Domanda del libro di testo
Looking ahead in Chapter 4, we explain that molecules like CH3+ are Lewis acids or electron pair acceptors. Into which orbital would the new electron pair go?
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Ch. 2 - General Chemistry Translated: Finding the Electrons
Mullins1st EditionOrganic Chemistry: A Learner Centered ApproachISBN: 9780137566471
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TOC.tableOfContents
- Ch. 2 - General Chemistry Translated: Finding the Electrons114
- Ch. 3 - Alkanes and Cycloalkanes: Properties and Conformational Analysis109
- Ch. 4 - Acids and Bases/Electron Flow144
- Ch. 5 - Chemical Reaction Analysis: Thermodynamics and Kinetics118
- Ch. 6 - Stereoisomerism: Arrangement of Atoms in Space112
- Ch. 7 - Principles of Green (Organic) Chemistry3
- Ch. 8 - Alkenes 1: Properties and Electrophilic Additions158
- Ch. 9 - Alkenes 2: Oxidation and Reduction150
- Ch. 10 - Alkynes: Electrophilic Addition and Redox Reactions101
- Ch. 11 - Properties and Synthesis of Alkyl Halides: Radical Reactions108
- Ch. 12 - Substitution and Elimination: Reactions of Haloalkanes172
- Ch. 13 - Alcohols, Ethers and Related Compounds: Substitution and Elimination239
- Ch. 14 - Structural Identification 1: Infrared Spectroscopy and Mass Spectrometry54
- Ch. 15 - Structural Identification 2: Nuclear Magnetic Resonance Spectroscopy93
- Ch. 16 - Metals in Organic Chemistry48
- Ch. 17 - Carbonyl Addition Reactions: Aldehydes and Ketones45
- Ch. 18 - Nucleophilic Acyl Substitution 1: Carboxylic Acids18
- Ch. 19 - Nucleophilic Acyl Substitution 2: Carboxylic Acid Derivatives39
- Ch. 20 - Enolates: Carbonyl Addition and Substitution13
- Ch. 21 - Conjugated Systems 1: Stability and Addition Reactions56
- Ch. 22 - Conjugated Systems 2: Pericyclic Reactions54
- Ch. 23 - Benzene 1: Aromatic Stability and Substitution Reactions64
- Ch. 24 - Benzene 2: Reactions Influenced by the Aromatic Ring62
- Ch. 25 - Amines: Structure, Reactions, and Synthesis27
- Ch. 26 - Amino Acids, Proteins, and Peptide Synthesis9
- Ch. 27 - Carbohydrates, Nucleic Acids, and Lipids54
Mullins1st EditionOrganic Chemistry: A Learner Centered ApproachISBN: 9780137566471Non è quello che usi tu?Cambia libro di testo
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Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblema 80
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblema 80Capitolo 1, Problema 80
The C―H σ bond length in ethane is 1.09 Å. The C―H σ bond in ethene is 1.07 Å. Explain.
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The bond length of a C―H σ bond is influenced by the hybridization of the carbon atom involved in the bond. In ethane, the carbon atoms are sp³ hybridized, while in ethene, the carbon atoms are sp² hybridized.
The sp³ hybridization in ethane results in orbitals with 25% s-character and 75% p-character. In contrast, sp² hybridization in ethene results in orbitals with 33% s-character and 67% p-character.
Orbitals with higher s-character (as in sp² hybridization) are closer to the nucleus, leading to shorter bond lengths. This explains why the C―H bond in ethene (1.07 Å) is shorter than the C―H bond in ethane (1.09 Å).
The increased s-character in sp² hybridized orbitals also results in stronger and more tightly held bonds, contributing to the shorter bond length in ethene compared to ethane.
In summary, the difference in C―H bond lengths between ethane and ethene is due to the difference in hybridization of the carbon atoms, which affects the orbital characteristics and bond strength.
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Bond Length
Bond length is the distance between the nuclei of two bonded atoms. It is influenced by the type of bond (single, double, or triple) and the atomic radii of the involved elements. In general, shorter bond lengths indicate stronger bonds due to increased overlap of atomic orbitals.
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Single bonds, double bonds, and triple bonds.
Hybridization
Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate bonding. In ethane (C2H6), carbon undergoes sp3 hybridization, resulting in single C―H bonds. In contrast, ethene (C2H4) features sp2 hybridization, leading to a double bond between carbons, which affects bond lengths.
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10:43Using bond sites to predict hybridization
Bond Order
Bond order refers to the number of chemical bonds between a pair of atoms. A higher bond order typically results in a shorter bond length and greater bond strength. Ethene has a bond order of 1.5 for the C―H bonds due to the presence of a double bond between the carbon atoms, which contributes to the shorter bond length compared to ethane.
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06:00Single bonds, double bonds, and triple bonds.
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There is free rotation around the C―C bond in ethane. There is an extremely high barrier to rotation around the C=C bond in in ethene. Explain.
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In propene, the indicated C―C bond length is 1.51 Å. In the allyl cation, the indicated C―C bond length is 1.41 Å. Explain.
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Carbon dioxide (CO2) has no dipole moment (μ = 0 D). The related molecule sulfur dioxide (SO2) does have a dipole moment (μ = 1.6 D) Explain this observation.
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In comparison to CH3+ in Assessment 2.82, the related molecule H3O+ is not a Lewis acid at oxygen. Why?
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Domanda del libro di testo
Given the Lewis structures, indicate the direction of the dipole moment, if there is one.
(e)
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