Domanda del libro di testo
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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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 82
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblema 82Capitolo 1, Problema 82
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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Understand the context: CH₃⁺ is a carbocation, which means it has a positively charged carbon atom. This positive charge arises because the carbon atom has only six electrons in its valence shell, making it electron-deficient and a Lewis acid (electron pair acceptor).
Recall the electronic configuration of carbon: Carbon has an atomic number of 6, so its ground-state electronic configuration is 1s² 2s² 2p². In CH₃⁺, the carbon atom is sp² hybridized, leaving one unhybridized p orbital.
Visualize the molecular geometry: CH₃⁺ has a trigonal planar geometry due to sp² hybridization. The three sp² orbitals form sigma bonds with the three hydrogen atoms, while the unhybridized p orbital remains empty and perpendicular to the plane of the molecule.
Determine the orbital that can accept the electron pair: The empty unhybridized p orbital on the carbon atom is the orbital that can accept the incoming electron pair. This is because it is the only orbital available and not involved in bonding.
Conclude: The new electron pair would go into the empty p orbital of the carbon atom in CH₃⁺, which is aligned perpendicular to the plane of the molecule.
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Lewis Acids and Bases
Lewis acids are defined as substances that can accept an electron pair, while Lewis bases donate an electron pair. This concept is crucial for understanding how certain molecules, like CH₃⁺, interact with other species in chemical reactions. The ability of a Lewis acid to accept electrons is fundamental in predicting the outcome of reactions involving these species.
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02:49
The Lewis definition of acids and bases.
Molecular Orbitals
Molecular orbitals are formed by the combination of atomic orbitals when atoms bond together. In the case of CH₃⁺, the molecular orbitals determine where the new electron pair will reside after it is accepted by the Lewis acid. Understanding the arrangement and energy levels of these orbitals is essential for predicting the behavior of the molecule in chemical reactions.
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08:41Review of Molecular Orbitals
Orbital Hybridization
Orbital hybridization is the process by which atomic orbitals mix to form new hybrid orbitals that can accommodate bonding. In CH₃⁺, the carbon atom undergoes sp³ hybridization, resulting in four equivalent orbitals that can form bonds. Recognizing the type of hybridization helps in determining the geometry of the molecule and the orbital into which the new electron pair will be accepted.
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04:58Bond sites, hybridization, and intermediate orbitals
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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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The C―N bond in the following amide is much stronger than the C―N bond in the amine. 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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Looking ahead in Chapter 3, we describe how the formal charge on an atom can be used to predict the number of lone pairs. Given the charge, or lack of charge, on each atom, fill in the electron pairs.
(a)
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Domanda del libro di testo
In comparison to CH3+ in Assessment 2.82, the related molecule H3O+ is not a Lewis acid at oxygen. Why?
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