Zinc fluoride

Zinc fluoride
Names
	IUPAC name Zinc(II) fluoride
	Other names Zinc difluoride
Identifiers
CAS Number	7783-49-5 ; 13986-18-0 (tetrahydrate) ;
3D model (JSmol)	Interactive image;
ChemSpider	22957 ;
ECHA InfoCard	100.029.092
PubChem CID	24551;
RTECS number	ZH3200000;
UNII	L9V334775I ; SQ7815WXFB (tetrahydrate) ;
CompTox Dashboard (EPA)	DTXSID20894882 ;
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Properties
Chemical formula	ZnF2
Molar mass	103.406 g/mol (anhydrous) ; 175.45 g/mol (tetrahydrate)
Appearance	white needles ; hygroscopic
Density	4.95 g/cm3 (anhydrous) ; 2.30 g/cm3 (tetrahydrate)
Melting point	872 °C (1,602 °F; 1,145 K) (anhydrous); 100 °C, decomposes (tetrahydrate)
Boiling point	1,500 °C (2,730 °F; 1,770 K) (anhydrous)
Solubility in water	.000052 g/100 mL (anhydrous) ; 1.52 g/100 mL, 20 °C (tetrahydrate)
Solubility	sparingly soluble in HCl, HNO3, ammonia
Magnetic susceptibility (χ)	−38.2·10−6 cm3/mol
Structure
Crystal structure	tetragonal (anhydrous), tP6
Space group	P42/mnm, No. 136
Hazards
EU classification (DSD) (outdated)	T+ Xn N
NFPA 704 (fire diamond)	3 0 0
Related compounds
Other anions	Zinc(II) bromide ; Zinc(II) chloride ; Zinc(II) iodide
	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

Zinc fluoride (ZnF₂) is an inorganic chemical compound. It is encountered as the anhydrous form and also as the tetrahydrate, ZnF₂ · 4H₂O (rhombohedral crystal structure).^[1] It has a high melting point and has the rutile structure containing 6 coordinate zinc, which suggests appreciable ionic character in its chemical bonding.^[2] Unlike the other zinc halides, ZnCl₂, ZnBr₂ and ZnI₂, it is not very soluble in water.^[2]

Preparation and reactions[]

Zinc fluoride can be synthesized several ways.

Reaction of a fluoride salt with zinc chloride, to yield zinc fluoride and a chloride salt, in aqueous solution.^{[citation needed]}
The reaction of zinc metal with fluorine gas.^[2]
Reaction of hydrofluoric acid with zinc, to yield hydrogen gas (H₂) and zinc fluoride (ZnF₂).^[2]

Zinc fluoride can be hydrolysed by hot water to form the zinc hydroxyfluoride, Zn(OH)F.^[3]

References[]

^ Perry, D. L.; Phillips, S. L. (1995). Handbook of Inorganic Compounds. CRC Press. ISBN 0-8493-8671-3.
^ Jump up to: ^a ^b ^c ^d Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
^ Srivastava, O. K.; Secco, E. A. (1967). "Studies on Metal Hydroxy Compounds. I. Thermal Analyses of Zinc Derivatives ε-Zn(OH)₂, Zn₅(OH)₈Cl₂ · H₂O, β-ZnOHCl, and ZnOHF". Canadian Journal of Chemistry. 45 (6): 579–583. doi:10.1139/v67-096.

External links[]

"Zinc Fluoride". American Elements.

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[1] Perry, D. L.; Phillips, S. L. (1995). Handbook of Inorganic Compounds. CRC Press. ISBN 0-8493-8671-3.

[Greenwood-2] Jump up to: ^a ^b ^c ^d Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.

[3] Srivastava, O. K.; Secco, E. A. (1967). "Studies on Metal Hydroxy Compounds. I. Thermal Analyses of Zinc Derivatives ε-Zn(OH)₂, Zn₅(OH)₈Cl₂ · H₂O, β-ZnOHCl, and ZnOHF". Canadian Journal of Chemistry. 45 (6): 579–583. doi:10.1139/v67-096.

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