Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 9: Problem 30

Distinguish among single, double, and triple bonds in a molecule, and give an example of each.

Short Answer

Expert verified
A single bond shares one pair of electrons, double bond shares two pairs, and triple bond shares three pairs. Examples are hydrogen gas (H_2) for single bond, carbon dioxide (CO_2) for double bond, and nitrogen gas (N_2) for triple bond.

Step by step solution

01

Defining Bond Types

A single bond in a molecule is where one pair of electrons are shared between two atoms. In contrast, a double bond shares two pairs of electrons between two atoms and a triple bond is the sharing of three pairs of electrons between two atoms.
02

Examples: Single Bonds

A good example of a molecule with a single bond is hydrogen gas (H_2), where two hydrogen atoms are linked by sharing one pair of electrons.
03

Examples: Double Bonds

For double bonds, consider carbon dioxide (CO_2). In this molecule, each oxygen atom shares two pairs of electrons with the central carbon atom, creating two double bonds.
04

Examples: Triple Bonds

An example of a molecule with a triple bond is nitrogen gas (N_2). Here, two nitrogen atoms share three pairs of electrons to form a triple 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

What is lattice energy and what role does it play in the stability of ionic compounds?

Write Lewis structures for the reaction $$ \mathrm{AlCl}_{3}+\mathrm{Cl}^{-} \longrightarrow \mathrm{AlCl}_{4}^{-} $$ What kind of bond is between \(\mathrm{Al}\) and \(\mathrm{Cl}\) in the product?

Explain why the bond enthalpy of a molecule is usually defined in terms of a gas-phase reaction. Why are bond-breaking processes always endothermic and bond-forming processes always exothermic?

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.)

List these bonds in order of increasing ionic character: cesium to fluorine, chlorine to chlorine, bromine to chlorine, silicon to carbon.
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

The Earths Atmosphere

Read Explanation

Inorganic Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Chemical Analysis

Read Explanation

Organic 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