Textbook Question
(c) What happens to a gas if you put it under extremely high pressure?
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Ch.11 - Liquids and Intermolecular Forces
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 11, Problem 10a
(a) How does the average kinetic energy of molecules com- pare with the average energy of attraction between mole- cules in solids, liquids, and gases?
Verified step by step guidance1
1. The average kinetic energy of molecules is a measure of how fast the molecules are moving. This energy is related to the temperature of the substance. The higher the temperature, the higher the average kinetic energy of the molecules.
2. The average energy of attraction between molecules, also known as intermolecular forces, is a measure of how strongly the molecules are attracted to each other. This energy is related to the phase of the substance. In solids, the intermolecular forces are strong enough to keep the molecules in a fixed position. In liquids, the intermolecular forces are weaker, allowing the molecules to slide past each other. In gases, the intermolecular forces are very weak or negligible, allowing the molecules to move freely.
3. In solids, the average energy of attraction between molecules is greater than the average kinetic energy of the molecules. This is why the molecules are held in a fixed position.
4. In liquids, the average kinetic energy of the molecules is comparable to the average energy of attraction between molecules. This is why the molecules can slide past each other but are still held together to some extent.
5. In gases, the average kinetic energy of the molecules is much greater than the average energy of attraction between molecules. This is why the molecules can move freely and are not held together.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Kinetic Molecular Theory
The Kinetic Molecular Theory explains the behavior of gases in terms of the motion of their molecules. It posits that gas molecules are in constant, random motion and that the temperature of a gas is directly proportional to the average kinetic energy of its molecules. This theory helps to understand how kinetic energy varies in solids, liquids, and gases, influencing their physical properties.
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Intermolecular Forces
Intermolecular forces are the attractive forces between molecules that influence the physical state of a substance. In solids, these forces are strong, keeping molecules closely packed; in liquids, they are moderate, allowing for some movement; and in gases, they are weak, resulting in free movement of molecules. Understanding these forces is crucial for comparing them to kinetic energy in different states of matter.
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Phase Changes
Phase changes refer to the transitions between solid, liquid, and gas states, which occur due to changes in temperature and pressure. During these changes, the balance between kinetic energy and intermolecular forces shifts, affecting the average energy of attraction. For instance, as a solid melts into a liquid, the kinetic energy increases, overcoming some intermolecular forces, which is essential for understanding the energy dynamics in different phases.
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Related Practice
Textbook Question
List the three states of matter in order of (a) increasing molecular disorder
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Textbook Question
At three different temperatures, T1, T2, and T3, the molecules in a liquid crystal align in these ways:
(a) At which temperature or temperatures is the substance in a liquid crystalline state? At those temperatures, which type of liquid crystalline phase is depicted?
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