Chemistry:Zinc fluoride

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Short description: Chemical compound
Zinc fluoride
Zinc fluoride
IUPAC name
Zinc(II) fluoride
Other names
Zinc difluoride
3D model (JSmol)
EC Number
  • 232-001-9
RTECS number
  • ZH3200000
UN number 3077
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 pictograms GHS05: CorrosiveGHS06: ToxicGHS07: Harmful
GHS Signal word Danger
H301, H315, H318, H335
P261, P264, P270, P271, P280, P301+310, P302+352, P304+340, P305+351+338, P310, P312, P330, P332+313, P337+313, P362, P403+233, P405, P501
NFPA 704 (fire diamond)
Flammability code 0: Will not burn. E.g. waterHealth code 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no codeNFPA 704 four-colored diamond
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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Infobox references

Zinc fluoride is an inorganic chemical compound with the chemical formula ZnF
. It is encountered as the anhydrous form and also as the tetrahydrate, ZnF
 · 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, ZnCl
, ZnBr
and ZnI
, it is not very soluble in water.[3]

Like some other metal difluorides, ZnF
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" (in en). 
  2. Perry, D. L.; Phillips, S. L. (1995). Handbook of Inorganic Compounds. CRC Press. ISBN 0-8493-8671-3. 
  3. 3.0 3.1 3.2 3.3 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, 

External links