Trisulfuryl fluoride

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Trisulfuryl fluoride
Trisulfuryl fluoride.svg
Names
Preferred IUPAC name
bis(fluorosulfonyl) sulfate
Other names
Trisulfuryl difluoride
Identifiers
3D model (JSmol)
PubChem CID
  • InChI=1S/F2O8S3/c1-11(3,4)9-13(7,8)10-12(2,5)6
    Key: UOBKEQZSWBMYKP-UHFFFAOYSA-N
  • O=S(=O)(OS(=O)(=O)F)OS(=O)(=O)F
Properties
F2O8S3
Molar mass 262.17 g·mol−1
Appearancecolorless liquid
Density 1.86 g/cm3 [1]
Boiling point 120 °C [1]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Trisulfuryl fluoride is an inorganic compound of fluorine, oxygen, and sulfur with the chemical formula S3O8F2. [2] [3] [4]

Contents

Synthesis

The compound is obtained by the thermal disassociation of KBF4·4SO3 or via reaction of potassium tetrafluoroborate (KBF4) with sulfur trioxide (SO3) at 70 °C. [5]

Also, trisulfuryl fluoride is formed in a reaction of sulfur trioxide (SO3), boron trifluoride (BF3), and 70% sulfuric acid (H2SO4) at 70 °C. [1]

Chemical properties

Trisulfuryl fluoride is a reactive compound. It is known to decompose into disulfuryl fluoride when heated. The compound reacts with certain compounds, like the sodium cyanohydrin salt, to form other fluorosulfates. [6]

It slowly hydrolizes in the solution of potassium hydroxide (KOH): [5]

S3O8F2 + 4KOH → 2KSO3F + K2SO4 + 2H2O

Physical properties

The compound forms a colorless liquid. It fumes in air and is insoluble in the concentrated H2SO4. [7] [8]

See also

References

  1. 1 2 3 Simons, J. H. (2 December 2012). Fluorine Chemistry V5. Elsevier. p. 71. ISBN   978-0-323-14724-8 . Retrieved 20 August 2025.
  2. ↑ Lustig, Max (January 1, 1970). "Synthesis of fluorosulfates and difluorophosphates by the heterolytic cleavage of polysulfuryl fluorides and pyrophosphoryl fluoride with 2-substituted perfluoroisopropoxide and fluoroalkoxide anions" . ACS Publications : 104. doi:10.1021/ic50083a021 . Retrieved 20 August 2025.
  3. ↑ Ruff, John K. (1 May 2002). "Sulfur Oxyfluoride Derivatives. II" . ACS Publications . 4 (4): 567. doi:10.1021/ic50026a027 . Retrieved 20 August 2025.
  4. ↑ Macintyre, Jane E. (23 July 1992). Dictionary of Inorganic Compounds. CRC Press. p. 3158. ISBN   978-0-412-30120-9 . Retrieved 20 August 2025.
  5. 1 2 Ryss, Iosif Grigorʹevich (1960). The Chemistry of Fluorine and Its Inorganic Compounds. U. S. Atomic Energy Commission, Technical Information Service Extension. p. 186. Retrieved 20 August 2025.
  6. ↑ Ruff, John K. (1 May 2002). "Sulfur Oxyfluoride Derivatives. II" . ACS Publications . 4 (4): 567. doi:10.1021/ic50026a027 . Retrieved 20 August 2025.
  7. ↑ Brauer, Georg (2 December 2012). Handbook of Preparative Inorganic Chemistry V1. Elsevier. p. 174. ISBN   978-0-323-16127-5 . Retrieved 20 August 2025.
  8. ↑ Advances in Inorganic Chemistry and Radiochemistry. Academic Press. 1960. p. 123. ISBN   978-0-08-057851-4 . Retrieved 20 August 2025.{{cite book}}: ISBN / Date incompatibility (help)
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