Ch.9 - Molecular Geometry and Bonding Theories

Brown - Chemistry: The Central Science 14th Edition

Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook

Brown 14th Edition

Ch.9 - Molecular Geometry and Bonding Theories

Problem 101

Chapter 9, Problem 101

For one of the resonance forms of ozone, O3, which of the orbitals are used to make bonds and which are used to hold nonbonding pairs of electrons?

Name: Chemistry: The Central Science
Author: Brown
ISBN: 9780134414232

Verified step by step guidance

Identify the molecular structure of ozone (O3), which consists of three oxygen atoms arranged in a bent shape.

Recognize that ozone has resonance structures, meaning that the actual structure is a hybrid of multiple possible structures.

In one resonance form, consider the central oxygen atom forming a double bond with one of the terminal oxygen atoms and a single bond with the other terminal oxygen atom.

Determine that the sigma (σ) bonds are formed using sp2 hybrid orbitals on the central oxygen atom, while the pi (π) bond is formed using unhybridized p orbitals.

Identify that the nonbonding pairs of electrons (lone pairs) on the central oxygen atom are held in the remaining sp2 hybrid orbitals.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Resonance Structures

Resonance structures are different ways of drawing the same molecule that illustrate the delocalization of electrons. In ozone (O3), resonance forms show how the double bond can shift between the oxygen atoms, affecting the distribution of electrons. Understanding resonance is crucial for predicting molecular behavior and stability.

Molecular Orbitals

Molecular orbitals are formed by the combination of atomic orbitals when atoms bond together. In ozone, the bonding involves the overlap of p orbitals from the oxygen atoms, which create bonding and antibonding molecular orbitals. Recognizing which orbitals participate in bonding versus those that hold lone pairs is essential for understanding the molecule's structure.

Lone Pairs and Bonding Pairs

Lone pairs are pairs of valence electrons that are not involved in bonding, while bonding pairs are shared between atoms to form covalent bonds. In ozone, certain p orbitals are occupied by lone pairs, influencing the molecule's geometry and reactivity. Identifying these pairs helps in visualizing the electron distribution and predicting molecular properties.

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Related Practice

Textbook Question

Sodium azide is a shock-sensitive compound that releases N2 upon physical impact. The compound is used in automobile airbags. The azide ion is N3-. (a) Draw the Lewis structure of the azide ion that minimizes formal charge (it does not form a triangle). Is it linear or bent?

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Textbook Question

Butadiene, C4H6, is a planar molecule that has the following carbon–carbon bond lengths:

(b) From left to right, what is the hybridization of each carbon atom in butadiene?

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Textbook Question

(b) The anion IO₄^- has a tetrahedral structure: three oxygen atoms form double bonds with the central iodine atom and one oxygen atom which carries a negative charge forms a single bond. Predict the molecular geometry of IO₆^5-.

Textbook Question

Sodium azide is a shock-sensitive compound that releases N2 upon physical impact. The compound is used in automobile airbags. The azide ion is N3-. (b) State the hybridization of the central N atom in the azide ion.

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Textbook Question

Butadiene, C4H6, is a planar molecule that has the following carbon–carbon bond lengths:

(a) Predict the bond angles around each of the carbon atoms and sketch the molecule.

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Textbook Question

In ozone, O3, the two oxygen atoms on the ends of the molecule are equivalent to one another. (d) How many electrons are delocalized in the p system of ozone?

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