Perbromate

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Ion

title: "Perbromate" type: doc version: 1 created: 2026-02-28 author: "Wikipedia contributors" status: active scope: public tags: ["perbromates"] description: "Ion" topic_path: "general/perbromates" source: "https://en.wikipedia.org/wiki/Perbromate" license: "CC BY-SA 4.0" wikipedia_page_id: 0 wikipedia_revision_id: 0

::summary Ion ::

|ImageFile=Perbromate-3D-vdW.png |ImageCaption=Space-filling model of the perbromate anion, |Section1={{Chembox Identifiers | CASNo = 16474-32-1 | CASNo_Ref = | ChEBI = 29246 | ChemSpiderID = 4574125 | PubChem = 5460630 | StdInChI=1S/BrHO4/c2-1(3,4)5/h(H,2,3,4,5)/p-1 | StdInChIKey = LLYCMZGLHLKPPU-UHFFFAOYSA-M | SMILES = [O-]Br(=O)(=O)=O |Section2={{Chembox Properties | Formula_Charge=− | Br=1|O=4 |Section8={{Chembox Related |OtherCompounds=bromide hypobromite bromite bromate

In chemistry, the perbromate ion is the anion with the chemical formula . It is an oxyanion of bromine, the conjugate base of perbromic acid, in which bromine has the oxidation state +7.{{Cite book | title = Inorganic chemistry | author1 = Egon Wiberg | author2 = Nils Wiberg | author3 = Arnold Frederick Holleman | publisher = Academic Press | year = 2001 | isbn = 0-12-352651-5 | page = 439

The term perbromate also refers to a compound that contains the anion or the functional group.

The perbromate ion is a strong oxidizing agent. The reduction potential for the / couple is +0.68 V at pH 14. This is comparable to selenite's reduction potential.

Synthesis

Attempted syntheses of perbromates were unsuccessful until 1968, when it was finally obtained by the beta decay of selenium-83 in a selenate salt by chemist Evan H. Appelman:

: → + β−

Subsequently, it was successfully synthesized again by the electrolysis of , although only in low yield. | doi = 10.1021/ja01009a040 | title = Synthesis of perbromates | year = 1968 | last1 = Appelman | first1 = E. H. | journal = Journal of the American Chemical Society | volume = 90 | issue = 7 | pages = 1900–1901 | title = Introduction to modern inorganic chemistry | author1 = Kenneth Malcolm Mackay | author2 = W. Henderson | editor = Rosemary Ann Mackay | edition = 6th | publisher = CRC Press | year = 2002 | isbn = 0-7487-6420-8 | page = 488

One effective method of producing perbromate is by the oxidation of bromate with fluorine under alkaline conditions:{{Cite book | title = Main group chemistry (Volume 3 of Tutorial chemistry texts) | author = W. Henderson | publisher = Royal Society of Chemistry | year = 2000 | isbn = 0-85404-617-8 | pages = 136–137

: + + 2 → + 2 +

This synthesis is much easier to perform on a large scale than the electrolysis route or oxidation by xenon difluoride.

In 2011 a new, more effective synthesis was discovered: perbromate ions were formed through the reaction of hypobromite and bromate ions in an alkaline sodium hypobromite solution. The reaction (and its perchlorate analogue) occurs naturally, but very slowly, requiring several days to complete. |first1=Aleksey N.|last1=Pisarenko|first2=Robert |last2=Young|first3=Oscar |last3=Quiñones|first4=Brett |last4=J. Vanderford|first5=Douglas |last5=B. Mawhinney |title=Two New Methods of Synthesis for the Perbromate Ion: Chemistry and Determination by LC-MS/MS| journal = Inorg. Chem.|year=2011|volume=50|issue=18|pages=8691–8693|doi=10.1021/ic201329q |pmid=21780765

References

References

  1. (1973). "Nonexistent compounds. Two case histories". Accounts of Chemical Research.
  2. Kurt H. Stern. (2001). "High temperature properties and thermal decomposition of inorganic salts with oxyanions". CRC Press.
  3. (2001). "Inorganic chemistry". Academic Press.
  4. (1969). "Perbromic acid and perbromates: synthesis and some properties". Inorg. Chem..

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perbromates