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Chapter 23: Problem 12

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

Short Answer

Expert verified
Ligand Field Theory (LFT) focuses on molecular orbitals and covalent interactions for a more detailed picture of metal-ligand bonding. Crystal Field Theory (CFT) sees ligands as point charges with electrostatic interactions. Thus, while both are used to explain bonding in coordination complexes, they approach the interaction differently - CFT uses an electrostatic model, while LFT uses a model based on molecular orbitals.

Step by step solution

01

Title: Explain Ligand Field Theory

Ligand Field Theory (LFT) is a model used in inorganic chemistry to explain the bonding and properties of coordination complexes. It takes into account the understanding of molecular orbitals and overlaps them with the d-orbitals of the metal ion and the ligand orbitals to form bonding, non-bonding, and anti-bonding orbitals.
02

Title: Explain Crystal Field Theory

Crystal Field Theory (CFT) is a model in which the interaction between a central metal ion and its surrounding ligands is explained by the points of negative charges. In this model, these negatively charged points are directly arranged towards the central metal ion leading to the splitting of degenerate d-orbitals into two different energy levels.
03

Compare and Contrast LFT and CFT

The main difference between Ligand Field Theory and Crystal Field Theory is their approach in treating the metal-ligand interaction. In Crystal Field Theory, the ligands are considered as point charges and only electrostatic interactions are considered. In contrast, Ligand Field Theory goes beyond this and treats the metal-ligand interaction covalently and takes into account the overlap of molecular orbitals. Therefore, the Ligand Field Theory provides a more accurate and detailed picture of the metal-ligand bonding.

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Most popular questions from this chapter

Discuss Sidgwick's concept of effective atomic number with the help of suitable example.

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.

How does crystal field theory differ from valence bond theory?

What are the limitations of valence bond theory?

Discuss in brief the crystal field theory and represent the splitting of ' \(d\) ' orbitals in octahedral and tetrahedral fields.
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