Library

Notes: Abstract Charge transfer complexes between C60 and ternary aromatic amines (N,N,N,N′-tetramethyl-p-phenylenediamine,p-methoxy-N,N-dimethylaniline,p-methyl-N,N-dimethylaniline,N,N-diethylaniline,N,N-dimethylaniline, and triphenylamine) were studied in chlorobenzene solutions. The lifetimes of the excited state with charge transfer in these complexes were measured by the method of picosecond laser photolysis. The dependence of the rate constant of the back electron transfer on ΔG in the back electron transfer reaction with relaxation of the charge-transfer state exhibits the “Marcus-inverted” region.

Notes: Flash photolysis technique has been used to obtain the rate and thermodynamic parameters of the reversible dimerization reactions of a range of ten phenoxy radicals (I-X) in a toluene-dibutylphthalate mixture (0.6 cP ≤η≤18.4 cP): \documentclass{article}\pagestyle{empty}\begin{document}$$ {\rm R}^{.} + {\rm R}^{.} {\mathop{{\buildrel{-\!\!\longrightarrow}\over{\longleftarrow}}}\limits_{k_{-1}}^{k_1}}{\rm D} $$\end{document} The main reason for the difference in the k1 values are the different steric hindrances in radicals. It has been found that the values of k1 for 2,6-diphenyl-4-methoxy- (I), 2-phenyl-(III), and 2-methoxyphenoxy (IV) radicals are 3-5 times smaller than the respective diffusion constants calculated according to the Debye formula with regard to the spin-statistical factor: \documentclass{article}\pagestyle{empty}\begin{document}$$ k_{diff} = \sigma \frac{{8{\rm RT}}}{{3000{\rm \eta }}} $$\end{document} The resultant ΔH1≠values for these radicals in toluene and dibutylphthalate are close to the activation energies of the viscous flow of the solvents B. Linear relationships with a slope equal to unity are observed between log k1 and log(T/η). The recombination of radicals I, III, and IV is limited by translational diffusion. The k1 values for 2,6-diphenyl- (VII), 2,6-di-tert-butyl- (IX), and 2,6-di-tert-butyl-4-methylphenoxy (X) radicals are 10-60 times smaller than kdiff and Δ H≠ B. In the case of radical X in toluene ΔH1≠ 0. The recombination of these three radicals includes an intermediate step of complex formation: \documentclass{article}\pagestyle{empty}\begin{document}$${{\rm R}^\cdot+{\rm R}^\cdot}{\mathop {{\scriptstyle\longleftarrow}^{\hskip-13pt\longrightarrow}}}{\rm R^\cdot}\ldots {\rm R}^\cdot \rightarrow {\rm D}$$ \end{document} For 4-phenyl- (II), 2,6- dimethoxy- (V), 2,4-diphenyl- (VI), and radicals VII, IX, and X the linear relationships between log k1 and log (T/η) have a slope of from 0.5 ± 0.05 to 0.8 ± 0.05. The k1-1 versus η relationships for these radicals are not straight lines. The recombination of these six radicals is limited by translational and rotational diffusion. With the aid of theoretical models, the k1 versus η relationships have been used to derive the steric factor f in radical recombination and the angle θ between the axis and the solid angle generatrix. The solid angle defines the reaction spot on the radical-sphere surface. The recombination of the 2,6-diphenyl-4-diphenylmethylphenoxy radical (VIII) takes place in the region intermediate between the diffusion and the kinetic ones, and the relationship between log k1 and log (T/η) for this radical has a plateau portion. The log k-1 versus log (T/η) relationships have precisely the same form as the corresponding k1 relationships, which is quite in line with the theory of diffusion-controlled reversible recombination reactions.

Notes: Rate, equilibrium, and thermodynamic data for reaction (1) of 2,6-diphenyl-4R-phenoxyl radicals, where R==OCH3 (I), Ph (II), OC2H5 (III), O-n-C18H37 (IV), and 2,6-dicyclohexyl-4-phenylphenoxyl radical (V), in various solvents are obtained. The k1 values of radicals I to V are within (5.5 ± 1.0) × 107-(1.4 ± 0.3) × 109M-1·sec-1 in propanol. The solvent effect on k1 for radicals I and II was studied. The dimerization of radical I is diffusion-controlled in all solvent studies. The dimerization of radical II is viscosity-dependent but not diffusion-controlled. Plots of k1 against ET have a V shape. Specific solvent-solute interactions are seeming to be responsible for numerical k1 values of radicals I and II. The solvent effect is more pronounced for “slow” dimerization of radicals II than for “fast” dimerization of radicals I. The minimum k1 values correspond to pyridine and chloroform. The reaction (1) rate strongly depends upon the composition of a chloroform (S)-cosolvent binary mixture. Besides reaction (1) the following reactions proceed in binary mixture: \documentclass{article}\pagestyle{empty}\begin{document}$$ K_{14} = 0.18 \pm 0.05M^{ - 1},k_{15} = (2.0 \pm 1.0) \times 10^8 M^{ - 1} \cdot \sec ^{ - 1} $$\end{document} (radical I, S-CCL4 mixture) \documentclass{article}\pagestyle{empty}\begin{document}$$ K_{14} = 0.9 \pm 0.2M^{ - 1},k_{15} = (1.2 \pm 0.5) \times 10^7 M^{ - 1} \cdot \sec ^{ - 1} $$\end{document}(radical II, S-C6H14 mixture) \documentclass{article}\pagestyle{empty}\begin{document}$$ K_{14} = 0.45 \pm 0.10M^{ - 1},k_{15} = (9.0 \pm 2.0) \times 10^6 M^{ - 1} \cdot \sec ^{ - 1} $$\end{document}(radical II, S-CCL4 mixture)In all cases k16 ≪ k15. Factors influencing dimerization rates in strongly nonideal mixtures CH3OH-CCL4 and CH3OH-CHCl3 are discussed.