Textbook Question
(c) Which is generally stronger, a s bond or a p bond? Explain.
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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 Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 9, Problem 56b
(b) Imagine that you could hold two atoms that are bonded together, twist them, and not change the bond length. Would it be easier to twist (rotate) around a single s bond or around a double 1s plus p2 bond, or would they be the same?
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Identify the types of bonds in ethane and ethene. Ethane has a single bond (sigma bond) between the carbon atoms, while ethene has a double bond (one sigma bond and one pi bond) between the carbon atoms.
Understand the nature of sigma and pi bonds. Sigma bonds are formed by the head-on overlap of atomic orbitals, while pi bonds are formed by the side-to-side overlap of p orbitals.
Consider the rotational freedom around these bonds. Sigma bonds allow for free rotation around the bond axis because the electron density is symmetrically distributed along the axis.
Analyze the restriction imposed by pi bonds. Pi bonds restrict rotation because the electron density is above and below the plane of the atoms, making it harder to twist without breaking the pi bond.
Conclude that it is easier to twist around a single sigma bond (as in ethane) than around a double bond (as in ethene) because the pi bond in the double bond restricts rotation.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Types of Chemical Bonds
Chemical bonds can be classified into single, double, and triple bonds based on the number of shared electron pairs between atoms. A single bond, like that in ethane, involves one pair of shared electrons, while a double bond, as seen in ethene, consists of two pairs. The nature of these bonds affects molecular geometry and rotation.
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Bond Rotation and Rigidity
Bond rotation refers to the ability of atoms connected by a bond to rotate around that bond axis. Single bonds allow for free rotation due to less steric hindrance, while double bonds restrict rotation because of the presence of pi bonds, which create a planar structure. This rigidity impacts the overall shape and reactivity of molecules.
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Steric Hindrance
Steric hindrance is the repulsion between atoms that occurs when they are brought close together, affecting their ability to rotate around bonds. In the case of double bonds, the spatial arrangement of atoms creates more steric hindrance compared to single bonds, making it more difficult to twist or rotate around a double bond without breaking it.
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