/*! 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 2 Explain the term "polarizability... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 12: Problem 2

Explain the term "polarizability." What kind of molecules tend to have high polarizabilities? What is the relationship between polarizability and intermolecular forces?

Short Answer

Expert verified
Polarizability refers to the ability of a molecule to have its electron cloud distorted by an external electric field, forming a temporary dipole. Molecules with larger, more diffused electron clouds tend to have high polarizability. A direct relationship exists between polarizability and intermolecular forces such as dispersion forces, with higher polarizability leading to stronger forces.

Step by step solution

01

Defining Polarizability

Polarizability is the ability or tendency of a molecule (atom or ion) to be distorted by an external electric field. It involves the stretching or altering of the electron cloud, causing the molecule to establish a temporary dipole.
02

Molecules with High Polarizability

Molecules that tend to have high polarizabilities are those with large, more diffused electron clouds. This is often seen in atoms with a large number of electrons, such as larger molecules, or elements further down a group in the periodic table. The size and shape of the electron cloud play significant roles in polarizability.
03

Relationship between Polarizability and Intermolecular Forces

There is a direct and significant relationship between polarizability and the strength of intermolecular forces, particularly London dispersion forces. The larger the polarizability of a molecule, the stronger are its dispersion forces. This is because when an atom's or a molecule's electron cloud is more easily distorted (i.e., it has high polarizability), it can induce a dipole in its neighbor more effectively, leading to stronger intermolecular forces.

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

Which of these statements are false: (a) Dipole-dipole interactions between molecules are greatest if the molecules possess only temporary dipole moments. (b) All compounds containing hydrogen atoms can participate in hydrogen bond formation. (c) Dispersion forces exist between all atoms, molecules, and ions. (d) The extent of ion-induced dipole interaction depends only on the charge on the ion.

If you lived in Alaska, state which of these natural gases you would keep in an outdoor storage tank in winter and explain why: methane \(\left(\mathrm{CH}_{4}\right),\) propane \(\left(\mathrm{C}_{3} \mathrm{H}_{8}\right),\) or butane \(\left(\mathrm{C}_{4} \mathrm{H}_{10}\right)\)

A solid is very hard and has a high melting point. Neither the solid nor its melt conducts electricity. Classify the solid.

A solid contains \(X, Y,\) and \(Z\) atoms in a cubic lattice with \(X\) atoms in the corners, \(Y\) atoms in the bodycentered positions, and \(Z\) atoms on the faces of the cell. What is the empirical formula of the compound?

These compounds are liquid at \(-10^{\circ} \mathrm{C}\); their boiling points are given: butane, \(-0.5^{\circ} \mathrm{C}\); ethanol, \(78.3^{\circ} \mathrm{C}\); toluene, \(110.6^{\circ} \mathrm{C}\). At \(-10^{\circ} \mathrm{C}\), which of these liquids would you expect to have the highest vapor pressure? Which the lowest?
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

The Earths Atmosphere

Read Explanation

Making Measurements

Read Explanation

Physical Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Chemistry Branches

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.