Chemistry:Chloryl fluoride
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| Properties | |
| ClO 2F | |
| Molar mass | 86.45 g·mol−1 |
| Appearance | Colorless gas |
| Density | 3.534 g/L |
| Melting point | −115 °C |
| Boiling point | −6 °C |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 verify (what is   ?)
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Chloryl fluoride is the chemical compound with the formula ClO
2F. This compound is a gas boiling at −6 °C. It is commonly encountered as side-product in reactions of chlorine fluorides with oxygen sources.[1] It is the acyl fluoride of chloric acid.
Preparation
ClO
2F was first reported by Schmitz and Schumacher in 1942, who prepared it by the fluorination of ClO
2.[2] The compound is more conveniently prepared by reaction of sodium chlorate and chlorine trifluoride[3] and purified by vacuum fractionation, i.e. selectively condensing this species separately from other products.
Structure
In contrast to O
2F
2, ClO
2F is a pyramidal molecule as predicted by VSEPR. The differing structures reflects the greater tendency of chlorine to exist in positive oxidation states with oxygen and fluorine ligands. The related Cl-O-F compound perchloryl fluoride, ClO
3F, is tetrahedral.
The related bromine compound bromyl fluoride (BrO
2F) adopts the same structure as ClO
2F, whereas iodyl fluoride (IO
2F) forms a polymeric substance under standard conditions.[4]
Precautions
Rocket fuel chemist John Drury Clark reported in his book Ignition! that chloryl fluoride "is indecently reactive, and the hardest to keep of all the CI-O-F compounds, since it apparently dissolves the protective metal fluoride coatings that make the storage of ClF
3 comparatively simple."[5]
References
- ↑ Christe, K. O.; Wilson, R. D.; Schack, C. J. "Chloryl fluoride" Inorganic Syntheses, 1986, volume 24, pages 3–5. ISBN:0-471-83441-6 https://onlinelibrary.wiley.com/doi/10.1002/9780470132555.ch2
- ↑ Schmitz, H.; Schumacheb, H. J. (1942-04-29). "Über eine neue Reaktion des Chlordioxyds. Die Bildung einer Verbindung der Formel ClO2F" (in de). Zeitschrift für anorganische und allgemeine Chemie (Wiley) 249 (3): 238–244. doi:10.1002/zaac.19422490302. ISSN 0863-1786.
- ↑ Wiberg, Egon; Wiberg, Nils; Holleman, A. F. (2001). Inorganic chemistry. San Diego: Academic Press. p. 1797. ISBN 0-12-352651-5. OCLC 48056955.
- ↑ Holleman, A.F.; Wiberg, E.; Wiberg, N. (1995). Lehrbuch der anorganischen Chemie. de Gruyter. p. 501. ISBN 9783110126419. https://books.google.com/books?id=eGkvSDAqY9gC. Retrieved 2015-02-20.
- ↑ Clark, John Drury (23 May 2018). Ignition!: An Informal History of Liquid Rocket Propellants. Rutgers University Press. pp. 302. ISBN 978-0-8135-9918-2. OCLC 281664. https://books.google.com/books?id=BdU4DwAAQBAJ&q=perchloryl%20fluoride.
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