Textbook Question
(b) What is the hybridization of the carbon atoms in each molecule?
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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 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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