Textbook Question
(c) Calculate the bond order in H2-.
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Ch.9 - Molecular Geometry and Bonding Theories
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement111
- Ch.2 - Atoms, Molecules, and Ions166
- Ch.3 - Chemical Reactions and Reaction Stoichiometry138
- Ch.4 - Reactions in Aqueous Solution127
- Ch.5 - Thermochemistry104
- Ch.6 - Electronic Structure of Atoms109
- Ch.7 - Periodic Properties of the Elements107
- Ch.8 - Basic Concepts of Chemical Bonding102
- Ch.9 - Molecular Geometry and Bonding Theories120
- Ch.10 - Gases122
- Ch.11 - Liquids and Intermolecular Forces79
- Ch.12 - Solids and Modern Materials102
- Ch.13 - Properties of Solutions99
- Ch.14 - Chemical Kinetics153
- Ch.15 - Chemical Equilibrium83
- Ch.16 - Acid-Base Equilibria109
- Ch.17 - Additional Aspects of Aqueous Equilibria117
- Ch.18 - Chemistry of the Environment60
- Ch.19 - Chemical Thermodynamics109
- Ch.20 - Electrochemistry113
- Ch.21 - Nuclear Chemistry79
- Ch.22 - Chemistry of the Nonmetals52
- Ch.23 - Transition Metals and Coordination Chemistry57
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry7
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 9, Problem 71e
Consider the H2+ ion. (e) Suppose that the ion is excited by light so that an electron moves from a lower-energy to a higher-energy MO. Would you expect the excited-state H2+ ion to be stable or to fall apart?
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Identify the molecular orbitals (MOs) of the H2+ ion. In H2+, there are two key molecular orbitals to consider: the bonding molecular orbital (σ1s) and the antibonding molecular orbital (σ*1s).
Understand the electron configuration of the ground state and the excited state of H2+. In its ground state, the single electron of H2+ occupies the lower energy σ1s orbital. When excited by light, the electron transitions to the higher energy σ*1s orbital.
Analyze the stability of the molecular orbitals. The bonding orbital (σ1s) has a lower energy and contributes to the stability of the molecule by lowering the overall energy. In contrast, the antibonding orbital (σ*1s) has higher energy and tends to destabilize the molecule.
Consider the effect of the electron in the antibonding orbital. With the electron in the σ*1s orbital, the electron density between the nuclei decreases, reducing the attractive forces that hold the nuclei together and increasing the repulsive forces.
Conclude on the stability of the excited-state H2+ ion. Given that the electron in the excited state occupies an antibonding orbital, which destabilizes the molecule, it is likely that the excited-state H2+ ion would be less stable and could potentially dissociate or fall apart.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molecular Orbitals (MOs)
Molecular orbitals are regions in a molecule where electrons are likely to be found. They are formed from the combination of atomic orbitals and can be classified as bonding, antibonding, or non-bonding. In the case of H2+, the bonding molecular orbital is lower in energy and stabilizes the molecule, while the antibonding orbital is higher in energy and can destabilize it if occupied.
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Excitation of Electrons
When an electron absorbs energy, such as from light, it can be promoted from a lower-energy molecular orbital to a higher-energy one. This process is known as excitation. In the context of H2+, if an electron is excited to a higher-energy molecular orbital, it may lead to changes in the stability of the ion, potentially making it less stable.
Stability of Ions
The stability of ions, such as H2+, depends on the balance between attractive and repulsive forces within the molecule. If an electron is excited to a higher-energy state, it may occupy an antibonding orbital, which can weaken the bond between the hydrogen nuclei. This can lead to the ion becoming unstable and potentially dissociating into separate hydrogen atoms.
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Related Practice
Textbook Question
Draw a picture that shows all three 2p orbitals on one atom and all three 2p orbitals on another atom. (c) How many antibonding orbitals, and of what type can be made from the two sets of 2p orbitals?
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Textbook Question
Consider the H2+ ion. (c) Write the electron configuration of the ion in terms of its MOs. (d) What is the bond order in H2+?
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Textbook Question
What hybridization do you expect for the atom indicated in red in each of the following species? (a) CH3CO2-
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Textbook Question
Draw a picture that shows all three 2p orbitals on one atom and all three 2p orbitals on another atom. (b) How many p bonds can the two sets of 2p orbitals make with each other?
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Textbook Question
Consider the H2+ ion. (a) Sketch the molecular orbitals of the ion and draw its energy-level diagram.
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