Textbook Question
(a) Two pans of water are on different burners of a stove. One pan of water is boiling vigorously, while the other is boiling gently. What can be said about the temperature of the water in the two pans?
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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 Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 11, Problem 51
(a) Place the following substances in order of increasing volatility: CH4, CBr4, CH2Cl2, CH3Cl, CHBr3, and CH2Br2. (b) How do the boiling points vary through this series? (c) Explain your answer to part (b) in terms of intermolecular forces.
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Identify the types of intermolecular forces present in each substance: CH_4, CBr_4, CH_2Cl_2, CH_3Cl, CHBr_3, and CH_2Br_2. Consider London dispersion forces, dipole-dipole interactions, and hydrogen bonding.
Recognize that volatility is inversely related to the strength of intermolecular forces. Substances with weaker intermolecular forces are more volatile.
Arrange the substances in order of increasing volatility by comparing the strength of their intermolecular forces. Consider molecular weight and polarity.
For boiling points, note that they are directly related to the strength of intermolecular forces. Substances with stronger intermolecular forces have higher boiling points.
Explain the variation in boiling points by discussing the role of molecular weight and polarity in determining the strength of London dispersion forces and dipole-dipole interactions.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Volatility
Volatility refers to the tendency of a substance to vaporize. It is influenced by the strength of intermolecular forces; substances with weaker forces tend to be more volatile. For example, lighter molecules with weaker London dispersion forces will evaporate more readily than heavier molecules with stronger dipole-dipole interactions or hydrogen bonds.
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Boiling Point
The boiling point of a substance is the temperature at which its vapor pressure equals the external pressure, allowing it to transition from liquid to gas. Generally, higher boiling points indicate stronger intermolecular forces. In the context of the given substances, as molecular weight and polarity increase, boiling points typically rise due to enhanced van der Waals forces.
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Intermolecular Forces
Intermolecular forces are the forces of attraction or repulsion between molecules. They include London dispersion forces, dipole-dipole interactions, and hydrogen bonds. The type and strength of these forces significantly affect both volatility and boiling points; for instance, substances with stronger intermolecular forces will have lower volatility and higher boiling points compared to those with weaker forces.
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Related Practice
Textbook Question
The critical temperatures and pressures of a series of halogenated methanes are as follows: (c) Predict the critical temperature and pressure for CCl4 based on the trends in this table. Look up the experimentally determined critical temperatures and pressures for CCl4, using a source such as the CRC Handbook of Chemistry and Physics, and suggest a reason for any discrepancies.
Textbook Question
The critical temperatures and pressures of a series of halogenated methanes are as follows:
(a) List the intermolecular forces that occur for each compound.