/*! 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 13 Which type of intermolecular att... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 11: Problem 13

Which type of intermolecular attractive force operates between (a) all molecules, (b) polar molecules, (c) the hydrogen atom of a polar bond and a nearby small electronegative atom?

Short Answer

Expert verified
The types of intermolecular attractive forces operating between different molecules are as follows: (a) London dispersion forces operate between all molecules, (b) dipole-dipole forces operate between polar molecules, and (c) hydrogen bonding operates between the hydrogen atom of a polar bond and a nearby small electronegative atom (usually nitrogen, oxygen, or fluorine).

Step by step solution

01

Identify the force operating between all molecules.

London dispersion forces are the weakest intermolecular forces and act between all types of molecules, whether they are polar or nonpolar. They arise due to the temporary fluctuations in the electron distribution around the molecules, which creates a temporary dipole. Hence, the type of intermolecular attractive force that operates between all molecules is London dispersion forces.
02

Identify the force operating between polar molecules.

Dipole-dipole forces are the intermolecular forces present between polar molecules. Polar molecules have a permanent dipole moment due to the presence of polar bonds, which leads to the formation of partial positive and partial negative charges within the molecule. These charges are responsible for the attraction between the molecules. The type of intermolecular attractive force operating between polar molecules is dipole-dipole forces.
03

Identify the force operating between the hydrogen atom of a polar bond and a nearby small electronegative atom.

Hydrogen bonding is a special type of intermolecular attractive force that occurs when a hydrogen atom is bonded to a highly electronegative atom (such as nitrogen, oxygen, or fluorine) and is also attracted to a nearby electronegative atom (usually nitrogen, oxygen, or fluorine). This creates a strong, directional force between the molecules. The type of intermolecular attractive force operating between the hydrogen atom of a polar bond and a nearby small electronegative atom is hydrogen bonding.

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

Name the phase transition in each of the following situations, and indicate whether it is exothermic or endothermic: (a) Bromine vapor turns to bromine liquid as it is cooled. (b) Crystals of iodine disappear from an evaporating dish as they stand in a fume hood. (c) Rubbing alcohol in an open container slowly disappears. (d) Molten lava from a volcano turns into solid rock.

(a) What atoms must a molecule contain to participate in hydrogen bonding with other molecules of the same kind? (b) Which of the following molecules can form hydrogen bonds with other molecules of the same kind: \(\mathrm{CH}_{3} \mathrm{~F}, \mathrm{CH}_{3} \mathrm{NH}_{2}, \mathrm{CH}_{3} \mathrm{OH}, \mathrm{CH}_{3} \mathrm{Br} ?\)

Acetone, \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{CO}\), is widely used as an industrial solvent. (a) Draw the Lewis structure for the acetone molecule, and predict the geometry around each carbon atom. (b) Is the acetone molecule polar or nonpolar? (c) What kinds of intermolecular attractive forces exist between acetone molecules? (d) 1-Propanol, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{OH}\), has a molecular weight that is very similar to that of acetone, yet acetone boils at \(56.5^{\circ} \mathrm{C}\) and 1 -propanol boils at \(97.2^{\circ} \mathrm{C}\). Explain the difference.

Amorphous silica has a density of about \(2.2 \mathrm{~g} / \mathrm{cm}^{3}\), whereas the density of crystalline quartz is \(2.65 \mathrm{~g} / \mathrm{cm}^{3}\) Account for this difference in densities.

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

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Organic Chemistry

Read Explanation

Making Measurements

Read Explanation

Nuclear Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Chemical Analysis

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.