Mercury(II) fluoride

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Mercury(II) fluoride
Mercury(II) fluoride
Names
IUPAC name
Mercury(II) fluoride
Other names
Mercuric fluoride
Identifiers
ECHA InfoCard 100.029.085
EC Number 231-994-6
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]
−62.0·10−6 cm3/mol
Structure
Fluorite (cubic), cF12
Fm3m, No. 225
Hazards
Main hazards highly toxic
GHS pictograms The skull-and-crossbones pictogram in the Globally Harmonized System of Classification and Labelling of Chemicals (GHS)The health hazard pictogram in the Globally Harmonized System of Classification and Labelling of Chemicals (GHS)The environment pictogram in the Globally Harmonized System of Classification and Labelling of Chemicals (GHS)
NFPA 704
Flammability code 0: Will not burn. E.g., waterHealth code 4: Very short exposure could cause death or major residual injury. E.g., VX gasReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogenSpecial hazards (white): no codeNFPA 704 four-colored diamond
0
4
0
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).
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Infobox references

Mercury(II) fluoride has the molecular formula HgF2 as a chemical compound of one atom of mercury with 2 atoms of fluorine.

Synthesis[edit]

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 of mercury(II) oxide:[2]

2 HgO + 2 F2 → 2 HgF2 + O2

with oxygen as byproduct.

Applications[edit]

Mercury(II) fluoride is a selective fluorination agent.[3]

References[edit]

  1. ^ Lide, David R (1998), Handbook of Chemistry and Physics (87th ed.), Boca Raton, Florida: CRC Press, pp. 4–69, ISBN 0-8493-0594-2
  2. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9.
  3. ^ 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.