Chlorine trifluoride dioxide is an inorganic compound of chlorine, fluorine, and oxygen with the chemical formula ClO2F3.[1]
| Names | |
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| Other names
Chloryl trifluoride, chlorine dioxytrifluoride, trifluorodioxychlorine
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| Identifiers | |
3D model (JSmol)
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| Properties | |
| ClF3O2 | |
| Molar mass | 124.44 g·mol−1 |
| Appearance | colorless gas |
| Density | 5.087 g/L |
| Melting point | −81 °C (−114 °F; 192 K) |
| Boiling point | −22 °C (−8 °F; 251 K) |
| reacts with water | |
| Related compounds | |
Related compounds
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Iodyl trifluoride Bromyl trifluoride |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Synthesis
editSynthesis of chlorine trifluoride dioxide can be by a reaction of chlorine monofluoride with dioxygen difluoride:[2]
- ClF + O2F2 → ClO2F3
Alternatively it can be made by a reaction of chlorine trifluoride with oxygen gas:[2]
- ClF3 + O2 → ClO2F3
Physical properties
editChlorine trifluoride dioxide is a colorless gas at standard conditions.[3]
Chemical properties
editClO2F3 reacts with water.[4]
References
edit- ^ Rode, B. M.; Engelbrecht, A. (15 September 1972). "LCAO MO SCF calculations on ClO2F3". Chemical Physics Letters. 16 (1): 26–27. Bibcode:1972CPL....16...26R. doi:10.1016/0009-2614(72)80448-2. ISSN 0009-2614. Retrieved 6 June 2023.
- ^ a b Downs, A. J.; Adams, C. J. (4 May 2017). The Chemistry of Chlorine, Bromine, Iodine and Astatine: Pergamon Texts in Inorganic Chemistry, Volume 7. Elsevier. p. 1395. ISBN 978-1-4831-5832-7. Retrieved 6 June 2023.
- ^ Haupt, Axel (22 March 2021). Organic and Inorganic Fluorine Chemistry: Methods and Applications. Walter de Gruyter GmbH & Co KG. ISBN 978-3-11-065950-4. Retrieved 6 June 2023.
- ^ Lide, David R. (29 June 2004). CRC Handbook of Chemistry and Physics, 85th Edition. CRC Press. p. 4-52. ISBN 978-0-8493-0485-9. Retrieved 6 June 2023.