Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 6: Problem 13

Discuss Lewis concept of acids and bases.

Short Answer

Expert verified
The Lewis concept of acids and bases is an extension of the traditional definition of acids and bases. It defines a Lewis acid as a species that can accept an electron pair and a Lewis base as a species that can donate an electron pair. This concept includes a wider range of substances that can act as acids or bases. It is useful in explaining a broad range of chemical reactions, including those that do not involve protons, by focusing on the movement of electron pairs.

Step by step solution

01

Define Lewis Acids and Lewis Bases

A Lewis acid is a species that can accept an electron pair, whereas a Lewis base is a species that can donate an electron pair. This concept is much broader than the traditional definition of acids and bases and includes more substances that can act as acids or bases. Except hydrogen ions, other positively charged ions, or cations, can also act as Lewis acids, such as Fe3+ and Al3+. At the same time, molecules with at least one lone pair of electrons can behave as Lewis bases, such as NH3 and H2O.
02

Discuss typical examples of Lewis acid-base reactions

Consider the reaction between NH3 (ammonia) and BF3 (boron trifluoride): \[ BF3 + NH3 \rightarrow F3B:NH3 \] Here, the ammonia (NH3) donates a lone pair of electrons to the boron in boron trifluoride (BF3), forming a dative covalent bond (also called a coordinate bond). Therefore, according to the Lewis concept, BF3 acts as an acid and NH3 acts as a base in this reaction.
03

Discuss the importance of Lewis concept

The Lewis concept is particularly useful because it extends our ability to talk about reactions, beyond just protons and hydroxide ions, by focusing on the movement of electron pairs. This makes the concept widely applicable to a broad range of chemical reactions, including those that do not involve protons at all.

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

Give reasons for the following: (a) Acetamide is basic in water but acidic in liquid \(\mathrm{NH}_{3}\). (b) \(\mathrm{SbF}_{6}\) behaves as an acid in \(\mathrm{HF}\). (c) Alkali metals dissolve in liquid \(\mathrm{NH}_{3}\) to give reducing solutions. (d) Solution of \(\mathrm{KNH}_{2}\) in liquid \(\mathrm{NH}_{3}\) gives pink colour to phenolphthalein. (e) Solution of \(\mathrm{Hg}\left(\mathrm{ClO}_{A}\right)_{2}\) in \(\mathrm{HgCl}_{2}\) is acidic.

Discuss the following reactions in liquid HF and anhydrous \(\mathrm{H}_{2} \mathrm{SO}_{4}\). (a) Acid-base reactions (b) Auto-ionisation

Discuss the important characteristics of solvents.

What is HSAB principle? What are its applications?

What do you mean by levelling and differentiating solvents?
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Chemical Analysis

Read Explanation

Physical Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Making Measurements

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