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Chapter 10: Problem 67

Briefly compare the VSEPR and hybridization approaches to the study of molecular geometry.

Short Answer

Expert verified
The VSEPR and hybridization theories both tackle molecular geometry, albeit using different lenses. VSEPR theory is based on the repulsion between the pairs of electrons surrounding a central atom, thus predicting the 3D shape of the molecules. In contrast, hybridization is concerned with how atomic orbitals mix and form newly hybridized orbitals, exerting influence over the shape and properties of molecules. Hence, while VSEPR is more spatial, hybridization provides a more atomic perspective.

Step by step solution

01

Define VSEPR

The VSEPR theory is a model used to predict the geometry of individual molecules from the number of electron pairs surrounding central atoms. This theory posits that electron pairs, bound or unbound, in the outermost shells of atoms, or valence shells, extend outwards from the central atom and repel each other. These repulsions result in the unique 3D shape or geometry of a molecule.
02

Define Hybridization

Hybridization in chemistry refers to the idea that atomic orbitals fuse to form newly hybridized orbitals, which influence the shape and reactivity of the molecules. These new orbitals result from the mixing of at least two nonequivalent atomic orbitals (s-orbitals, p-orbitals, d-orbitals) from the same atom.
03

Compare both approaches

While both theories are used in the explanation of molecular geometry, their approaches are different. The VSEPR theory is more about spatial considerations. It looks at electron pairs as they repel each other, leading to the formation of the molecular shape. The Hybridization Theory, on the other hand, is more atomic-level focused. It is concerned with the blending or mixing of individual atomic orbitals to form new hybrid orbitals. In essence, it helps to explain how atomic orbitals blend to accommodate the shape and bonding of molecules.

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Most popular questions from this chapter

What is the angle between these two hybrid orbitals on the same atom? (a) \(s p\) and \(s p\) hybrid orbitals, (b) \(s p^{2}\) and \(s p^{2}\) hybrid orbitals, (c) \(s p^{3}\) and \(s p^{3}\) hybrid orbitals.

Define these terms: bonding molecular orbital, antibonding molecular orbital, pi molecular orbital, sigma molecular orbital.

Predict the geometries of these species: (a) \(\mathrm{AlCl}_{3}\) (b) \(\mathrm{ZnCl}_{2},\) (c) \(\mathrm{ZnCl}_{4}^{2-}\)

Draw the Lewis structure of ketene \(\left(\mathrm{C}_{2} \mathrm{H}_{2} \mathrm{O}\right)\) and describe the hybridization states of the \(\mathrm{C}\) atoms. The molecule does not contain \(\mathrm{O}-\mathrm{H}\) bonds. On separate diagrams, sketch the formation of sigma and pi bonds.

The allene molecule \(\mathrm{H}_{2} \mathrm{C}=\mathrm{C}=\mathrm{CH}_{2}\) is linear (the three \(\mathrm{C}\) atoms lie on a straight line). What are the hybridization states of the carbon atoms? Draw diagrams to show the formation of sigma bonds and pi bonds in allene.
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