Zinc fluoride
| Names | |
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| IUPAC name
Zinc(II) fluoride
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| Other names
Zinc difluoride
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| Identifiers | |
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3D model (JSmol)
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| ChemSpider | |
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| E number | Lua error in Module:Wikidata at line 880: attempt to index field 'wikibase' (a nil value). |
PubChem CID
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| UN number | 3077 |
CompTox Dashboard (EPA)
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| 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) | |
| Related compounds | |
Other anions
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Other cations
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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
[edit | edit source]Zinc fluoride can be synthesized several ways.
- The reaction of zinc metal with fluorine gas.[3]
- Reaction of hydrofluoric acid with zinc, to yield hydrogen gas (H2) and zinc fluoride (ZnF2).[3]
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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External links
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