Textbook Question
Consider the following hydrocarbon:
d. Identify all the 120° bond angles in the molecule.
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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 10a
The following is part of a molecular orbital energy-level diagram for MOs constructed from 1s atomic orbitals.
(a) What labels do we use for the two MOs shown?
Verified step by step guidance1
Identify the atomic orbitals involved in the formation of molecular orbitals. In this case, the diagram shows molecular orbitals formed from 1s atomic orbitals.
Recognize that the two molecular orbitals formed from 1s atomic orbitals are the bonding and antibonding molecular orbitals.
Label the lower energy molecular orbital as the bonding molecular orbital, denoted as σ(1s).
Label the higher energy molecular orbital as the antibonding molecular orbital, denoted as σ*(1s).
Note that the bonding molecular orbital (σ(1s)) is lower in energy and more stable, while the antibonding molecular orbital (σ*(1s)) is higher in energy and less stable.
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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 formed by the linear combination of atomic orbitals (LCAO) when atoms bond. In the case of diatomic molecules, the 1s atomic orbitals from each atom combine to create two types of molecular orbitals: bonding and antibonding. The bonding molecular orbital is lower in energy and stabilizes the molecule, while the antibonding molecular orbital is higher in energy and can destabilize it.
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Molecular Orbital Theory
Bonding and Antibonding Orbitals
Bonding orbitals are formed when atomic orbitals combine constructively, leading to increased electron density between the nuclei, which stabilizes the molecule. Antibonding orbitals, on the other hand, result from destructive interference, creating a node between the nuclei and leading to decreased electron density in that region, which can destabilize the molecule. The labels for these orbitals are typically denoted as σ (sigma) for bonding and σ* (sigma star) for antibonding.
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Energy-Level Diagrams
Energy-level diagrams visually represent the relative energies of molecular orbitals. In these diagrams, bonding orbitals are placed lower in energy than their corresponding antibonding orbitals. The arrangement helps predict the stability of the molecule based on the number of electrons in each type of orbital, guiding the understanding of molecular structure and reactivity.
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Related Practice
Textbook Question
For each of these contour representations of molecular orbitals, identify (b) the type of MO (s or p) (iii)
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Textbook Question
For each of these contour representations of molecular orbitals, identify (a) the atomic orbitals (s or p) used to construct the MO (iii)
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Textbook Question
For each of these contour representations of molecular orbitals, identify (a) the atomic orbitals (s or p) used to construct the MO (i)
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Textbook Question
The drawing below shows the overlap of two hybrid orbitals to form a bond in a hydrocarbon. (a) Which of the following types of bonds is being formed: (i) C¬C s, (ii) C¬C p, or (iii) C¬H s?
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Textbook Question
The drawing below shows the overlap of two hybrid orbitals to form a bond in a hydrocarbon. (b) Which of the following could be the identity of the hydrocarbon: (i) CH4, (ii) C2H6, (iii) C2H4, or (iv) C2H2?
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