Oxidative activation hydroperoxide

Metal-Catalyzed Oxidation. Trace quantities of transition metal ions catalyze the decomposition of hydroperoxides to radical species and greatiy accelerate the rate of oxidation. Most effective are those metal ions that undergo one-electron transfer reactions, eg, copper, iron, cobalt, and manganese ions (9). The metal catalyst is an active hydroperoxide decomposer in both its higher and its lower oxidation states. In the overall reaction, two molecules of hydroperoxide decompose to peroxy and alkoxy radicals (eq. 5). 

Optically active hydroperoxides 244 were found285 to oxidize prochiral sulphides into the corresponding sulphoxides in higher optical yields (up to 27%) in comparison with those observed with peracids (equation 132). Moreover, the optical purity of the sulphoxides formed may be enhanced by addition of Ti(OPr-i)4. The oxidation of racemic 2-methyl-2,3-dihydrobenzothiophene 246 with these peroxides gave a mixture of cis and trans-sulphoxides 247 (equation 133). In all cases of the oxidation with the hydroperoxide alone the formation of the trans-isomer was strongly preferred and the e.e. value (up to 42%) of the cis-isomer was always higher than that of the trans-isomer. Moreover, the addition of Ti(OPr-i)4 furthermore promoted the selective formation of the frans-sulphoxide 247 and remarkably enhanced the e.e. value of both isomers. 

In the initial period the oxidation of hydrocarbon RH proceeds as a chain reaction with one limiting step of chain propagation, namely reaction R02 + RH. The rate of the reaction is determined only by the activity and the concentration of peroxyl radicals. As soon as the oxidation products (hydroperoxide, alcohol, ketone, etc.) accumulate, the peroxyl radicals react with these products. As a result, the peroxyl radicals formed from RH (R02 ) are replaced by other free radicals. Thus, the oxidation of hydrocarbon in the presence of produced and oxidized intermediates is performed in co-oxidation with complex composition of free radicals propagating the chain [4], A few examples are given below. 

Antioxidants possess the reducing activity and can be oxidized by hydroperoxide formed in the oxidizing substance [23,31,32,38,51]. This reaction produces an active radical... 

Sulfur(II)-containing compounds possess the reducing activity and react with hydroperoxides and peroxyl radicals [1-5]. They are employed as components of antioxidant additives to lubricants and polymers [30-35]. Denison and Condit [36] were the first to show that dialkyl sulfides are oxidized by hydroperoxides to sulfoxides and then to sulfones... 

Hydroperoxides play an important role as oxidants in organic synthesis [56-58]. Although several methods are available for the preparation of racemic hydroperoxides, no convenient method of a broad scope was until recently [59] known for the synthesis of optically active hydroperoxides. Such peroxides have potential as oxidants in the asymmetric oxidation of organic substrates, currently a subject of intensive investigations in synthetic organic chemistry [60, 61]. The application of lipoxygenase [62-65] and lipases [66,67] facilitated the preparation of optically active hydroperoxides by enzymes for the first time. 

Oxidation of phenols and aromatic amines using HRP is generally of little synthetic value, as oligomers and polymers are the main products (5, 260). Under certain conditions oxidative coupling of phenols or naphthols to give biaryls can be achieved, but with low selectivity (262). In contrast, HRP can catalyze a number of useful oxidative N-and 0-deaIkyIation reactions that are relatively difficult to carry out synthetically. This area has been described in detail by Meunier (263). A method for the preparation of optically active hydroperoxides using HRP C has been developed (264). Optically pure (S)-hydroperoxides... 

A different approach to the metal peroxo-mediated asymmetric oxidations of sulfides was proposed by Chmielewski and coworkers and more recently by Korb, Adam and coworkers based on the use of optically active hydroperoxides. First attempts to use... 

Horseradish peroxidase catalysed kinetic resolution of racemic secondary hydroperoxides has been described by Adam et al. [79]. The reaction yields (i )-hy-droperoxides up to ee>99% and (S)-alcohols up to ee>97%. Optically active hydroperoxides as potential stereoselective oxidants can be obtained by this process. 

The stabilization does not occur through a single process but a combination of all the above proposed processes and their combined effect is known as synergism when the cooperative action is greater than their individual effects [177] taken independently. The mechanism of synergism is unknown. The synergism [178] between UV absorbers (hydroxybenzotriazoles) and antioxidant [tris(3,5-di-with free radicals or oxidation products (hydroperoxide or peroxide) which may be formed even in the presence of ultra-violet stabilizers. 

The origin of the catalytic oxidative activity of the the Sn-siljcalites is not clear at the moment. It may be due to the reduction of isolated Sn " to Sn, which is then oxidised back with H2O2. Also, many hydroperoxides of tin have been known from the action of H2O2 upon solutions of Sn2+ and Sn4+. With our Sn-silicalites, however, there was no evidence for the dissolution of Sn under the reaction conditions as they have been regenerated after the reaction and reused several times without significant loss of catalytic activity. Surface tin hydroperoxides may be the active species but further detailed studies are required before possible mechanisms of oxidation involving Sn could be discussed. 

During the inhibited self-initiated autoxidation of methyl linoleate by a-Toc in solution, Niki and coworkers made the interesting observation that a-Toc acts as an antioxidant at low concentrations, but high concentrations (up to 18.3 mM) actually increased hydroperoxide formation due to a pro-oxidant effect. The pro-oxidant effect of a-Toc was observed earlier by Cillard and coworkers in aqueous micellar systems and they found that the presence of co-antioxidants such as cysteine, BHT, hydroquinone or ascor-byl palmitate inverted the reaction into antioxidant activity, apparently by reduction of a-To" to a-Toc . Liu and coworkers ° found that a mixture of linoleic acid and linoleate hydroperoxides and a-Toc in SDS micelles exhibited oxygen uptake after the addition of a-Toc. The typical ESR spectrum of the a-To" radical was observed from the mixture. They attributed the rapid oxidation to decomposition of linoleate hydroperoxides, resulting in the formation of linoleate oxy radicals which initiated reactions on the lipid in the high concentration of the micellar micro-environment. Niki and coworkers reported pro-oxidant activity of a-Toc when it was added with metal ions, Fe3+25i Qj. jjj (jjg oxidation of phosphatidyl choline liposomes. a-Toc was found... 

Scheme 1.70. Pro-oxidant activity of alkyl mercaptans (a) and both pro-oxidant and delayed antioxidant activity of diphenyl disulfides (b) during melt processing of polymer PH containing hydroperoxide groups POOH. After Scott (1993b).

The epoxidation using optically active hydroperoxide both as chiral source and oxidant has also been studied as an alternative approach to metal-mediated AE of allylic alcohols, but there is still much room for improvement in this approach [13]. 

Radicals NC H2 are formed intermediately and are oxidized via hydroperoxide 121 into the formate salt 122. The ROOH and radical attacks are more prone to thermal processes taking part in heat stabilizing activity of HAS. Mechanism involving 102 and excited CTC fits participation of NCH3 in the photo-oxidation mechanism [43,111]. 

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