Refraction bonds involving hydrogen

From an examination of the refractivity of propionitrile-amine systems in water, Oda et al. (1960) concluded that hydrogen bonding involved an a -hydrogen, and indeed isobutyronitrile (a proton donor ) was deemed to use an a-hydrogen in hydrogen-bonding with the electron donor site of benzonitrile (called a proton acceptor ) ... 

Here E is the solute excess molar refractivity, S is the solute dipolarity/ polarizability A and B are the overall or summation hydrogen-bond acidity and basicity, respectively and V is the McGowan characteristic volume lower-case letters stand for respective coefficients which are characteristic of the solvent, c is the constant. By help of sfafisfical methods like the principal component analysis and nonlinear mapping, the authors determined the mathematical distance (i.e., measure of dissimilarify) from an IL fo seven conventional solvents immiscible with water. It appears that the closest to the IL conventional solvent is 1-octanol. Even more close to IL is an aqueous biphasic system based on PEG-200 and ammonium sulfate (and even closer are ethylene glycol and trifluoroethanol, as calculated for hypofhefical water-solvenf sysfems involving fhese solvenfs). 

Abraham developed what is termed a general solvation equation. The main idea behind the model involves the creation of a cavity in the solvent, incorporation of the solvent in the cavity, and turning on solute-solvent interactions. These interactions require a relevant solute parameter, and the ones chosen were the excess molar refraction, ttf the solute dipolarity/polarizability, flf and Pf the hydrogen-bond acidity and basicity, respectively, and a characteristic volume. Applying this general equation to 132 solutes in aqueous SDS, Abraham et al. obtained the following equation for the partition coefQcient ... 

---