Perbromate Ion Research Articles

ChemInform Abstract: Two New Methods of Synthesis for the Perbromate Ion: Chemistry and Determination by LC‐MS/MS.

AbstractThe formation of perbromate ions by reactions of hypobromite and bromate ions in an alkaline sodium hypobromite solution is demonstrated by liquid chromatography tandem mass spectrometry.

Two New Methods of Synthesis for the Perbromate Ion: Chemistry and Determination by LC-MS/MS

Historically, the synthesis of perbromate ion through conventional oxidation routes has proven elusive. Herein, we report perbromate ion formation through the reaction of hypobromite and bromate ions in an alkaline sodium hypobromite solution. Formation was established via LC-MS/MS analysis of the bromate and perbromate ions in the reaction solutions over a 13-day period. Furthermore, it was discovered that the perbromate ion was also formed as a result of the electrospray ionization process. Selective reduction of the bromate ion prior to analysis was used to confirm the two formation pathways.

Mechanism of Reaction of the Hydrated Electron with Ozone, Perbromate, and Other Strongly Oxidizing Inorganic Oxocompounds

A model is proposed for the mechanism of reaction of the hydrated electron with strongly oxidizing inorganic oxocompounds, according to which such reactions comprise three steps: (1) a primary split-off of O- occurring immediately upon the transfer of the electron to the oxocompound, (2) after which O- becomes fully solvated, acquiring properties as in the bulk phase, and (3) finally, the solvated O- either escapes from the cage or forms an electron adduct by reacting back within the cage with its partner. The model is based on studies of the photochemistry of aqueous solution of the oxoanions O3- and ClO3- (Walhaut, P. K.; Silva, C.; Barbara, P. F. J. Phys. Chem. 1996, 100, 5188. Klaning, U. K.; Sehested, K. J. Phys. Chem. 1991, 95, 740.), which suggest that solvation of the photoproduct O- precedes cage-back reactions. Measurements of the reactions of the hydrated electron with the perbromate ion and the periodate ion and of the reactions of O- with the bromate and iodate ion support the model by verif...

Lithium Perbromate Monohydrate at 296 and 173 K

Lithium tetraoxobromate(1-) monohydrate, LiBrO4.-H2O, whose perchlorate analog has not yet been described, is found to be isomorphic with NaBrO4.H2O and NaClO4.H2O. Each of the two inequivalent Li ions is coordinated by six O atoms, thus forming distorted octahedra, each of which has three inequivalent Li-O distances. At room temperature, the average Li(1)-O and Li(2)-O distances are 2.150 and 2.164 A, respectively. The perbromate ion displays very nearly regular tetrahedral geometry, although it is not subject to symmetry constraints. At 296 K the average observed Br-O distance is 1.610 (4) A and the average O-Br-O angle is 109.5 (6) degrees, while at 173 K the corresponding values are 1.613 (4) A and 109.5 (7) degrees. The perbromate ion shows rigid-body behavior but the lithium coordination polyhedra do not. At 296 K, the average rigid-body corrected Br-O distance in the perbromate ion is 1.624 (3) A, in excellent agreement with the corresponding value reported for NaBrO4.H2O. Refinement of the two inequivalent H atoms allowed detailed analysis of the hydrogen bonding, which is more extensive than in NaBrO4.H2O or in NaClO4.H2O. The average observed B values for the H atoms [2.9 (3) A2 at 296 K and 2.8 (3) A2 at 173 K] are sufficiently small to suggest that dynamic disordering of the H atoms (determined by magnetic resonance methods for NaClO4.H2O) is not significant in the title salt.

Comparative multinuclear (35Cl,79Br,81Br,127I and17O) magnetic resonance study of the perhalate anions XO4−(X  Cl, Br or I) in acetonitrile solution

AbstractThe NMR spectra (35Cl,79Br,81Br,127I and17O) of the tetrahedral perhalate anions XO4−(X  Cl, Br and I) were compared for the first time in acetonitrile solution, a medium in which the resonances are relatively sharp and in which no oxygen exchange occurs. Relaxation studies of the quadrupolar nuclei in these solutions at 24°C are reported and show that excellent spectra may be obtained at 0.1 M concentration; thus the observation of separate resonances for Cl16O4−and Cl18O16O3−represents the first reported instance of a35Cl secondary isotopic shift [1Δ35Cl(18.16O) = ‐0.090 ppm]. Enrichment with17O of all three ions was carried out and the1J(127I,17O) coupling constant (489 Hz) has been observed for the first time. The chemical shifts and coupling constants are discussed, especially in connection with the anomalous properties of the perbromate ion. Halogen chemical shifts for BrO3F, IF7and IF6+AsF6−are reported for the first time.

Roles for paramagnetic substances in MRI: contrast agents, molecular amplifiers, and indicators for redox and pH mapping

A “molecular amplifier” is a substance which at high dilution can significantly influence the magnetic resonance (MR) properties of water; its “gain” can be controlled by varying either its chemical or magnetic properties. If the “gain” of that amplifier is sensitive to the chemical potential of its molecular environment, then it can be used as an “MRI-active chemical indicator.” Three examples are described: (a) the use of the ethylenediaminetetraacetic acid-copper(II) complex to map the spatial distribution of pH; (b) the use of Fe(II)/Fe(III) ions to map redox potential and thereby reducing species such as ascorbic acid or oxidants such as perbromate ion; (c) similar use of a stable nitroxide free radical to map reducing agents. The mass transport diffusion of those species can be visualized in hydrocolloid gels and in articular cartilage by MR imaging and the diffusion coefficients measured quantitatively using the null-point MR imaging method.

Structure of sodium perbromate monohydrate.

NaBrO4.H2O, Mr = 184.90, monoclinic, C2/c, a = 15.7575 (19), b = 5.7373 (15), c = 11.3390 (19) A, beta = 111.193 (10)degrees, V = 955.8 (3) A3, Z = 8, Dx = 2.570 g cm-3, lambda(Mo K alpha) = 0.71073 A, mu = 85.2 cm-1, F(000) = 704, T = 296 K, R = 0.039 for 1137 unique reflections having I greater than sigma I. In this structure, there are two inequivalent Na ions, each coordinated by six O atoms. In each of the two types of distorted octahedra, there are three inequivalent Na--O distances; the average Na(1)--O and Na(2)--O distances are 2.379 (10) and 2.405 (23) A, respectively. The perbromate ion in this structure displays very nearly regular tetrahedral geometry, although it is subject to no symmetry constraints; the average observed Br--O distance is 1.601 (4) A, while the average observed O--Br--O angle is 109.5 (9)degrees. These values agree well with previously reported values. The perbromate ion, but neither of the sodium coordination polyhedra, shows rigid-body behavior. The average rigid-body corrected Br--O distance in the perbromate ion is 1.624 (3) A. Refinement of the two inequivalent H atoms permitted detailed analysis of the hydrogen bonding, which is slightly different from that reported for the isomorphic sodium perchlorate monohydrate. Dynamic disordering of the H atoms as detailed by magnetic resonance methods for sodium perchlorate monohydrate is not clearly indicated in our X-ray study of sodium perbromate monohydrate.

Structure of nickel(II) perbromate hexahydrate at 296 K

Ni(BrO4)2.6H2O, Mr = 454.61, trigonal, P3, a = 7.874 (1), c = 5.423 (2) A, V = 291.2 (1) A3, Z = 1, D chi = 2.59 g cm-3, lambda(Mo K alpha) = 0.71069 A, mu = 85.36 cm-1, F(000) = 222, T = 296 K, R = 0.029 for 457 unique reflections having I greater than 0. The room-temperature structure is very similar to that reported previously for a sample at 169 K. The water O atoms form a very slightly distorted octahedron about nickel while the perbromate-ion geometry is virtually regular tetrahedral. Both the coordination polyhedron and the perbromate ion were tested and found to behave as rigid bodies. Corrected for rigid-body motion, the Ni--O(2) distance is 2.064 (2) A and the mean Br--O distance in the perbromate ion is 1.629 (3) A. A detailed account of the hydrogen bonding is presented. The structure previously determined at 169 K is most probably not the stable structure at that temperature.

ChemInform Abstract: ELECTRON‐TRANSFER REACTIONS BETWEEN THE PERBROMATE ION AND IRON(II) COMPLEXES OF 2,2′‐BIPYRIDINE AND SUBSTITUTED 1,10‐PHENANTHROLINES

Chemischer InformationsdienstVolume 13, Issue 49 Organoelement Compounds ChemInform Abstract: ELECTRON-TRANSFER REACTIONS BETWEEN THE PERBROMATE ION AND IRON(II) COMPLEXES OF 2,2′-BIPYRIDINE AND SUBSTITUTED 1,10-PHENANTHROLINES A. M. KJAER, A. M. KJAERSearch for more papers by this authorJ. ULSTRUP, J. ULSTRUPSearch for more papers by this author A. M. KJAER, A. M. KJAERSearch for more papers by this authorJ. ULSTRUP, J. ULSTRUPSearch for more papers by this author First published: December 7, 1982 https://doi.org/10.1002/chin.198249280AboutPDF ToolsRequest permissionExport citationAdd to favoritesTrack citation ShareShare Give accessShare full text accessShare full-text accessPlease review our Terms and Conditions of Use and check box below to share full-text version of article.I have read and accept the Wiley Online Library Terms and Conditions of UseShareable LinkUse the link below to share a full-text version of this article with your friends and colleagues. Learn more.Copy URL Share a linkShare onFacebookTwitterLinked InRedditWechat No abstract is available for this article. Volume13, Issue49December 7, 1982 RelatedInformation

Electron-transfer reactions between the perbromate ion and iron(II) complexes of 2,2'-bipyridine and substituted 1,10-phenanthrolines

Electron-transfer reactions between the perbromate ion and iron(II) complexes of 2,2'-bipyridine and substituted 1,10-phenanthrolines

Some reactions of the perbromate ion in aqueous solution

ADVERTISEMENT RETURN TO ISSUEPREVArticleNEXTSome reactions of the perbromate ion in aqueous solutionEvan H. Appelman, Ulrik K. Klaening, and Richard C. ThompsonCite this: J. Am. Chem. Soc. 1979, 101, 4, 929–934Publication Date (Print):February 1, 1979Publication History Published online1 May 2002Published inissue 1 February 1979https://doi.org/10.1021/ja00498a022RIGHTS & PERMISSIONSArticle Views98Altmetric-Citations7LEARN ABOUT THESE METRICSArticle Views are the COUNTER-compliant sum of full text article downloads since November 2008 (both PDF and HTML) across all institutions and individuals. These metrics are regularly updated to reflect usage leading up to the last few days.Citations are the number of other articles citing this article, calculated by Crossref and updated daily. Find more information about Crossref citation counts.The Altmetric Attention Score is a quantitative measure of the attention that a research article has received online. Clicking on the donut icon will load a page at altmetric.com with additional details about the score and the social media presence for the given article. Find more information on the Altmetric Attention Score and how the score is calculated. Share Add toView InAdd Full Text with ReferenceAdd Description ExportRISCitationCitation and abstractCitation and referencesMore Options Share onFacebookTwitterWechatLinked InReddit PDF (758 KB) Get e-Alerts Get e-Alerts

A Clean, Sensitive and Lasting New Spot Test for Paper and Thin-Layer Chromatograms of Perbromate Ion

Abstract Benzidine in dilute acetic acid reacts with perbromate ion to give initially a blue colored spot which, on further heating, changes to a dark bluish-grey spot. The latter serves as a sensitive clean test for the detection of perbromate ion on paper and thin-layer chromatograms and electrophoregrams. The reagent can also be used to detect bromate, iodate and periodate ions as well as free halogens.

The analytical reactions of the perbromate ion : II. Spot tests, partition and ion-exchange thin-layer chromatography

Spot tests and partition and anion-exchange thin-layer chromatography data for the perbromate ion are given. The sequence of the perhalo acids in the various systems is discussed.

Raman intensity of the A1 line and bond order of the perbromate ion

Raman intensity of the A1 line and bond order of the perbromate ion

The chromatography and electrophoresis of the perbromate ion

The chromatography and electrophoresis of the perbromate ion

Microanalytical method for determination of perbromate ion in the presence of macro amounts of other bromine anions

Microanalytical method for determination of perbromate ion in the presence of macro amounts of other bromine anions

Heats of formation of potassium perbromate and of the perbromate ion, and the potential of the BrO3--BrO4- electrode

ADVERTISEMENT RETURN TO ISSUEPREVArticleNEXTHeats of formation of potassium perbromate and of the perbromate ion, and the potential of the BrO3--BrO4- electrodeJohn Robert Brand and Steven A. BunckCite this: J. Am. Chem. Soc. 1969, 91, 23, 6500–6502Publication Date (Print):November 1, 1969Publication History Published online1 May 2002Published inissue 1 November 1969https://doi.org/10.1021/ja01051a060RIGHTS & PERMISSIONSArticle Views58Altmetric-Citations6LEARN ABOUT THESE METRICSArticle Views are the COUNTER-compliant sum of full text article downloads since November 2008 (both PDF and HTML) across all institutions and individuals. These metrics are regularly updated to reflect usage leading up to the last few days.Citations are the number of other articles citing this article, calculated by Crossref and updated daily. Find more information about Crossref citation counts.The Altmetric Attention Score is a quantitative measure of the attention that a research article has received online. Clicking on the donut icon will load a page at altmetric.com with additional details about the score and the social media presence for the given article. Find more information on the Altmetric Attention Score and how the score is calculated. Share Add toView InAdd Full Text with ReferenceAdd Description ExportRISCitationCitation and abstractCitation and referencesMore Options Share onFacebookTwitterWechatLinked InReddit PDF (394 KB) Get e-Alerts Get e-Alerts