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Chapter 11: Problem 1

Indicate several ways in which the valence-bond method is superior to Lewis structures in describing covalent bonds.

Short Answer

Expert verified
The valence-bond method is superior to Lewis structures in several ways. This method accounts for the types of atomic orbital overlaps (sigma and pi bonds) that occur during bond formation. It also emphasizes the spatial orientation of atomic orbitals which is not taken into account in Lewis structures. Thus, providing a more comprehensive and realistic molecular description.

Step by step solution

01

Defining Lewis Structures

Lewis structures, also known as electron dot diagrams, are graphical representations of the bonding between atoms in a molecule and the lone pairs of electrons that may exist in the molecule. It clearly shows the number of valence electrons in each atom, and how these valence electrons participate in bond formation. It is widely used due to its simplicity but has its own set of limitations.
02

Understanding Valence-Bond Theory

The valence-bond method, on the other hand, is a model of covalent bond formation which includes more details, such as the overlapping of atomic orbitals and the types of overlaps resulting in sigma and pi bonds. Unlike Lewis structures, this method includes an understanding of the electronic structure and atomic orbitals.
03

Comparing Lewis Structures with the Valence-Bond Method

Upon comparison, it can be seen that the Valence-bond method provides a more detailed description of covalent bond formation. It accounts for the spatial orientation of the atomic orbitals involved in bonding, and it can explain the formation of sigma and pi bonds in multiple bond situations, which Lewis structures cannot describe accurately. This makes it superior in describing covalent bonds compared to Lewis structures.

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Most popular questions from this chapter

Explain why the concept of delocalized molecular orbitals is essential to an understanding of bonding in the benzene molecule, $\mathrm{C}_{6} \mathrm{H}_{6}$

Explain why the molecular structure of \(\mathrm{BF}_{3}\) cannot be adequately described through overlaps involving pure \(s\) and \(p\) orbitals.

Of the following, the species with a bond order of 1 is (a) \(\mathrm{H}_{2}^{+} ;\) (b) \(\mathrm{Li}_{2} ;\) (c) \(\mathrm{He}_{2} ;\) (d) \(\mathrm{H}_{2}^{-}\)

Construct the molecular orbital diagram for CaF. Would you expect the bond length of \(\mathrm{CaF}^{+}\) to be longer or shorter than that of CaF?

Explain how it is possible to avoid the concept of resonance by using molecular orbital theory.
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