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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
From the given information that the complex MA₂B₂ has two different isomers, we can determine that the complex is square planar. This is because, in a square planar geometry, there can be two isomers - cis (A and B ligands are adjacent) and trans (A and B ligands are opposite). In contrast, a tetrahedral complex would have only one isomer with no distinction between cis or trans.

Step by step solution

01

Analyze the isomers in both geometries

Let's first analyze the possible isomers for both square planar and tetrahedral geometries. Square planar: - Cis: A and B ligands are adjacent to each other - Trans: A and B ligands are opposite each other Tetrahedral: - There are no separate cis or trans isomers, as all ligand positions are equivalent.
02

Compare the isomer possibilities to the given information

We have determined the possible isomers for both square planar and tetrahedral complexes. We are given that the complex has two different isomers. By comparing this information to our analysis, we can draw the following conclusions: - If the complex is square planar, it can have two isomers: cis and trans. - If the complex is tetrahedral, it has only one isomer, and no distinction between cis or trans.
03

Conclude the geometry

Since the given complex has two different isomers, it must be square planar, as the tetrahedral complex only has one isomer. Thus, the complex is square planar.

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Most popular questions from this chapter

A Zn electrode is immersed in a solution that is \(1.00 \mathrm{M}\) in \(\left[\mathrm{Zn}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}\) 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 \(+1.04 \mathrm{~V}\). What is the formation constant for \(\left[\mathrm{Zn}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+} ?\)

Draw the crystal-field energy-level diagrams and show the placement of \(d\) electrons for each of the following: (b) \(\left[\mathrm{Mn}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\), (a) \(\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) (four unpaired electrons), (a high-spin complex), (c) $\left[\mathrm{Ru}\left(\mathrm{NH}_{3}\right)_{5}\left(\mathrm{H}_{2} \mathrm{O}\right)\right]^{2+}$ (a low-spin complex), (d) \(\left[\mathrm{IrCl}_{6}\right]^{2-}\) (a low-spin complex), (e) \(\left[\mathrm{Cr}(\mathrm{en})_{3}\right]^{3+}\), (f) \(\left[\mathrm{NiF}_{6}\right]^{4-}\).

For each of the following pairs, identify the molecule or ion that is more likely to act as a ligand in a metal complex: (a) carbonic acid \(\left(\mathrm{H}_{2} \mathrm{CO}_{3}\right)\) or carbonate \(\left(\mathrm{CO}_{3}^{2-}\right),(\mathbf{b})\) water $\left(\mathrm{H}_{2} \mathrm{O}\right)\( or hydronium ion \)\left(\mathrm{H}_{3} \mathrm{O}^{+}\right),(\mathbf{c})\( phosphine \)\left(\mathrm{PH}_{3}\right)$ or phosphoric acid \(\left(\mathrm{H}_{3} \mathrm{PO}_{4}\right)\).

Give the number of (valence) \(d\) electrons associated with the central metal ion in each of the following complexes: (a) $\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\right] \mathrm{Cl}_{2},$, (b) $\mathrm{K}_{2}\left[\mathrm{Cu}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{2}\right]$, (c) \(\left[\mathrm{Os}(\mathrm{en})_{3}\right] \mathrm{Cl}_{3}\), (d) $[\mathrm{Cr}(\mathrm{EDTA})] \mathrm{SO}_{4},(\mathbf{e})\left[\mathrm{Cd}\left(\mathrm{H}_{2} ,\mathrm{O}\right)_{6}\right] \mathrm{Cl}_{2}$.

Which species are more likely to act as ligands? (a) Positively charged ions or negatively charged ions? (b) Neutral molecules that are polar or those that are nonpolar?
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