPJDDSLD-UHFFFAOYSA-L^Y InChI=1/Cd.2FH/h;21H/q+2;;/p-2 Key: LVEULQCPJDDSLD-NUQVWONBAG
SMILES [Cd+2].[F-].[F-]
Properties
Chemical formula	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)
Solubility in water	4.35 g/100 mL
Solubility product (K_sp)	0.00644^[1]
Solubility	soluble in acid insoluble in ethanol alcohol and liquid ammonia
Magnetic susceptibility (χ)	-40.6·10⁻⁶ cm³/mol
Structure
Crystal structure	Fluorite (cubic), cF12
Space group	Fm3m, No. 225
Thermochemistry
Std enthalpy of formation (Δ_fH^⦵₂₉₈)	-167.39 ± 0.23 kcal. mole-1 at 298.15 (K, C?)
Gibbs free energy (Δ_fG^⦵)	-155.4 ± 0.3 kcal. mole-1 at 298.15 (K, C?)
Hazards
GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H301, H330, H340, H350, H360, H372, H410
Precautionary statements	P201, P202, P260, P264, P270, P271, P273, P281, P284, P301+P310, P304+P340, P308+P313, P310, P314, P320, P321, P330, P391, P403+P233, P405, P501
NIOSH (US health exposure limits):
PEL (Permissible)	[1910.1027] TWA 0.005 mg/m³ (as Cd)^[2]
REL (Recommended)	Ca^[2]
IDLH (Immediate danger)	Ca [9 mg/m³ (as Cd)]^[2]
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 otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Y verify (what is ^YN ?) 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.^[3] 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.^[4]^[5]

Preparation

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.^[6]

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.^[7]

Uses

Electronic conductor

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.^[8]

Safety

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

Cadmium fluoride can cause potential health issues if it is not handled properly. It can cause irritation to the skin and the eyes, so gloves and protective eyewear are advised. The MSDS, or Material Safety Data Sheet, also includes warnings for ingestion and inhalation. Under acidic conditions, at high temperatures, and in moist environments, hydrogen fluoride and cadmium vapors may be released into the air. Inhalation may cause irritation of the respiratory system as well as congestion, fluorosis, and even pulmonary edema in extreme cases. Cadmium fluoride also has the same potential hazards caused by cadmium and fluoride.^[9]

References

^ John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–188. ISBN 978-1138561632.
^ ^a ^b ^c NIOSH Pocket Guide to Chemical Hazards. "#0087". National Institute for Occupational Safety and Health (NIOSH).
^ "Cadmium Fluoride". Retrieved 2009-06-06.
^ Rudzitis, Edgars; Feder, Harold; Hubbard, Ward (November 1963). "Fluorine Bomb Calorimetry. VII. The Heat of Formation of Cadmium Difluoride". Journal of Physical Chemistry. 67 (11): 2388–2390. doi:10.1021/j100805a031.
^ Besenbruch, G.; Kana'an, A. S.; Margrave, J. L. (March 3, 1965). "Knudson and Langmuir Measurements of the Sublimation Pressure of Cadmium (II) Fluoride". Journal of Physical Chemistry. 69 (9): 3174–3176. doi:10.1021/j100893a505.
^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
^ Haendler, Helmut; Bernard, Walter (November 1951). "The Reaction of Fluorine with Cadmium and Some of its Binary Compounds. The Crystal Structure, Density and Melting Points of Cadmium Fluoride". Journal of the American Chemical Society. 73. doi:10.1021/ja01155a064.
^ Weller, Paul (June 1, 1965). "Electrical and Optical Properties of Rare Earth Doped Cadmium Fluoride Single Crystals". Inorganic Chemistry. 4 (11): 1545–1551. doi:10.1021/ic50033a004.
^ "Cadmium Fluoride [CdF2]". MSDS Solutions Center. Advance Research Chemicals Inc. / A.R.C. 2011-04-01. Retrieved 2014-12-12.^{[permanent dead link‍]}

External links

v t e Cadmium compounds
Cadmium(I)	Cd₂(AlCl₄)₂
Cadmium(II)	Cd(BF₄)₂ CdF₂ CdCl₂ CdBr₂ CdI₂ Cd(CN)₂ CdH₂ CdO CdS CdSe CdTe Cd(OH)₂ Cd₃N₂ Cd(NO₃)₂ CdSO₄ CdSeO₄ CdCrO₄ CdWO₄ CdTeO₃ Cd(C₃H₅O₃)₂ Cd₃As₂ Cd₃P₂ CsCdCl₃ CsCdBr₃ Cd(CH₃CO₂)₂ Cd(O₂CC₁₇H₃₅)₂

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