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Thiothionyl fluoride

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Thiothionyl fluoride
Names
IUPAC name difluoro(sulfanylidene)-λ-sulfane
Other names Sulphur(IV) sulfide difluoride
Thiosulfinic difluoride
Identifiers
CAS Number
3D model (JSmol)
ChemSpider
PubChem CID
CompTox Dashboard (EPA)
InChI
  • InChI=1S/F2S2/c1-4(2)3Key: KBYVSSUWTLBZTB-UHFFFAOYSA-N
SMILES
  • FS(=S)F
Properties
Chemical formula S=SF2
Molar mass 102.12 g·mol
Appearance colorless gas
Melting point −164.6 °C (−264.3 °F; 108.5 K)
Boiling point −10.6 °C (12.9 °F; 262.5 K)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). Infobox references
Chemical compound

Thiothionyl fluoride is a chemical compound of fluorine and sulfur, with the chemical formula S=SF2. It is an isomer of disulfur difluoride (difluorodisulfane) F−S−S−F.

Preparation

Thiothionyl fluoride can be obtained from the reaction between disulfur dichloride with potassium fluoride at about 150 °C or with mercury(II) fluoride at 20 °C.

S2Cl2 + 2 KF → S=SF2 + 2 KCl

Another possible preparation is by the reaction of nitrogen trifluoride with sulfur.

NF3 + 3 S → S=SF2 + NSF

It also forms from disulfur difluoride when in contact with alkali metal fluorides.

S=SF2 can also be synthesized with the reaction of potassium fluorosulfite and disulfur dichloride:

2 KSO2F + S2Cl2 → S=SF2 + 2 KCl + 2 SO2

Properties

Thiothionyl fluoride is a colorless gas. At high temperatures and pressures, it decomposes into sulfur tetrafluoride and sulfur.

2 S=SF2 → SF4 + 3 S

With hydrogen fluoride, it forms sulfur tetrafluoride and hydrogen sulfide.

S=SF2 + 2 HF → SF4 + H2S

It condenses with sulfur difluoride at low temperatures to yield 1,3-difluoro-trisulfane-1,1-difluoride.

S=SF2 + SF2 → FS−S−SF3

References

  1. ^ Brauer, Georg; Baudler, Marianne (1975). Handbuch der Präparativen Anorganischen Chemie. Band I. (3rd ed.). Stuttgart: Ferdinand Enke. p. 182. ISBN 3-432-02328-6.
  2. ^ Holleman, A. F.; Wiberg, E.; Wiberg, N. (1995). Lehrbuch der Anorganischen Chemie (101st ed.). Berlin: Walter de Gruyter. p. 379. ISBN 3-11-012641-9.
  3. Steudel, Ralf (2008). Chemie der Nichtmetalle: Von Struktur und Bindung zur Anwendung. Walter de Gruyter. p. 475. ISBN 978-311021128-3.
  4. 张青莲 (1991). 《无机化学丛书》第五卷：氧、硫、硒分族 (in Chinese). Beijing: Science Press. p. 179. ISBN 978-7-03-002238-7.
  5. Kolditz, Lothar (1983). Anorganische Chemie. Berlin: Deutscher Verlag der Wissenchaften. p. 468.
  6. Lösking, O.; Willner, H.; Baumgärtel, H.; Jochims, H. W.; Rühl, E. (November 1985). "Chalkogenfluoride in niedrigen Oxydationsstufen. X Thermochemische Daten und Photoionisations-Massenspektren von SSF2, FSSF, SF3SF und SF3SSF". Zeitschrift für anorganische und allgemeine Chemie. 530 (11): 169–177. doi:10.1002/zaac.19855301120.
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