Selenium hexafluoride

Structural formula
General
Surname	Selenium hexafluoride
Molecular formula	SeF 6
Brief description	colorless gas with a pungent odor
External identifiers / databases
EC number	620-577-8
ECHA InfoCard	100.149.506
PubChem	24558
Wikidata	Q425217
properties
Molar mass	192.95 g mol −1
Physical state	gaseous
density	8.69 kg m −3
Melting point	−34.7 ° C
Sublimation point	−46.6 ° C
solubility	insoluble in water (slow hydrolysis)
safety instructions
H and P phrases	H: 280-330-314
	EUH: 071
	P: ?
Toxicological data	10 ppm 1h −1 ( LC Lo , mouse , inh. ) ; 10 ppm 4h −1 ( LC Lo , rabbit , inh. ) ; 10 ppm 1h −1 ( LC Lo , rat , inh. ) ;
Thermodynamic properties
ΔH f 0	−1030 kJ mol −1
	As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions .

Selenium hexafluoride (SeF ₆ ) is an inorganic chemical compound of the elements selenium and fluorine . Selenium is in its highest oxidation state + VI. Under normal conditions , selenium hexafluoride is a colorless, poisonous, easily condensable gas.

presentation

Similar to sulfur hexafluoride, selenium hexafluoride can be produced from the elements (direct synthesis).

{\ displaystyle {\ ce {Se + 3 F2 -> SeF6}}}

properties

Physical Properties

Selenium hexafluoride is physically interesting due to its relatively high density in gas form . The sublimation point is −46.6 ° C at normal pressure. Under pressure and in a closed system, the solid substance also shows a melting and boiling point. Its critical temperature is 72.4 ° C, the triple point temperature is −34.7 ° C.

Chemical properties

Due to its symmetrical , dense molecular structure, selenium hexafluoride is just as inert as sulfur hexafluoride , although it is thermally somewhat more unstable. In contrast to its higher homologue tellurium hexafluoride , it is only very slowly hydrolyzed by water , producing hydrogen fluoride and selenic acid .

use

Selenium hexafluoride is used as an electrical insulator in arc lamp electrodes and the like.

Individual evidence

↑ ^a ^b ^c ^d ^e ^f ^g ^h Entry on selenium hexafluoride in the GESTIS substance database of the IFA , accessed on February 1, 2016(JavaScript required) .
↑ ^a ^b ^c Georg Kimmerle: “Comparative studies of the inhalation toxicity of sulfur, selenium and tellurium hexafluoride”, in: Archiv für Toxikologie , 1960 , 18 (2), pp. 140–144; doi : 10.1007 / BF00605645 .
↑ ^a ^b ^c Entry on selenium hexafluoride in the ChemIDplus database of the United States National Library of Medicine (NLM) .
^ ^A ^b A. F. Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 102nd edition. Walter de Gruyter, Berlin 2007, ISBN 978-3-11-017770-1 , pp. 628-629.
^ Agency for Toxic Substances and Disease Registry (ATSDR): ToxFAQs for Selenium Hexafluoride .

literature

Gmelin's Handbook of Inorganic Chemistry , System No. 10, Selenium, Part B 2, pp. 39-66.

[GESTIS-1] ↑ ^a ^b ^c ^d ^e ^f ^g ^h Entry on selenium hexafluoride in the GESTIS substance database of the IFA , accessed on February 1, 2016(JavaScript required) .

[arctox-2] Georg Kimmerle: “Comparative studies of the inhalation toxicity of sulfur, selenium and tellurium hexafluoride”, in: Archiv für Toxikologie , 1960 , 18 (2), pp. 140–144; doi : 10.1007 / BF00605645 .

[chemid-3] Entry on selenium hexafluoride in the ChemIDplus database of the United States National Library of Medicine (NLM) .

[howi-4] A ^b A. F. Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 102nd edition. Walter de Gruyter, Berlin 2007, ISBN 978-3-11-017770-1 , pp. 628-629.

[5] Agency for Toxic Substances and Disease Registry (ATSDR): ToxFAQs for Selenium Hexafluoride .