Oxides of bromine
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The oxides of bromine are far less stable than their chlorine or iodine analogues. Of the seventeen binary species that have been described, none is stable at room temperature and pressure: the reality of many of these species is dubious.[1]
| Formula | Structure | Thermochemistry | Notes | |||||
|---|---|---|---|---|---|---|---|---|
| r(Br–O) | r(Br–Br) | r(O–O) | Ref. | ΔfH |
Ref. | |||
| BrO | ||||||||
| BrO2 | OBrO | |||||||
| BrO2 | BrOO | |||||||
| BrO3 | C3v | |||||||
| BrO4 | ||||||||
| Br2O | BrOBr | |||||||
| Br2O | BrBrO | |||||||
| Br2O2 | BrOOBr | |||||||
| Br2O3 | OBrOBrO | |||||||
| Br2O4 | BrOBrO3 | |||||||
| Br2O4 | O2BrBrO2 | |||||||
| Br2O4 | O2BrOBrO | |||||||
| Br2O5 | O2BrOBrO2 | |||||||
| Br2O6 | ||||||||
| Br2O7 | ||||||||
| Br2O3 | ||||||||
References
- ↑ Chase, Malcolm W. NIST–JANAF Thermochemical Tables for the Bromine Oxides. J. Phys. Chem. Ref. Data 1996, 25 (4), 1069–1111, <http://www.nist.gov/data/PDFfiles/jpcrd508.pdf>.
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