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Chapter 9: Problem 17

(a) How does one determine the number of electron domains in a molecule or ion? (b) What is the difference between a bonding electron domain and a nonbonding electron domain?

Short Answer

Expert verified
To determine the number of electron domains in a molecule or ion, first, identify the central atom and count the electron regions around it, including single, double, or triple bonds and lone pairs. A bonding electron domain is a region of electron density involved in covalent bonds between atoms (single, double, or triple bonds). In contrast, a nonbonding electron domain is a region of electron density not involved in bonding between atoms, typically as lone pairs or unshared pairs of electrons on the central atom.

Step by step solution

01

(a) Determining the number of electron domains in a molecule or ion

To determine the number of electron domains in a molecule or ion, first, identify the central atom. Then, count the regions around the central atom where electrons are found, keeping in mind that these electrons can be involved in bonding (either single, double, or triple bonds) or present as lone pairs. An electron domain can be: 1. A single bond (e.g., in CH4, the bond between C and each H counts as an electron domain) 2. A double bond (e.g., in CO2, each double bond between C and O counts as a single electron domain) 3. A triple bond (e.g., in N2, the triple bond between the two N atoms counts as a single electron domain) 4. A lone pair (e.g., in NH3, the lone pair on N counts as an electron domain) The total number of such electron domains gives us the electron-domain geometry of the molecule.
02

(b) Difference between a bonding and nonbonding electron domain

A bonding electron domain is a region of electron density that is involved in covalent bonds between atoms, which can be single, double, or triple bonds. In each case, the bonding electron domain counts as one region of electron density, regardless of the number of bonds involved. A nonbonding electron domain, on the other hand, is a region of electron density that is not involved in bonding between atoms. These are usually in the form of lone pairs or unshared pairs of electrons on the central atom. The presence of nonbonding electron domains can influence the shape of the molecule as they can cause repulsion with the bonding electron domains.

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Most popular questions from this chapter

Antibonding molecular orbitals can be used to make bonds to other atoms in a molecule. For example, metal atoms can use appropriate \(d\) orbitals to overlap with the \(\pi_{2 p}^{*}\) orbitals of the carbon monoxide molecule. This is called \(d-\pi\) backbonding. (a) Draw a coordinate axis system in which the \(y\)-axis is vertical in the plane of the paper and the \(x\)-axis horizontal. Write " \(\mathrm{M}^{"}\) at the origin to denote a metal atom. (b) Now, on the \(x\) axis to the right of \(M\), draw the Lewis structure of a CO molecule, with the carbon nearest the \(M\). The CO bond axis should be on the \(x\)-axis. (c) Draw the \(\mathrm{CO} \pi_{2 p}^{*}\) orbital, with phases (see the "Closer Look" box on phases) in the plane of the paper. Two lobes should be pointing toward M. (d) Now draw the \(d_{x y}\) orbital of \(\mathrm{M}\), with phases. Can you see how they will overlap with the \(\pi_{2}^{*}\) orbital of \(\mathrm{CO}\) ? (e) What kind of bond is being made with the orbitals between \(M\) and \(\mathrm{C}_{,} \sigma\) or \(\pi\) ? (f) Predict what will happen to the strength of the CO bond in a metal\(\mathrm{CO}\) complex compared to \(\mathrm{CO}\) alone.

How does a trigonal pyramid differ from a tetrahedron so far as molecular geometry is concerned?

The energy-level diagram in Figure 9.36 shows that the sideways overlap of a pair of porbitals produces two molecular orbitals, one bonding and one antibonding. In ethylene there is a pair of electrons in the bonding \(\pi\) orbital between the two carbons. Absorption of a photon of the appropriate wavelength can result in promotion of one of the bonding electrons from the \(\pi_{2 p}\) to the $\pi_{2 p}^{\star}$ molecular orbital. (a) Assuming this electronic transition corresponds to the HOMO-LUMO transition, what is the HOMO in ethylene? (b) Assuming this electronic transition corresponds to the HOMO-LUMO transition, what is the LUMO in ethylene? (c) Is the C-Cbond in ethylene stronger or weaker in the excited state than in the ground state? Why? (d) Is the \(C-C\) bond in ethylene easier to twist in the ground state or in the excited state?

{An} \mathrm{} \mathrm{AB}_{3}$ molecule is described as having a trigonal- bipyramidal electron-domain geometry. (a) How many nonbonding domains are on atom A? (b) Based on the information given, which of the following is the molecular geometry of the molecule: (i) trigonal planar, (ii) trigonal pyramidal, (iii) T-shaped, or (iv) tetrahedral?

Draw the Lewis structure for each of the following molecules or ions, and predict their electron-domain and molecular geometries: (a) \(\mathrm{AsF}_{3}\), (b) \(\mathrm{CH}_{3}^{+}\), (c) \(\mathrm{BrF}_{3}\), (d) \(\mathrm{ClO}_{3}^{-}\), (e) \(\mathrm{XeF}_{2}\), (f) \(\mathrm{BrO}_{2}^{-}\).
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