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
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 9, Problem 55d
Which of the following statements are true? d. A π bond has two regions of overlap on opposite sides of the internuclear axis.
Verified step by step guidance1
Understand the nature of a π bond: A π bond is formed by the sideways overlap of p orbitals.
Visualize the overlap: In a π bond, the electron density is concentrated above and below the plane of the nuclei of the bonding atoms.
Identify the regions of overlap: The overlap occurs in two distinct regions, one above and one below the internuclear axis.
Compare with a π bond: Unlike a π bond, which has a single region of overlap along the internuclear axis, a π bond has these two separate regions.
Conclude the statement: Based on the above understanding, determine if the statement about the π bond having two regions of overlap on opposite sides of the internuclear axis is true.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Pi Bonding
A pi bond is a type of covalent bond formed when two lobes of one involved atomic orbital overlap with two lobes of another, typically occurring in double or triple bonds. Unlike sigma bonds, which have end-to-end overlap, pi bonds involve side-to-side overlap of p orbitals, resulting in a bond that is generally weaker and more reactive.
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Orbital Overlap
Orbital overlap is a fundamental concept in molecular chemistry that describes how atomic orbitals combine to form bonds. The extent and orientation of this overlap determine the strength and type of bond formed, with sigma bonds resulting from head-on overlap and pi bonds from lateral overlap of orbitals.
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Internuclear Axis
The internuclear axis is an imaginary line that connects the nuclei of two bonded atoms. In the context of bonding, it is crucial for understanding the orientation of bonds; sigma bonds are aligned along this axis, while pi bonds are formed above and below it, leading to distinct geometrical arrangements in molecules.
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Related Practice
Textbook Question
(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?
Textbook Question
Shown here are three pairs of hybrid orbitals, with each set at a characteristic angle. For each pair, determine the type of hybridization, if any, that could lead to hybrid orbitals at the specified angle. (a)
(b)
(c)
Textbook Question
Which of the following statements are true? c. A π bond is made from the sideways overlap of two p orbitals.
Textbook Question
What is the hybridization of the central atom in d. TeCl2?