Disulfur decafluoride
Chemical compound
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Through Sulfur, Valence (chemistry) and Toxicity
It is a colorless liquid with a burnt match smell similar to sulfur dioxide.
Production
Disulfur decafluoride is produced by photolysis of SF5Br:
- 2 SF5Br → S2F10 + Br2
Disulfur decafluoride arises by the decomposition of sulfur hexafluoride. 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.
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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, S
2F
10 decomposes slowly (disproportionation) into SF
6 and SF
4:
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.
- S
2F
10 + N
2F
4 → 2 SF
5NF
2
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. The reversibility of this reaction can be used to synthesize S
2F
10 from SF
5Br.
Ammonia is oxidised by S
2F
10 into NSF
3.
Toxicity
S
2F
10 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 SF
6, which is inert, and SF
4, which reacts with moisture to form sulfurous acid and hydrofluoric acid.