Kinetics and Mechanism of Monomolecular Heterolysis of Commercial Organohalogen Compounds: XXXI. Solvent Effect on the Rate of 1-Methyl-1-chlorocyclopentane Heterolysis. Correlation Analysis of Solvation Effects

Heterolysis of 1-methyl-1-chlorocyclopentane in protic and aprotic solvents occurs by the E1 mechanism. The reaction rate in aprotic solvents or in a set of protic and aprotic solvents is satisfactorily described by the parameters of the polarity and electrophilicity or ionizing power of the solvents. In protic solvents, the reaction rate grows with increasing polarity or ionizing power of the solvent and decreases with increasing nucleophilicity.     

Kinetics and Mechanism of Monomolecular Heterolysis of Commercial Organohalogen Compounds: XLII. Effect of Aprotic Solvent on the Rate of 3-Methyl-3-chloro-1-butene Dehydrochlorination. Correlation Analysis of Solvation Effects

The kinetics of 3-methyl-3-chloro-1-butene dehydrochlorination in propylene carbonate, γ-butyrolactone, sulfolane, acetone, MeCN, PhNO₂, PhCN, PhCOMe, MeCOEt, cyclohexanone, o-dichlorobenzene, PhCl, PhBr, 1,2-dichloroethane, dioxane, and AcOEt were studied; v = k[C₅H₉Cl], E1 mechanism. The reaction rate is satisfactorily described by the parameters of the polarity, electrophilicity, and cohesion of the solvent; the solvent nucleophilicity and polarizability exert no effect on the reaction rate.     

Kinetics and Mechanism of Monomolecular Heterolysis of Commercial Organohalogen Compounds: XLI. Solvent Effect on the Rate of 3-Methyl-3-chloro-1-butene Solvolysis. Correlation Analysis of Solvation Effects and Role of Solvent Nucleophilicity

The kinetics of 3-methyl-3-chloro-1-butene solvolysis at 25°C in MeOH, EtOH, BuOH, i-BuOH, PentOH, 2-PrOH, 2-BuOH, HexOH, OctOH, t-BuOH, t-PentOH, cyclohexanol, and allyl alcohol was studied by the verdazyl method; v = k[C₅H₉Cl], SN1 + E1 mechanism. The reaction rate shows a satisfactory correlation with the parameter of the solvent ionizing power E _T and is independent of the solvent nucleophilicity.     

Kinetics and Mechanism of Monomolecular Heterolysis of Commercial Organohalogen Compounds: XXX.1 Correlation Analysis of Solvation Effects in Heterolysis of tert-Butyl Chloride

Quantitative analysis of the effect of solvent parameters on the rate of heterolysis of tert-butyl chloride was performed; the reaction rate is fairly described by the polarity, polarizability, and electrophilicity parameters or by the ionizing ability parameter, while the nucleophilicity of the solvent has no rate effect. A negative effect of nucleophilic solvation was revealed in protic solvents.     

Kinetics and Mechanism of Monomolecular Heterolysis of Commercial Organohalogen Compounds: XXXII.1 Solvent Effects on Activation Parameters of Heterolysis of 1-Chloro-1-methylcyclopentane. Correlation Analysis of Solvation Effects

Kinetics of heterolysis of 1-chloro-1-methylcyclopentane in MeOH, BuOH, cyclohexane, i-PrOH, t-BuOH, tert-C₅H₁₁OH, -butyrolactone, MeCN, PhCN, PhNO₂, acetone, PhCOMe, cyclohexanone, and 1,2-dichloroethane at 25-50°C were studied by the verdazyl method. Correlation analysis of solvent effects on activation parameters of the reaction in 8 protic (additionally, AcOH and CF₃CH₂OH) and 8 aprotic solvents together and separately in either group of solvents was performed. In all the solvents studied, two H -S compensation effects were revealed.     

Kinetics and Mechanism of Monomolecular Heterolysis of Commercial Organohalogen Compounds: XXXIV. Solvent Effect on the Heterolysis Rate of 1-Chloro-1-methylcyclohexane. Correlation Analysis of Solvation Effects in Heterolysis of 1-Chloro-1-methylcyclohexane and 1-Chloro-1-methylcyclopentane

The kinetics of heterolysis of 1-chloro-1-methylcyclohexane in 9 protic and 25 aprotic solvents at 25°C were studied by the verdazyl method. The kinetic equation is v = k[RCl] (E1 mechanism). The heterolysis rate of 1-chloro-1-methylcyclohexane in protic solvents is two orders of magnitude lower than that of 1-chloro-1-methylcyclopentane, whereas in low-polarity and nonpolar aprotic solvents the rates are close. A correlation analysis was made to reveal the solvation effects in heterolysis of both chlorides in a set of 9 protic and 25 aprotic solvents, and separately in protic and aprotic solvents.     

Kinetics and Mechanism of Monomolecular Heterolysis of Commercial Organohalogen Compounds: XXIX. Solvent Effects on the Activation Parameters of Heterolysis of tert-Butyl Chloride

The kinetics of heterolysis of t-BuCl in sulfolane, PhCN, PhNO₂, acetophenone, cyclohexanone, chloroform, and 1,2-dichloroethane at 30-50°C were studied by the verdazyl method. Quantitative analysis of the effect of solvent parameters on the G , H , S , and log k _{2 5} values for heterolysis of t-BuCl in a set of 15 protic and 16 aprotic solvents and separately in either group of solvents was performed. In the above set of solvents, three H -S compensation effects are observed, associated with jump changes in the potential energy of the reaction.     

Kinetics and Mechanism of Monomolecular Heterolysis of Commercial Organohalogen Compounds: XXXV.1 Solvation Effects on the Activation Parameters of Heterolysis of 1-Bromo-1-methylcyclopentane and 1-Bromo-1-methylcyclohexane. Correlation Analysis of Solvation Effects

Kinetics of heterolysis of 1-bromo-1-methylcyclopentane and -cyclohexane in protic and aprotic solvents were studied. Correlation analysis of the effect of solvent parameters on G , H , and S was performed.     

Kinetics and Mechanism of Monomolecular Heterolysis of Commercial Organohalogen Compounds: XXXVI.1 Solvent Effect on the Activation Parameters of Heterolysis of 1-Methyl-1-chlorocyclohexane. Correlation Analysis of Solvation Effects in Heterolysis of 1-Methyl-1-chlorocyclohexane and 1-Methyl-1-chlorocyclopentane

The kinetics of heterolysis of 1-methyl-1-chlorocyclohexane in six protic and eight aprotic solvents at 25-50°C was studied by the verdazyl method; v = k[RCl], E1 mechanism. The correlation analysis of the solvent effects on the activation free energy G , enthalpy H , and entropy S of heterolysis of 1-methyl-1-chlorocyclohexane and 1-methyl-1-chlorocyclopentane was performed for the same sets of solvents.     

Kinetics and Mechanism of Monomolecular Heterolysis of Commercial Organohalogen Compounds: XXXVII.1 Effect of Nucleofuge and Solvent of the Relative Rates of Heterolysis of 1-Halo-1-methylcyclopentanes and 1-Halo-1-methylcyclohexanes. Correlation Analysis of Solvation Effects

The effect of solvent ionizing ability on heterolysis rate enhances in the series 1-chloro-1-methylcyclohexane < 1-bromo-1-methylcyclohexane 1-chloro-1-methylcyclopentane < 1-bromo-1-methyl- cyclopentane. The lower sensitivity of cyclohexyl substrates compared with cyclopentyl is determined by conformational effects. Bromides are more sensitive to solvent effects than chlorides because of the stronger polarizability of the C-Br bond.     

Kinetics and Mechanism of Monomolecular Heterolysis of Commercial Organohalogen Compounds: XL. Nature of Salt Effects in Dehydrobromination of 3-Bromocyclohexene in γ-Butyrolactone. Role of Solvation Effects of Dipolar Aprotic Solvents

The influence of neutral salts on the rate of heterolysis of 3-bromocyclohexene at 31°C in γ-butyrolactone was studied by the verdazyl method; ν = k[C₆H₉Br], E1 mechanism. Additions of lithium picrate do not affect the reaction rate; those of LiClO₄ and Et₄NClO₄ increase it; and those of LiCl, Et₄NCl, and KNCS decelerate the reaction. The nature of salt and solvation effects in the heterolysis of 3-bromocyclohexene in γ-butyrolactone, MeCN, and PhNO₂ is discussed.__________Translated from Zhurnal Obshchei Khimii, Vol. 75, No. 6, 2005, pp. 937–944.Original Russian Text Copyright © 2005 by Ponomarev, Stambirskii, Dvorko.     

Kinetics and Mechanism of Monomolecular Heterolysis of Commercial Organohalogen Compounds: XXVIII. Effect of the Nature of the Verdazyl Indicator on Salt Effects in Dehydrobromination of 3-Bromocyclohexene in Nitrobenzene

The salt effect on the rate of dehydrobromination of 3-bromocyclohexene in PhNO2 depends on the nature of the verdazyl indicator. With triphenylverdazyl and its chloro and nitro derivatives in the presence of Et₄NClO₄, a normal salt effect is observed, in the presence of bromides, a superposition of normal and special salt effects, while in the presence of chlorides, a superposition of normal and special negative salt effects. With the dimethoxy verdazyl derivative, a normal salt effect is always observed.     

Kinetics and Mechanism of Monomolecular Heterolysis of Commercial Organohalogen Compounds: XXXIII.1 Correlation Analysis of Solvation Effects in Monomolecular Heterolysis of 1-Bromo-1-methylcyclopentane, 1-Bromo-1-methylcyclohexane, and 2-Bromo-2-methyladamantane

The rate of heterolysis of 1-bromo-1-methylcyclopentane and 1-bromo-1-methylcyclohexane is determined by the equation v = k[RBr], mechanism E1. Comparative correlation analysis of solvation effects in heterolysis of these substrates and 2-brom-2-methyladamantane was performed.     

Kinetics and Mechanism of Monomolecular Heterolysis of Commercial Organohalogen Compounds: XXXIX. Salt Effect of LiClO<Subscript>4</Subscript>in Heterolysis of Ph<Subscript>2</Subscript>CHCl in γ-Butyrolactone

Additions of LiClO₄ accelerate the heterolysis of Ph₂CHCl in γ-butyrolactone; v = k[Ph₂CHCl], SN1 mechanism. The salt effect increases with an increase in the electron-acceptor properties of the verdazyl indicator. A superposition of three salt effects (normal, special, and negative special) is observed.__________Translated from Zhurnal Obshchei Khimii, Vol. 75, No. 1, 2005, pp. 105–110.Original Russian Text Copyright © 2005 by Dvorko, Ponomareva, Golovko, Pervishko.     

Effect of Solvation on the Decomposition Rate of Azodiisobutyronitrile

The log rate constants of monomolecular decomposition of azodiisobutyronitrile can be quantitatively correlated with solvent properties by means of linear multiparameter equations including various solvation effects; the key factors are the ability of solvents for electrophilic solvation, which favors decomposition, and cohesive energy density, which unfavors the reaction.__________Translated from Zhurnal Obshchei Khimii, Vol. 75, No. 2, 2005, pp. 196–200.Original Russian Text Copyright © 2005 by Makitra, Polyuzhin, Golovata.     

Kinetics and Mechanism of Unimolecular Heterolysis of Framework Compounds: XVII. Solvation Effects in Dehydrobromination of <Emphasis Type="Italic">tert</Emphasis>-Butyl Bromide, 1-Bromo-1-Methylcyclohexane,and 2-Bromo-2-methyladamantane in Dipolar Aprotic Solvents

Dehydrobromination rate of tert-butyl bromide, 1-bromo-1-methylcyclohexane, and 2-bromo-2-methyladamantane grows with increasing polarity and dipole moment of solvents. No correlation was found between rate constants of the process and electrophilicity or ionizing power of the solvents. The observed solvation effects are due mainly to dispersion interactions.     

Effect of the Hydrogen Bond and the Solvent on Kinetics and the Mechanism of Intermolecular Proton Transitions

Abstracts A reaction involving an intermolecular proton transition RAH + BR₁ → RA^? + HB⁺ in a polar solvent is considered as a process of many consecutive steps. The formation of a hydrogen-bonded complex and stepwise vibrational proton excitation in a double minimum well play a basic part in the reaction. Vibrational transitions occur under the effect of a random force imparted from the medium. A general expression for the rate constant of the multistep reaction is obtained without making the quasistationarity assumption. The rate constant for the reaction considered is obtained from the theory of random processes. By comparing it with experimental data conclusions are made about the overbarrier or tunnelling nature of some proton-transfer reactions. Une réaction comportant une transition protonique intermoléculaire RAH + BR₁ RA^- + HB⁺ dans un dissolvant polaire peut être considéréé comme un procès de plusieurs pas consécutifs. Dans cette réaction la formation d'un complexe avec des liaisons d'hydrogène ainsi que l'excitation vibrationelle graduelle du proton dans le puits de potentiel à deux minimums joue un rôle essentiel. Les transitions vibrationelles résultent d'une force aléatoire provenant de milieu. On obtient une expression générale de la vitesse de la réaction à plusieurs pas sans aucun recours à l'hypothèse de quasi-stationarité. Les methodes employées sont basées sur la théorie des procès aléatoires. On compare la valeur théorique de cette vitesse aux données expérimentales et on discute la nature de quelques réactions de transfert protonique. Eine Reaktion die intermolekulare Protonübergänge RAH + BR₁ → RA^- + HB⁺ in einem polaren Lösungsmittel mit sick bringt, wird als ein Prozess vieler aufeinanderfolgende Stufen angesehen. In dieser Reaktion spielt die Bildung eines Komplexes mit Wasserstoffbrücken and stufenweise Schwingungsanregungen des Protons eine fundamentale Rolle. Schwingungsübergänge geschehen, die von Kraften zufälliger Art erzeugt sind. Ein allgemeiner Ausdruck der Reaktionsrate für diese Reaktion wird mittels der Theorie von Zufalisprozessen ohne die Quasistationaritätsannahme hergeleitet. Dieser theoretische Ausdruck wird mit experimentellen Werten verglichen; die Natur gewisser Protontransferreaktionen wird diskutiert.     

Solvent Effect on the Rate of Dimerization of Cyclopentadiene

The rate of dimerization of cyclopentadiene and some other cycloaddition reactions is determined by electrophilic solvation of the substrate with some contribution of other solvation factors, primarily nonspecific solvation. The corresponding dependence is described by multiparameter equations.     

The Effect of Solvation on the Radiation Damage Rate Constants for Adenine

It is well known that water plays an important part in almost all biological systems and that inclusion of solvation effects might therefore be of utmost importance in studies of radiation damage to DNA. In the present investigation, we have studied the effect of different solvation models in calculations of Gibbs free energies and reaction rates for the reaction between the OH radical and the DNA nucleobase adenine by conducting density functional theory calculations at the ωB97X‐D/6‐311++G(2df,2pd) level with the Eckart tunnelling correction. The solvent, water, was included through either the implicit polarizable continuum model (PCM) or through explicit modelling of micro‐solvation by a single water molecule at the site of reaction as well as by the combination of both. Scrutiny of the thermodynamics and kinetics of the individual sub‐reactions suggests that the qualitative differences introduced by the solvation models do not significantly alter the conclusions made based solely on simple gas‐phase calculations. Abstraction of the amine hydrogen atoms H₆₁ and H₆₂ and addition onto C₈ remain the most likely reaction pathways.     

Nitrosation of Phenolic Compounds: Effects of Alkyl Substituents and Solvent

 Nitrosation reactions of phenol, o-cresol, 2,6-dimethylphenol, o-tert-butylphenol, 2-hydroxyacetophenone, and 2-allylphenol in water and water/acetonitrile were studied. Kinetic monitoring of the reactions was accomplished by spectrophotometric analysis of the nitrosated products at 345 nm. The dominant reaction was C-nitrosation via a mechanism consisting of an attack on the nitrosatable substrate by NO⁺/NO₂H₂ ⁺ followed by a slow proton transfer. The values of the rate constants of phenolic C-nitrosation were increased by electron donating substituents, and a good Hammett correlation was observed with ρ = −6.1. The results also revealed the strong effect of pH and the permitivity of the reaction medium on the rate constant, whose maximum values were observed for pH ≈ 3, decreasing strongly for higher pH values. The study in water/acetonitrile with up to 25% acetonitrile showed that it is possible to inhibit the reaction strongly by increasing the percentage of the organic component. The conclusions drawn show that (i) it is possible to predict the rate of nitrosation of phenolics as a function of the meta-substituents on the phenol ring and (ii) the nitrosation of phenolics can be strongly inhibited by increasing the pH of the reaction medium as well as by lowering its dielectric constant.