A | B | C | D | E | F | G | H | CH | I | J | K | L | M | N | O | P | Q | R | S | T | U | V | W | X | Y | Z | 0 | 1 | 2 | 3 | 4 | 5 | 6 | 7 | 8 | 9
Names | |
---|---|
IUPAC name
Dibromine trioxide
| |
Other names
Bromine trioxide
Bromine bromate | |
Identifiers | |
3D model (JSmol)
|
|
ChemSpider | |
PubChem CID
|
|
| |
| |
Properties | |
Br2O3 | |
Molar mass | 207.806 g/mol |
Appearance | orange needles |
Melting point | decomposes around −40°C[1] |
Structure[2] | |
monoclinic | |
P21/c | |
a = 1186.6 pm, b = 762.9 pm, c = 869.3 pm α = 90°, β = 106.4°, γ = 90°
| |
Related compounds | |
Other anions
|
Bromine dioxide Bromine trifluoride Bromine pentafluoride |
Other cations
|
Oxygen difluoride Dichlorine monoxide Chlorine dioxide Iodine dioxide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa).
|
Dibromine trioxide is the chemical compound composed of bromine and oxygen with the formula Br2O3. It is an orange solid that is stable below −40 °C. It has the structure Br−O−BrO2 (bromine bromate).[3] It was discovered at 1993.[2] The bond angle of Br−O−Br is 111.7°, the bond angle of O−Br=O is 103.1°, and the bond angle of O=Br=O is 107.6°. The Br−OBrO2 bond length is 1.845Å, the O−BrO2 bond length is 1.855Å, and the Br=O bond length is 1.612Å.[4]
Reactions
Dibromine trioxide can be prepared by reacting a solution of bromine in dichloromethane with ozone at low temperatures.[3][5]
It disproportionates in alkali solutions to Br−
and BrO−
3.[5]
References
- ^ Perry, Dale L.; Phillips, Sidney L. (1995), Handbook of Inorganic Compounds, CRC Press, p. 255, ISBN 0-8493-8671-3, retrieved 2015-08-25
- ^ a b Kuschel, Raimund; Seppelt, Konrad (1993). "Brombromat Br2O3". Angewandte Chemie. 105 (11). Wiley: 1734–1735. doi:10.1002/ange.19931051141. ISSN 0044-8249.
- ^ a b Henderson, K. M. Mackay; R. A. Mackay; W. (2002). Introduction to modern inorganic chemistry (6th ed.). Cheltenham: Nelson Thornes. ISBN 9780748764204.
{{cite book}}
: CS1 maint: multiple names: authors list (link) - ^ Jansen, Martin; Kraft, Thorsten (1997). "The Structural Chemistry of Binary Halogen Oxides in the Solid State". Chemische Berichte. 130 (3). Wiley: 307–316. doi:10.1002/cber.19971300302. ISSN 0009-2940.
- ^ a b Wiberg, Egon (2001). Wiberg, Nils (ed.). Inorganic chemistry (1st ed.). San Diego, Calif.: Academic Press. p. 464. ISBN 9780123526519.
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