Amino acids can act as ligands toward transition metal ions. The simplest amino acid is glycine $\left(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{CO}_{2} \mathrm{H}\right) .$ Draw a structure of the glycinate anion \(\left(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{CO}_{2}^{-}\right)\) acting as a bidentate ligand. Draw the structural isomers of the square planar complex \(\mathrm{Cu}\left(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{CO}_{2}\right)_{2}\)

The glycinate anion structure is formed by deprotonating the carboxyl group in glycine, resulting in NH2CH2CO2-. As a bidentate ligand, glycinate forms two coordination bonds with metal ions; one through the amine nitrogen (N) and the other through the carboxylate oxygen (O). There are two structural isomers of the square planar complex Cu(NH2CH2CO2)2: 1. Cis configuration: The two amine nitrogen (N) atoms are adjacent in the complex, with the carboxylate oxygen (O) atoms also adjacent, occupying the other two corners of the square. 2. Trans configuration: The two amine nitrogen (N) atoms are opposite each other in the complex, with the carboxylate oxygen (O) atoms also opposite, occupying the other two corners of the square.