Bromine dioxide
{{redirect|BrO2|the oxyanion with the formula BrO{{su|b=2|p=−}}|Bromite}}
{{chembox
| Verifiedfields = changed
| Watchedfields = changed
| verifiedrevid = 428832706
| Name = Bromine dioxide
| ImageFile1 = Bromine-dioxide-radical-resonance-hybrid-2D.png
| ImageSize1 = 150px
| ImageName1 =
| ImageFile2 = Bromine-dioxide-MP2-CM-3D-balls.png
| ImageSize2 = 150px
| IUPACName = Bromine dioxide
| OtherNames =
| Section1 = {{Chembox Identifiers
| CASNo_Ref = {{cascite|correct|??}}
| CASNo = 21255-83-4
| RTECS =
| PubChem = 5460629
| ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}}
| ChemSpiderID = 4574124
| SMILES = O=Br=O
| InChI = 1/BrO2/c2-1-3
| InChIKey = SISAYUDTHCIGLM-UHFFFAOYAZ
| StdInChI_Ref = {{stdinchicite|changed|chemspider}}
| StdInChI = 1S/BrO2/c2-1-3
| StdInChIKey_Ref = {{stdinchicite|changed|chemspider}}
| StdInChIKey = SISAYUDTHCIGLM-UHFFFAOYSA-N
}}
| Section2 = {{Chembox Properties
| Formula = BrO2
{{Citation
| last1 = Perry
| first1 = Dale L.
| last2 = Phillips
| first2 = Sidney L.
| year = 1995
| title = Handbook of Inorganic Compounds
| publisher = CRC Press
| isbn = 0-8493-8671-3
| pages = 74
| url = https://books.google.com/books?id=0fT4wfhF1AsC&q=%22Bromine+dioxide%22&pg=PA74
| access-date = 17 March 2009
}}
| Appearance = unstable yellow crystals
| Density =
| Solubility =
| MeltingPt = decomposes around 0°C
{{Citation
| last = Lide
| first = David R.
| year = 1998
| title = Handbook of Chemistry and Physics
| edition = 87
| location = Boca Raton, Florida
| publisher = CRC Press
| isbn = 0-8493-0594-2
| pages = 447
}}
| BoilingPt =
}}
| Section3 = {{Chembox Structure
| MolShape =
| Coordination =
| CrystalStruct =
| Dipole =
}}
| Section7 = {{Chembox Hazards
| NFPA-H =
| NFPA-F =
| NFPA-R =
| FlashPt =
}}
| Section8 = {{Chembox Related
| OtherAnions = Bromine monoxide
Bromine trifluoride
Bromine pentafluoride
| OtherCations = Oxygen difluoride
Dichlorine monoxide
Chlorine dioxide
Iodine dioxide
}}
}}
Bromine dioxide is the chemical compound composed of bromine and oxygen with the formula BrO2. It forms unstable yellow to yellow-orange crystals. It was first isolated by R. Schwarz and M. Schmeißer in 1937 and is hypothesized to be important in the atmospheric reaction of bromine with ozone.{{cite journal|last1=Müller|first1=Holger S. P.|last2=Miller|first2=Charles E.|last3=Cohen|first3=Edward A.|title=The rotational spectrum and molecular properties of bromine dioxide, OBrO|journal=The Journal of Chemical Physics|volume=107|issue=20|year=1997|pages=8292|issn=0021-9606|doi=10.1063/1.475030|bibcode=1997JChPh.107.8292M }}
It is similar to chlorine dioxide, the dioxide of its halogen neighbor one period higher on the periodic table.{{cn|date=September 2023}}
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Reactions
Bromine dioxide is formed when an electric current is passed through a mixture of bromine and oxygen gases at low temperature and pressure.
{{Citation
| last =Arora
| first = M.G.
| year = 1997
| title = P-Block Elements
| location = New Delhi
| publisher = Anmol Publications
| isbn = 978-81-7488-563-0
| pages = 256
| url = https://books.google.com/books?id=QR3TCaKaykEC&q=%22Bromine+dioxide%22&pg=PA256
| access-date = 17 March 2009
}}
Bromine dioxide can also be formed by the treatment of bromine gas with ozone in trichlorofluoromethane at −50 °C.
When mixed with a base, bromine dioxide gives the bromide and bromate anions:
References
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{{bromine compounds}}
{{oxides}}
{{oxygen compounds}}
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{{DEFAULTSORT:Bromine Dioxide}}