Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 12: Problem 9

What kinds of attractive forces exist between particles in (a) molecular crystals, (b) covalent-network crystals, (c) ionic crystals, (d) metallic crystals?

Short Answer

Expert verified
In (a) molecular crystals, the attractive forces are London dispersion forces (Van der Waals forces) or, for polar molecules, dipole-dipole forces or hydrogen bonding. In (b) covalent-network crystals, strong covalent bonds form a three-dimensional network between atoms. In (c) ionic crystals, electrostatic forces between oppositely charged ions form ionic bonds. In (d) metallic crystals, metallic bonds arise from the interaction of positively charged metal ions with a delocalized "sea" of electrons.

Step by step solution

01

(a) Molecular Crystals

In molecular crystals, the primary attractive force between the particles is the London dispersion forces (also known as Van der Waals forces) or in case of polar molecules, dipole-dipole forces or hydrogen bonding can also be present. These forces are due to temporary fluctuations in electron distribution around the molecules, creating temporary dipoles that attract other nearby molecules. In case of polar molecules, there are permanent dipoles that interact with the dipoles of nearby molecules.
02

(b) Covalent-Network Crystals

Covalent-network crystals have a different structure as compared to molecular crystals. In covalent-network crystals, the atoms are connected through covalent bonds forming a three-dimensional network. The attractive forces between the atoms in these crystals are strong covalent bonds, which make these crystals very hard, with high melting and boiling points.
03

(c) Ionic Crystals

Ionic crystals are composed of positive and negative ions arranged in a lattice structure. The attractive forces between the particles in ionic crystals are electrostatic forces between the oppositely charged ions, also known as ionic bonds. These ionic bonds result in the formation of an ordered and repeating pattern of ions, which gives ionic crystals their characteristic crystal structure.
04

(d) Metallic Crystals

Metallic crystals have a different arrangement of atoms compared to the other three types of crystals. In metallic crystals, metal atoms are bonded together through metallic bonds, where electrons are delocalized and free to move throughout the lattice. This delocalization of electrons creates a "sea" of electrons around the metal ions, and the attractive forces between the positively charged metal ions and the negatively charged electron cloud hold the particles together in a metallic crystal lattice. So, the attractive forces in metallic crystals are metallic bonds.

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

If you want to dope GaAs to make an \(n\) -type semiconductor with an element to replace Ga, which element(s) would you pick?

Cadmium telluride, CdTe, takes the zinc blende structure (Figure 12.26 ) with a unit cell edge length of \(6.49 \AA\). There are four cadmium atoms and four tellurium atoms per unit cell. How many of each type of atom are there in a cubic crystal with an edge length of \(5.00 \mathrm{nm} ?\)

Which element or elements are alloyed with gold to make the following types of "colored gold" used in the jewelry industry? For each type indicate what type of alloy is formed: (a) white gold, (b) rose gold, (c) blue gold, (d) green gold.

Briefly describe each of the following: (a) elastomer, (b) thermoplastic, (c) thermosetting plastic.

Iridium crystallizes in a face-centered cubic unit cell that has an edge length of \(3.833 \AA\). (a) Calculate the atomic radius of an iridium atom. (b) Calculate the density of iridium metal.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Chemistry Branches

Read Explanation

The Earths Atmosphere

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.

Sign-up for free