<Tr> <Td> <P> </P> </Td> </Tr> <P> (2) </P> <P> In (1) the bidentate ligand ethylene diamine forms a chelate complex with the copper ion . Chelation results in the formation of a five - membered ring . In (2) the bidentate ligand is replaced by two monodentate methylamine ligands of approximately the same donor power, meaning that the enthalpy of formation of Cu--N bonds is approximately the same in the two reactions . Under conditions of equal copper concentrations and when then concentration of methylamine is twice the concentration of ethylenediamine, the concentration of the complex (1) will be greater than the concentration of the complex (2). The effect increases with the number of chelate rings so the concentration of the EDTA complex, which has six chelate rings, is much higher than a corresponding complex with two monodentate nitrogen donor ligands and four monodentate carboxylate ligands . Thus, the phenomenon of the chelate effect is a firmly established empirical fact: under comparable conditions, the concentration of a chelate complex will be higher than the concentration of an analogous complex with monodentate ligands . </P> <P> The thermodynamic approach to explaining the chelate effect considers the equilibrium constant for the reaction: the larger the equilibrium constant, the higher the concentration of the complex . </P>

Why do chelating ligands have higher formation constants for metal complexes
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