Disulfur decafluoride
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| MeSH | Disulfur+decafluoride |
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| RTECS number | Template:Unbulleted list |
| UN number | 3287 |
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| Template:Longitem | Template:Chem2 |
| Molar mass | Template:Chem molar mass |
| Appearance | colorless liquid |
| Odor | like sulfur dioxide[1] |
| Density | 2.08 g/cm3 |
| Melting point | Template:Chembox CalcTemperatures |
| Boiling point | Template:Chembox CalcTemperatures |
| Vapor pressure | 561 mmHg (20 °C)[1] |
| NFPA 704 (fire diamond) | Template:NFPA 704 diamond |
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Disulfur decafluoride is a chemical compound with the formula Template:Chem2. It was discovered in 1934 by Denbigh and Whytlaw-Gray.[4] Each sulfur atom of the Template:Chem2 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 Template:Chem2 molecule, the oxidation state of each sulfur atoms is +5, but their valency is 6 (they are hexavalent). Template:Chem2 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 Template:Chem2:[6]
Disulfur decafluoride arises by the decomposition of sulfur hexafluoride. It is produced by the electrical decomposition of sulfur hexafluoride (Template:Chem2)—an essentially inert insulator used in high voltage systems such as transmission lines, substations and switchgear. Template:Chem2 is also made during the production of Template:Chem2.
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, Template:Chem/link decomposes slowly (disproportionation) into Template:Chem/link and Template:Chem/link:
Template:Chem/link reacts with [[Tetrafluorohydrazine|Template:Chem/link]] to give [[Difluoroamino sulfur pentafluoride|Template:Chem/link]]. It reacts with Template:Chem/link to form Template:Chem/link in the presence of ultraviolet radiation.
In the presence of excess chlorine gas, Template:Chem/link reacts to form sulfur chloride pentafluoride (Template:Chem/link):
The analogous reaction with bromine is reversible and yields Template:Chem/link.[7] The reversibility of this reaction can be used to synthesize Template:Chem/link from Template:Chem/link.[8]
Ammonia is oxidised by Template:Chem/link into [[Thiazyl trifluoride|Template:Chem/link]].[9]
Toxicity
Template:Chem/link 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.[10] It is about four times as poisonous as phosgene. Its toxicity is thought to be caused by its disproportionation in the lungs into Template:Chem/link, which is inert, and Template:Chem/link, which reacts with moisture to form sulfurous acid and hydrofluoric acid.[11]
See also
References
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External links
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