| 词条 | Bromine dioxide |
| 释义 |
| 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 | MolarMass = 111.903 g/mol[1] | Appearance = unstable yellow crystals | Density = | Solubility = | MeltingPt = decomposes around 0°C[2] | BoilingPt = | Section3 = {{Chembox Structure | MolShape = | Coordination = | CrystalStruct = | Dipole = | Section7 = {{Chembox Hazards | NFPA-H = | NFPA-F = | NFPA-R = | EUClass = | RPhrases = | SPhrases = | 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[2] to yellow-orange[1] 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.[3] It is similar to chlorine dioxide, the dioxide of its halogen neighbor one period higher on the periodic table. ReactionsBromine dioxide is formed when an electric current is passed through a mixture of bromine and oxygen gases at low temperature and pressure.[4] Bromine dioxide can also be formed by the treatment of bromine gas with ozone in trichlorofluoromethane at −50 °C.[1] When mixed with a base, bromine dioxide gives the bromide and bromate anions:[4] 6 BrO2 + 6 NaOH → NaBr + 5 NaBrO3 + 3 H2O References1. ^1 2 {{Citation | last = Perry | first = Dale L. | author-link = | last2 = Phillips | first2 = Sidney L. | author2-link = | publication-date = | year = 1995 | title = Handbook of Inorganic Compounds | edition = | volume = | series = | publication-place = | place = | publisher = CRC Press | id = | isbn = 0-8493-8671-3 | doi = | oclc = | pages = 74 | url = https://books.google.com/books?id=0fT4wfhF1AsC&pg=PA74&dq=%22Bromine+dioxide%22 | accessdate = 17 March 2009}} {{bromine compounds}}{{oxygen compounds}}{{Use dmy dates|date=March 2018}}{{DEFAULTSORT:Bromine Dioxide}}{{inorganic-compound-stub}}2. ^1 {{Citation | last = Lide | first = David R. | author-link = | last2 = | first2 = | author2-link = | publication-date = | year = 1998 | title = Handbook of Chemistry and Physics | edition = 87 | volume = | series = | publication-place = Boca Raton, Florida | place = | publisher = CRC Press | id = | isbn = 0-8493-0594-2 | doi = | oclc = | pages = 447 | url = | accessdate =}} 3. ^{{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}} 4. ^1 {{Citation | last =Arora | first = M.G. | author-link = | last2 = | first2 = | author2-link = | publication-date = | year = 1997 | title = P-Block Elements | edition = | volume = | series = | publication-place = New Delhi | place = | publisher = Anmol Publications | id = | isbn = 978-81-7488-563-0 | doi = | oclc = | pages = 256 | url = https://books.google.com/books?id=QR3TCaKaykEC&pg=PA256&dq=%22Bromine+dioxide%22 | accessdate = 17 March 2009}} 2 : Bromine compounds|Oxides |
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