Thiazyl trifluoride
Names
IUPAC name
Thiazyl trifluoride
Other names
Sulfur(VI) nitride trifluoride
Trifluorosulfanenitrile
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
  • InChI=1S/F3NS/c1-5(2,3)4 checkY
    Key: UQUPGRNSXINWBS-UHFFFAOYSA-N checkY
  • InChI=1/F3NS/c1-5(2,3)4
    Key: UQUPGRNSXINWBS-UHFFFAOYAR
  • FS(F)(F)#N
Properties
NSF3
Molar mass 103.06 g·mol−1
Appearance Colourless gas
Melting point −72.6 °C (−98.7 °F; 200.6 K)
Boiling point −27.1 °C (−16.8 °F; 246.1 K)
Structure
Tetrahedral at the S atom
Hybridisation sp3
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Thiazyl trifluoride is a chemical compound of nitrogen, sulfur, and fluorine, having the formula NSF3. It exists as a stable, colourless gas, and is an important precursor to other sulfur-nitrogen-fluorine compounds.[1] It has tetrahedral molecular geometry around the sulfur atom, and is regarded to be a prime example of a compound that has a sulfur-nitrogen triple bond.[2]

Preparation

NSF3 can be synthesised by the fluorination of thiazyl fluoride, NSF, with silver(II) fluoride, AgF2:

NSF + 2 AgF2 → NSF3 + 2 AgF

or by the oxidative decomposition of FC(O)NSF2 by silver(II) fluoride:[3]

FC(O)NSF2 + 2 AgF2 → NSF3 + 2 AgF + COF2

It is also a product of the oxidation of ammonia by S2F10.[4]

Reactions

NSF3 is much more stable than thiazyl fluoride, does not reacts with ammonia and hydrogen chloride, and only reacts with sodium at 400 °C.[5] It reacts with carbonyl fluoride (COF2) in the presence of hydrogen fluoride to form pentafluorosulfanyl isocyanate (SF5NCO).[6]

References

  1. ^ Oskar Glemser and Rüdiger Mews (1980). "Chemistry of Thiazyl Fluoride (NSF) and Thiazyl Trifluoride (NSF3): A Quarter Century of Sulfur-Nitrogen-Fluorine Chemistry". Angew. Chem. Int. Ed. Engl. 19 (11): 883–899. doi:10.1002/anie.198008831.
  2. ^ Borrmann, T.; Lork, E.; Mews, R. D.; Parsons, S.; Petersen, J.; Stohrer, W. D.; Watson, P. G. (2008). "The crystal structures of NSF
    3     and (NSF2N(CH3)CH2–)2: How short is the 'Crystallographic' N≡S triple bond?". Inorganica Chimica Acta. 361 (2): 479–486. doi:10.1016/j.ica.2007.05.016.
  3. ^ Chivers, Tristram; Laitinen, Risto S. (2006). "Chalcogen–Nitrogen Chemistry". In Devillanova, Francesco (ed.). Handbook of Chalcogen Chemistry. London: The Royal Society of Chemistry. p. 238. doi:10.1039/9781847557575. ISBN 978-0-85404-366-8.
  4. ^ Steve Mitchell (1996). Steve Mitchell (ed.). Biological interactions of sulfur compounds. CRC Press. p. 14. ISBN 0-7484-0245-4.
  5. ^ Huheey, James E.; Keiter, Ellen A.; Keiter, Richard L. (2003). Anorganische Chemie (in German). Berlin: Walter de Gruyter. p. 1021. ISBN 978-3-11-017903-3.
  6. ^ US patent 3,666,784, Alan F. Clifford, Thomas C. Rhyne and James W. Thompson, "Process For Preparing .alpha.,.alpha.-Fluorinated Alkyl Isocyanates", issued 1972-05-30 

[1]

  1. ^ Li, Bing‐Yu; Su, Kexin; Van Meervelt, Luc; Verhelst, Steven H. L.; Ismalaj, Ermal; De Borggraeve, Wim M.; Demaerel, Joachim (2023-07-17). "Ex situ Generation of Thiazyl Trifluoride (NSF 3 ) as a Gaseous SuFEx Hub**". Angewandte Chemie International Edition. 62 (29). doi:10.1002/anie.202305093. ISSN 1433-7851.
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