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| Names | ||
|---|---|---|
| Preferred IUPAC name
Disulfur decafluoride | ||
| Systematic IUPAC name
Decafluoro-1λ6,2λ6-disulfane | ||
| Identifiers | ||
CAS Number
|
5714-22-7 | |
| ChemSpider | 56348 
| |
| EC Number | 227-204-4 | |
| Jmol 3D model | Interactive image | |
| MeSH | Disulfur+decafluoride | |
| PubChem | 62586 | |
InChI
| ||
SMILES
| ||
| Properties | ||
| Appearance | colorless liquid | |
| Melting point | ||
| Boiling point | ||
Solubility in water
|
insoluble[1] | |
| Hazards | ||
| Main hazards | Poisonous | |
| NFPA 704 | 
3
4
2 | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | ||
| Infobox references | ||
Disulfur decafluoride (S2F10) is a gas discovered in 1934 by Denbigh and Whytlaw-Gray.[2] Each S of the S2F10 molecule is octahedral, and surrounded by 5 fluorines.[3] S2F10 is highly toxic, with toxicity 4 times that of phosgene. It 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. It is produced by the electrical decomposition of sulfur hexafluoride (SF6)—an essentially inert insulator used in high voltage systems such as transmission lines, substations and switchgear. S2F10 is also made during the production of SF6, but is distilled out.
Production[]
Disulfur decafluoride is produced primarily by the decomposition of sulfur hexafluoride:
2 SF6 → S2F10 + F2
Properties[]
This compound contains sulfur in the +5 oxidation state.
At temperatures above 150 °C, S
2F
10 decomposes slowly to SF
6 and SF
4:
S2F10 → SF6 + SF4
S
2F
10 reacts with N
2F
4 to give SF
5NF
2. It reacts with SO
2 to form SF
5OSO
2F in the presence of ultraviolet radiation.
In the presence of excess chlorine gas, S
2F
10 reacts to form sulfur chloride pentafluoride (SF
5Cl):
- S
2F
10 + Cl
2 → 2 SF
5Cl
The analogous reaction with bromine is reversible and yields SF
5Br.[4] The reversibility of this reaction can be used to synthesize S
2F
10 from SF
5Br.[5]
Ammonia is oxidised by S
2F
10 into NSF
3.[6]
Toxicity[]
S
2F
10 Sulfur pentafluoride is a colorless gas or liquid with a sulfur-dioxide-like odor.[7] It is about 4 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.[8] Disulfur decafluoride itself is not toxic due to hydrolysis products, since it is hardly hydrolysed by water and most aqueous solutions.
External links[]
- "Sulfur Pentaflu". 1988 OSHA PEL Project. CDC NIOSH. http://www.cdc.gov/niosh/pel88/5714-22.html.
References[]
- ↑ http://www.chemicalbook.com/ChemicalProductProperty_EN_CB0751782.htm
- ↑ Denbigh, K. G.; Whytlaw-Gray, R. (1934). "The Preparation and Properties of Disulphur Decafluoride". pp. 1346–1352. Digital object identifier:10.1039/JR9340001346.
- ↑ doi: 10.1021/ja01108a015
This citation will be automatically completed in the next few minutes. You can jump the queue or expand by hand - ↑ doi: 10.1021/ic50034a025
This citation will be automatically completed in the next few minutes. You can jump the queue or expand by hand - ↑ doi: 10.1016/S0022-1139(97)00096-1
This citation will be automatically completed in the next few minutes. You can jump the queue or expand by hand - ↑ Mitchell, S. (1996). Biological Interactions of Sulfur Compounds. CRC Press. p. 14. ISBN 0-7484-0245-4.
- ↑ "Sulfur Pentaflu". 1988 OSHA PEL Project. CDC NIOSH. http://www.cdc.gov/niosh/pel88/5714-22.html.
- ↑ Johnston, H. (2003). A Bridge not Attacked: Chemical Warfare Civilian Research During World War II. World Scientific. pp. 33–36. ISBN 981-238-153-8.
- Christophorou, L. G.; Sauers, I. (1991). Gaseous Dielectrics VI. Plenum Press. ISBN 0-306-43894-1.
The original article can be found at Disulfur decafluoride and the edit history here.