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Chapter 23: Problem 46

Determine if each of the following metal complexes is chiral and therefore has an optical isomer: (a) square planar \(\left[\mathrm{Pd}(\mathrm{en})(\mathrm{CN})_{2}\right],(\mathbf{b})\) octahedral $\left[\mathrm{Ni (\mathrm{en})\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+},$ (c) octahedral cis-[V(en) \(\left._{2} \mathrm{ClBr}\right]\).

Short Answer

Expert verified
The square planar complex \([\mathrm{Pd}(\mathrm{en})(\mathrm{CN})_{2}]\) and the octahedral complex \([\mathrm{Ni}(\mathrm{en})(\mathrm{NH}_{3})_{4}]^{2+}\) are achiral due to the presence of planes of symmetry. In contrast, the octahedral complex cis-\([\mathrm{V}(\mathrm{en})_{2} \mathrm{ClBr}]\) is chiral and has an optical isomer, as it lacks any plane of symmetry.

Step by step solution

01

(Step 1: Analyzing Complex (a))

The first complex is a square planar complex, \([\mathrm{Pd}(\mathrm{en})(\mathrm{CN})_{2}]\). Here, the coordination geometry of the Pd metal center is square planar. The ligands are one ethylenediamine (en) molecule and two cyanide (CN) ions. To determine if it's chiral or not, we need to check if there's a plane of symmetry present in this complex.
02

(Step 2: Assessing Symmetry in Complex (a))

In this complex, both cyanide ions are in trans positions, and ethylenediamine ligand spans opposite corners of the square. Therefore, there are two planes of symmetry. This means that this metal complex is achiral.
03

(Step 3: Analyzing Complex (b))

The second complex is an octahedral complex, \([\mathrm{Ni}(\mathrm{en})(\mathrm{NH}_{3})_{4}]^{2+}\). The coordination geometry of the Ni metal center is octahedral. The ligands are one ethylenediamine (en) molecule and four ammonia (NH\(_3\)) molecules. To determine if it's chiral or not, we need to check if there's a plane of symmetry present in this complex.
04

(Step 4: Assessing Symmetry in Complex (b))

In this complex, the four ammonia molecules occupy equatorial positions, and the ethylenediamine ligand spans the axial positions. Therefore, there is a plane of symmetry along the plane containing the four ammonia molecules. This means that this metal complex is achiral.
05

(Step 5: Analyzing Complex (c))

The third complex is an octahedral complex, cis-\([\mathrm{V}(\mathrm{en})_{2} \mathrm{ClBr}]\). The coordination geometry of the V metal center is octahedral. The ligands are two ethylenediamine (en) molecules, one chloride (Cl) ion, and one bromide (Br) ion. To determine if it's chiral or not, we need to check if there's a plane of symmetry present in this complex.
06

(Step 6: Assessing Symmetry in Complex (c))

In this cis complex, the ethylenediamine ligands lie next to each other, while the chloride and bromide ions occupy trans dihalide positions. There is no plane of symmetry in this complex. This means that this metal complex is chiral and has an optical isomer. In conclusion, among the given metal complexes, only complex (c) is chiral and has an optical isomer, while complexes (a) and (b) are achiral.

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Most popular questions from this chapter

Consider the following three complexes: \(\left(\right.\) Complex 1) $\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{SCN}\right]^{2+}$ \(\left(\right.\) Complex 2) $\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{3} \mathrm{Cl}_{3}\right]^{2+}$ \(\left(\right.\) Complex 3) \(\mathrm{CoClBr} \cdot 5 \mathrm{NH}_{3}\) Which of the three complexes can have (a) geometric isomers, (b) linkage isomers, (c) optical isomers, (d) coordination-sphere isomers?

Draw the structure for $\mathrm{Pt}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)\left(\mathrm{NH}_{3}\right)_{2}$ and use it to answer the following questions: (a) What is the coordination number for platinum in this complex? (b) What is the coordination geometry? (c) What is the oxidation state of the platinum? (d) How many unpaired electrons are there? [Sections 23.2 and 23.6\(]\)

Write the formula for each of the following compounds, being sure to use brackets to indicate the coordination sphere: (a) hexaammineiron(II) nitrate (b) tetraaquadibromochromium(III) perchlorate (c) ammonium hexachloropalladate(IV) (d) diammineoxolatonickel(II) (e) Hexaamminemolybdenum(III) tetrachlorocuprate(II)

For each of the following metals, write the electronic configuration of the atom and its \(3+\) ion: (a) Fe, (b) Mo, (c) Co. Draw the crystal-field energy-level diagram for the \(d\) orbitals of an octahedral complex, and show the placement of the \(d\) electrons for each \(3+\) ion, assuming a weak-field complex. How many unpaired electrons are there in each case?

Consider the following three complexes: \(\left(\right.\) Complex 1) $\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Br}_{2}\right] \mathrm{Cl}$ 2) \(\left[\mathrm{Pd}\left(\mathrm{NH}_{3}\right)_{2}(\mathrm{ONO})_{2}\right]\) (Complex (Complex 3) $\left[\mathrm{V}(\mathrm{en})_{2} \mathrm{Cl}_{2}\right]^{+},$ Which of the three complexes can have (a) geometric isomers, (b) linkage isomers, (c) optical isomers, (d) coordinationsphere isomers?
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