Recent Lessons

Show all results for ""

Feature Overview

Ace your exams with our all-in-one platform for creating and sharing quizzes and tests.

Quizzes

Create quizzes and tests automatically from your content using AI.

Flashcards

Automatically turn your notes into digital flashcards.

Share, Export & Embed

Share with classmates or export to Excel and your learning management system.

Stats & Reporting

Auto-grading quizzes and tests with detailed stats and reports.

Mobile Apps

The smarter way to study – wherever you are.

Pricing

Search...

5 Questions

1 Views

Lewis Acids and Bases Quiz

Choose a study mode

Play Quiz

Study Flashcards

Spaced Repetition

Chat to lesson

Podcast

Play an AI-generated podcast conversation about this lesson

Questions and Answers

Provide an example of a Lewis base and explain why it is a Lewis base.

An example of a Lewis base is NH3 because it can donate its lone pair of electrons, making it capable of forming a dative bond with a Lewis acid to form a Lewis adduct.

What is a Lewis acid?

A Lewis acid is a chemical species that contains an empty orbital capable of accepting an electron pair from a Lewis base to form a Lewis adduct.

Define a Lewis base.

A Lewis base is any species that has a filled orbital containing an electron pair which is not involved in bonding but may form a dative bond with a Lewis acid to form a Lewis adduct.

Identify a substance mentioned in the text that is a Lewis acid and explain why it is classified as such.

<p>Trimethylborane (Me3B) is a Lewis acid because it is capable of accepting a lone pair, making it suitable for forming a dative bond with a Lewis base to form a Lewis adduct.</p> Signup and view all the answers

Describe the formation of a Lewis adduct and provide an example from the text.

<p>In a Lewis adduct, the Lewis acid and base share an electron pair furnished by the Lewis base, forming a dative bond. For example, in the reaction between NH3 and Me3B, a lone pair from NH3 forms a dative bond with the empty orbital of Me3B to form the adduct NH3 BMe3.</p> Signup and view all the answers

Study Notes

Lewis Acids and Bases

Lewis Bases

A Lewis base is an electron pair donor, capable of forming a covalent bond with an electron acceptor (Lewis acid).
Example: Ammonia (NH3) is a Lewis base because it has a lone pair of electrons that can be donated to form a covalent bond.
In ammonia, the nitrogen atom has a lone pair of electrons that can be shared with a Lewis acid.

Lewis Acids

A Lewis acid is an electron pair acceptor, capable of forming a covalent bond with an electron donor (Lewis base).
Example: Boron trifluoride (BF3) is a Lewis acid because it has an incomplete octet and can accept an electron pair to form a covalent bond.

Lewis Adduct Formation

A Lewis adduct is a compound formed by the reaction of a Lewis acid with a Lewis base.
Example: The reaction of ammonia (NH3) with boron trifluoride (BF3) forms a Lewis adduct, H3NBF3.
In this reaction, the nitrogen atom of ammonia donates a lone pair of electrons to the boron atom of boron trifluoride, forming a covalent bond.

Studying That Suits You

Use AI to generate personalized quizzes and flashcards to suit your learning preferences.

Description

Test your knowledge of Lewis acids and bases with this quiz. Explore the concepts of electron pair acceptance and dative bonding as you identify and understand the properties of these important chemical species.