Aspects of Homogeneous Catalysis: A Series of Advances - download pdf or read online

By James E. Lyons (auth.), Renato Ugo (eds.)

ISBN-10: 9401011990

ISBN-13: 9789401011990

ISBN-10: 9401012016

ISBN-13: 9789401012010

In fresh years, the liquid part oxidation of natural substrates utilizing transition steel compounds as catalysts has turn into a ecocnomic technique of acquiring industrially very important chemical compounds. thousands of lots of important petrochemicals are produced during this demeanour each year [1]. ordinary examples of such procedures are the creation of vinyl acetate or acetaldehyde through the Wacker approach, equations (1) and (2); the Mid­ Century method for the oxidation of methyl aromatics, akin to p-xylene to tereph­ thalic acid, equation (3); and the construction of propylene oxide from propylene utilizing alkyl hydroperoxides, equation (4). PdCI , CuCI 2 2 (1) CH2 = CH2 + 0.5 O2 -H zero ~ CH3CHO 2 (2) Co(OAcjz ~ (3) (4) nearly all of liquid part transition steel catalyzed oxidations of natural compounds fall into those 3 vast different types: (a) loose radical autoxidation reactions, (b) reactions related to nucleophilic assault on coordinated substrate equivalent to the Wacker method, or (c) steel catalyzed reactions of natural substrates with hydroperoxides. of those 3 sessions of oxidations merely the 1st represents the particular interplay of dioxygen with an natural substrate. The functionality of oxygen within the Wacker procedure is just to re-oxidize the catalyst after each one cycle [2].

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However, the stoichiometry of one step and the relative rates of several other steps appear to be somewhat different. The observed rate laws are quite different from those of the platinum complex. The rate equations for the proposed mechanism are shown in equation (71) for the dioxygen complex and equation (72) for the carbonyl complex (RU02 = [Ru(NCS)(NOXPPh3M02)]; RuCO = [Ru(NCSXCOXNO)(pPh 3)2]). 63 x 10- 2 1mol-1. In contrast to the observations of Halpern and coworkers who found that the rate of triphenylphosphine oxidation catalyzed by [Pt(02XPPh 3h] depended linearly on [PPh 3] , the above two rate equations require that the reciprocal of the rate depends on [Ph 3P] -1 .

By the use of optical absorption spectroscopy it has been shown that the predominant species present in a benzene solution of [Pt(PPh 3)41 is [Pt(PPh 3)31, equation (60). (60) Subsequent dissociation to [Pt(PPh 3h 1 and triphenylphosphine or recombination with triphenylphosphine occur to only a minor extent over a rather wide range of phosphine concentrations. The complex, [Pt(PPh 3)31, has been shown to add molecular oxygen with expulsion of triphenylphosphine to give a dioxygen complex, equation (61).

8. 1. Complexes of Ni, Pd and Pt as catalysts A large number of transition metal complexes have been found to catalyze the oxidation of organic phosphines to phosphine oxides. Wilke, Schott and Heimbach [85] showed that complexes of the type: [M(PPh 3)4] catalyze the oxidation of triphenylphosphine to triphenylphosphine oxide in toluene solution, equation (59). 2PPh 3 + O2 [M(PPh 3 l 41) 20PPh 3 (59) When Mis Ni reaction occurs at temperatures above - 35 °c whereas the corresponding Pd and Pt complexes show catalytic activity when warmed at temperatures above 90°C.

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Aspects of Homogeneous Catalysis: A Series of Advances Volume 3 by James E. Lyons (auth.), Renato Ugo (eds.)

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