/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 18 An \(\mathrm{AB}_{3}\) molecule ... [FREE SOLUTION] | 91影视

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Chapter 9: Problem 18

An \(\mathrm{AB}_{3}\) molecule is described as having a trigonalbipyramidal electron-domain geometry. How many nonbonding domains are on atom A? Explain.

Short Answer

Expert verified
In an AB3 molecule with a trigonal bipyramidal electron-domain geometry, there are 2 nonbonding electron domains on atom A. This is because there are 3 bonding domains (B atoms) and a total of 5 electron domains required for the trigonal bipyramidal geometry, which results in the difference of 2 nonbonding electron domains for the central atom A.

Step by step solution

01

Understand the trigonal bipyramidal geometry

First, let's have a quick understanding of trigonal bipyramidal geometry. In this geometry, there are five electron domains around the central atom (A). Three of these domains lie in the same plane and are referred to as the equatorial domains, while the other two are perpendicular to this plane and lie above and below (referred to as axial domains).
02

Determine the total electron domains for atom A

In an AB3 molecule with a trigonal bipyramidal geometry, there are three bonding domains (B atoms) connected to the central atom A. This implies that there are at least three electron domains around atom A.
03

Determine the number of nonbonding electron domains on atom A

To reach five electron domains (the number required for a trigonal bipyramidal geometry), we need to consider the presence of nonbonding electron domains. The difference between the total number of electron domains in trigonal bipyramidal geometry (5) and the number of bonding electron domains we have in AB3 (3) will give us the number of nonbonding electron domains. 5 total electron domains - 3 bonding electron domains = 2 nonbonding electron domains
04

Conclusion

There are 2 nonbonding electron domains on atom A in this AB3 molecule with a trigonal bipyramidal electron-domain geometry. The presence of these nonbonding electron domains is necessary to achieve the desired geometry around the central atom (A).

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Most popular questions from this chapter

Consider the molecule \(\mathrm{PF}_{4} \mathrm{Cl}\). (a) Draw a Lewis structure for the molecule, and predict its electron-domain geometry. (b) Which would you expect to take up more space, a. \(\mathrm{P}-\mathrm{F}\) bond or a \(\mathrm{P}-\mathrm{Cl}\) bond? Explain. (c) Predict the molecular geometry of \(\mathrm{PF}_{4} \mathrm{Cl}\). How did your answer for part (b) influence your answer here in part (c)? (d) Would you expect the molecule to distort from its ideal electron-domain geometry? If so, how would it distort?

You can think of the bonding in the \(\mathrm{Cl}_{2}\) molecule in several ways. For example, you can picture the Cl- -Cl bond containing two electrons that each come from the \(3 p\) orbitals of a \(\mathrm{Cl}\) atom that are pointing in the appropriate direction. However, you can also think about hybrid orbitals. (a) Draw the Lewis structure of the \(\mathrm{Cl}_{2}\) molecule. (b) What is the hybridization of each \(\mathrm{Cl}\) atom? (c) What kind of orbital overlap, in this view, makes the Cl- -Cl bond? (d) Imagine if you could measure the positions of the lone pairs of electrons in \(\mathrm{Cl}_{2}\). How would you distinguish between the atomic orbital and hybrid orbital models of bonding using that knowledge? (e) You can also treat \(\mathrm{Cl}_{2}\) using molecular orbital theory to obtain an energy level diagram similar to that for \(\mathrm{F}_{2}\). Design an experiment that could tell you if the MO picture of \(\mathrm{Cl}_{2}\) is the best one, assuming you could easily measure bond lengths, bond energies, and the light absorption properties for any ionized species.

(a) What is the difference between a localized \(\pi\) bond and a delocalized one? (b) How can you determine whether a molecule or ion will exhibit delocalized \(\pi\) bonding? (c) Is the \(\pi\) bond in \(\mathrm{NO}_{2}^{-}\) localized or delocalized?

(a) What does the term diamagnetism mean? (b) How does a diamagnetic substance respond to a magnetic field? (c) Which of the following ions would you expect to be diamagnetic: \(\mathrm{N}_{2}{ }^{2-}, \mathrm{O}_{2}{ }^{2-}, \underline{\mathrm{Be}_{2}}^{2+}, \mathrm{C}_{2}{ }^{-} ?\)

(a) The \(\mathrm{PH}_{3}\) molecule is polar. How does this offer experimental proof that the molecule cannot be planar? (b) It tums out that ozone, \(\mathrm{O}_{3}\), has a small dipole moment. How is this possible, given that all the atoms are the same?
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