Ch.11 - Liquids and Intermolecular Forces

Brown - Chemistry: The Central Science 15th Edition

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Brown 15th Edition

Ch.11 - Liquids and Intermolecular Forces

Problem 17b

Chapter 11, Problem 17b

(b) Which type of intermolecular attractive force operates only between polar molecules?

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Identify the types of intermolecular forces: London dispersion forces, dipole-dipole interactions, hydrogen bonding, and ion-dipole interactions.

Understand that polar molecules have a permanent dipole moment due to the difference in electronegativity between atoms.

Recognize that dipole-dipole interactions occur between the positive end of one polar molecule and the negative end of another polar molecule.

Note that dipole-dipole interactions are specific to polar molecules because they rely on the presence of a permanent dipole.

Conclude that the type of intermolecular attractive force that operates only between polar molecules is dipole-dipole interactions.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Intermolecular Forces

Intermolecular forces are the attractive forces that occur between molecules, influencing their physical properties such as boiling and melting points. These forces are weaker than covalent or ionic bonds and include various types such as hydrogen bonding, dipole-dipole interactions, and London dispersion forces.

Polar Molecules

Polar molecules have an uneven distribution of electron density, resulting in a partial positive charge on one end and a partial negative charge on the other. This polarity arises from differences in electronegativity between atoms, leading to dipole moments that affect how these molecules interact with each other.

Dipole-Dipole Interactions

Dipole-dipole interactions are a type of intermolecular force that occurs specifically between polar molecules. These forces arise from the attraction between the positive end of one polar molecule and the negative end of another, contributing to the overall stability and properties of polar substances.

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Related Practice

Textbook Question

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

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Textbook Question

At standard temperature and pressure, the molar volumes of Cl₂ and NH₃ gases are 22.06 and 22.40 L, respectively. (c) The densities of crystalline Cl₂ and NH₃ at 160 K are 2.02 and 0.84 g/cm³, respectively. Calculate their molar volumes.

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Textbook Question

(a) Which type of intermolecular attractive force operates between all molecules?

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Textbook Question

At standard temperature and pressure, the molar volumes of Cl2 and NH3 gases are 22.06 and 22.40 L, respectively. (d) Are the molar volumes in the solid state as similar as they are in the gaseous state?

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Textbook Question

Which type of intermolecular force accounts for each of these differences? (a) CH₃OH boils at 65 °C; CH₃SH boils at 6 °C. (d) Acetone boils at 56 °C, whereas 2-methylpropane boils at -12 °C.

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Textbook Question

(b) Which of these kinds of interactions are broken when a liquid is converted to a gas?

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