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Chapter 9: Problem 17

Use the localized electron model to describe the bonding in \(\mathrm{H}_{2} \mathrm{O}\).

Short Answer

Expert verified
In H鈧侽, the bonding can be described using the localized electron model as follows: the molecule has a bent molecular geometry with an H-O-H bond angle of approximately 104.5掳 and the central oxygen atom exhibits sp鲁 hybridization. The O-H bonds are 蟽 bonds formed due to the head-on overlap of orbitals.

Step by step solution

01

Determine the Lewis structure

First, we need to find out the total number of valence electrons in the H鈧侽 molecule. Oxygen has 6 valence electrons, while hydrogen has 1 valence electron each. Thus, we have a total of 8 valence electrons (6 from oxygen and 2 from the two hydrogen atoms). Now, we will place the oxygen atom in the center and two hydrogen atoms on either side of it. Distributing the valence electrons in the molecule, we give 2 electrons to each H-O bond (totaling 4 electrons) and the remaining 4 electrons are distributed as lone pairs on the oxygen atom. The Lewis structure is as follows: O / \ H - H
02

Determine the molecular geometry and bond angles

The molecular geometry of a molecule can be identified using the Valence Shell Electron Pair Repulsion (VSEPR) theory. H鈧侽 has 2 bonding electron pairs (between O and H atoms) and 2 lone electron pairs on the central oxygen atom. This corresponds to an AX鈧侲鈧� (A = central atom, X = atoms bonded to central atom, E = lone electron pairs) geometry in the VSEPR model with molecular geometry being bent (angular). The bond angle (H-O-H) in H鈧侽 is approximately 104.5掳. This is less than the ideal bond angle of 109.5掳 in a tetrahedral geometry due to the repulsion between the lone electron pairs on the central oxygen atom, which compresses the H-O-H bond angle.
03

Determine the hybridization of the central atom

To identify the hybridization of the central oxygen atom, we need to look at the number of electron domains (regions of electron density) around the atom. In the case of H鈧侽, there are 4 electron domains (2 bonding pairs and 2 lone pairs). Hence, the oxygen atom exhibits sp鲁 hybridization.
04

Identify the type of chemical bonds (蟽 and 蟺 bonds)

In H鈧侽, there are two O-H bonds. Each of these bonds is formed by the overlap of orbitals, one from the oxygen atom and one from the hydrogen atom. The sigma (蟽) bond is formed by the axial head-on overlap of orbitals, which is the case for both O-H bonds in H鈧侽. Since there is no sideways overlap of orbitals to form additional, parallel bonds (蟺 bonds), both O-H bonds are solely classified as 蟽 bonds. In conclusion, using the localized electron model, we can describe the bonding in H鈧侽 as follows: H鈧侽 has a bent molecular geometry, with an H-O-H angle of 104.5掳, and the central oxygen atom exhibits sp鲁 hybridization. The O-H bonds are 蟽 bonds formed due to the head-on overlap of orbitals.

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Most popular questions from this chapter

Using molecular orbital theory, explain why the removal of one electron in \(\mathrm{O}_{2}\) strengthens bonding, while the removal of one electron in \(\mathrm{N}_{2}\) weakens bonding.

\(\mathrm{FClO}_{2}\) and \(\mathrm{F}_{3} \mathrm{ClO}\) can both gain a fluoride ion to form stable anions. \(\mathrm{F}_{3} \mathrm{ClO}\) and \(\mathrm{F}_{3} \mathrm{ClO}_{2}\) will both lose a fluoride ion to form stable cations. Draw the Lewis structures and describe the hybrid orbitals used by chlorine in these ions.

Use the MO model to explain the bonding in \(\mathrm{BeH}_{2}\). When constructing the MO energy-level diagram, assume that the Be's \(1 s\) electrons are not involved in bond formation.

For each of the following molecules or ions that contain sulfur, write the Lewis structure(s), predict the molecular structure (including bond angles), and give the expected hybrid orbitals for sulfur. a. \(\mathrm{SO}_{2}\) b. \(\mathrm{SO}_{3}\) e. \(\mathrm{SO}_{3}^{2-}\) f. \(\mathrm{SO}_{4}^{2-}\) g. \(\mathrm{SF}_{2}\) h. \(\mathrm{SF}_{4}\) i. \(\mathrm{SF}_{6}\) j. \(\mathrm{F}_{3} \mathrm{~S}-\mathrm{SF}\) k. \(\mathrm{SF}_{5}{ }^{+}\)

Determine the molecular structure and hybridization of the central atom \(\mathrm{X}\) in the polyatomic ion \(\mathrm{XY}_{3}{ }^{+}\) given the following information: A neutral atom of \(X\) contains 36 electrons, and the element Y makes an anion with a 1 - charge, which has the electron configuration \(1 s^{2} 2 s^{2} 2 p^{6}\).
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