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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
Based on the given information that the four-coordinate complex MA2B2 has two different isomers, it is possible to determine that the complex is square planar. This is because a square planar arrangement can have two possible isomers (cis and trans), whereas a tetrahedral arrangement can only have one isomer. Thus, the complex is square planar.

Step by step solution

01

Understand the given information

We know that the complex is composed of four ligands, with two of each type (A and B). Two different isomers are found, which implies that there are two different ways to arrange these ligands around the metal.
02

Consider square planar arrangement

In a square planar arrangement, the ligands are at the corners of a square, with the metal ion at the center. In this case, there are two possible isomers: cis and trans. These two isomers occur when the same type of ligands (either A or B) are either adjacent to each other (cis) or directly opposite each other (trans).
03

Consider tetrahedral arrangement

In a tetrahedral arrangement, the ligands are placed at the corners of a tetrahedron, with the metal ion at the center. In this case, there is only one possible isomer, as all the corners are equivalent. Any arrangement of the ligands A and B will be the same isomer.
04

Identify the type of complex

Since we are given that the four-coordinate complex MA2B2 has two different isomers, this implies that the complex must be square planar (with cis and trans isomers). A tetrahedral arrangement would only have one isomer. Therefore, the complex is square planar.

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Most popular questions from this chapter

For each of the following metals, write the electronic configuration of the atom and its \(2+\) ion: (a) \(\mathrm{Mn}\), (b) \(\mathrm{Ru}\), (c) \(\mathrm{Rh}\). Draw the crystal-field energy-level diagram for the \(d\) orbitals of an octahedral complex, and show the placement of the \(d\) electrons for each \(2+\) ion, assuming a strong-field complex. How many unpaired electrons are there in each case?

Consider the tetrahedral anions \(\mathrm{VO}_{4}^{3-}\) (orthovanadate ion), \(\mathrm{CrO}_{4}^{2-}\) (chromate ion), and \(\mathrm{MnO}_{4}^{-}\)(permanganate ion). (a) These anions are isoelectronic. What does this statement mean? (b) Would you expect these anions to exhibit \(d-d\) transitions? Explain. (c) As mentioned in "A Closer Look" on charge- transfer color, the violet color of \(\mathrm{MnO}_{4}^{-}\)is due to a ligand- to-metal charge transfer (LMCT) transition. What is meant by this term? (d) The LMCT transition in \(\mathrm{MnO}_{4}^{-}\)occurs at a wavelength of \(565 \mathrm{~nm}\). The \(\mathrm{CrO}_{4}^{2}\) ion is yellow. Is the wavelength of the LMCT transition for chromate larger or smaller than that for \(\mathrm{MnO}_{4}^{-}\)? Explain. (e) The \(\mathrm{VO}_{4}^{3-}\) ion is colorless. Do you expect the light absorbed by the LMCT to fall in the UV or the IR region of the electromagnetic spectrum? Explain your reasoning.

A Cu electrode is immersed in a solution that is \(1.00 \mathrm{M}\) in \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}\) and \(1.00 \mathrm{M}\) in \(\mathrm{NH}_{3}\). When the cathode is a standard hydrogen electrode, the emf of the cell is found to be \(+0.08 \mathrm{~V}\). What is the formation constant for \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}\) ?

(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 \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6} \mathrm{Cl}_{2}\). (e) What are the most common coordination numbers for metal complexes?

Polydentate ligands can vary in the number of coordination positions they occupy. In each of the following, identify the polydentate ligand present and indicate the probable number of coordination positions it occupies: (a) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4}(o-\mathrm{phen})\right] \mathrm{Cl}_{3}\) (b) $\left[\mathrm{Cr}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}\right] \
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