Chlorite, iodine oxidation

C) Chlorite-iodine species-reductant. Several subclasses may be distinguished within this category according to the oxidation number of the iodine species involved ... 

TELLURIUM (13494-80-9) Finely divided powder or dust may be flammable and explosive. Violent reaction with strong oxidizers, bromine pentafluoride, halogens, interhalogens, iodine pentafluoride, hexalithium disilicide, lithium silicide, nitrosyl fluoride, oxygen difluoride, sodium peroxide, sulfur, zinc. Incompatible with cadmium, cesium, hafnium, strong bases, chemically active metals, iodic acid, iodine oxide, lead chlorite, lead oxide, mercury oxides, nitric acid, peroxyformic acid, platinum, silver bromate/iodate/ fluoride, nitryl fluoride, sodium nitrate. 

Chlorite ion oxidizes iodine to iodate, a well-known clock reaction, equation (25). The proposed mechanism postulates the intermediate ICIO2,... 

Operated in a CSTR, the CIMA reaction produces, as a function of iodide or chlorite feed concentrations, bistability between an iodine reduced state (high iodine, high iodide concentration) and an iodine oxidized state (low iodide concentration) at relatively low malonic acid feed concentration. Sustained oscillations are produced at higher concentration [14,59]. Using starch as iodine color indicator, the reduced state colors daric blue while the oxidized state is clear or pale yellow. 

Identify the oxidation number of the halogen atoms in (a) iodine heptafluoride (b) sodium periodate (c) hypobromous acid (d) sodium chlorite. 

Iodine dioxide trifluoride, 4328 Iodine(V) oxide, 4622 Iodine(VII) oxide, 4623 Iridium hexafluoride, 4356 Lead chromate, 4237 Lead(II) nitrate, 4744 Lead(II) oxide, 4818 Lead(IV) oxide, 4828 Lithium chlorite, 4014 Magnesium nitrate, 4688 Magnesium nitrite, 4687 Magnesium permanganate, 4686... 

The methods commonly used for preparation of disodium dihydrogen hypophosphate depend upon the oxidation of yellow or red phosphorus. Yellow phosphorus may be oxidized by air1 or by copper(II) nitrate.2,3 Red phosphorus may be oxidized by chlorite,4 hypochlorite,5,6 alkaline permanganate,7 hydrogen peroxide,7 or iodine.8 The phosphorus (III) halides, upon hydrolysis and treatment with iodine, yield some hypophosphate.9-11 Electrolytic oxidation of a phosphide of copper, nickel, or silver3 has also been used. 

As an aid to understanding the mechanism of oxidation of aldoses by alkaline iodine,126,127 bromine,128 and acidified sodium chlorite,129... 

Hydrolysis of the 1,3-oxathiane moiety has been accomplished under mild conditions (0°C, 5 min) by the use of N-Chlorosuccinimide-Silver(l) Nitrate. This oxidative hydrolysis produces a-hydroxy aldehydes in good yields and, in addition, two diastereomeric sultines (19) (eq 8). The use of Iodine-for the oxidative hydrolysis of 1,3-oxathianes has also recently been reported. The tertiary a-hydroxy aldehydes are easily oxidized directly to the acids (Sodium Chlorite) or methyl esters (MeOH, I2, KOH) or are conveniently reduced to the diols by direct reduction of the hydrolysis mixture with Sodium Borohydride. The secondary a-hydroxy aldehydes could likewise be reduced to the glycols without racemization however, oxidation required pro-... 

Other alternatives for the oxidant for stoichiometric oxidations include the use of a selenoxide [99], including a photochemical oxidation of catalytic selenium [100], iodine [101], sodium chlorite [102], hypochlorite [103], and electrochemical methods [101,104]. Even air can be used as the oxidant [99,100], but care has to be taken with regard to the choice of solvent as cleavage of the product 1,2-diol can occur, especially when the alkene has an aryl substituent [53, 105, 106]. 

Oxidation of an aldehyde group to a carboxyl group has often been used for identification of the compounds. As far as can be judged from the results, such oxidations, using chromium trioxide/acetic acid, bromine-water, - peroxy acids, - or chlorite, have not been accompanied by any important side-reactions. Hypoiodite titration, using the iodine in sodium bicarbonate-sodium carbonate procedure, has sometimes been used, giving almost stoichiometric aldehyde determinations. - - Reduction by the Meerwein-Ponndorf reaction, with borohydride - - ... 

TIN or TIN POWDER (7440-31-5) Sn Finely divided material is combustible and forms explosive mixture with air [autoignition temp (dust cloud) 1166°F/630°C]. Contact with moisture in 911 forms tin dioxide. A reducing agent the powder is very reactive. Violent reaction with strong acids, strong oxidizers, ammonium perchlorate, ammonium nitrate, bis-o-azido benzoyl peroxide, bromates, bromine, bromine pentafluoride, bromine trifluoride, bromine azide, cadmium, carbon tetrachloride + water, chlorine, chlorine monofluoride, chlorine nitrate, chlorine pentafluoride, chlorites, copper(II) nitrate, dimethylarsinic acid, fluorine, hydriodic acid, iodine heptafluoride, nitrosyl fluoride, oxygen difluoride, perchlorates, perchloroethylene, potassium dioxide, phosphorus pentoxide, sulfur, sulfur dichloride, turpentine (fire or explosion). 

BENSULFOID (7704-34-9) Combustible solid (flash point 405°F/207°C). Finely divided dry materia forms explosive mixture with air. The vapor reacts violently with lithium carbide. Reacts violently with many substances, including strong oxidizers, aluminum powders, boron, bromine pentafluoride, bromine trifluoride, calcium hypochlorite, carbides, cesium, chlorates, chlorine dioxide, chlorine trifluoride, chromic acid, chromyl chloride, dichlorine oxide, diethylzinc, fluorine, halogen compounds, hexalithium disilicide, lampblack, lead chlorite, lead dioxide, lithium, powdered nickel, nickel catalysis, red phosphorus, phosphorus trioxide, potassium, potassium chlorite, potassium iodate, potassium peroxoferrate, rubidium acetylide, ruthenium tetraoxide, sodium, sodium chlorite, sodium peroxide, tin, uranium, zinc, zinc(II) nitrate, hexahydrate. Forms heat-, friction-, impact-, and shock-sensitive explosive or pyrophoric mixtures with ammonia, ammonium nitrate, barium bromate, bromates, calcium carbide, charcoal, hydrocarbons, iodates, iodine pentafluoride, iodine penloxide, iron, lead chromate, mercurous oxide, mercury nitrate, mercury oxide, nitryl fluoride, nitrogen dioxide, inorganic perchlorates, potassium bromate, potassium nitride, potassium perchlorate, silver nitrate, sodium hydride, sulfur dichloride. Incompatible with barium carbide, calcium, calcium carbide, calcium phosphide, chromates, chromic acid, chromic... 

Halobenziodoxoles l-Chloro-l,2-benziodoxol-3-(l//)-one (88, 2X = O, Y = Cl) can be easily prepared by direct chlorination of 2-iodobenzoic acid [233], or by the oxidation of 2-iodobenzoic acid with sodium chlorite (NaC102) in aqueous hydrochloric acid media [267]. The original X-ray single-crystal analysis of l-chloro-l,2-benziodoxol-3-(l//)-one reported in 1976 was relatively imprecise [268]. More recently, Koser and coworkers reported the single-crystal X-ray structure of a 1 1 complex of l-chloro-1,2-benziodoxol-3-(l/7)-one and tetra-n-butylammonium chloride [262], The primary bond distances at iodine in this compound are consistent with expectations for a X -iodane. In particular, the I—Cl and I—O bond distances of 2.454 and 2.145 A, respectively, are greater than the sums of the appropriate covalent radii and reflect the... 

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