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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 complex \(\mathrm{MA}_{2}\mathrm{B}_{2}\) has two different isomers, it can be concluded that the complex is square planar. This is because a square planar complex can exhibit two isomers (cis and trans), while a tetrahedral complex with the same formula would only have one possible configuration.

Step by step solution

01

Understand isomers in square planar complexes

In a square planar complex, the central metal atom is surrounded by 4 ligands in a square plane. For the given complex \(\mathrm{MA}_{2}\mathrm{B}_{2}\), we would have two possible isomers. The cis-isomer, in which the A ligands are adjacent to each other and the B ligands are also adjacent to each other, and the trans-isomer, in which the A ligands are opposite to each other and the B ligands are also opposite to each other. Since the complex can exhibit two different isomers, the possibility of having a square planar complex is valid.
02

Understand isomers in tetrahedral complexes

In a tetrahedral complex, the central metal atom is surrounded by 4 ligands in a tetrahedron geometry. For the given complex \(\mathrm{MA}_{2}\mathrm{B}_{2}\) in a tetrahedral arrangement, there is only one possible configuration where 2 A ligands and 2 B ligands are positioned around the central metal atom. In a tetrahedral complex, there are no cis or trans isomers because all ligands are equidistant from each other. Therefore, having two isomers for the given complex with a tetrahedral geometry is not possible.
03

Determine whether the complex is square planar or tetrahedral

Since it was found that the given complex \(\mathrm{MA}_{2}\mathrm{B}_{2}\) has two different isomers, and only a square planar complex allows for the formation of these two isomers (cis and trans), we can conclude that the complex is square planar and not tetrahedral.

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Most popular questions from this chapter

Explain why the transition metals in periods 5 and 6 have nearly identical radii in each group.

(a) Sketch a diagram that shows the definition of the crystal-field splitting energy \((\Delta)\) for an octahedral crystal-field. (b) What is the relationship between the magnitude of \(\Delta\) and the energy of the \(d\)-\(d\) transition for a \(d^{1}\) complex? (c) Calculate \(\Delta\) in \(\mathrm{k} J / \mathrm{mol}\) if a \(d^{1}\) complex has an absorption maximum at 545 \(\mathrm{nm} .\)

(a) In early studies it was observed that when the complex \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Br}_{2}\right] \mathrm{Br}\) was placed in water, the electrical conductivity of a 0.05\(M\) solution changed from an initial value of 191 \(\mathrm{ohm}^{-1}\) to a final value of 374 \(\mathrm{ohm}^{-1}\) over a period of an hour or so. Suggest an explanation for the observed results.(See Exercise 23.69 for relevant comparison data.) (b) Write a balanced chemical equation to describe the reaction. (c) \(A 500\)-mL solution is made up by dissolving 3.87g of the complex. As soon as the solution is formed, and before any change in conductivity has occurred, a 25.00-mL portion of the solution is titrated with 0.0100 \(\mathrm{M} \mathrm{AgNO}_{3}\) solution. What volume of AgNO \(_{3}\) solution do you expect to be required to precipitate the free \(\operatorname{Br}^{-}(a q) ?(\mathbf{d})\) Based on the response you gave to part (b), what volume of \(\mathrm{AgNO}_{3}\) solution would be required to titrate a fresh 25.00 -mL sample of \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Br}_{2}\right] \mathrm{Br}\) after all conductivity changes have occurred?

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

The lanthanide contraction explains which of the following periodic trends? (a) The atomic radii of the transitionmetals first decrease and then increase when moving horizontally across each period. (b) When forming ions the period 4 transition metals lose their 4\(s\) electrons before their 3\(d\) electrons. (c) The radii of the period 5 transition metals \((\mathrm{Y}-\mathrm{Cd})\) are very similar to the radii of the period 6 transition metals \((\mathrm{Lu}-\mathrm{Hg}).\)
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