Disulfur decafluoride is a chemical compound with the formula S2F10. It was discovered in 1934 by Denbigh and Whytlaw-Gray.[4] Each sulfur atom of the S2F10 molecule is octahedral, and surrounded by five fluorine atoms[5] and one sulfur atom. The two sulfur atoms are connected by a single bond. In the S2F10 molecule, the oxidation state of each sulfur atoms is +5, but their valency is 6 (they are hexavalent). S2F10 is highly toxic, with toxicity four times that of phosgene.
It is a colorless liquid with a burnt match smell similar to sulfur dioxide.[1]
Production
Disulfur decafluoride is produced by photolysis of SF5Br:[6]
The analogous reaction with bromine is reversible and yields SF 5Br.[7] The reversibility of this reaction can be used to synthesize S 2F 10 from SF 5Br.[8]
S 2F 10 was considered a potential chemical warfarepulmonary agent in World War II because it does not produce lacrimation or skin irritation, thus providing little warning of exposure.
Disulfur decafluoride is a colorless gas or liquid with a SO2-like odor.[10] It is about four times as poisonous as phosgene. Its toxicity is thought to be caused by its disproportionation in the lungs into SF 6, which is inert, and SF 4, which reacts with moisture to form sulfurous acid and hydrofluoric acid.[11]
^Denbigh, K. G.; Whytlaw-Gray, R. (1934). "The Preparation and Properties of Disulphur Decafluoride". Journal of the Chemical Society. 1934: 1346–1352. doi:10.1039/JR9340001346.
^Harvey, R. B.; Bauer, S. H. (June 1953). "An Electron Diffraction Study of Disulfur Decafluoride". Journal of the American Chemical Society. 75 (12): 2840–2846. doi:10.1021/ja01108a015.