Domanda del libro di testo
Write a hybridization and bonding scheme for each molecule or ion. Sketch the structure, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. d. I3-
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Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving136
- Ch.2 - Atoms & Elements112
- Ch.3 - Molecules, Compounds & Chemical Equations159
- Ch.4 - Chemical Quantities & Aqueous Reactions140
- Ch.5 - Gases118
- Ch.6 - Thermochemistry106
- Ch.7 - Quantum-Mechanical Model of the Atom62
- Ch.8 - Periodic Properties of the Elements103
- Ch.9 - Chemical Bonding I: The Lewis Model104
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory89
- Ch.11 - Liquids, Solids & Intermolecular Forces73
- Ch.12 - Solids and Modern Material59
- Ch.13 - Solutions110
- Ch.14 - Chemical Kinetics140
- Ch.15 - Chemical Equilibrium78
- Ch.16 - Acids and Bases155
- Ch.17 - Aqueous Ionic Equilibrium176
- Ch.18 - Free Energy and Thermodynamics108
- Ch.19 - Electrochemistry118
- Ch.20 - Radioactivity and Nuclear Chemistry82
- Ch.21 - Organic Chemistry150
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
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Tro 4th EditionCh.10 - Chemical Bonding II: Molecular Shapes & Valence Bond TheoryProblema 63
Tro 4th EditionCh.10 - Chemical Bonding II: Molecular Shapes & Valence Bond TheoryProblema 63Capitolo 10, Problema 63
Write a hybridization and bonding scheme for each molecule or ion. Sketch the structure, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7.
a. COCl2 (carbon is the central atom)
b. BrF5
c. XeF2
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Identify the central atom and count the number of regions of electron density around it. For COCl_2, carbon is the central atom with three regions of electron density: one double bond with oxygen and two single bonds with chlorine atoms.
Determine the hybridization of the central atom based on the number of regions of electron density. With three regions, the hybridization of carbon is sp^2.
Sketch the structure of COCl_2, showing the central carbon atom with sp^2 hybrid orbitals forming sigma bonds with the oxygen and chlorine atoms. The double bond with oxygen consists of one sigma bond and one pi bond.
Label the bonds: the C=O bond consists of a sigma bond (sp^2-p overlap) and a pi bond (p-p overlap), while each C-Cl bond is a sigma bond (sp^2-p overlap).
Draw the overlapping orbitals: show the sp^2 hybrid orbitals on carbon overlapping with the p orbitals of oxygen and chlorine, and the unhybridized p orbital on carbon overlapping with the p orbital on oxygen to form the pi bond.
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Hybridization
Hybridization is the process of mixing atomic orbitals to form new hybrid orbitals that can accommodate the bonding requirements of a molecule. In the case of COCl2, the central carbon atom undergoes sp2 hybridization, resulting in three equivalent hybrid orbitals that form sigma bonds with the two chlorine atoms and one oxygen atom, while the remaining p orbital can participate in pi bonding.
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00:51
Hybridization
Bonding and Molecular Geometry
The bonding in molecules involves the formation of sigma (σ) and pi (π) bonds between atoms. In COCl2, the molecular geometry is trigonal planar due to the sp2 hybridization of carbon, which allows for 120-degree bond angles between the bonds. Understanding the geometry helps predict the physical and chemical properties of the molecule.
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01:33Molecular Geometry with Two Electron Groups
Orbital Overlap
Orbital overlap is a key concept in chemical bonding, where atomic orbitals from different atoms combine to form bonds. In COCl2, the overlap of the sp2 hybrid orbitals of carbon with the p orbitals of chlorine and oxygen leads to the formation of sigma bonds, while any remaining p orbitals can form pi bonds, illustrating the importance of orbital interactions in molecular structure.
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03:06Molecular Orbital Theory
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