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? Explain.
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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 15c
(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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Identify the type of intermolecular force described in the question. The force is specific to interactions involving hydrogen atoms and electronegative atoms like oxygen, nitrogen, or fluorine.
Recognize that this intermolecular force occurs when hydrogen is covalently bonded to a highly electronegative atom, making the hydrogen partially positive.
Understand that the partially positive hydrogen atom is attracted to the lone pair electrons of a nearby electronegative atom in another molecule, forming a special type of dipole-dipole interaction.
Recall the name of this intermolecular force, which is named after the elements typically involved: hydrogen and an electronegative atom such as nitrogen, oxygen, or fluorine.
Conclude that this type of force is known as hydrogen bonding, which is a strong type of dipole-dipole attraction and crucial in many biological and chemical systems.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Hydrogen Bonding
Hydrogen bonding is a specific type of intermolecular force that occurs when a hydrogen atom, covalently bonded to a highly electronegative atom like oxygen, nitrogen, or fluorine, interacts with another electronegative atom. This interaction is characterized by a strong dipole-dipole attraction due to the significant difference in electronegativity, leading to a partial positive charge on the hydrogen and a partial negative charge on the electronegative atom.
Polar Bonds
Polar bonds form when there is a significant difference in electronegativity between two atoms, resulting in an uneven distribution of electron density. This creates a dipole moment, where one end of the bond becomes partially negative and the other partially positive. In the context of hydrogen bonding, the polar bond is crucial as it allows the hydrogen atom to participate in attractive interactions with other electronegative atoms.
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Molecular Polarity
Intermolecular Forces
Intermolecular forces are the forces of attraction or repulsion between neighboring particles (atoms, molecules, or ions). These forces are weaker than covalent or ionic bonds and play a significant role in determining the physical properties of substances, such as boiling and melting points. Understanding the different types of intermolecular forces, including hydrogen bonds, dipole-dipole interactions, and London dispersion forces, is essential for predicting the behavior of substances in various states.
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01:59Intermolecular vs Intramolecular Forces
Related Practice
Textbook Question
(a) Which type of intermolecular attractive force operates between all molecules?
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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 type of intermolecular attractive force operates only between polar molecules?
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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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