Domanda del libro di testo
(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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TOC.tableOfContents
- 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: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 9, Problema 56
(a) If the valence atomic orbitals of an atom are sp hybridized, how many unhybridized p orbitals remain in the valence shell? How many p bonds can the atom form?
Guida verificata passo dopo passo1
Understand the concept of hybridization: Hybridization is the process of mixing atomic orbitals to form new hybrid orbitals suitable for the pairing of electrons to form chemical bonds in molecules.
Identify the type of hybridization: In sp hybridization, one s orbital and one p orbital mix to form two equivalent sp hybrid orbitals.
Determine the number of unhybridized p orbitals: Since one p orbital is used in hybridization, there are two remaining unhybridized p orbitals in the valence shell.
Understand the formation of pi bonds: Pi (π) bonds are formed by the sideways overlap of unhybridized p orbitals.
Calculate the number of pi bonds: With two unhybridized p orbitals available, the atom can form two pi bonds.
Concetti chiave
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Hybridization
Hybridization is the process of combining atomic orbitals to form new hybrid orbitals that are suitable for the pairing of electrons to form chemical bonds. In sp hybridization, one s orbital and one p orbital mix to create two equivalent sp hybrid orbitals, which are oriented 180 degrees apart, suitable for forming linear geometries.
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00:51
Hybridization
Valence Shell and Orbitals
The valence shell is the outermost shell of an atom that contains the valence electrons, which are involved in chemical bonding. In the case of sp hybridization, two of the three p orbitals are used in hybridization, leaving one unhybridized p orbital in the valence shell, which can participate in bonding.
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00:47Valence Shell Electron Pair Repulsion Theory
P Bonds
P bonds, or pi bonds, are a type of covalent bond that occurs when two lobes of one involved atomic orbital overlap with two lobes of another, typically involving unhybridized p orbitals. An atom with one unhybridized p orbital can form one pi bond, which is often found in double or triple bonds alongside sigma bonds.
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01:53Bond Angles
Pratica correlata
Domanda del libro di testo
(c) Which is generally stronger, a s bond or a p bond? Explain.
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Domanda del libro di testo
(a) Draw a picture showing how two p orbitals on two different atoms can be combined to make a σ bond. (b) Sketch a π bond that is constructed from p orbitals.
Domanda del libro di testo
(d) Can two s orbitals combine to form a p bond? Explain.
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Domanda del libro di testo
(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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Domanda del libro di testo
(a) Draw Lewis structures for chloromethane (CH3Cl), chloroethene (C2H3Cl), and chloroethyne (C2HCl).