/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 88 CC(=O)[O-] can act a鈥� # Many... [FREE SOLUTION] | 91影视

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Chapter 23: Problem 88

CC(=O)[O-] can act a鈥� # Many trace metal ions exist in the blood complexed with amino acids or small peptides. The anion of the amino acid glycine (gly), N#CC(=O)[O-] can act as a bidentate ligand, coordinating to the metal through nitrogen and oxygen atoms. How many isomers are possible for (a) \(\left[\mathrm{Zn}(\mathrm{gly})_{2}\right]\) (tetrahedral), (b) \(\left[\mathrm{Pt}(\mathrm{gly})_{2}\right]\) (square planar), (c) \(\left[\mathrm{Co}(\mathrm{gly})_{3}\right]\) (octahedral)? Sketch all possible isomers. Use the symbol \(\mathrm{N}\) O to represent the ligand.

Short Answer

Expert verified
For the given metal complexes with glycine as the ligand, there is only one possible isomer for each: (a) Zn(gly)\(_2\): 1 isomer (tetrahedral) (b) Pt(gly)\(_2\): 1 isomer (square planar) (c) Co(gly)\(_3\): 1 isomer (octahedral)

Step by step solution

01

Determine the coordination geometries of the complexes

(a) Zn(gly)\(_2\): Coordination geometry is tetrahedral with a central metal ion and two bidentate glycine ligands. (b) Pt(gly)\(_2\): Coordination geometry is square planar with a central metal ion and two bidentate glycine ligands. (c) Co(gly)\(_3\): Coordination geometry is octahedral with a central metal ion and three bidentate glycine ligands.
02

Find the isomers for the tetrahedral complex Zn(gly)\(_2\)

Since the coordination geometry is tetrahedral and we have two bidentate ligands, only one isomer is possible. The metal binds to the oxygen atom from the carboxylate group and the nitrogen atom from the amino group in each ligand. Sketch: ``` O \ O-Zn-N / \ (NH3)C \ || \ C N // (NH3)C N==C /\. \ O O ```
03

Find the isomers for the square planar complex Pt(gly)\(_2\)

For the square planar complex, we have two bidentate ligands. We only have one possible geometrical isomer. Each ligand will bind to the metal through nitrogen and oxygen atoms. Sketch: ``` O \ O-Pt-N \ (NH3)C \ || \ C N // (NH3)C N==C /\. \ O O ```
04

Find the isomers for the octahedral complex Co(gly)\(_3\)

For the octahedral complex, we have three bidentate ligands. Since each ligand will bind through nitrogen and oxygen atoms, there is only one possible geometrical isomer. Sketch: ``` O \ O-Co-N / \ (NH3)C / \ || / \ C / N //\/ (NH3)C N=\O \ / \.\ N-Co-O O O / \ N O (NH3)C / || / C / // / N==C /^\ \ O O ``` To summarize, we found that there is only one possible isomer for each of the complexes: - (a) Zn(gly)\(_2\): 1 isomer (tetrahedral) - (b) Pt(gly)\(_2\): 1 isomer (square planar) - (c) Co(gly)\(_3\): 1 isomer (octahedral)

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Most popular questions from this chapter

Polydentate ligands can vary in the number of coordination positions they occupy. In each of the following, identify the polydentate ligand present and indicate the probable number of coordination positions it occupies: (a) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4}(o\) -phen \()\right] \mathrm{Cl}_{3}\) (b) \(\left[\mathrm{Cr}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}\right] \mathrm{Br}\) (c) \(\left[\mathrm{Cr}(\mathrm{EDTA})\left(\mathrm{H}_{2} \mathrm{O}\right)\right]^{-}\) (d) \(\left[\mathrm{Zn}(\mathrm{en})_{2}\right]\left(\mathrm{ClO}_{4}\right)_{2}\)

For each of the following polydentate ligands, determine (i) the maximum number of coordination sites that the ligand can occupy on a single metal ion and (ii) the number and type of donor atoms in the ligand: (a) ethylenediamine (en), (b) bipyridine (bipy), (c) the oxalate anion \(\left(\mathrm{C}_{2} \mathrm{O}_{4}{ }^{2-}\right),(\mathrm{d})\) the \(2-\) ion of the porphine molecule (Figure 23.13 ); (e) [EDTA] \(]\) -

Distinguish among a ferromagnetic substance, an antiferromagnetic substance, and a ferrimagnetic substance.

Generally speaking, for a given metal and ligand, the stability of a coordination compound is greater for the metal in the +3 rather than in the +2 oxidation state (for metals that form stable +3 ions in the first place). Suggest an explanation, keeping in mind the Lewis acid-base nature of the metal-ligand bond.

A certain complex of metal \(\mathrm{M}\) is formulated as \(\mathrm{MCl}_{3} \cdot 3 \mathrm{H}_{2} \mathrm{O}\). The coordination number of the complex is not known but is expected to be 4 or 6. (a) Would conductivity measurements provide information about the coordination number? (b) In using conductivity measurements to test which ligands are bound to the metal ion, what assumption is made about the rate at which ligands enter or leave the coordination sphere of the metal? (c) Suppose you experimentally determine that this complex exists in aqueous solution as a single species. Suggest a likely coordination number and the number and type of each ligand.
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