Mercury(II) fluoride
-fluoride-xtal-3D-sticks.png) | |
| Names | |
|---|---|
| IUPAC name
Mercury(II) fluoride | |
| Other names
Mercuric fluoride | |
| Identifiers | |
7783-39-3  = | |
| ECHA InfoCard | 100.029.085 |
| PubChem | 82209 |
| Properties | |
| HgF2 | |
| Molar mass | 238.587 g/mol |
| Appearance | hygroscopic white cubic crystals |
| Density | 8.95 g/cm3 |
| Melting point | decomposes at 645°C |
| reacts[1] | |
| Structure | |
| Fluorite (cubic), cF12 | |
| Fm3m, No. 225 | |
| Related compounds | |
| Other anions |
Mercury(II) chloride Mercury(II) bromide Mercury(II) iodide |
| Other cations |
Mercury(I) fluoride Zinc fluoride Cadmium fluoride Thallium(I) fluoride |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 verify (what is ?) | |
| Infobox references | |
- "Mercuric fluoride" redirects here.
Mercury(II) fluoride has the molecular formula HgF2.
Synthesis
Mercury(II) fluoride is most commonly produced by the reaction of mercury(II) oxide and hydrogen fluoride:
- HgO + 2 HF → HgF2 + H2O
Mercury(II) fluoride can also be produced through the fluorination of mercury(II) chloride:
- HgCl2 + F2 → HgF2 + Cl2
or mercury(II) oxide:.[2]
- 2 HgO + 2 F2 → 2 HgF2 + O2
Applications
Mercury(II) fluoride is a selective fluorination agent.[3]
References
- ↑ Lide, David R. (1998), Handbook of Chemistry and Physics (87 ed.), Boca Raton, FL: CRC Press, pp. 4–69, ISBN 0-8493-0594-2
- ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9.
- ↑ Habibi, Mohammed H.; Mallouk, Thomas E. (1991). "Photochemical selective fluorination of organic molecules using mercury (II) fluoride". Journal of Fluorine Chemistry. 51 (2): 291. doi:10.1016/S0022-1139(00)80299-7.
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