Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 2: Q63P (page 83)

Given that the ions in LiF and MgO are of similar size, which compound has stronger ionic bonding? Use Coulomb’s law in your explanation.

Short Answer

Expert verified

MgO the compound has stronger ionic bonding.

Step by step solution

01

Define Coulomb’s law

Coulomb’s law is defined as the interaction force between two ions (cation and anion) in an ionic bond is directly proportional to the product of charges of ions and inversely proportional to the distance between two ions.

F=αq1q2r2

Here,

Fis the interaction between two ions.

q1is the charge of an ion (cation).

q2is the charge of an ion (anion).

r is the distance between two ions.

02

Apply the Coulomb’s law

In , MgO the charge of Mg2+cation is +2 while the charge of O2anion is -2. In the case of LiF , the charge of Li+cation is +1 while the charge of F anion is -1. So, the product of charges of two ions in MgO is greater than that of two ions in . Hence,MgOthe compound has stronger ionic 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.

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

Describe the type and nature of the bonding that occurs between reactive metals and nonmetals.

The radii of the lithium and magnesium ions are 76 pm and 72 pm, respectively. Which compound has stronger ionic attractions, lithium oxide or magnesium oxide?

Each scene below represents a mixture. Describe each one in terms of the number of elements and/or compounds present.

Chlorine has two naturally occurring isotopes, 35Cl and 37Cl. What is the mass number of each isotope? How many protons, neutrons, and electrons are present in each?

Fluorite, a mineral of calcium, is a compound of the metal with fluorine. Analysis shows that a 2.76-g sample of fluorite contains 1.42 g of calcium. Calculate the (a) mass of fluorine in the sample; (b) mass fractions of calcium and fluorine in fluorite; (c) mass percents of calcium and fluorine in fluorite.
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Chemical Reactions

Read Explanation

The Earths Atmosphere

Read Explanation

Chemistry Branches

Read Explanation

Chemical Analysis

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