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| Names | |
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| IUPAC name Zinc(II) fluoride | |
| Other names Zinc difluoride | |
| Identifiers | |
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3D model (JSmol) | |
| ChemSpider | |
| ECHA InfoCard | 100.029.092  |
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CompTox Dashboard (EPA) | |
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| 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) |
| .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 | |
Crystal structure | tetragonal (anhydrous), tP6 |
| P42/mnm, No. 136 | |
| Hazards | |
EU classification (DSD) (outdated) | ){kind=small} T+){kind=small} Xn){kind=small} N |
| NFPA 704 (fire diamond) | |
| Related compounds | |
Other anions | Zinc(II) bromide Zinc(II) chloride Zinc(II) iodide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
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).[1] It has a high melting point and has the rutile structure containing 6 coordinate zinc, which suggests appreciable ionic character in its chemical bonding.[2] Unlike the other zinc halides, ZnCl2, ZnBr2 and ZnI2, it is not very soluble in water.[2]
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.[2]
- Reaction of hydrofluoric acid with zinc, to yield hydrogen gas (H2) and zinc fluoride (ZnF2).[2]
Zinc fluoride can be hydrolysed by hot water to form the zinc hydroxyfluoride, Zn(OH)F.[3]
References
- ^ 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.
- ^ 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.
External links
- "Zinc Fluoride". American Elements.