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Like most amino acid complexes, the glycinate forms a 5-membered chelate ring, with the glycinato ligand serving as a bidentate (κ 2 Ο,Ν) species. [2] [5] The chelating ligands assume a square planar configuration around the copper atom as is common for tetracoordinate d 9 complexes, calculated to be much lower in energy than the alternative tetrahedral arrangement.
The chelate effect is the greater affinity of chelating ligands for a metal ion than that of similar nonchelating (monodentate) ligands for the same metal. The thermodynamic principles underpinning the chelate effect are illustrated by the contrasting affinities of copper(II) for ethylenediamine (en) vs. methylamine.
Complexes with the 2:1 stoichiometry are illustrated by copper(II) glycinate [Cu(O 2 CC(R)HNH 2) 2], which exists both in anhydrous and pentacoordinate geometries. When the metal is square planar, these complexes can exist as cis and trans isomers.
A Zn chelate supplement was compared with zinc sulfate in broiler chickens. Weight gain and feed intake increased quadratically (p<0.05) with increasing Zn concentrations from the chelate and linearly with Zn sulfate. The relative bioavailability of the Zn chelate was 183% and 157% of Zn sulfate for weight gain and tibia Zn, respectively. The ...
The chelate effect increases as the number of chelate rings increases. For example, the complex [Ni(dien) 2 )] 2+ is more stable than the complex [Ni(en) 3 )] 2+ ; both complexes are octahedral with six nitrogen atoms around the nickel ion, but dien ( diethylenetriamine , 1,4,7-triazaheptane) is a tridentate ligand and en is bidentate.
Then they can determine if magnesium citrate or magnesium glycinate is the way to go. Also, if you still have questions, don’t be afraid to speak up. “Registered dietitians are here to help ...