Trisulfuryl fluoride

  1. Home
  2. Wiki
Trisulfuryl fluoride
Names
Preferred IUPAC name
bis(fluorosulfonyl) sulfate
Other names
Trisulfuryl difluoride
Identifiers
3D model (JSmol)
  • 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
Appearance colorless 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]

Synthesis

[edit]

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

[edit]

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

[edit]

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

See also

[edit]

References

[edit]
  1. ^ a b c 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. ^ a b 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)