Zinc fluoride
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Template:Chembox image cellTemplate:Chembox image cellTemplate:Chembox AllOtherNamesTemplate:Chembox headerbarTemplate:Chembox IndexlistTemplate:Chembox JmolTemplate:Chembox ChEMBLTemplate:Chembox ECHATemplate:Chembox E numberTemplate:Chembox IUPHAR ligandTemplate:Chembox UNIITemplate:Chembox CompToxTemplate:Chembox headerbarTemplate:Chembox SolubilityInWaterTemplate:Chembox headerbarTemplate:Chembox headerbarTemplate:Chembox GHS (set)Template:Chembox headerbarTemplate:Chembox Datapage checkTemplate:Chembox Footer| Template:Longitem | Template:Unbulleted list |
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| UN number | 3077 |
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| Template:Longitem | Template:Chem2 |
| 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 | Template:Chembox CalcTemperatures |
| Boiling point | Template:Chembox CalcTemperatures |
| Solubility | sparingly soluble in HCl, HNO3, ammonia |
| Template:Longitem | −38.2·10−6 cm3/mol |
| Template:Longitem | tetragonal (anhydrous), tP6 |
| Template:Longitem | P42/mnm, No. 136 |
| NFPA 704 (fire diamond) | Template:NFPA 704 diamond |
| Template:Longitem | Template:Ubl |
| Template:Longitem | Template:Ubl |
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Zinc fluoride is an inorganic chemical compound with the chemical formula Template:Chem2. It is encountered as the anhydrous form and also as the tetrahydrate, Template:Chem2 (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, [[Zinc chloride|Template:Chem2]], [[Zinc bromide|Template:Chem2]] and [[Zinc iodide|Template:Chem2]], it is not very soluble in water.[2]
Like some other metal difluorides, Template:Chem2 crystallizes in the rutile structure, which features octahedral Zn cations and trigonal planar fluorides.[3]
Preparation and reactions
Zinc fluoride can be synthesized several ways.
- The reaction of zinc metal with fluorine gas.[2]
- Reaction of hydrofluoric acid with zinc, to yield hydrogen gas (Template:Chem2) and zinc fluoride (Template:Chem2).[2]
Zinc fluoride can be hydrolysed by hot water to form the zinc hydroxide fluoride, Zn(OH)F.[4]
The salt is believed to form both a tetrahydrate and a dihydrate.[5]
References
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External links
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