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Dioxygen difluoride
From Wikipedia, the free encyclopedia
| Oxygen difluoride | |
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| Systematic name | oxygen(I) fluoride |
| Other names | difluorine dioxide fluorine dioxide dioxygen difluoride perfluoroperoxide |
| Molecular formula | O2F2 |
| Molar mass | 69.996 g mol−1 |
| CAS number | [7783-44-0] |
| Density | 1.45 g cm−3 |
| Solubility (in water) | ? |
| Melting point | −154°C |
| Boiling point | −57°C |
| Color | yellow (solid and liquid) |
| O−O bond dissociation energy | 430 kJ mol−1 |
| O−F bond dissociation energy | 75 kJ mol−1 |
| Related compounds | FClO2 S2Cl2 |
| Disclaimer and references | |
Dioxygen difluoride, O2F2, is a gaseous fluoride of oxygen. In the solid and liquid phases, it is yellow. It is unique amongst oxygen compounds in that oxygen has an oxidation state of +1. In all its other compounds (other than peroxides and superoxides), oxygen has an oxidation state of −2, except in oxygen difluoride, OF2, where it is +2. O2F2 is considerably less stable than OF2 and rapidly decomposes to the latter, even at very low temperatures.
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Dioxygen difluoride can be obtained by subjecting a 1:1 mixture of gaseous fluorine and oxygen at low pressure (7-17 mmgHg is optimal) to an electric discharge of 25-30 mA at 2.1-2.4 kV. Another synthesis involves mixing O2 and F2 in a stainless steel vessel cooled to −196°C, then exposing the elements to 3 MeV bremsstrahlung for several hours.
The structure of dioxygen difluoride resembles that of hydrogen peroxide, H2O2, in its large dihedral angle, which approaches 90°. The O−O bond is particularly short, remarkably close to the 120.7 pm distance for the O=O double bond in dioxygen, O2.
- N. N. Greenwood, A. Earnshaw, Chemistry of the Elements, Elsevier Butterworth-Heinemann, Oxford, UK, 1997.
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