Zinc fluoride

(Redirected from Zinc difluoride)

Zinc fluoride is an inorganic chemical compound with the chemical formula ZnF2. 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]

Zinc fluoride
Zinc fluoride
Names
IUPAC name
Zinc(II) fluoride
Other names
Zinc difluoride
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.092 Edit this at Wikidata
EC Number
  • 232-001-9
RTECS number
  • ZH3200000
UNII
UN number 3077
  • InChI=1S/2FH.Zn/h2*1H;/q;;+2/p-2 checkY
    Key: BHHYHSUAOQUXJK-UHFFFAOYSA-L checkY
  • F[Zn]F
Properties
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)
.000052 g/(100 mL) (anhydrous)
1.52 g/(100 mL), 20 °C (tetrahydrate)
Solubility sparingly soluble in HCl, HNO3, ammonia
−38.2·10−6 cm3/mol
Structure
tetragonal (anhydrous), tP6
P42/mnm, No. 136
Hazards
GHS labelling:[1]
GHS05: CorrosiveGHS06: ToxicGHS07: Exclamation mark
Danger
H301, H315, H318, H335
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)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
3
0
0
Related compounds
Other anions
Other cations
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Like some other metal difluorides, ZnF2 crystallizes in the rutile structure, which features octahedral Zn cations and trigonal planar fluorides.[4]

Preparation and reactions

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Zinc fluoride can be synthesized several ways.

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

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  1. ^ "ZINC fluoride". pubchem.ncbi.nlm.nih.gov.
  2. ^ Perry, D. L.; Phillips, S. L. (1995). Handbook of Inorganic Compounds. CRC Press. ISBN 0-8493-8671-3.
  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.
  4. ^ 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.
  5. ^ 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.
  6. ^ 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
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