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Chapter 24: Problem 8

What are the limitations of valence bond theory?

Short Answer

Expert verified
The primary limitations of Valence Bond Theory include its inability to explain the shapes of molecules, the limitation of electron pair sharing to two atoms, and ineffective contrasting of sigma and pi bonds.

Step by step solution

01

Identifying Limitation #1 - Molecular Shapes

Valence Bond Theory was unable to explain the shapes of molecules. This is due to the theory's focus on the overlapping of orbitals, which doesn't account for how those orbitals orient themselves in space to form distinct molecular shapes.
02

Identifying Limitation #2 - Restrictions on Electron Pair-Sharing

The theory assumes that covalent bond formation involves the sharing of electron pairs only between two atoms. However, there are certain situations where electrons are delocalized or shared by more than two atoms. This phenomenon isn't explained by Valence Bond Theory.
03

Identifying Limitation #3 - Sigma and Pi Bonds

The theory is not very effective in contrasting the different properties of Sigma and Pi bonds. In reality, sigma (σ) bonds are directional and stronger, while pi (π) bonds are weaker and more diffused, but the theory does not make this distinction clear.

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Most popular questions from this chapter

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

Discuss the molecular orbital diagram of a tetrahedral complex with the help of a suitable example.

Discuss the factors affecting the magnitude of crystal field splitting.

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 ligand field theory describe the origin of charge transfer spectra in coordination complexes.
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