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 71a
Consider the H2+ ion. (a) Sketch the molecular orbitals of the ion and draw its energy-level diagram.
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Identify the atomic orbitals of the hydrogen atoms that will combine to form molecular orbitals. In the case of H2+, each hydrogen atom contributes one 1s orbital.
Understand the concept of molecular orbital theory, which states that atomic orbitals combine to form new orbitals called molecular orbitals. These can be bonding or antibonding orbitals.
Sketch the molecular orbitals for H2+. The combination of two 1s orbitals results in the formation of a bonding molecular orbital (σ1s) and an antibonding molecular orbital (σ*1s).
Draw the energy-level diagram for H2+. Place the σ1s orbital at a lower energy level than the original 1s atomic orbitals, indicating a more stable (lower energy) state. Place the σ*1s orbital at a higher energy level than the original 1s atomic orbitals, indicating a less stable (higher energy) state.
Fill the molecular orbitals with the available electrons. H2+ has a total of one electron, which will occupy the lower energy σ1s orbital, indicating a bond formation in the molecular ion.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molecular Orbitals
Molecular orbitals (MOs) are formed by the linear combination of atomic orbitals (LCAO) when atoms bond together. In the case of diatomic molecules like H2+, the MOs can be classified as bonding or antibonding. Bonding MOs lower the energy of the system and stabilize the molecule, while antibonding MOs increase energy and destabilize it. Understanding the arrangement and energy levels of these orbitals is crucial for predicting the stability and properties of the ion.
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Molecular Orbital Theory
Energy-Level Diagram
An energy-level diagram visually represents the relative energies of molecular orbitals in a molecule or ion. In the case of H2+, the diagram will show the bonding molecular orbital (σ) at a lower energy level and the antibonding molecular orbital (σ*) at a higher energy level. The placement of electrons in these orbitals, according to the Aufbau principle and Hund's rule, helps determine the overall stability and magnetic properties of the ion.
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H2+ Ion Characteristics
The H2+ ion is a simple molecular ion consisting of two hydrogen nuclei and one electron. Its unique characteristics arise from the presence of only one electron, which allows for a straightforward analysis of its molecular orbitals. The ion's behavior can be understood through quantum mechanics, particularly in how the single electron occupies the bonding molecular orbital, leading to a net attractive force between the nuclei, thus influencing its stability and energy.
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Related Practice
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
Consider the following Lewis structure:
a. Does the Lewis structure depict a neutral molecule or an ion? If it is an ion, what is the charge on the ion?
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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
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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Textbook Question
Predict the molecular geometry of each of the following molecules: (b) H O C O C O O H
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