Textbook Question
For each molecule (a)–(f), indicate how many different electron-domain geometries are consistent with the molecular geometry shown. a.
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Ch.9 - Molecular Geometry and Bonding Theories
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 9, Problem 5c
The following plot shows the potential energy of two Cl atoms as a function of the distance between them. (c) If the Cl2 molecule is compressed under higher and higher pressure, does the Cl–Cl bond become stronger or weaker?
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Observe the graph showing the potential energy of two Cl atoms as a function of the interatomic distance.
Identify the point where the potential energy is at its minimum; this corresponds to the equilibrium bond length of the Cl2 molecule.
Understand that the depth of the potential energy well at this point represents the bond energy, which is the energy required to break the bond.
Consider what happens when the Cl2 molecule is compressed under higher pressure: the interatomic distance decreases, moving left on the graph from the equilibrium point.
Note that as the interatomic distance decreases from the equilibrium point, the potential energy increases, indicating that the bond becomes weaker under higher pressure.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Potential Energy Curve
The potential energy curve illustrates how the potential energy of a system changes with the distance between two atoms. In the case of Cl atoms, the curve shows a minimum point where the bond is most stable, indicating the bond energy. As the distance decreases, potential energy decreases until it reaches a minimum, after which it increases sharply, indicating repulsion when atoms are too close.
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Bond Strength and Distance
Bond strength is related to the energy required to break a bond. As the interatomic distance decreases, the bond becomes stronger until the equilibrium distance is reached. If the Cl–Cl bond is compressed further, the bond may weaken due to increased repulsion between the electron clouds of the atoms, which can lead to bond breaking if the pressure is excessive.
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Effect of Pressure on Molecular Bonds
Applying pressure to a molecule can influence the bond length and strength. In the case of Cl2, increasing pressure can initially strengthen the bond by bringing atoms closer, but excessive pressure may lead to a weakening of the bond due to repulsive forces. Understanding this balance is crucial for predicting molecular behavior under varying conditions.
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Related Practice
Textbook Question
The orbital diagram that follows presents the final step in the formation of hybrid orbitals by a silicon atom. (a) Which of the following best describes what took place before the step pictured in the diagram: (i) Two 3p electrons became unpaired, (ii) An electron was promoted from the 2p orbital to the 3s orbital, or (iii) An electron was promoted from the 3s orbital to the 3p orbital?
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Textbook Question
In the hydrocarbon
(a) What is the hybridization at each carbon atom in the molecule?
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Textbook Question
The orbital diagram that follows presents the final step in the formation of hybrid orbitals by a silicon atom. (b) What type of hybrid orbital is produced in this hybridization?
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