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Chapter 23: Problem 41

A four-coordinate complex \(\mathrm{MA}_{2} \mathrm{~B}_{2}\) is prepared and found to have two different isomers. Is it possible to determine from this information whether the complex is square planar or tetrahedral? If so, which is it?

Short Answer

Expert verified
The complex MA₂B₂ can be either square planar or tetrahedral. However, considering the number of isomers, a square planar complex has two isomers (cis- and trans-), while a tetrahedral complex has no isomers. Since the given information states that the complex has two different isomers, it can be concluded that the complex MA₂B₂ is square planar.

Step by step solution

01

Identify possible isomers for square planar geometry

In a square planar complex, the molecule is arranged in a planar fashion with the 4 ligands at the vertices of a square. The possible isomers for a square planar complex are cis- and trans-isomers. Cis-isomers have the two A ligands and the two B ligands adjacent to each other, whereas trans-isomers have one A and one B ligand adjacent to each other. Therefore, there are two different isomers for a square planar complex.
02

Identify possible isomers for tetrahedral geometry

In a tetrahedral complex, the molecule is arranged in a three-dimensional tetrahedral configuration with 4 ligands at the vertices of a tetrahedron. In the case of the MA₂B₂ complex with a tetrahedral geometry, there is no possibility of having different isomers because all vertices of a tetrahedron are adjacent. Regardless of the positioning of the A and B ligands, they always possess a single arrangement.
03

Comparing isomer numbers

Now, we have determined that a square planar MA₂B₂ complex has two isomers (cis- and trans-) while a tetrahedral MA₂B₂ complex doesn't have any isomers. The given information implies that the complex has two different isomers, which matches the isomer count for a square planar MA₂B₂ complex.
04

Conclusion

Based on the given information and the analysis of the isomers for square planar and tetrahedral geometries, we can conclude that the complex MA₂B₂ is square planar.

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Most popular questions from this chapter

Draw the crystal-field energy-level diagrams and show the placement of electrons for the following complexes: (a) \(\left[\mathrm{VCl}_{6}\right]^{3-}\) (b) \(\left[\mathrm{FeF}_{6}\right]^{3-}(\) a high-spin complex \(),(\mathrm{c})\left[\mathrm{Ru}(\mathrm{bipy})_{3}\right]^{3+}\) (a low- spin complex), (d) \(\left[\mathrm{NiCl}_{4}\right]^{2-}\) (tetrahedral), (e) \(\left[\mathrm{PtBr}_{6}\right]^{2-}\) (f) \(\left[\mathrm{Ti}(\mathrm{en})_{3}\right]^{2+}\)

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) \(\left[\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{CO}_{3}\right] \mathrm{Cl}\) (d) \(\left[\operatorname{Ir}\left(\mathrm{NH}_{3}\right)_{4}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right]\left(\mathrm{NO}_{3}\right)_{3}\)

Sketch a plot of atomic radius versus number of valence \(d\) electrons for the period 5 transition metals, and explain the trend.

(a) What is the meaning of the term coordination number as it applies to metal complexes? (b) Give an example of a ligand that is neutral and one that is negatively charged. (c) Would you expect ligands that are positively charged to be common? Explain. (d) What type of chemical bonding is characteristic of coordination compounds? Illustrate with the compound \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6} \mathrm{Cl}_{3}\) (e) What are the most common coordination numbers for metal complexes?

(a) Draw the structure for \(\mathrm{Pt}(\mathrm{en}) \mathrm{Cl}_{2} .\) (b) What is the coordination number for platinum in this complex, and what is the coordination geometry? (c) What is the oxidation state of the platinum? [Section 23.2]
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