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Chapter 15: Problem 21

Which of the following octahedral complexes show geometric isomerism? If geometric isomers are possible, draw their structures. (a) \(\left[\mathrm{Co}(e n) \mathrm{Cl}_{4}\right]^{-}\) (b) \(\left[\mathrm{Ni}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{2} \mathrm{ClBr}\right]^{4-}\) (c) \(\left[\mathrm{Cd}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{4}\right]^{2-}\)

Short Answer

Expert verified
Short Answer: Only the complexes (b) \(\left[\mathrm{Ni}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{2} \mathrm{ClBr}\right]^{4-}\) and (c) \(\left[\mathrm{Cd}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{4}\right]^{2-}\) show geometric isomerism. For complex (b), both cis and trans isomers have the Cl and Br ligands trans to each other; the difference is the arrangement of the two oxalate(C2O4) ligands, which are adjacent in the cis-isomer and opposite in the trans-isomer. In the case of complex (c), the geometric isomers have two NH3 ligands adjacent in the cis-isomer and opposite in the trans-isomer.

Step by step solution

01

Identifying geometric isomerism for (a)

The given complex is \(\left[\mathrm{Co}(e n) \mathrm{Cl}_{4}\right]^{-}\). The central metal ion is Co, surrounded by one ethylenediamine (en) ligand and four Cl ligands in an octahedral geometry. Since there is only one type of ligand occupying the remaining positions, geometric isomerism is not possible for this complex.
02

Drawing structures for (a)

There is no need to draw any structures for (a) as it doesn't show geometric isomerism.
03

Identifying geometric isomerism for (b)

The given complex is \(\left[\mathrm{Ni}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{2} \mathrm{ClBr}\right]^{4-}\). The central metal ion is Ni, surrounded by two oxalato (C2O4) ligands, one Cl ligand, and one Br ligand in an octahedral geometry. Since there are two identical oxalate ligands, we can have geometric isomers in this case.
04

Drawing structures for (b)

The cis-isomer will have both the oxalate(C2O4) ligands adjacent to each other, while the trans-isomer will have the oxalate ligands opposite each other. In both cases, the Cl and Br ligands are also trans to each other. Draw both the cis and trans isomers.
05

Identifying geometric isomerism for (c)

The given complex is \(\left[\mathrm{Cd}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{4}\right]^{2-}\). The central metal ion, Cd, is surrounded by two NH3 ligands and four Cl ligands in an octahedral geometry. Since there are two identical NH3 ligands, geometric isomerism is possible here.
06

Drawing structures for (c)

The cis-isomer will have both NH3 ligands adjacent to each other, while the trans-isomer will have the NH3 ligands opposite each other. Draw both the cis and trans isomers.

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Most popular questions from this chapter

In the \(\mathrm{Ti}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}{ }^{3+}\) ion, the splitting between the \(\mathrm{d}\) levels, \(\Delta_{\mathrm{o}}\) is \(55 \mathrm{kcal} / \mathrm{mol}\). What is the color of this ion? Assume that the color results from a transition between upper and lower d levels.

\(\mathrm{Ti}\left(\mathrm{NH}_{3}\right)_{6}{ }^{3+}\) has a d-orbital electron transition at \(399 \mathrm{~nm}\). Find \(\Delta_{o}\) at this wavelength.

Bipyridyl (Bipy) is a molecule commonly used as a bidentate ligand. When \(0.17 \mathrm{~mol}\) of bipyridyl is dissolved in \(2.4 \mathrm{~L}\) of a solution that contains \(0.052 \mathrm{M} \mathrm{Fe}^{2+},\left[\mathrm{Fe}(\mathrm{bipy})_{3}\right]^{2+}\left(K_{\mathrm{f}}=1.6 \times 10^{17}\right)\) is formed. What are the con- centrations of all species when equilibrium is established?

Analysis of a coordination compound gives the following results: \(22.0 \% \mathrm{Co}, 31.4 \% \mathrm{~N}, 6.78 \% \mathrm{H}\), and \(39.8 \% \mathrm{Cl} .\) One mole of the compound dissociates in water to form four moles of ions. (a) What is the simplest formula of the compound? (b) Write an equation for its dissociation in water.

\(\mathrm{MnF}_{6}{ }^{2-}\) has a crystal field splitting energy, \(\Delta_{0}\) of \(2.60 \times 10^{2} \mathrm{~kJ} / \mathrm{mol}\). What is the wavelength responsible for this energy?
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