Zinc fluoride

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Zinc fluoride

From Wikipedia, the free encyclopedia

Zinc fluoride
Names

IUPAC name Zinc(II) fluoride
Other names Zinc difluoride
Identifiers
CAS Number	7783-49-5^Y 13986-18-0 (tetrahydrate)^Y
3D model (JSmol)	Interactive image
ChemSpider	22957^Y
ECHA InfoCard	100.029.092
EC Number	232-001-9
PubChem CID	24551
RTECS number	ZH3200000
UNII	L9V334775I^Y SQ7815WXFB (tetrahydrate)^Y
UN number	3077
CompTox Dashboard (EPA)	DTXSID20894882
InChI InChI=1S/2FH.Zn/h2*1H;/q;;+2/p-2^Y Key: BHHYHSUAOQUXJK-UHFFFAOYSA-L^Y
SMILES F[Zn]F
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
GHS labelling:^[1]
Pictograms
Signal word	Danger
Hazard statements	H301, H315, H318, H335
Precautionary statements	P261, P264, P270, P271, P280, P301+P310, P302+P352, P304+P340, P305+P351+P338, P310, P312, P330, P332+P313, P337+P313, P362, P403+P233, P405, P501
NFPA 704 (fire diamond)	3 0 0
Related compounds
Other anions	Zinc(II) bromide Zinc(II) chloride Zinc(II) iodide
Other cations	Cadmium(II) fluoride Mercury(II) fluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). N verify (what is ^YN ?) Infobox references

Zinc fluoride is an inorganic chemical compound with the chemical formula Zn F₂. It is encountered as the anhydrous form and also as the tetrahydrate, ZnF₂·4H₂O (rhombohedral crystal structure).^[2] It has a high melting point and has the rutile structure containing 6 coordinate zinc, which suggests appreciable ionic character in its chemical bonding.^[3] Unlike the other zinc halides, ZnCl₂, ZnBr₂ and ZnI₂, it is not very soluble in water.^[3]

Like some other metal difluorides, ZnF₂ crystallizes in the rutile structure, which features octahedral Zn cations and trigonal planar fluorides.^[4]

Preparation and reactions

[edit]

Zinc fluoride can be synthesized several ways.

The reaction of zinc metal with fluorine gas.^[3]
Reaction of hydrofluoric acid with zinc, to yield hydrogen gas (H₂) and zinc fluoride (ZnF₂).^[3]

Zinc fluoride can be hydrolysed by hot water to form the zinc hydroxide fluoride, Zn(OH)F.^[5]

The salt is believed to form both a tetrahydrate and a dihydrate.^[6]

References

[edit]

^ "ZINC fluoride". pubchem.ncbi.nlm.nih.gov.
^ Perry, D. L.; Phillips, S. L. (1995). Handbook of Inorganic Compounds. CRC Press. ISBN 0-8493-8671-3.
^ ^a ^b ^c ^d Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
^ Stout, J. W.; Reed, Stanley A. (1954). "The Crystal Structure of MnF₂, FeF₂, CoF₂, NiF₂ and ZnF₂". J. Am. Chem. Soc. 76 (21): 5279–5281. doi:10.1021/ja01650a005.
^ 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.
^ Lindahl, Charles B.; Mahmood, Tariq (2000), "Fluorine compounds, inorganic, zinc", Kirk-Othmer Encyclopedia of Chemical Technology, New York: John Wiley, doi:10.1002/0471238961.2609140312091404.a01, ISBN 9780471238966

External links

[edit]

"Zinc Fluoride". American Elements.

Zinc compounds

Zinc(I)

Organozinc(I) compounds	Zn₂(C₅(CH₃)₅)₂

Zinc(II)

Organozinc(II) compounds	Zn(CH₃)₂ Zn(C₂H₅)₂ Zn(CH₃COO)₂ Zn(CH(CH₃)₂)₂ Zn(C(CH₃)₃)₂ Zn(C₆H₅)₂ Zn(C₃H₅O₃)₂ ZnICH₂I

C
₂₄H
₄₆ZnO
₄

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