Textbook Question
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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Table of contents
- 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 I: Properties and Electrophilic Additions158
- Ch. 9 - Alkenes II: 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 I: Infrared Spectroscopy and Mass Spectrometry54
- Ch. 15 - Structural Identification II: Nuclear Magnetic Resonance Spectroscopy93
- Ch. 16 - Metals in Organic Chemistry48
- Ch. 17 - Carbonyl Addition Reactions: Aldehydes and Ketones45
- Ch. 18 - Nucleophilic Acyl Substitution I: Carboxylic Acids18
- Ch. 19 - Nucleophilic Acyl Substitution II: Carboxylic Acid Derivatives39
- Ch. 20 - Enolates: Carbonyl Addition and Substitution13
- Ch. 21 - Conjugated Systems I: Stability and Addition Reactions56
- Ch. 22 - Conjugated Systems II: Pericyclic Reactions54
- Ch. 23 - Benzene I: Aromatic Stability and Substitution Reactions64
- Ch. 24 - Benzene II: 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: 9780137566471Not the one you use?Change textbook
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Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 77e
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 77eChapter 1, Problem 77e
Given the Lewis structures, indicate the direction of the dipole moment, if there is one.
(e) 
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Examine the Lewis structure provided. The molecule consists of a methyl group (CH₃) attached to a positively charged nitrogen (N⁺), which is bonded to two oxygen atoms. One oxygen is double-bonded, and the other is single-bonded with a negative charge (O⁻).
Identify the electronegativity of the atoms involved. Oxygen is more electronegative than nitrogen, and nitrogen is more electronegative than carbon. This difference in electronegativity will influence the direction of the dipole moment.
Analyze the bonds individually. The N⁺-O double bond will have a dipole moment pointing toward the oxygen atom due to its higher electronegativity. Similarly, the N⁺-O⁻ single bond will also have a dipole moment pointing toward the oxygen atom, but the negative charge on the oxygen intensifies this dipole.
Consider the overall molecular geometry. The molecule is not symmetrical, and the dipole moments of the N⁺-O bonds do not cancel out. Additionally, the CH₃ group contributes a small dipole moment pointing toward the nitrogen due to the electronegativity difference between carbon and nitrogen.
Combine the dipole moments to determine the net dipole direction. The dipole moments from the N⁺-O bonds dominate, and the overall dipole moment will point toward the oxygen atoms, away from the CH₃ group.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Lewis Structures
Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They help visualize the arrangement of electrons and the connectivity of atoms, which is crucial for understanding molecular geometry and polarity.
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Drawing the Lewis Structure for N2H4.
Dipole Moment
A dipole moment is a measure of the separation of positive and negative charges in a molecule, indicating its polarity. It arises when there is an uneven distribution of electron density, leading to a partial positive charge on one end and a partial negative charge on the other, which can be represented as an arrow pointing from the positive to the negative end.
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01:46How dipole-dipole forces work.
Molecular Polarity
Molecular polarity refers to the distribution of electrical charge over the atoms in a molecule. A molecule is polar if it has a net dipole moment due to differences in electronegativity between bonded atoms, which affects its physical properties and interactions with other molecules, such as solubility and boiling point.
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Related Practice
Textbook Question
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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Textbook Question
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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Textbook Question
For the following partial structures, the σ bond is shown. Add the indicated number of π bonds, being sure to specify the orientation (that is, x, y, or z axis) of the p orbitals used.
(e)
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Textbook Question
Given the Lewis structures, indicate the direction of the dipole moment, if there is one.
(b)
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Textbook Question
Given the Lewis structures, indicate the direction of the dipole moment, if there is one.
(a)
5
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