|Jmol-3D images||Image 1|
|Molar mass||103.406 g/mol (anhydrous)
175.45 g/mol (tetrahydrate)
|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|
|Crystal structure||tetragonal (anhydrous), tP6|
|Space group||P42/mnm, No. 136|
|EU Index||Not listed|
|Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)|
|(what is: / ?)|
Zinc fluoride (ZnF2) is an inorganic chemical compound. It is encountered as the anydrous form and also as the tetrahydrate, ZnF2 · 4H2O (rhombohedral crystal structure). It has a high melting point and has the rutile structure containing 6 coordinate zinc, which suggests appreciable ionic character in its chemical bonding. Unlike the other zinc halides, ZnCl2, ZnBr2 and ZnI2, it is not very soluble in water.
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.
- The reaction of zinc metal with fluorine gas.
- Reaction of hydrofluoric acid with zinc, to yield hydrogen gas (H2) and zinc fluoride (ZnF2).
Zinc fluoride can be hydrolysed by hot water to form the zinc hydroxyfluoride, Zn(OH)F.
- Perry, D. L.; Phillips, S. L. (1995). Handbook of Inorganic Compounds. CRC Press. ISBN 0-8493-8671-3.
- Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0080379419.
- 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" (pdf). Canadian Journal of Chemistry 45 (6): 579–583. doi:10.1139/v67-096.
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