Mononuclear metal complexes in aqueous solution lie at the heart of coordination chemistry. Their significance is evident in areas ranging from simple textbook chemistry to sophisticated applications in fields of current interest. Water as a solvent is the most important medium in biochemistry and environmental chemistry. When the challenges that it poses have been met, water could be an especially advantageous solvent for technical catalysis, particularly in green chemistry. The chemistry of mononuclear coordination complexes in water, as characterized by the variety of multidentate organic chelators that may bind to a metal center, is most extensive for the medium oxidation states of a metal, typically + II and + III. This statement also holds for metalloenzymes, in which protein side chains act as ligands. The chemistry of higher metal oxidation states in water is, however, usually severely restricted. Hydrolytic reactions lead to replacement of the mononuclear metal/chelator core with mono-and polynuclear (hydr)oxido metal species and, finally, (hydrated) oxide phases. This is the case for main-group-metal as well as transition-metal centers, examples being tin(IV) and manganese(IV). The latter shows another property of high-oxidation-state centers that may prohibit the formation of stable mononuclear coordination compounds with organic ligands, namely, its reactivity as an oxidant. The combination of these properties results in decidedly restricted chemistry in water. A good example is lead(IV), whose coordination chemistry in