Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 9: Problem 41

Summarize the essential features of the Lewis octet rule.

Short Answer

Expert verified
The Lewis Octet Rule is a rule in the field of chemistry which reflects the observation that atoms of the main group elements tend to bond in a manner that results in each atom having eight electrons in its valence shell, giving it the same electronic configuration as a noble gas. The rule is used to predict and explain the nature of chemical bonding and element reactions, despite there being some exceptions.

Step by step solution

01

Define the Lewis Octet Rule

The Lewis octet rule is a chemical rule of thumb that reflects observation that atoms of the main group elements tend to combine in such a way that each atom has eight electrons in its valence shell, giving it the same electron configuration as a noble gas.
02

Describe the Significance of the Lewis Octet Rule

This rule is significant because it helps predict and explain the nature of chemical bonding and how elements will react with one another. It aids in predicting the types of bonds an element will form and the number of atoms it can bond with.
03

Note the Exceptions to the Lewis Octet Rule

Despite its widespread use, there are exceptions to the Lewis octet rule. Some elements are capable of expanding their valence shell to accommodate more than eight electrons, while elements like hydrogen are stable with two electrons, and elements such as boron and aluminum are stable with six electrons in their valence shell.

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

Oxygen forms three types of ionic compounds in which the anions are oxide \(\left(\mathrm{O}^{2-}\right),\) peroxide \(\left(\mathrm{O}_{2}^{2-}\right),\) and superoxide \(\left(\mathrm{O}_{2}^{-}\right) .\) Draw Lewis structures of these ions.

Most organic acids can be represented as \(\mathrm{RCOOH}\) where \(\mathrm{COOH}\) is the carboxyl group and \(\mathrm{R}\) is the rest of the molecule. (For example, \(\mathrm{R}\) is \(\mathrm{CH}_{3}\) in acetic acid, \(\mathrm{CH}_{3} \mathrm{COOH} .\) ) (a) Draw a Lewis structure for the carboxyl group. (b) Upon ionization, the carboxyl group is converted to the carboxylate group, \(\mathrm{COO}^{-}\). Draw resonance structures for the carboxylate group.

Write the formulas of the binary hydride for the second-period elements LiH to HF. Comment on the change from ionic to covalent character of these compounds. Note that beryllium behaves differently from the rest of the Group 2 A metals (see Section 8.6 ).

Write the Lewis dot symbols of the reactants and products in the following reactions. (First balance the equations.) (a) \(\mathrm{Sr}+\mathrm{Se} \longrightarrow \mathrm{SrSe}\) (b) \(\mathrm{Ca}+\mathrm{H}_{2} \longrightarrow \mathrm{CaH}_{2}\) (c) \(\mathrm{Li}+\mathrm{N}_{2} \longrightarrow \mathrm{Li}_{3} \mathrm{~N}\) (d) \(\mathrm{Al}+\mathrm{S} \longrightarrow \mathrm{Al}_{2} \mathrm{~S}_{3}\)

The triiodide ion \(\left(\mathrm{I}_{3}^{-}\right)\) in which the I atoms are arranged in a straight line is stable, but the corresponding \(\mathrm{F}_{3}^{-}\) ion does not exist. Explain.
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Organic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Chemical Reactions

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