Solvent Effects on Methyl Transfer Reactions. 2. The Reaction of Amines with Trimethylsulfonium Salts

• Published in: Journal of the American Chemical Society 2001-06, Vol.123 (25), p.6092-6097
• Main Authors: Castejon, Henry, Wiberg, Kenneth B, Sklenak, Stepan, Hinz, Wolfgang
• Format: Article
• Language: English
• Subjects: Amines - chemistry; Ammonia - chemistry; Cyclohexanes; Dimethyl Sulfoxide; Indicators and Reagents; Kinetics; Methylation; Models, Molecular; Molecular Conformation; Pyridines - chemistry; Salts - chemistry; Solvents; Sulfonium Compounds - chemistry; Water
• ISSN: 0002-7863; 1520-5126
• DOI: 10.1021/ja0042940

The reaction of ammonia and pyridine with trimethylsulfonium ion has been studied in gas phase and solution. Density functional theory at the B3LYP/6-31+G* level was used to describe the energy changes along the reaction coordinate in the gas phase, and the self-consistent isodensity polarizable continuum model (SCI-PCM) was used to calculate the effect of cyclohexane and dimethyl sulfoxide as the solvent on the energy changes. The effect of water as the solvent was studied using the Monte Carlo free energy perturbation method. The reaction with both ammonia and pyridine follows a similar rather convoluted path in gas phase, with the formation of several reaction complexes before and after the formation of the transition state. All the species found in gas phase persist in cyclohexane, yielding a reaction path very similar to that in gas phase but with significant differences in the relative energy of the critical points. In DMSO, the energy profile is greatly simplified by the disappearance of several of the species found in gas phase and in cyclohexane. The activation free energy increases with the polarity of the solvent in both reactions. Increasing the polarity of the solvent also increases the exothermicity of the reaction of trimethylsulfonium ion with ammonia and reduces it in the reaction with pyridine. In water, the free energy profile follows the same trend as found for DMSO, and free energy of activation is calculated to be larger by about 2−3 kcal/mol. This is in good agreement with an experimental measurement of the effect of solvent on the rate of reaction.