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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. Weak-field ligands cause a small splitting of the d-orbital energy levels in a transition-metal complex, making it energetically favorable for electrons to occupy higher energy orbitals rather than pairing up in the same orbital. This leads to the formation of high-spin complexes, which follow Hund's rule and have a greater number of unpaired electrons.

Step by step solution

01

Understanding Weak-field Ligands and High-spin Complexes

Weak-field ligands are those that cause a small splitting of the d-orbital energy levels in a transition-metal complex. In such a complex, the difference in energy between the d-orbitals is small, and it becomes easy for electrons to be promoted to higher energy orbitals. High-spin complexes are those in which the electrons of a transition-metal complex occupy all available energy levels (orbitals) before going into a double-occupancy state (i.e., two electrons with opposite spins in the same orbital). This behavior follows Hund's rule, which states that for a given electron configuration, the term with maximum multiplicity (greatest number of unpaired electrons) has the lowest energy.
02

Connecting Weak-field Ligands and High-spin Complexes

Weak-field ligands lead to a smaller splitting of d-orbitals, meaning that the energy difference between the orbitals is less significant. Consequently, it becomes energetically favorable for electrons to move up to the higher energy orbital rather than pairing with another electron in the same orbital. This results in the formation of high-spin complexes, with more unpaired electrons occupying the available orbitals.
03

Assessing the Classmate's Statement

The classmate's statement is indeed correct. Generally, weak-field ligands are associated with high-spin complexes, which means that they cause a small splitting of the d-orbital energy levels. As a result, electrons can easily be promoted to higher energy orbitals, giving rise to high-spin complexes with more unpaired electrons occupying the available orbitals according to Hund's rule.

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Most popular questions from this chapter

Consider the following three complexes: \(\left(\right.\) Complex 1) $\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Br}_{2}\right] \mathrm{Cl}$ 2) \(\left[\mathrm{Pd}\left(\mathrm{NH}_{3}\right)_{2}(\mathrm{ONO})_{2}\right]\) (Complex (Complex 3) $\left[\mathrm{V}(\mathrm{en})_{2} \mathrm{Cl}_{2}\right]^{+},$ Which of the three complexes can have (a) geometric isomers, (b) linkage isomers, (c) optical isomers, (d) coordinationsphere isomers?

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?

An iron complex formed from a solution containing hydrochloric acid and bipyridine is purified and analyzed. It contains $9.38 \% \mathrm{Fe}, 60.53 \%\( carbon, \)4.06 \%\( hydrogen, and \)14.12 \%$ nitrogen by mass. The remainder of the compound is chlorine. An aqueous solution of the complex has about the same electrical conductivity as an equimolar solution of \(\mathrm{K}_{2}\left[\mathrm{CuCl}_{4}\right] .\) Write the formula of the compound, using brackets to denote the iron and its coordination sphere.

The complexes \(\left[\mathrm{CrBr}_{6}\right]^{3-}\) and \(\left[\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}\) are both known. (a) Draw the \(d\) -orbital energy-level diagram for octahedral \(\mathrm{Cr}(\mathrm{III})\) complexes. (b) What gives rise to the colors of these complexes? (c) Which of the two complexes would you expect to absorb light of higher energy?

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