Abstract
An expression is derived for the entropy of solvation of a solvated electron that can be evaluated directly from (1) an established correlation between the spectral energy and solvent energy of the solvated-electron system and (2) the entropy of the pure solvent. The theory predicts that entropies of solvation of solvated electrons should be positive in all pure solvents, under the usual standard conditions, in marked contrast with the negative values obtained for the hydration of conventional ions. This is supported by current experimental results: for NH3, the theory yields a value of +120 J/(mol-K), while the most recently reported experimental value is +154 ± 20 J/(mol-K); for H20, the theory yields a value of +118 J/(mol-K), while the most recently reported experimental value is +118 ± 20 J/(mol-K).