Solution chemistry
Aqueous chemistry is completely dominated through the M+ ions. The M+/M electrode potentials are all very negative, that of Li being little more so than the others due to the large solvation energy consequently of its small size. The higher solvation of lithium can be observed in the ionic mobilities determined by the ionic conductivities of dissolved salts. It might be supposed that the smallest ion would be the most mobile, but actually Li+ is the least mobile and it shows that the smallest 'bare' ion becomes the biggest on solvation.
The M+ ions have only weak complexing trends, but these can be improved by properly sized macrocyclic ligands. Ligands with dissimilar cavity sizes can be employed to discriminate among alkali ions. The metallic elements dissolve in liquid ammonia and associated amines (example ethylamine C2H5NH2) to give solutions that consist of solvated electrons in addition to cations. In a number of solvents there is proof for equilibria involving alkali anions M-. The solutions are helpful reducing agents for the preparation of not usually low oxidation states (example [Ni0(CN)4]4-) including anionic compounds of the alkali elements themselves.