Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 9: Problem 14

The atoms in a single bond can rotate about the internuclear axis without breaking the bond. The atoms in a double and triple bond cannot rotate about the internuclear axis unless the bond is broken. Why?

Short Answer

Expert verified
In summary, single bonds can rotate about the internuclear axis without breaking the bond due to their symmetric electron distribution and the presence of only sigma bonds. On the other hand, double and triple bonds have more complex electron distributions involving pi bonds, which do not allow for free rotation about the internuclear axis without breaking the bond.

Step by step solution

01

Understanding single, double, and triple bonds

In a covalent bond, atoms share electrons to gain stability. A single bond forms when two atoms share one pair of electrons, a double bond forms when two atoms share two pairs of electrons, and a triple bond forms when two atoms share three pairs of electrons. The electron distribution in single, double, and triple bonds plays a crucial role in their flexibility.
02

Electron distribution in single bond

In a single bond, electrons are shared in the form of a sigma bond, which is formed by the direct overlap of atomic orbitals. The electron density is symmetric along the internuclear axis, and this allows the atoms to rotate around the bond without much resistance or change in energy. This is why a single bond can rotate freely about the internuclear axis.
03

Electron distribution in double and triple bonds

In double and triple bonds, the electron distribution is more complex. In addition to the sigma bond present in single bonds, double and triple bonds also involve one or more pi bonds. A pi bond is formed by the parallel overlap of atomic orbitals. The electron cloud is distributed above and below the internuclear axis, causing more electron density and a higher energy state.
04

Double and triple bonds rotation restriction

Unlike single bonds, the electron distribution in double and triple bonds does not allow for rotation about the internuclear axis. The pi bonds rely on the atomic orbitals maintaining fixed orientations relative to each other. If one atom in the bond starts to rotate, the overlap of orbitals forming the pi bond would be disrupted, leading to a rise in energy and the possible breaking of the bond. Hence, atoms in double and triple bonds cannot rotate about the internuclear axis without breaking the bond.
05

Conclusion

In summary, single bonds can rotate about the internuclear axis without breaking the bond due to their symmetric electron distribution and the presence of only sigma bonds. On the other hand, double and triple bonds have more complex electron distributions involving pi bonds, which do not allow for free rotation about the internuclear axis without breaking the bond.

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

A variety of chlorine oxide fluorides and related cations and anions are known. They tend to be powerful oxidizing and fluorinating agents. \(\mathrm{FClO}_{3}\) is the most stable of this group of compounds and has been studied as an oxidizing component in rocket propellants. Draw a Lewis structure for \(\mathrm{F}_{3} \mathrm{ClO}\) , $\mathrm{F}_{2} \mathrm{ClO}_{2}^{+},\( and \)\mathrm{F}_{3} \mathrm{ClO}_{2}$ . What is the molecular structure for each species, and what is the expected hybridization of the central chlorine atom in each compound or ion?

The diatomic molecule OH exists in the gas phase. OH plays an important part in combustion reactions and is a reactive oxidizing agent in polluted air. The bond length and bond energy have been measured to be 97.06 \(\mathrm{pm}\) and 424.7 \(\mathrm{kJ} / \mathrm{mol}\) respectively. Assume that the OH molecule is analogous to the HF molecule discussed in the chapter and that the MOs result from the overlap of a \(p_{z}\) orbital from oxygen and the 1\(s\) orbital of hydrogen (the O-H bond lies along the z axis). a. Draw pictures of the sigma bonding and antibonding molecular orbitals in OH. b. Which of the two MOs has the greater hydrogen 1\(s\) character? c. Can the 2\(p_{x}\) orbital of oxygen form MOs with the 1\(s\) orbital of hydrogen? Explain. d. Knowing that only the 2\(p\) orbitals of oxygen interact significantly with the 1\(s\) orbital of hydrogen, complete the MO energy-level diagram for OH. Place the correct number of electrons in the energy levels. e. Estimate the bond order for OH. f. Predict whether the bond order of \(\mathrm{OH}^{+}\) is greater than, less than, or the same as that of OH. Explain.

Complete the Lewis structures of the following molecules. Predict the molecular structure, polarity, bond angles, and hybrid orbitals used by the atoms marked by asterisks for each molecule. a. \(\mathrm{BH}_{3}\) a. \(\mathrm{BH}_{3}\) b. \(\mathrm{N}_{2} \mathrm{F}_{2}\) c. \(\mathrm{C}_{4} \mathrm{H}_{6}\)

Indigo is the dye used in coloring blue jeans. The term navy blue is derived from the use of indigo to dye British naval uniforms in the eighteenth century. The structure of the indigo molecule is a. How many \(\sigma\) bonds and \(\pi\) bonds exist in the molecule? b. What hybrid orbitals are used by the carbon atoms in the indigo molecule?

Show how a hydrogen 1\(s\) atomic orbital and a fluorine 2\(p\) atomic orbital overlap to form bonding and antibonding molecular orbitals in the hydrogen fluoride molecule. Are these molecular orbitals \(\sigma\) or \(\pi\) molecular orbitals?
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Physical Chemistry

Read Explanation

Kinetics

Read Explanation

Organic Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Analysis

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