From Surf Wiki (app.surf) — the open knowledge base

Disulfur decafluoride

TL-70 Agent Z | NFPA-H = 4 | NFPA-F = 0 | NFPA-R = 0 | NFPA-S = OX 1000 mg/m3 (mouse, 10 min) 4000 mg/m3 (rabbit, 10 min) 4000 mg/m3 (guinea pig, 10 min) 4000 mg/m3 (dog, 10 min) Disulfur decafluoride is a chemical compound with the formula . It was discovered in 1934 by Denbigh and Whytlaw-Gray. Each sulfur atom of the molecule is octahedral, and surrounded by five fluorine atoms and one sulfur atom. The two sulfur atoms are connected by a single bond. In the molecule, the oxidation state of each sulfur atoms is +5, but their valency is 6 (they are hexavalent). is highly toxic, with toxicity four times that of phosgene.

It is a colorless liquid with a burnt match smell similar to sulfur dioxide.

Production

Disulfur decafluoride is produced by photolysis of , or in H2: : :

Disulfur decafluoride arises by the decomposition of sulfur hexafluoride. It is produced by the electrical decomposition of sulfur hexafluoride ()—an essentially inert insulator used in high voltage systems such as transmission lines, substations and switchgear. is also made during the production of .

Properties

The S-S bond dissociation energy is 305 ± 21 kJ/mol, about 80 kJ/mol stronger than the S-S bond in diphenyldisulfide.

At temperatures above 150 °C, decomposes slowly (disproportionation) into and : :S2F10 → SF6 + SF4

reacts with to give . It reacts with to form in the presence of ultraviolet radiation.

: + → 2

In the presence of excess chlorine gas, reacts to form sulfur chloride pentafluoride ():

: + → 2

The analogous reaction with bromine is reversible and yields . The reversibility of this reaction can be used to synthesize from .

Ammonia is oxidised by into .

Toxicity

was considered a potential chemical warfare pulmonary 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. It is about four times as poisonous as phosgene. Its toxicity is thought to be caused by its disproportionation in the lungs into , which is inert, and , which reacts with moisture to form sulfurous acid and hydrofluoric acid.

References

{{PGCH. 0579
"Disulphur Decafluoride | 5714-22-7".
{{IDLH. 5714227. Sulfur pentafluoride
(1934). "The Preparation and Properties of Disulphur Decafluoride". Journal of the Chemical Society.
(June 1953). "An Electron Diffraction Study of Disulfur Decafluoride". Journal of the American Chemical Society.
(1998). "A new preparation of disulfur decafluoride". Journal of Fluorine Chemistry.
(2015). "Preparation and utility of organic pentafluorosulfanyl-containing compounds". Chemical Reviews.
(December 1965). "Chemical Properties of Disulfur Decafluoride". Inorganic Chemistry.
(January 1998). "A new preparation of disulfur decafluoride". Journal of Fluorine Chemistry.
Mitchell, S.. (1996). "Biological Interactions of Sulfur Compounds". CRC Press.
(28 February 2020). "Sulfur Pentaflu". CDC NIOSH.
Johnston, H.. (2003). "A Bridge not Attacked: Chemical Warfare Civilian Research During World War II". World Scientific.

Info: Wikipedia Source

This article was imported from Wikipedia and is available under the Creative Commons Attribution-ShareAlike 4.0 License. Content has been adapted to SurfDoc format. Original contributors can be found on the article history page.

pulmonary-agents sulfur-fluorides hypervalent-molecules

Want to explore this topic further?

Ask Mako anything about Disulfur decafluoride — get instant answers, deeper analysis, and related topics.

Research with Mako

Free with your Surf account

Content sourced from Wikipedia, available under CC BY-SA 4.0.

This content may have been generated or modified by AI. CloudSurf Software LLC is not responsible for the accuracy, completeness, or reliability of AI-generated content. Always verify important information from primary sources.

Report