Textbook Question
Write orbital diagrams (boxes with arrows in them) to represent the electron configurations of carbon before and after sp hybridization.
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Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving107
- Ch.2 - Atoms & Elements100
- Ch.3 - Molecules, Compounds & Chemical Equations127
- Ch.4 - Chemical Quantities & Aqueous Reactions114
- Ch.5 - Gases103
- Ch.6 - Thermochemistry92
- Ch.7 - Quantum-Mechanical Model of the Atom50
- Ch.8 - Periodic Properties of the Elements89
- Ch.9 - Chemical Bonding I: The Lewis Model84
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory74
- Ch.11 - Liquids, Solids & Intermolecular Forces60
- Ch.12 - Solids and Modern Material50
- Ch.13 - Solutions90
- Ch.14 - Chemical Kinetics111
- Ch.15 - Chemical Equilibrium65
- Ch.16 - Acids and Bases135
- Ch.17 - Aqueous Ionic Equilibrium145
- Ch.18 - Free Energy and Thermodynamics92
- Ch.19 - Electrochemistry100
- Ch.20 - Radioactivity and Nuclear Chemistry68
- Ch.21 - Organic Chemistry121
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Tro 4th EditionCh.10 - Chemical Bonding II: Molecular Shapes & Valence Bond TheoryProblem 61a
Tro 4th EditionCh.10 - Chemical Bonding II: Molecular Shapes & Valence Bond TheoryProblem 61aChapter 10, Problem 61a
Write a hybridization and bonding scheme for each molecule. Sketch the molecule, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. a. CCl4
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Identify the central atom in the molecule. In CCl_4, carbon (C) is the central atom.
Determine the number of valence electrons for the central atom. Carbon has 4 valence electrons.
Count the number of atoms bonded to the central atom. In CCl_4, there are 4 chlorine atoms bonded to carbon.
Determine the hybridization of the central atom. Since carbon forms 4 sigma bonds with chlorine, it undergoes sp^3 hybridization.
Sketch the molecule: Draw the carbon atom in the center with four sp^3 hybrid orbitals. Each orbital overlaps with a p orbital from a chlorine atom to form a sigma (σ) bond. Label each C-Cl bond as a σ bond.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Hybridization
Hybridization is the process of combining atomic orbitals to form new hybrid orbitals that can accommodate the bonding requirements of a molecule. In the case of CCl4, the carbon atom undergoes sp3 hybridization, resulting in four equivalent hybrid orbitals that arrange themselves in a tetrahedral geometry to minimize electron pair repulsion.
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Hybridization
Bonding and Molecular Geometry
Bonding refers to the interactions between atoms that result in the formation of molecules. In CCl4, each of the four sp3 hybrid orbitals of carbon overlaps with the p orbitals of chlorine atoms, forming four sigma (σ) bonds. The molecular geometry is tetrahedral, which is crucial for understanding the spatial arrangement of the atoms and the overall shape of the molecule.
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Orbital Overlap Theory
Orbital overlap theory explains how atomic orbitals combine to form bonds in a molecule. In CCl4, the overlap of carbon's sp3 hybrid orbitals with chlorine's p orbitals leads to the formation of sigma bonds. This concept is essential for visualizing the bonding interactions and understanding the strength and characteristics of the bonds formed in the molecule.
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Related Practice
Textbook Question
Write a hybridization and bonding scheme for each molecule. Sketch the molecule, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7.a. CH2Br2 b. SO2 c. NF3 d. BF3
Textbook Question
Write a hybridization and bonding scheme for each molecule. Sketch the molecule, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. b. NH3
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Textbook Question
Which hybridization scheme allows the central atom to form more than four bonds? sp3, sp3d, sp2
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Textbook Question
Write a hybridization and bonding scheme for each molecule. Sketch the molecule, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. c. OF2 d. CO2
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Textbook Question
Write orbital diagrams (boxes with arrows in them) to represent the electron configurations—without hybridization—for all the atoms in SF2. Circle the electrons involved in bonding. Draw a three-dimensional sketch of the molecule and show orbital overlap. What bond angle do you expect from the unhybridized orbitals? How well does valence bond theory agree with the experimentally measured bond angle of 98.2° ?
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