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Chapter 23: Problem 59

A classmate says, "A weak-field ligand usually means the complex is high spin." Is your classmate correct? Explain.

Short Answer

Expert verified
Yes, your classmate is correct. Generally, weak-field ligands cause small splits in the d-orbital energy levels, leading to high-spin complexes. This is because electrons tend to occupy all available d-orbitals with parallel spins before pairing up due to the small energy gap between the orbitals. However, it is important to note that this statement may not be true for every case, as there could be exceptions depending on the specific metal ion and ligands involved.

Step by step solution

01

Understand weak-field and strong-field ligands

A ligand is a molecule or ion that binds to a central metal atom or ion, forming a coordination complex. Ligands can be classified as weak-field or strong-field ligands based on their ability to split the d-orbital energy levels in a transition metal complex. Weak-field ligands cause a small splitting of the d-orbitals, while strong-field ligands cause a large splitting of the d-orbitals. The crystal field stabilization energy (CFSE) is used to quantify the energy stabilization resulting from this splitting.
02

Understand high-spin and low-spin complexes

High-spin and low-spin complexes refer to the distribution of electrons in the d-orbitals of a metal complex. For a high-spin complex, electrons will occupy all available d-orbitals with parallel spins (i.e., unpaired electrons) before pairing up. This happens when the energy difference between the d-orbitals is small. On the other hand, a low-spin complex will have electrons filling the lower-energy d-orbitals, pairing up before occupying the higher-energy d-orbitals. Low-spin complexes are formed when the energy difference between the d-orbitals is large. The difference in the energy gap between the orbitals is largely due to the ligands and their ability to split the d-orbitals.
03

Establish the relationship between ligands and their complexes

Now that we understand the terms "weak-field ligand," "strong-field ligand," "high-spin complex," and "low-spin complex," we can establish their relationships. Generally, weak-field ligands bind to metal centers in such a way that the energy gap between the d-orbitals remains small. Therefore, weak-field ligands usually result in high-spin complexes. Conversely, strong-field ligands produce large energy gaps in the d-orbitals, which, in turn, result in low-spin complexes.
04

Evaluate the accuracy of the classmate's statement

The classmate's statement, "A weak-field ligand usually means the complex is high spin," is generally correct, as weak-field ligands are known to cause small splits in the d-orbital energy levels, leading to high-spin complexes. However, it is crucial to remember that this statement is not universally true for every case, as there may be some exceptions depending on the specific metal ion and ligands involved.

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Most popular questions from this chapter

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 \((\mathrm{Lu}-\mathrm{Hg}).\)

Draw the crystal-field energy-level diagrams and show the placement of electrons for the following complexes: (a) \(\left[\mathrm{VCl}_{6}\right]^{3-},\) (b) \(\left[\mathrm{FeF}_{6}\right]^{3-}\) | (a high-spin complex) \((\mathbf{c})\left[\mathrm{Ru}(\mathrm{bipy})_{3}\right]^{3+}\) (a low-spin complex), \((\mathbf{d})\left[\mathrm{NiCl}_{4}\right]^{2-}\) (tetrahedral), ( e) \(\left[\mathrm{PtBr}_{6}\right]^{2-},(\mathbf{f})\left[\mathrm{Ti}(\mathrm{en})_{3}\right]^{2+}\).

As shown in Figure 23.26, the \(d-d\) transition of \(\left[\mathrm{Ti}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) produces an absorption maximum at a wavelength of about 500 \(\mathrm{nm}\) . (a) What is the magnitude of \(\Delta\) for \(\left[\mathrm{Ti}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) in \(\mathrm{kJ} / \mathrm{mol} ?\) (b) How would the magnitude of \(\Delta\)change if the \(\mathrm{H}_{2} \mathrm{O}\) ligands in \(\left[\mathrm{Ti}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) were replaced with \(\mathrm{NH}_{3}\) ligands?

Indicate the coordination number and the oxidation number of the metal for each of the following complexes: (a) \(\mathrm{Na}_{2}\left[\mathrm{CdCl}_{4}\right]\) (b) \(\mathrm{K}_{2}\left[\mathrm{MoOCl}_{4}\right]\) (c) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right] \mathrm{Cl}\) (d) \(\left[\mathrm{Ni}(\mathrm{CN})_{5}\right]^{3-}\) (e) \(\mathrm{K}_{3}\left[\mathrm{V}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}\right]\) (f) \(\left[\mathrm{Zn}(\mathrm{en})_{2}\right] \mathrm{Br}_{2}\)

Which type of substance is attracted by a magnetic field, a diamagnetic substance or a paramagnetic substance?
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