Mercury (II) fluoride

Crystal structure
__ Hg 2+      __ F -
General
Surname	Mercury (II) fluoride
other names	Mercury difluoride
Ratio formula	HgF 2
Brief description	white solid
External identifiers / databases
CAS number 7783-39-3 EC number 231-994-6 ECHA InfoCard 100,029,085 PubChem 82209 Wikidata Q172914
properties
Molar mass	238.61 g mol −1
Physical state	firmly
density	8.95 g cm −3
Melting point	645 ° C (decomposition)
solubility	Hydrolysis in water soluble in hydrofluoric acid and dilute nitric acid somewhat soluble in ethanol
safety instructions
GHS labeling of hazardous substances danger H and P phrases H: 300-310-330-373-410 P: 260-301 + 310-304 + 340-320-330-361-405-501
As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions .

Mercury (II) fluoride is an inorganic chemical compound of mercury from the group of fluorides .

Extraction and presentation

Mercury (II) fluoride can be obtained by reacting mercury (II) chloride with fluorine .

${\displaystyle \mathrm {HgCl_{2}+F_{2}\longrightarrow HgF_{2}+Cl_{2}} }$

It is also possible to display it by reacting mercury (II) oxide with hydrogen fluoride

${\displaystyle \mathrm {HgO+2\ HF\longrightarrow HgF_{2}+H_{2}O} }$

or by fluorination of mercury (I) fluoride .

${\displaystyle \mathrm {Hg_{2}F_{2}+2\ NOF\cdot 3HF\longrightarrow 2\ HgF_{2}+2\ NO+6\ HF} }$

properties

Mercury (II) fluoride is a white, light-sensitive and very moisture-sensitive solid that is immediately hydrolyzed by water to turn yellow. It has a cubic crystal structure of the fluorite type ( space group Fm 3 m (space group no. 225) ).

use

Mercury (II) fluoride can be used as a selective fluorinating agent .

Individual evidence

1. ↑ David R. Lide (Ed.): CRC Handbook of Chemistry and Physics . 90th edition. (Internet version: 2010), CRC Press / Taylor and Francis, Boca Raton, FL, Properties of the Elements and Inorganic Compounds, pp. 4-76.
2. ↑ ^{a b c d e f} data sheet Mercury (II) fluoride, 95% from AlfaAesar, accessed on September 28, 2013 ( PDF )(JavaScript required) .
3. ↑ ^{a b c d e} Georg Brauer (Ed.), With the collaboration of Marianne Baudler u. a .: Handbook of Preparative Inorganic Chemistry. 3rd, revised edition. Volume I, Ferdinand Enke, Stuttgart 1975, ISBN 3-432-02328-6 , p. 252.
4. ↑ ^{a b c} Roger Blachnik (Ed.): Pocket book for chemists and physicists . Volume III: Elements, Inorganic Compounds and Materials, Minerals . founded by Jean d'Ans, Ellen Lax. 4th, revised and revised edition. Springer, Berlin 1998, ISBN 3-540-60035-3 , pp. 484 ( limited preview in Google Book search).
5. ^ Dale L. Perry: Handbook of Inorganic Compounds, Second Edition . Taylor & Francis, 2011, ISBN 1-4398-1462-7 , pp. 273 ( limited preview in Google Book search).
6. ↑ Mohammed H. Habibi, Thomas E. Mallouk : Photochemical selective fluorination of organic molecules using mercury (II) fluoride. In: Journal of Fluorine Chemistry . 51, 1991, pp. 291-294, doi : 10.1016 / S0022-1139 (00) 80299-7 .