The photoelectron spectra of the gas phase negative cluster ions NH2-(NH3)1 and NH2-(NH3)2 are reported. The spectra imply that these ions consist of intact amide ions solvated by ammonia. Vertical detachment energies and ion-solvent dissociation energies are obtained. In addition, spectral features are also observed that indicate that the ammonia moiety in these cluster anions is distorted from the equilibrium configuration of the free ammonia molecule. The spectra are compared to the photoelectron spectra of H-(NH~)I and H-(NH3)2. Gas phase basicities are determined for N H~-( N H~) I , NH-(NH3)2, H-(NH3),, and H-(NH3)2.While NH2-is a stronger base than H-in the gas phase, our data show that the addition of only two ammonia solvent molecules reverses the relative basicities of these two species.
IntroductionThe governing influence of solvation on the energetics, equilibria, and rates of chemical reactions occurring in solution has long been recogni~ed.'-~ There are many cases in which a change in solvent medium changes the rate or equilibrium constant of a reaction by several orders of magnit~de.~ In order to understand solution phase chemistry, a knowledge of the primary reaction chemistry must be supplemented by information on the interactions between reactant and product molecules with the solvent. Distinguishing between the intrinsic properties of reacting chemical species and the effects attributable to solvation, however, is often difficult.The development in the mid-1960s of experimental methods for studying ion-molecule reactions in the gas phase, in the absence of a solvent medium, profoundly influenced our understanding of chemical r e a~t i v i t y .~-~ Using ion cyclotron resonance mass ~pectrometry,~ high-pressure mass spectrometry,* and flowing afterglow methods? it became possible to make thermodynamic and kinetic measurements for a wide variety of chemical reactions without the complicating effects of solvation. Since solvation energies are often large enough to dominate over differences in intrinsic reactivities, the data generated revealed subtle yet important chemical differences for the first time. During the course of these studies, gas phase acid-base chemistry received considerable a t t e n t i~n .~,~. '~-'~ By measuring equilibrium constants for proton transfer reactions, relative acidities and basicities were determined and anchored to an absolute scale (see tables in refs 5, 6, and 16). Of particular significance, it was found that the ordering of relative acidities for a number of alcohols in the gas phase is the reverse of their ordering in s~l u t i o n . '~ Likewise, for a given list of related bases, it was found that the ordering of their basicities in the gas phase often differs from their ordering in s~l u t i o n . '~