Perbromate

Perhalates. Whereas silver perchlorate [7783-93-9] AgClO, and silver periodate [15606-77-6] AglO, are well known, silver perbromate [54494-97-2] AgBrO, has more recendy been described (18). Silver perchlorate is prepared from silver oxide and perchloric acid, or by treating silver sulfate with barium perchlorate. Silver perchlorate is one of the few silver salts that is appreciably soluble in organic solvents such as glycerol, toluene, and chlorobenzene. 

The structure has recently been shown by EXAFS to be bromine perbromate BrOBrOs with Br -0 186.2pm, Br -0 160.5 pm and angle BrOBr 110 3° d °) (cf. CIOCIO3 and Br0C103). Br0Br03 is thermally unstable above —40°C and decomposes violently to the elements at 0°C slower warming yields B1O2 (see above). Alkaline hydrolysis leads to disproportionation ... 

The quest for perbromic acid and perbromates and the various reasons adduced for their apparent non-existence make fascinating and salutary reading. " The esoteric radiochemical synthesis of Br04 in 1968 using the /3-decay of radioactive Se, whilst not providing a viable route to macroscopic quantities of perbromate. 

This stimulated the search for a chemical synthesis. Electrolytic oxidation of aqueous LiBrOs produced a 1% yield of perbromate, but the first isolation of a solid perbromate salt (RbBr04) was achieved by oxidation of BrOs with aqueous XeF2 ... 

Per-aciditat, /. superaeidity. -ameisensaure, /. performic (peroxyformie) acid, -benzoe-s ure, /. perbenzoic (peroxybenzoic) acid, -borsaure, /. perboric acid, -bromsiure, /. perbromic acid, -buttersaure, /. perbutyrie (peroxybutyric) acid. 

The rigorous temperature of these procedures can be avoided when 5-bromo-5 -(bromomcth-yl)dipyrrylmethene hydrobromides 12 a, 5-bromo-5 -(bromomethyl)dipyrrylmethene perbrom-ides 12b or a mixture of both are used, instead of 5-bromo-5 -methyldipyrrylmethene hydrobromides 6. These compounds 12 can be cyclodimerized by heating in formic acid to produce porphyrins. 

Only a few perbromates have so far been prepared [844] the stability of Br04 is about the same [851] as C104 and I04. KBr04 decomposes (548—553 K) exothermally to KBr03 which is stable [852]. Potassium metaperiodate decomposes [853] (529—561 K)... 

Chlorine, bromine, and iodine each form four different oxoanions that are distinguished by prefixes and suffixes. The nomenclature of these ions is illustrated for bromine, but it applies to chlorine and iodine as well BrO, hypohromite Br02, bromzte Br03, bromate and Br04, perbromate. 

C03-0067. Write chemical formulas for these compounds (a) sodium sulfate (b) potassium sulfide (c) potassium dihydrogen phosphate (d) cobalt(II) fluoride tetrahydrate (e) lead(IV) oxide (Q sodium hydrogen carbonate and (g) lithium perbromate. 

Write formulas for each of the following compounds (a) sodium bromide, (b) sodium bromate, (c) sodium bromite, (d) sodium hypobromite, and (e) sodium perbromate. 

The solid produced at —5°C by interaction of bromine and ozone is only stable at —80°C or in presence of ozone, and decomposition may be violently explosive in presence of trace impurities [1], The structure may be the dimeric bromyl perbromate, analogous to Cl206 [2],... 

The oxidation of alkaline bromate by fluorine to perbromate is not smooth and small explosions may occur in the vapour above the solution. The reaction should not be run unattended. 

Perbromic acid was first prepared in 1969 in a very unusual way that made use of the conversion of... 

Potassium pentafluoroaluminate monohydrate, 2 371 Potassium perbromate, 4 335 Potassium perchlorate, 18 277 Potassium permanganate, 9 635-636 crystallographic studies on, 15 601 as a detoxicant, 15 621 decomposition of, 15 597 as an ignitable waste, 15 615 industrial-scale production of, 15 606 manufacture of, 15 601-606 for purifying carbon dioxide streams, 4 815... 

Sodium perborate trihydrate in detergent formulations, 8 419 Sodium perbromate, 4 335 Sodium percarbonate, 28 413 Sodium perchlorate, 6 133... 

Tetrafluoroammonium hexafluoromanganate, 4384 Tetrafluoroammonium hexafluoronickelate, 4385 Tetrafluoroammonium octafluoroxenate, 4386 Tetrafluoroammonium perbromate, 0242 Tetrafluoroammonium perchlorate, 3986 Tetrafluoroammonium tetrafluoroborate, 0133 Tetrafluorodiaziridine, 0351 f Tetrafluorohydrazine, 4345... 

Though metal perbromates and periodates are known (but not perfluorates), the perchlorates have most frequently been involved in hazardous incidents over a long period. These usually stable salts are powerful oxidants and contact with combustible materials or reducants must be under controlled conditions. A severe restriction on the use of metal perchlorates in laboratory work has been recommended [1], Attention has been drawn, on the basis of experience with cobalt(II) perchlorate, to the possibility of stable hydrated metal perchlorates being converted by unintentional dehydration to unstable (endothermic) lower hydrates capable of explosive decomposition in absence of impurities. Great care to avoid dehydration (or desolvation) is urged [2],... 

Oxidation of [Fe(phen)3] + by concentrated nitric acid is autocatalytic. " T e hen)3] + reacts with bromate by rate-determining oxidation at high bromate concentration, [Fe(bipy)3] + and ligand-substituted [Fe(phen)3] + cations react with perbromate by rate-limiting dissocia-587 Reactions of [Fe(diimine)3] + with peroxodiphosphate also involve rate-limiting dissocia-... 

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