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Chapter 23: Problem 43

Determine if each of the following complexes exhibits geometric isomerism. If geometric isomers exist, determine how many there are. (a) tetrahedral \(\left[\operatorname{Cd}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2} \mathrm{Cl}_{2}\right],(\mathbf{b})\) square-planar \(\left[\operatorname{IrCl}_{2}\left(\mathrm{PH}_{3}\right)_{2}\right]^{-},(\mathbf{c})\) octahedral \(\left[\mathrm{Fe}(o-\mathrm{phen})_{2} \mathrm{Cl}_{2}\right]^{+}.\)

Short Answer

Expert verified
a) Tetrahedral complex \(\left[\operatorname{Cd}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2} \mathrm{Cl}_{2}\right]\) does not exhibit geometric isomerism. b) Square-planar complex \(\left[\operatorname{IrCl}_{2}\left(\mathrm{PH}_{3}\right)_{2}\right]^{-}\) exhibits geometric isomerism with 2 isomers: cis and trans. c) Octahedral complex \(\left[\mathrm{Fe}(o-\mathrm{phen})_{2} \mathrm{Cl}_{2}\right]^{+}\) exhibits geometric isomerism with 2 isomers: cis and trans.

Step by step solution

01

Analyze the geometry and ligands of each complex

For each complex, determine the geometry, the central atom and its ligands, and check if there are two or more different types of ligands in the complex. a) \(\left[\operatorname{Cd}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2} \mathrm{Cl}_{2}\right]\) has a tetrahedral geometry with the central atom Cd and ligands \(\mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{Cl}\). b) \(\left[\operatorname{IrCl}_{2}\left(\mathrm{PH}_{3}\right)_{2}\right]^{-}\) has a square-planar geometry with the central atom Ir and ligands \(\mathrm{Cl}\) and \(\mathrm{PH}_3\). c) \(\left[\mathrm{Fe}(o-\mathrm{phen})_{2} \mathrm{Cl}_{2}\right]^{+}\) has an octahedral geometry with the central atom Fe and ligands \(o-\mathrm{phen}\) and \(\mathrm{Cl}\).
02

Determine if geometric isomerism is possible

To determine if geometric isomerism is possible, analyze if there are two or more different types of ligands in the complex. a) \(\left[\operatorname{Cd}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2} \mathrm{Cl}_{2}\right]\) - Geometric isomerism is not possible as tetrahedral complexes do not exhibit geometric isomerism. b) \(\left[\operatorname{IrCl}_{2}\left(\mathrm{PH}_{3}\right)_{2}\right]^{-}\) - Geometric isomerism is possible in square-planar complexes with two different types of ligands. c) \(\left[\mathrm{Fe}(o-\mathrm{phen})_{2} \mathrm{Cl}_{2}\right]^{+}\) - Geometric isomerism is possible in octahedral complexes with two different types of ligands.
03

Determine the number of geometric isomers in complexes showing isomerism

For each complex showing geometric isomerism, determine the number of geometric isomers. b) \(\left[\operatorname{IrCl}_{2}\left(\mathrm{PH}_{3}\right)_{2}\right]^{-}\) - There are two geometric isomers: cis and trans. c) \(\left[\mathrm{Fe}(o-\mathrm{phen})_{2} \mathrm{Cl}_{2}\right]^{+}\) - There are two geometric isomers: cis and trans. #Final answer# a) Tetrahedral complex \(\left[\operatorname{Cd}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2} \mathrm{Cl}_{2}\right]\) does not exhibit geometric isomerism. b) Square-planar complex \(\left[\operatorname{IrCl}_{2}\left(\mathrm{PH}_{3}\right)_{2}\right]^{-}\) exhibits geometric isomerism with 2 isomers: cis and trans. c) Octahedral complex \(\left[\mathrm{Fe}(o-\mathrm{phen})_{2} \mathrm{Cl}_{2}\right]^{+}\) exhibits geometric isomerism with 2 isomers: cis and trans.

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Most popular questions from this chapter

(a) A compound with formula \(\mathrm{RuCl}_{3}\) \(\cdot 5 \mathrm{H}_{2} \mathrm{O}\) is dissolved in water, forming a solution that is approximately the same color as the solid. Immediately after forming the solution, the addition of excess AgNO \(_{3}(a q)\) forms 2 mol of solid AgCl per mole of complex. Write the formula for the compound, showing which ligands are likely to be present in the coordination sphere. (b) After a solution of \(\mathrm{RuCl}_{3}\) \(\cdot 5 \mathrm{H}_{2} \mathrm{O}\) has stood for about a year, addition of \(\mathrm{AgNO}_{3}(a q)\) precipitates 3 mol of AgCl per mole of complex. What has happened in the ensuing time?

Sketch the structure of the complex in each of the following compounds and give the full compound name: (a) \(\operatorname{cis}-\left[\operatorname{Co}\left(\mathrm{NH}_{3}\right)_{4}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right]\left(\mathrm{NO}_{3}\right)_{2}\) (b) \(\mathrm{Na}_{2}\left[\mathrm{Ru}\left(\mathrm{H}_{2} \mathrm{O}\right) \mathrm{Cl}_{5}\right]\) (c) \(\operatorname{trans} \mathrm{NH}_{4}\left[\mathrm{Co}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right]\) (d) \(\operatorname{cis}-\left[\operatorname{Ru}(\mathrm{en})_{2} \mathrm{Cl}_{2}\right]\)

The \(E^{\circ}\) values for two low-spin iron complexes in acidic solution are as follows: \(\left[\mathrm{Fe}(o-\mathrm{phen})_{3}\right]^{3+}(a q)+\mathrm{e}^{-} \Longrightarrow\) \(\quad\quad\quad\quad\quad\quad\quad\) \(\left[\mathrm{Fe}(o-\mathrm{phen})_{3}\right]^{2+}(a q) \quad E^{\circ}=1.12 \mathrm{V}\) \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-}(a q)+\mathrm{e}^{-} \rightleftharpoons\) \(\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\) \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}(a q) \quad E^{\circ}=0.36 \mathrm{V}\) (a) Is it thermodynamically favorable to reduce both Fe(III) complexes to their Fe(II) analogs? Explain. (b) Which complex, \(\left[\mathrm{Fe}(o-\mathrm{phen})_{3}\right]^{3+}\) or \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-},\) is more difficult to reduce? (c) Suggest an explanation for your answer to (b).

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?

Write names for the following coordination compounds: (a) \(\left[\mathrm{Cd}(\mathrm{en}) \mathrm{Cl}_{2}\right]\) (b) \(\mathrm{K}_{4}\left[\mathrm{Mn}(\mathrm{CN})_{6}\right]\) (c) \(\left[\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{5}\left(\mathrm{CO}_{3}\right)\right] \mathrm{Cl}\) (d) \(\left[\operatorname{Ir}\left(\mathrm{NH}_{3}\right)_{4}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right]\left(\mathrm{NO}_{3}\right)_{3}\)
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