Chemistry:Chlorine fluorosulfate
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3D model (JSmol)
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PubChem CID
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| Properties | |
| ClFO3S | |
| Molar mass | 134.51 g·mol−1 |
| Appearance | Light yellow liquid |
| Density | 1.71 g/cm³ |
| Melting point | −84.3 °C |
| Boiling point | 43.4 °C |
| reacts with water | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Chlorine fluorosulfate is an inorganic compound with the chemical formula ClFO
3S.[1] This is a derivative of fluorosulfonic acid.
Synthesis
Chlorine fluorosulfonate can be prepared by reacting sulfur trioxide and chlorine monofluoride at low temperatures:[2]
- SO
3 + ClF → ClOSO
2F
- SO
The compound can also be prepared by reacting sulfonyl fluoride peroxide with chlorine at 125 °C under high pressure:
- Cl
2 + S
2O
6F
2 → 2ClOSO
2F
- Cl
Physical properties
The compound is a highly reactive, and forms a pale yellow liquid that reacts violently with water.[3] The compound decomposes upon warming to room temperature, turning red.
Chemical properties
Chlorine trifluoride oxide reacts with chlorine fluorosulfate:
- ClOF
3 + 2ClOSO
2F → S
2O
5F
2 + FClO
2 + 2ClF
- ClOF
The reaction also produces SO
2F
2.[4]
The compound also reacts with nitronium perchlorate to produce chlorine perchlorate:[5]
- 2ClOSO
2F + NO
2ClO
4 → ClClO
4 + NO
2SO
3F
- 2ClOSO
Uses
The compound is used as a chlorinating agent, fluorosulfating agent, and oxidizer.[6]
See also
- Bromine fluorosulfate
- Fluorine fluorosulfate
- Iodine fluorosulfate
- Triiodine fluorosulfate
References
- ↑ Aubke, Friedhelm; Casper, Bernd; Müller, Holger S. P.; Oberhammer, Heinz; Willner, Helge (15 February 1995). "Vibrational spectra and gas phase structures of fluorine fluorosulfate (FOSO2F) and chlorine fluorosulfate (ClOSO2F)". Journal of Molecular Structure 346: 111–120. doi:10.1016/0022-2860(94)08421-D. ISSN 0022-2860. https://www.sciencedirect.com/science/article/abs/pii/002228609408421D. Retrieved 9 August 2025.
- ↑ Hardin, C. V.; Ratcliffe, Charles T.; Anderson, Lowell Ray; Fox, William B. (1 August 1970). "Preparing chlorine fluorosulfate". Inorganic Chemistry 9 (8): 1938–1939. doi:10.1021/ic50090a035. ISSN 0020-1669. https://pubs.acs.org/doi/10.1021/ic50090a035. Retrieved 9 August 2025.
- ↑ (in en) Inorganic Syntheses. John Wiley & Sons. 22 September 2009. p. 8. ISBN 978-0-470-13290-6. https://books.google.com/books?id=xLP_KevavOkC&dq=Chlorine+fluorosulfate&pg=PA8. Retrieved 9 August 2025.
- ↑ (in en) Advances in Inorganic Chemistry and Radiochemistry. Academic Press. 9 July 1976. pp. 331–333. ISBN 978-0-08-057867-5. https://books.google.com/books?id=EWlBFTxYth4C&pg=PA331. Retrieved 9 August 2025.
- ↑ Steudel, Ralf (20 April 2011) (in en). Chemistry of the Non-Metals: With an Introduction to Atomic Structure and Chemical Bonding. Walter de Gruyter. p. 266. ISBN 978-3-11-083082-8. https://books.google.com/books?id=Z7_-lFZbxi0C&dq=Chlorine+fluorosulfate&pg=PA266. Retrieved 9 August 2025.
- ↑ Schack, Carl J.; Wilson, Richard D.; Totsch, W. (1986). "Chlorine Fluorosulfate" (in en). Inorganic Syntheses. John Wiley & Sons, Ltd. pp. 6–8. doi:10.1002/9780470132555.ch3. ISBN 978-0-470-13255-5. https://onlinelibrary.wiley.com/doi/10.1002/9780470132555.ch3. Retrieved 9 August 2025.
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