Insights
into the influence of solvent on hydride transfer emerge
from a study of iridium complexes with the formula [Cp*Ir(bpy-X)H]+ (bpy-X = 4,4′-X2-2,2′-bipyridine,
X = H, Me, tBu, OMe, CO2Me, and CF3). Hydricity (or hydride donor ability) is found to be equally
sensitive to bipyridine ligand electronic structure in both CH3CN and H2O. In contrast, hydride transfer is found
to be more strongly influenced by subsequent chloride ion binding
to the metal center in CH3CN than in H2O. With
thermochemical parameters for six iridium complexes available in both
CH3CN and H2O, a general approach to comparing
thermodynamic parameters across solvents was developed. The free energy
to transfer the free hydride ion from water to eight organic solvents
(acetonitrile, methanol, ethanol, ethylene glycol, dimethyl sulfoxide, N-methylpyrrolidin-2-one, ethylene carbonate, and tetrahydrofuran)
was estimated. An equation based on the solvent transfer free energies
of the hydride ion and the organometallic species involved in hydride
transfer was developed, enabling accurate and quantitative predictions
of the change in hydricity moving between solvents.