Cerium complexes, reaction with peroxides

Catalysis of the decomposition by several metal ions has been reported . The order in peroxomonosulphate was found to be one, except for reaction with cobalt(II) and cerium(IV) (both second-order in the sulphate) and manga-nese(II) (half-order). Formation of a complex with cerium(IV) and peroxomonosulphate has been both asserted and denied . Catalysis by copper(II) is not significant unless manganese is also added, at least in the presence of some hydrogen peroxide ... 

The e.s.r. spectra of oxovanadium ions in redox systems have been reported. The interaction of free-radicals generated using the reactions of cerium(iv) or ferrous ions with hydrogen peroxide with oxovanadium(v), produces a complex which decays in a first-order manner (k = 6-2 s at 22 °C) with the formation of vanadium(iv). The oxidation of phenetidines by bromate is catalysed by vanadium(v) and kinetic parameters involved in the interactions of various substrates with vanadium(v) have been correlated with electron configurations. The redox behaviour of oxo-3,5-disulphocatecholatovanadium(v) has been studied and the acidity dependence in the reaction with phenylethyl alcohol reported. In the... 

Hiatt et a/.34a-d studied the decomposition of solutions of tert-butyl hydroperoxide in chlorobenzene at 25°C in the presence of catalytic amounts of cobalt, iron, cerium, vanadium, and lead complexes. The time required for complete decomposition of the hydroperoxide varied from a few minutes for cobalt carboxylates to several days for lead naphthenate. The products consisted of approximately 86% tert-butyl alcohol, 12% di-fe/T-butyl peroxide, and 93% oxygen, and were independent of the catalysts. A radical-induced chain decomposition of the usual type,135 initiated by a redox decomposition of the hydroperoxide, was postulated to explain these results. When reactions were carried out in alkane solvents (RH), shorter kinetic chain lengths and lower yields of oxygen and di-te/T-butyl peroxide were observed due to competing hydrogen transfer of rm-butoxy radicals with the solvent. 

Alternatively, 5-allyl-2(5/f)-furanones can be obtained from TMSOF and allylic acetates using lithium perchlorate in ether. 5-Propargyl-2(5//)-furanones are prepared by coupling with bex-acarbonyldicobalt complexes of propargylium cations (eq 5). Reaction of the intermediate complex with cerium(TV) ammonium nitrate removes the cobalt Fluoroalkylation is acbieved by using bis(fluoroalkanoyl) peroxides in 1,1,2-tricbloro-1,2,2-trifluoroethane (Freon 113) (eq 6). This process is believed to involve combination of a fluoroalkyl radical with the furan-derived radical cation. 

The fast reaction between cerium(IV) sulfate and hydrogen peroxide is useful to determine the concentration of hydrogen peroxide in solution by cerimetric titrations (see section 3). However, the decomposition of hydrogen peroxide by cerium(IV) in perchloric acid solution is slow at pH values above 0.7 (Baer and Stein, 1953 Ardon and Stein, 1956), at which colloid polymeric cerium(IV) complexes are formed. These are able to interact with hydrogen peroxide to afford colored complexes that are only slowly decomposed. At very low pH values, the polymeric complexes are not formed and decomposition of hydrogen peroxide is fast. 

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