Logout Open In App
Open In App
Warning: foreach() argument must be of type array|object, bool given in /var/www/html/web/app/themes/studypress-core-theme/template-parts/header/mobile-offcanvas.php on line 20

Chapter 7: Question 48 E (page 398)

In terms of the bonds present, explain why acetic acid, \(C{H_3}C{O_2}H\), contains two distinct types of carbon-oxygen bonds, whereas the acetate ion, formed by loss of a hydrogen ion from acetic acid, only contains one type of carbon-oxygen bond. The skeleton structures of these species are shown:

Short Answer

Expert verified

Acetic acid, \(C{H_3}C{O_2}H\), contains two distinct types of carbon-oxygen bonds, whereas the acetate ion, only contains one type of carbon-oxygen bond as there is resonance happening in acetate ion.

Step by step solution

01

Concept Introduction

Chemical bonding is a formation of chemical compound by initiating a chemical link between two or more atoms, molecules, or ions. The atoms in the consequent molecule are retained together by chemical bonds.

02

Bonds in Acetic Acid and Acetate Ion

The acetic acid molecule contains a\({\rm{C - O}}\)double bond and a\({\rm{C - O}}\)single bond.

There is resonance happening in case of acetate ion and it is described by two resonance structures that average the two\({\rm{C - O}}\)bonds.

So, it is because of resonance that acetate ion contains only one type of carbon-oxygen bond (average of two\({\rm{C - O}}\)bonds).

Therefore, both the acetate compounds contain different number of bonds due to resonance.

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

Identify the atoms that correspond to each of the following electron configurations. Then, write the Lewis symbol for the common ion formed from each atom: (a)\({\text{1}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{p}}^{\text{5}}}\)(b)\({\text{1}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{p}}^{\text{6}}}{\text{3}}{{\text{s}}^{\text{2}}}\)(c)\({\text{1}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{p}}^{\text{6}}}{\text{3}}{{\text{s}}^{\text{2}}}{\text{3}}{{\text{p}}^{\text{6}}}{\text{4}}{{\text{s}}^{\text{2}}}{\text{3}}{{\text{d}}^{{\text{10}}}}\)(d)\({\text{1}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{p}}^{\text{6}}}{\text{3}}{{\text{s}}^{\text{2}}}{\text{3}}{{\text{p}}^{\text{6}}}{\text{4}}{{\text{s}}^{\text{2}}}{\text{3}}{{\text{d}}^{{\text{10}}}}{\text{4}}{{\text{p}}^{\text{4}}}\)(e)\({\text{1}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{p}}^{\text{6}}}{\text{3}}{{\text{s}}^{\text{2}}}{\text{3}}{{\text{p}}^{\text{6}}}{\text{4}}{{\text{s}}^{\text{2}}}{\text{3}}{{\text{d}}^{{\text{10}}}}{\text{4}}{{\text{p}}^{\text{1}}}\).

Which of the following molecules have dipole moments?

  1. \({\rm{C}}{{\rm{S}}_{\rm{2}}}\)
  2. \({\rm{Se}}{{\rm{S}}_{\rm{2}}}\)
  3. \({\rm{CC}}{{\rm{l}}_{\rm{2}}}{\rm{\;}}{{\rm{F}}_{\rm{2}}}\)
  4. \({\rm{PC}}{{\rm{l}}_{\rm{3}}}{\rm{(P is the central atom)}}\)
  5. \({\rm{ClNO (N is the central atom)}}\)

How are single, double, and triple bonds similar? How do they differ?

Calculate the formal charge of chlorine in the molecules \({\rm{C}}{{\rm{l}}_{\rm{2}}}\), \({\rm{BeC}}{{\rm{l}}_{\rm{2}}}\), and \({\rm{Cl}}{{\rm{F}}_{\rm{5}}}\).

Question: Using the standard enthalpy of formation data in Appendix G, determine which bond is stronger: the \({\rm{P - Cl}}\) bond in \({\rm{PC}}{{\rm{l}}_{\rm{3}}}{\rm{(g)}}\) or in \({\rm{PC}}{{\rm{l}}_{\rm{5}}}{\rm{(g)}}\)?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Physical Chemistry

Read Explanation

Kinetics

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Reactions

Read Explanation

Inorganic Chemistry

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