Solubilities of alkali metal chlorides except lithium were determined in ammonia, EDA, methyl-and ethylamines, DME, and THF at three different temperatures. From these data, standard thermodynamic functions of solution and solvation with respect to ion formation were calculated. The standard free energies of solvation increased linearly as a function of D_1. However, the requirements of the Bom equation were not satisfied because the slopes and intercepts of these plots were not equal. Values of the entropies of solvation are roughly accounted for on the basis of the freezing out of a fixed number of solvent molecules. The superiority of ammonia as an agent for solvating ions is attributed to its relatively low molecular entropy compared to other solvents. A criterion for salt-like behavior is introduced and used to suggest that saturated alkali metal solutions are salt like and are probably dominated by the +• ~ion pairs. On this basis solubilities of metals in ammonia are too large to be accounted for without introducing additional species.
In the reaction of 2-chlorocyclohexanone or 2-bromo-~5-methyl-5-phenylcyclohexanone (cis or trans) with NaOMe in MeOH the yield of Favorskii ester has been found to increase markedly at the expense of or-methoxyoxirane and or-methoxy ketone products on increasing the methoxide concentration. 2-Chloro-and 2-bromo-4methyl-4-phenylcyclohexanones ( 6 ) are much less subject to this concentration effect, 407, yield of Favorskii ester being obtained even at low (-10-5 M ) methoxide concentrations. The ratio of stereoisomeric esters formed from 6 was found to be reversed in going from low to high (2 M ) methoxide concentrations. This result i3 rationalized in terms of equilibrating dipolar ion and cyclopropanone intermediates.
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