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| Names | |
|---|---|
| Other names chlorine dioxide fluoride | |
| Identifiers | |
3D model (JSmol) | |
| ChemSpider |
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| Properties | |
| ClFO2 | |
| Molar mass | 86.45 g·mol−1 |
| Density | 3.534 g/L |
| Melting point | −115 °C |
| Boiling point | −6 °C |
| Related compounds | |
Related compounds | Perchloryl fluoride Chloryl trifluoride |
Except where otherwise noted, data are given for materials in theirstandard state (at 25 °C [77 °F], 100 kPa). | |
Chloryl fluoride is thechemical compound with the formula ClO2F. It is commonly encountered as side-product in reactions ofchlorine fluorides with oxygen sources.[1] It is theacyl fluoride ofchloric acid.
ClO2F was first reported by Schmitz and Schumacher in 1942, who prepared it by the fluorination ofClO2.[2] The compound is more conveniently prepared by reaction ofsodium chlorate andchlorine trifluoride[3] and purified by vacuum fractionation, i.e. selectively condensing this species separately from other products. This species is a gas boiling at −6 °C:
In contrast toO2F2, ClO2F is a pyramidal molecule as predicted byVSEPR. 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 compoundperchloryl fluoride, ClO3F, is tetrahedral.The related bromine compoundbromyl fluoride (BrO2F) adopts the same structure as ClO2F, whereasiodyl fluoride (IO2F) forms a polymeric substance under standard conditions.[4]
Rocket fuel chemistJohn Drury Clark reported in his bookIgnition! that chloryl fluoride "is indecently reactive, and the hardest to keep of all the CI-O-F compounds, since it apparently dissolves theprotective metal fluoride coatings that make the storage of ClF3 comparatively simple."[5]
