/*! 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 47 What is a network solid? Give an... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 13: Problem 47

What is a network solid? Give an example of a network solid and describe the bonding in such a solid. How does a network solid differ from a molecular solid?

Short Answer

Expert verified
A network solid is a crystalline solid where atoms are covalently bonded together in a continuous three-dimensional network structure, such as diamond. In diamond, carbon atoms are bonded in a strong tetrahedral network, leading to high hardness and melting points. Molecular solids, on the other hand, consist of individual molecules held together by weaker intermolecular forces like hydrogen bonding or Van der Waals forces, resulting in lower melting and boiling points and increased susceptibility to deformation.

Step by step solution

01

Define a Network Solid

A network solid is a type of crystalline solid in which atoms are covalently bonded together in an extended three-dimensional network structure.
02

Provide an Example and Describe the Bonding

An example of a network solid is diamond, a form of carbon. In diamond, each carbon atom is covalently bonded to four other carbon atoms, forming a tetrahedron. This covalent bonding extends throughout the entire crystal, creating a strong interconnected network. The covalent bonds in a network solid are much stronger than the intermolecular forces found in molecular solids, resulting in network solids being harder and having higher melting points.
03

Define a Molecular Solid

A molecular solid is a type of crystalline solid that consists of molecules held together by relatively weak intermolecular forces such as hydrogen bonding, dipole-dipole interactions, and Van der Waals forces.
04

Compare and Contrast Network Solids and Molecular Solids

The key difference between network solids and molecular solids lies in the nature of the bonding between their constituent particles. In network solids, atoms are covalently bonded to one another, forming a continuous, strong, interconnected network. In contrast, molecular solids consist of individual molecules held together by weaker intermolecular forces. As a result, network solids generally have higher melting and boiling points, and are harder and less susceptible to deformation compared to molecular solids.

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

A common prank on college campuses is to switch the salt and sugar on dining hall tables, which is usually easy because the substances look so much alike. Yet, despite the similarity in their appearance, these two substances differ greatly in their properties, since one is a molecular solid and the other is an ionic solid. How do the properties differ and why?

What do we call the energies required, respectively, to melt and to vaporize 1 mol of a substance? Which of these energies is always larger for a given sub. stance? Why?

On the basis of the smaller units that make up the crystals, cite three types of crystalline solids. For each type of crystalline solid, give an example of a substance that forms that type of solid.

Which of the substances in each of the following sets would be expected to have the lowest melting point? Explain why. a. \(\mathrm{H}_{2}, \mathrm{N}_{2}, \mathrm{O}_{2}\) b. Xe, NaCl, C (diamond) c. \(C l_{2}, B r_{2}, I_{2}\)

Two molecules that contain the same number of each kind of atom but that have different molecular structures are said to be isomers of each other. For example, both ethyl alcohol and dimethyl ether (shown below) have the formula \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\) and are isomers. Based on considerations of intermolecular forces, which substance would you expect to be more volatile? Which would you expect to have the higher boiling point? Explain. $$\begin{array}{lc} \text { dimethyl ether } & \text { ethyl alcohol } \\ \mathrm{CH}_{3}-\mathrm{O}-\mathrm{CH}_{3} & \mathrm{CH}_{3}-\mathrm{CH}_{2}-\mathrm{OH} \end{array}$$
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Inorganic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Making Measurements

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.