/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 27 What is Lewis's contribution to ... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 9: Problem 27

What is Lewis's contribution to our understanding of the covalent bond?

Short Answer

Expert verified
Gilbert N. Lewis greatly contributed to our understanding of covalent bonds through his 'Lewis Dot Structures'. He proposed that atoms form covalent bonds by sharing electrons to complete their valence shell and achieve a stable noble gas configuration. His model is widely used to predict the structure, polarity, and reactivity of a molecule.

Step by step solution

01

Understand Covalent Bonds

Covalent bond is a chemical bond formed when two atoms share a pair of electrons. The presence of a shared pair of electrons in the valency shell of two atoms is the defining characteristic of a covalent bond.
02

Understand Lewis's Theory on Covalent bonds

Gilbert N. Lewis, in 1916, explained covalent bonding via his 'Lewis Dot Structures'. He proposed that atoms form bonds in order to complete their octet and reach a stable electronic configuration of a noble gas. This concept is also known as 'Octet Rule'. He demonstrated that shared electrons (represented by dots in the Lewis structures) between atoms result in a covalent bond.
03

Discuss the Impact of Lewis's Theory

Lewis's theory substantially contributed to the understanding of covalent bonds. His simple and visual representation method has helped to easily predict the structure of a molecule, its polarity, and its reactivity. His model affirmed the concept of electron sharing and emphasized the importance of the octet rule in covalent bonding.

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.

Over 30 million students worldwide already upgrade their learning with 91影视!

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

Draw Lewis structures of these organic molecules: (a) tetrafluoroethylene \(\left(\mathrm{C}_{2} \mathrm{~F}_{4}\right)\) (b) propane \(\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)\) (c) butadiene \(\left(\mathrm{CH}_{2} \mathrm{CHCHCH}_{2}\right.\) ), (d) propyne \(\left(\mathrm{CH}_{3} \mathrm{CCH}\right),\) (e) benzoic acid \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\right) .\) (Hint: To draw \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\), replace an \(\mathrm{H}\) atom in benzene with a COOH group.)

Use Lewis dot symbols to show the transfer of electrons between the following atoms to form cations and anions: (a) \(\mathrm{Na}\) and \(\mathrm{F},\) (b) \(\mathrm{K}\) and \(\mathrm{S},\) (c) \(\mathrm{Ba}\) and \(\mathrm{O}\), (d) \(\mathrm{Al}\) and \(\mathrm{N}\).

Write three reasonable resonance structures of the azide ion \(\mathrm{N}_{3}^{-}\) in which the atoms are arranged as NNN. Show formal charges.

Draw three resonance structures for the chlorate ion, \(\mathrm{ClO}_{3}^{-}\). Show formal charges.

Define bond enthalpy. Bond enthalpies of polyatomic molecules are average values. Why?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Inorganic Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Kinetics

Read Explanation

Physical Chemistry

Read Explanation

Nuclear 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.