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Chapter 24: Problem 13

If \(\mathrm{A}, \mathrm{B}, \mathrm{C},\) and \(\mathrm{D}\) are four different ligands, (a) how many geometric isomers will be found for square-planar \([\mathrm{PtABCD}]^{2+} ?\) (b) Will tetrahedral \([\mathrm{ZnABCD}]^{2+}\) display optical isomerism?

Short Answer

Expert verified
(a) For \([\mathrm{PtABCD}]^{2+}\), there are three geometric isomers. (b) The tetrahedral \([\mathrm{ZnABCD}]^{2+}\) cannot display optical isomerism.

Step by step solution

01

Identify Geometric Isomers of \([\mathrm{PtABCD}]^{2+}\)

In case of square-planar \([\mathrm{PtABCD}]^{2+}\), with four different ligands A, B, C, and D around platinum (Pt), there are two possibilities, depending on whether opposite positions are occupied by the same (cis) or different (trans) ligands. Geometric isomers for this complex can be generated by considering all possible unique arrangements of the ligands. These arrangements are: AB/CD, AC/BD, and AD/BC. Thus, there are three geometric isomers for \([\mathrm{PtABCD}]^{2+}\).
02

Identify Optical Isomers of \([\mathrm{ZnABCD}]^{2+}\)

Optical isomerism occurs when a compound can exist in two non-superimposable forms. These are mirror images of each other, much like your left hand is a non-superimposable mirror image of your right hand. However, in a tetrahedral complex like \([\mathrm{ZnABCD}]^{2+}\) with different ligands, the mirror images are always superimposable and are therefore the same. This means that tetrahedral complexes like \([\mathrm{ZnABCD}]^{2+}\) with all different ligands cannot exhibit optical isomerism.

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Most popular questions from this chapter

Write the names and formulas of three coordination isomers of \(\left[\mathrm{Co}(\mathrm{en})_{3}\right]\left[\mathrm{Cr}(\mathrm{ox})_{3}\right]\).

The number of unpaired electrons in the complex ion \(\left[\operatorname{Cr}\left(\mathrm{NH}_{3}\right)_{6}\right]^{2+}\) is (a) \(5 ;(\mathrm{b}) 4 ;(\mathrm{c}) 3 ;(\mathrm{d}) 2 ;(\mathrm{e}) 1\).

Of the following complex ions, the one that is optically active is (a) \(\operatorname{cis}-\left[\operatorname{CoCl}_{2}(\text { en })_{2}\right]^{+} ;\) (b) \(\left[\operatorname{CoCl}_{2}\left(\mathrm{NH}_{3}\right)_{4}\right]^{+}\) (c) \(\left[\mathrm{CoCl}_{4}\left(\mathrm{NH}_{3}\right)_{2}\right]^{-} ;(\mathrm{d})\left[\mathrm{CuCl}_{4}\right]^{-}\).

If the ion \(\mathrm{Co}^{2+}\) is linked with strong-field ligands to produce an octahedral complex, the complex has one unpaired electron. If \(\mathrm{Co}^{2+}\) is linked with weak-field ligands, the complex has three unpaired electrons. How do you account for this difference?

Describe how the crystal field theory explains the fact that so many transition metal compounds are colored.
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