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Chapter 9: Problem 75

(a) What is the physical basis for the VSEPR model? (b) When applying the VSEPR model, we count a double or triple bond as a single electron domain. Why is this justified?

Short Answer

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(a) The physical basis of the VSEPR model is the repulsion between electron pairs (both bonding pairs and lone pairs) around a central atom in a molecule due to their negative charges. The model predicts the geometric shape of a molecule by minimizing this repulsion. (b) Double or triple bonds are counted as a single electron domain in VSEPR because, despite the presence of additional pi bonds, the electron density remains localized and concentrated in the same region between the two bonded atoms. This electron density effectively causes repulsion in that specific region and does not increase the overall repulsive effect in other directions.

Step by step solution

01

(a) Physical Basis for VSEPR Model

The VSEPR (Valence Shell Electron Pair Repulsion) model is based on the idea that the electron pairs (both bonding pairs and lone pairs) around a central atom in a molecule will repel each other and try to move as far apart as possible. This repulsion is a result of the electron pairs' negative charges. The VSEPR model aims to predict the geometric shape of the molecule by minimizing this repulsion between electron pairs.
02

(b1) Understanding Single and Multiple Bonds

A single bond consists of one sigma bond formed by the head-on overlap of atomic orbitals between two atoms. A double bond consists of one sigma bond and one pi bond formed by the sideways overlap of atomic orbitals, while a triple bond is made up of one sigma bond and two pi bonds. It's important to understand that while multiple bonds involve more than one bonding interaction, they still occur between just two atoms.
03

(b2) Justifying Counting Multiple Bonds as a Single Domain

In VSEPR model, the electron domain represents a region of electron density. In both single and multiple bonds, this electron density lies between the two atoms involved in bonding. Despite the presence of additional pi bonds in double or triple bonds, the electron density remains localized and concentrated in the same region between the two bonded atoms. We can consider this electron density as a single domain because it effectively causes repulsion only in that particular region and does not increase the overall repulsive effect in other directions. Hence, counting a double or triple bond as a single electron domain is justified in the VSEPR model.

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Most popular questions from this chapter

Draw a picture that shows all three \(2 p\) orbitals on one atom and all three \(2 p\) orbitals on another atom. (a) Imagine the atoms coming close together to bond. How many \(\sigma\) bonds can the two sets of \(2 p\) orbitals make with each other? (b) How many \(\pi\) bonds can the two sets of \(2 p\) orbitals make with each other? (c) How many antibonding orbitals, and of what type, can be made from the two sets of \(2 p\) orbitals?

Shown below are three pairs of hybrid orbitals, with each set at a characteristic angle. For each pair, determine the type or types of hybridization that could lead to hybrid orbitals at the specified angle. |Section 9.5]

The azide ion, \(\mathrm{N}_{3}^{-}\), is linear with two \(\mathrm{N}-\mathrm{N}\) bonds of equal length, \(1.16 \mathrm{~A}\) (a) Draw a Lewis structure for the azide ion. (b) With reference to Table \(8.5\), is the observed \(\mathrm{N}-\mathrm{N}\) bond length consistent with your Lewis structure? (c) What hybridization scheme would you expect at each of the nitrogen atoms in \(\mathrm{N}_{3}^{-} ?\) (d) Show which hybridized and unhybridized orbitals are involved in the formation of \(\sigma\) and \(\pi\) bonds in \(\mathrm{N}_{3}^{-} .(\mathrm{e}) \mathrm{It}\) is often observed that \(\sigma\) bonds that involve an sp hybrid orbital are shorter than those that involve only \(s p^{2}\) or \(s p^{3}\) hybrid orbitals. Can you propose a reason for this? Is this observation applicable to the observed bond lengths in \(\mathrm{N}_{3}^{-}\) ?

The phosphorus trihalides \(\left(\mathrm{PX}_{3}\right)\) show the following variation in the bond angle \(\mathrm{X}-\mathrm{P}-\mathrm{X}: \mathrm{PF}_{3}, 96.3^{\mathrm{a}} ; \mathrm{PCl}_{3}\) \(100.3^{\circ} ; \mathrm{PBr}_{3}, 101.0^{\circ} ; \mathrm{Pl}_{3}, 102.0^{\circ} .\) The trend is generally at- tributed to the change in the electronegativity of the halogen. (a) Assuming that all electron domains are the same size, what value of the \(\mathrm{X}-\mathrm{P}-\mathrm{X}\) angle is predicted by the VSEPR model? (b) What is the general trend in the \(\mathrm{X}-\mathrm{P}-\mathrm{X}\) angle as the electronegativity increases? (c) Using the VSEPR model, explain the observed trend in \(X-P-X\) angle as the electronegativity of \(X\) changes. (d) Based on your answer to part (c), predict the structure of \(\mathrm{PBrCI}_{4}\)

Give the electron-domain and molecular geometries of a molecule that has the following electron domains on its central atom: (a) four bonding domains and no nonbonding domains, (b) three bonding domains and two nonbonding domains, (c) five bonding domains and one nonbonding domain, (e) four bonding domains and two nonbonding domains.
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