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Chapter 20: Problem 19

Draw structures of all the geometric and optical isomers of each of these cobalt complexes: (a) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}\) (b) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Cl}\right]^{2+}\) (c) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right]^{+}\) (d) \(\left[\mathrm{Co}(\mathrm{en})_{3}\right]^{3+}\) (e) \(\left[\mathrm{Co}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}\right]^{3-}\)

Short Answer

Expert verified
Complexes (a), (b), (d) and (e) do not show geometric isomerism, while complex (c) shows two geometric isomers, cis and trans. None of these complexes show optical isomerism.

Step by step solution

01

Defining Ligands

Ligands here are \(\mathrm{NH}_{3}\), \(\mathrm{Cl}\), ethane-1,2-diamine (en) and oxalate (\(\mathrm{C}_{2}\mathrm{O}_{4}^{2-}\)). Now consider the coordination number and charges for each complex in order to determine the potential geometries.
02

Drawing Geometric Isomers for Complex (a)

\(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}\) is an octahedral complex with identical ligands, hence it does not show geometrical isomerism.
03

Drawing Geometric Isomers for Complex (b)

\(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5}\mathrm{Cl}\right]^{2+}\) also does not express geometrical isomerism due to the octahedral complex with only one different ligand.
04

Drawing Geometric Isomers for Complex (c)

\(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4}\mathrm{Cl}_{2}\right]^{+}\) does express geometrical isomerism, there are two possible isomers: cis (where two Chlorines occupy the adjacent positions) and trans (where it occupies the opposite positions).
05

Drawing Geometric Isomers for Complex (d)

\(\left[\mathrm{Co}(\mathrm{en})_{3}\right]^{3+}\) does not show geometrical isomerism as it has symmetrical bidentate ligands.
06

Drawing Geometric Isomers for Complex (e)

\(\left[\mathrm{Co}\left(\mathrm{C}_{2}\mathrm{O}_{4}\right)_{3}\right]^{3-}\) does not show geometrical isomerism because it has symmetrical bidentate ligands.

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Most popular questions from this chapter

Complex ion formation has been used to extract gold, which exists in nature in the uncombined state. To separate it from other solid impurities, the ore is treated with a sodium cyanide (NaCN) solution in the presence of air to dissolve the gold by forming the soluble complex ion \(\left[\mathrm{Au}(\mathrm{CN})_{2}\right]^{-}\). (a) Balance the following equation: $$\mathrm{Au}+\mathrm{CN}^{-}+\mathrm{O}_{2}+\mathrm{H}_{2} \mathrm{O} \longrightarrow\left[\mathrm{Au}(\mathrm{CN})_{2}\right]^{-}+\mathrm{OH}^{-}$$ (b) The gold is obtained by reducing the complex ion with zinc metal. Write a balanced ionic equation for this process. (c) What is the geometry and coordination number of the \(\left[\mathrm{Au}(\mathrm{CN})_{2}\right]^{-}\) ion?

Briefly describe the crystal field theory. Define the following terms: crystal field splitting, high-spin complex, low-spin complex, spectrochemical series.

A student prepared a cobalt complex that has one of the following structures: \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right] \mathrm{Cl}_{3}\), \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Cl}\right] \mathrm{Cl}_{2},\) or \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right] \mathrm{Cl} .\) Explain how the student would distinguish among these possibilities by an electrical conductance experiment. At the student's disposal are three strong electrolytes: \(\mathrm{NaCl}, \mathrm{MgCl}_{2},\) and \(\mathrm{FeCl}_{3},\) which may be used for comparison purposes.

Why is zinc not considered a transition metal?

What factors determine whether a given complex will be diamagnetic or paramagnetic?
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