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Chapter 23: Problem 11

Discuss the factors affecting the magnitude of crystal field splitting.

Short Answer

Expert verified
The crystal field splitting is primarily affected by four factors: the metal ion's nature, including its charge; the type of ligands attached to the metal ion as per the spectrochemical series; the geometry of the complex; and the degree of orbital overlap with ligands.

Step by step solution

01

Understand Crystal Field Theory

The crystal field theory is a model used in inorganic chemistry to describe the electronic structure of transition metal complexes. The name 'crystal field' comes from the idea that the ions in a crystal lattice create an electric field that affects the energy of the five d-orbitals. It is the splitting of these d-orbitals when transitioning metal ions are in a complex that we refer to as 'crystal field splitting.'
02

Discuss the Nature of the Metal Ion

The first factor affecting the crystal field splitting is the nature of the metal ion. The magnitude of the splitting is larger for metal ions with a greater positive charge, because they pull the negatively charged ligands more strongly and cause greater splitting of the d-orbitals.
03

Discuss the Nature of the Ligands

Another essential factor is the type of ligand bounding to the metal ion. Different ligands cause different amounts of splitting. This is called the spectrochemical series, where stronger-field ligands cause greater splitting, while weaker-field ligands cause less splitting.
04

Consider the Geometry of the Complex

The geometry of the complex also affects the degree of splitting. Octahedral complexes, for example, experience splitting into two sets of orbitals (three below and two above), whereas in tetrahedral complexes (inverted variant of octahedral), the splitting results in two orbitals below and three above. Different complex geometries lead to variations in crystal field splitting.
05

Consider Orbital Overlap

The last factor is the overlap between the d-orbitals of the metal and the ligands' orbitals. Greater overlap leads to greater splitting because the interactions between the positively charged metal ion and negatively charged ligand are stronger.

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Most popular questions from this chapter

Discuss the crystal field splitting in a square planar complex.

Draw molecular orbital diagram of a square planar complex showing only \(\pi\) -bonding.

Explain the following: (a) \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) is paramagnetic and coloured. (b) \(\left(\mathrm{Ni}(\mathrm{CN})_{4}\right)^{2-}\) is square planar, but \(\left[\mathrm{Ni}(\mathrm{Cl})_{4}\right]^{2-}\) is tetrahedral. (c) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}\) is more stable than \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{2+}\), while \(\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) is more stable than \(\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) (d) Octahedral complexes are less stable than the square planar complexes. (e) \(\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3-}\) is a low-spin complex, but \(\left[\mathrm{CoF}_{6}\right]^{3-}\) is high-spin complex.

What are the limitations of valence bond theory?

Discuss the salient features of ligand field theory. How does it differ from crystal field theory?
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