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Chapter 24: Problem 15

Draw a structure for cis-dichlorobis(ethylenediamine)cobalt(III) ion. Is this ion chiral? Is the trans isomer chiral? Explain.

Short Answer

Expert verified
The cis-dichlorobis(ethylenediamine)cobalt(III) ion does have a plane of symmetry and therefore is not chiral. Likewise, the trans isomer also has a plane of symmetry and thus is not chiral.

Step by step solution

01

Identify the Components of the Complex Ion

This compound is called 'cis-dichlorobis(ethylenediamine)cobalt(III) ion'. In this, the cobalt(III) ion is the central metal ion, ethylenediamine (denoted as en, a bidentate ligand) is the ligand, and there are two chloride ions. The term 'cis' indicates that the two similar groups lie on the same side of a molecule.
02

Draw the Structure of the Complex Ion

Here, coordination number of the cobalt ion is 6 (4 from two ethylenediamine molecules and 2 from two chloride ions). As the coordination number is 6, the structure is likely to be octahedral. In the cis-configuration, arrange the two chloride ions at adjacent positions, and the two ethylenediamine ligands at the remaining positions.
03

Determine the Chirality of the Cis Isomer

For a molecule to be chiral, it should lack a plane of symmetry or a center of symmetry. Analyzing the drawn structure, it can be seen that the cis isomer does have a plane of symmetry and hence it is not chiral.
04

Draw the Structure of the Trans Isomer

In the trans isomer, the similar groups are arranged directly opposite to each other on the molecule. So position the two chloride ions opposite to each other and then place the ethylenediamine ligands at the remaining positions in the octahedral structure.
05

Determine the Chirality of the Trans Isomer

Just like the cis isomer, for the trans isomer to be chiral, it should not have a plane of symmetry. Looking closely at the structure, it can be noted that trans isomer does possess a plane of symmetry. Therefore, the trans isomer is also not chiral.

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Most popular questions from this chapter

Of the following, the one that is a Bronsted-Lowry acid is (a) \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+} ;\) (b) \(\left[\mathrm{FeCl}_{4}\right]^{-} ;\) (c) \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) (d) \(\left[\mathrm{Zn}(\mathrm{OH})_{4}\right]^{-}\).

Predict: (a) which of the complex ions, \(\left[\mathrm{MoCl}_{6}\right]^{3-}\) and \(\left[\mathrm{Co}(\mathrm{en})_{3}\right]^{3+},\) is diamagnetic and which is paramagnetic; (b) the number of unpaired electrons expected for the tetrahedral complex ion \(\left[\mathrm{CoCl}_{4}\right]^{2-}\).

Predict: (a) whether the square-planar complex ion \(\left[\mathrm{Cu}(\mathrm{py})_{4}\right]^{2+}\) is diamagnetic or paramagnetic (b) whether octahedral \(\left[\mathrm{Mn}(\mathrm{CN})_{6}\right]^{3-}\) or tetrahedral \(\left[\mathrm{FeCl}_{4}\right]^{-}\) has the greater number of unpaired electrons.

Briefly describe each of the following ideas, phenomena, or methods: (a) spectrochemical series; (b) crystal field theory; (c) optical isomer; (d) structural isomerism.

Which of these general structures for a complex ion would you expect to exhibit cis and trans isomerism? Explain. (a) tetrahedral (b) square-planar (c) linear
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