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Chapter 23: Problem 10

Two Fe(II) complexes are both low spin but have different ligands. A solution of one is green and a solution of the other is red. Which solution is likely to contain the complex that has the stronger-field ligand? [Section 23.6\(]\)

Short Answer

Expert verified
The red solution is likely to contain the complex with the stronger-field ligand because it absorbs green light, which has higher energy than the red light absorbed by the green solution. The energy of absorbed light is directly related to the crystal-field splitting energy in the complex, so a higher energy absorbed light indicates a larger crystal-field splitting energy associated with a stronger-field ligand.

Step by step solution

01

Determine the color of absorbed light

First, we need to determine the color of the light that is absorbed by each complex based on the color of their respective solutions. Colors that are observed result from the transmission of light in the complementary color of the absorbed light. The complementary color of green is red, meaning the green solution absorbs red light. And the complementary color of red is green, meaning the red solution absorbs green light.
02

Compare the energy of absorbed light

Based on the color wheel, the energy of the light increases from red to green. The equation connecting energy (E) and wavelength (λ) is given by the Planck's constant (h) and the speed of light (c): \[E = \dfrac{hc}{\lambda}\] Since the green solution absorbs red light, and the red solution absorbs green light, we can say that the green solution absorbs lower energy light and the red solution absorbs higher energy light.
03

Determine the stronger-field ligand

A stronger-field ligand will lead to a larger crystal-field splitting energy in the complex. Given that the energy of the absorbed light is directly related to the crystal-field splitting energy, we can conclude that the complex with the red solution (absorbing green, higher energy light) has the stronger-field ligand. So, the solution that contains the complex with the stronger-field ligand is the red solution.

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Most popular questions from this chapter

(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) 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?

How many electrons are in the valence \(d\) orbitals in these transition-metal ions? (a) \(\mathrm{Co}^{3+},(\mathbf{b}) \mathrm{Cu}^{+}\), (d) \(\mathrm{Os}^{3+}\). (c) \(\mathrm{Cd}^{2+}\)

A certain complex of metal \(\mathrm{M}\) is formulated as \(\mathrm{MCl}_{3} \cdot 3 \mathrm{H}_{2} \mathrm{O}\). The coordination number of the complex is not known but is expected to be 4 or 6. (a) Would conductivity measurements provide information about the coordination number? (b) In using conductivity measurements to test which ligands are bound to the metal ion, what assumption is made about the rate at which ligands enter or leave the coordination sphere of the metal? (c) Suppose you experimentally determine that this complex exists in aqueous solution as a single species. Suggest a likely coordination number and the number and type of each ligand.

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.
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