Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 9: Problem 11

In the hybrid orbital model, compare and contrast \(\sigma\) bonds with \(\pi\) bonds. What orbitals form the \(\sigma\) bonds and what orbitals form the \(\pi\) bonds? Assume the \(z\) -axis is the internuclear axis.

Short Answer

Expert verified
In the hybrid orbital model, \(\sigma\) bonds are formed by end-to-end overlap of atomic orbitals, such as s-s, s-p, and p-p (specifically p\(_z\)) combinations, while \(\pi\) bonds are formed by side-by-side overlap of p\(_x\) or p\(_y\) orbitals. The \(\sigma\) bond has electron density concentrated along the internuclear axis, while the \(\pi\) bond has two regions of electron density above and below the internuclear axis.

Step by step solution

01

Definition of Sigma and Pi bonds.

A \(\sigma\) bond is a covalent bond formed between two atoms by the end-to-end (head-on) overlapping of their atomic orbitals. This overlapping forms a region of high electron density along the internuclear axis, which is the z-axis in this case. A \(\pi\) bond, on the other hand, is another type of covalent bond formed between two atoms when their atomic orbitals overlap side-by-side. This overlapping creates two regions of high electron density above and below the internuclear axis.
02

Orbitals that form Sigma bonds

In the hybrid orbital model, the atomic orbitals involved in the formation of \(\sigma\) bonds are: 1. s orbitals: An s orbital can overlap with another s orbital head-on, forming an \(\text{s-s}\) \(\sigma\) bond. 2. s and p orbitals: An s orbital can also overlap with a p orbital along the internuclear axis, resulting in an \(\text{s-p}\) \(\sigma\) bond. 3. p orbitals: A p orbital, specifically the one aligned along the z-axis (p\(_z\)), can overlap with another p\(_z\) orbital head-on, creating a \(\text{p-p}\) \(\sigma\) bond.
03

Orbitals that form Pi bonds

In the hybrid orbital model, the atomic orbitals involved in the formation of \(\pi\) bonds are: 1. p orbitals: The p orbitals responsible for forming \(\pi\) bonds are the ones not aligned along the internuclear axis (z-axis). These are the p\(_x\) and p\(_y\) orbitals. They can interact with each other in a side-by-side fashion to form a \(\pi\) bond. In summary, the hybrid orbital model shows that \(\sigma\) and \(\pi\) bonds are formed by different types of atomic orbital overlap. \(\sigma\) bonds are created through end-to-end overlap of orbitals (like s, s-p, p-p), while \(\pi\) bonds are established by side-by-side overlap of p orbitals (p\(_x\) or p\(_y\)).

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

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. $$ \begin{array}{l}{\text { a. } \mathrm{SO}_{2}} \\ {\text { b. } \mathrm{SO}_{3}}\end{array} $$ $$ \text {c} \mathrm{s}_{2} \mathrm{O}_{3}^{2-}\left[\begin{array}{c}{\mathrm{o}} \\\ {\mathrm{s}-\mathrm{s}-\mathrm{o}} \\ {\mathrm{o}} \\\ {\mathrm{o}}\end{array}\right]^{2-} $$ 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. \(\mathrm{SF}_{5}+\)

Sodium can react with oxygen to form sodium peroxide $\left(\mathrm{Na}_{2} \mathrm{O}_{2}\right),\( which is composed of \)\mathrm{Na}^{+}$ and \(\mathrm{O}_{2} 2-\) ions. Potassium can react with oxygen to form potassium superoxide \(\left(\mathrm{KO}_{2}\right)\) which is composed of \(\mathrm{K}^{+}\) and \(\mathrm{O}_{2}-\) ions. Does the peroxide ion or the superoxide ion have the shorter bond length? Explain.

Describe the bonding in the \(\mathrm{CO}_{3}^{2-}\) ion using the localized electron model. How would the molecular orbital model describe the \(\pi\) bonding in this species?

Bond energy has been defined in the text as the amount of energy required to break a chemical bond, so we have come to think of the addition of energy as breaking bonds. However, in some cases the addition of energy can cause the formation of bonds. For example, in a sample of helium gas subjected to a high-energy source, some Holecules exist momentarily and then dissociate. Use MO theory (and diagrams) to explain why He_ molecules can come to exist and why they dissociate.

Use the MO model to explain the bonding in BeH. When con- structing the MO energy-level diagram, assume that the Be's 1 s electrons are not involved in bond formation.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Physical Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Organic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free