Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 6: Problem 15

Predict whether the bonds between the following pairs of elements are ionic, polar covalent, or nonpolar covalent. a. \(\mathrm{Na}-\mathrm{F}\) b. \(\mathrm{H}-\mathrm{I}\) c. \(\mathrm{N}-\mathrm{O}\) d. \(\mathrm{Al}-\mathrm{O}\) e. \(\mathrm{S}-\mathrm{O}\) f. \(\mathrm{H}-\mathrm{H}\)

Short Answer

Expert verified
Bond type predictions: \(\mathrm{Na}-\mathrm{F}\) is ionic, \(\mathrm{H}-\mathrm{I}\) is polar covalent, \(\mathrm{N}-\mathrm{O}\) is polar covalent, \(\mathrm{Al}-\mathrm{O}\) is ionic, \(\mathrm{S}-\mathrm{O}\) is polar covalent, and \(\mathrm{H}-\mathrm{H}\) is nonpolar covalent.

Step by step solution

01

Predict Bond Type for Na-F

In a pair \(\mathrm{Na}-\mathrm{F}\), F is much more electronegative than Na. The large electronegativity difference indicates the bond is ionic.
02

Predict Bond Type for H-I

For \(\mathrm{H}-\mathrm{I}\), I is more electronegative than H but the difference is not so large. The bond is polar covalent.
03

Predict Bond Type for N-O

In the \(\mathrm{N}-\mathrm{O}\) pair, the electronegativities of N and O are quite close. This suggests a polar covalent bond.
04

Predict Bond Type for Al-O

For \(\mathrm{Al}-\mathrm{O}\), O is much more electronegative than Al. The large electronegativity difference indicates the bond is ionic.
05

Predict Bond Type for S-O

In the \(\mathrm{S}-\mathrm{O}\) pair, the electronegativities of S and O are quite close. This suggests a polar covalent bond.
06

Predict Bond Type for H-H

In the \(\mathrm{H}-\mathrm{H}\) pair, the two atoms have identical electronegativities. This results in a nonpolar covalent bond.

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

How does an ionic compound differ from a molecular compound?

What is the difference between a dipole and electronegativity difference?

Draw Lewis structures for the following polyatomic ions. a. \(\mathrm{CO}_{3}^{2-}\) b. \(\mathrm{O}_{2}^{2-}\) c. \(\mathrm{PO}_{4}^{3-}\)

What term is used to describe the situation when two or more correct Lewis structures represent a molecule?

Natural rubber consists of long chains of carbon and hydrogen atoms covalently bonded together. When Goodyear accidentally dropped a mixture of sulfur and rubber on a hot stove, the energy joined these chains together to make vulcanized rubber. Vulcan was the Roman god of fire. The car-bon-hydrogen chains in vulcanized rubber are held together by two sulfur atoms that form covalent bonds between the chains. These covalent bonds are commonly called disulfide bridges. Explore other molecules that have such disulfide bridges. Present your findings to the class.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Physical Chemistry

Read Explanation

Chemical Analysis

Read Explanation

The Earths Atmosphere

Read Explanation

Organic Chemistry

Read Explanation

Ionic and Molecular Compounds

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