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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 MA鈧侭鈧� 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 MA鈧侭鈧� 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 MA鈧侭鈧� 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 MA鈧侭鈧� complex has two isomers (cis- and trans-) while a tetrahedral MA鈧侭鈧� 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 MA鈧侭鈧� 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 MA鈧侭鈧� is square planar.

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Most popular questions from this chapter

The red color of ruby is due to the presence of Cr(III) ions at octahedral sites in the close-packed oxide lattice of \(\mathrm{Al}_{2} \mathrm{O}_{3} .\) Draw the crystal-field splitting diagram for Cr(III) in this environment. Suppose that the ruby crystal is subjected to high pressure. What do you predict for the variation in the wavelength of absorption of the ruby as a function of pressure? Explain.

(a) What is the difference between a monodentate ligand and a bidentate ligand? (b) How many bidentate ligands are necessary to fill the coordination sphere of a six-coordinate complex? (c) You are told that a certain molecule can serve as a tridentate ligand. Based on this statement, what do you know about the molecule?

Explain the lanthanide contraction, and describe how it affects the properties of the transition-metal elements.

By writing formulas or drawing structures related to any one of these three complexes, \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Br}_{2}\right] \mathrm{Cl}\) \(\left[\mathrm{Pd}\left(\mathrm{NH}_{3}\right)_{2}(\mathrm{ONO})_{2}\right]\) cis-[ \(\left.\mathrm{V}(\mathrm{en})_{2} \mathrm{Cl}_{2}\right]^{+}\) illustrate (a) geometric isomerism, (b) linkage isomerism, (c) optical isomerism, (d) coordination-sphere isomerism.

Suppose that a transition-metal ion was in a lattice in which it was in contact with just two nearby anions, located on opposite sides of the metal. Diagram the splitting of the metal \(\bar{d}\) orbitals that would result from such a crystal field. Assuming a strong field, how many unpaired electrons would you expect for a metal ion with six \(d\) electrons? (Hint: Consider the linear axis to be the \(z\) -axis)
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