Zinc fluoride
Zinc fluoride
IUPAC name
Zinc(II) fluoride
Other names
Zinc difluoride
3D model (JSmol)
ECHA InfoCard 100.029.092 Edit this at Wikidata
EC Number
  • 232-001-9
RTECS number
  • ZH3200000
UN number 3077
  • InChI=1S/2FH.Zn/h2*1H;/q;;+2/p-2 checkY
  • F[Zn]F
Molar mass 103.406 g/mol (anhydrous)
175.45 g/mol (tetrahydrate)
Appearance white needles
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
tetragonal (anhydrous), tP6
P42/mnm, No. 136
GHS labelling:[1]
GHS05: CorrosiveGHS06: ToxicGHS07: Exclamation mark
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
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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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]

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

Preparation and reactions

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]


  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