Textbook Question
Determine whether the following pairs of structures are actually different compounds or simply resonance forms of the same compounds.
a.
b.
c.
d.
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Ch.1 - Structure and Bonding
Wade9th EditionOrganic ChemistryISBN: 9780135213728
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Table of contents
- Ch.1 - Structure and Bonding107
- Ch. 2 - Acids and Bases; Functional Groups115
- Ch.3 - Structure and Stereochemistry of Alkanes100
- Ch.4 - The Study of Chemical Reactions99
- Ch.5 - Stereochemistry93
- Ch.6 - Alkyl Halides; Nucleophilic Substitution118
- Ch. 7 - Structure and Synthesis of Alkenes; Elimination158
- Ch.8 - Reactions of Alkenes171
- Ch.9 - Alkynes91
- Ch.10 - Structure and Synthesis of Alcohols143
- Ch.11 - Reactions of Alcohols104
- Ch. 12 - Infrared Spectroscopy and Mass Spectrometry22
- Ch. 13 - Nuclear Magnetic Resonance Spectroscopy45
- Ch. 14 - Ethers, Epoxides, and Thioethers72
- Ch. 15 - Conjugated Systems, Orbital Symmetry, and Ultraviolet Spectroscopy89
- Ch. 16 - Aromatic Compounds74
- Ch. 17 - Reactions of Aromatic Compounds126
- Ch. 18 - Ketones and Aldehydes193
- Ch. 19 - Amines129
- Ch. 20 - Carboxylic Acids77
- Ch. 21 - Carboxylic Acid Derivatives141
- Ch. 22 - Condensations and Alpha Substitutions of Carbonyl Compounds175
- Ch. 23 - Carbohydrates and Nucleic Acids93
- Ch. 24 - Amino Acids, Peptides, and Proteins54
Chapter 1, Problem 41e-h
Determine whether the following pairs of structures are actually different compounds or simply resonance forms of the same compounds.
e. 
f. 
g. 
h. 
Verified step by step guidance1
Step 1: Understand the concept of resonance. Resonance structures are different ways of drawing the same molecule, showing the delocalization of electrons. They are not different compounds but different representations of the same compound.
Step 2: Analyze pair (e): CH₂=C-O⁻ and ⁻CH₂-C=O-H. Check if they can be interconverted by moving electrons without breaking any sigma bonds. The first structure has a negative charge on oxygen, while the second has a negative charge on carbon. These are not resonance forms but different compounds.
Step 3: Analyze pair (f): CH₃-C⁺=NH₂ and CH₃-C=NH₂⁺. Check if they can be interconverted by moving electrons. The positive charge is on different atoms in each structure, indicating they are not resonance forms but different compounds.
Step 4: Analyze pair (g): CH₂=CH-CH₂⁺ and ⁺CH₂-CH=CH₂. Check if they can be interconverted by moving electrons. The positive charge can be moved between the carbon atoms through resonance, indicating they are resonance forms of the same compound.
Step 5: Analyze pair (h): CH₂=C=O and H-C≡C-OH. Check if they can be interconverted by moving electrons. The connectivity of atoms is different, indicating they are not resonance forms but different compounds.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Resonance Structures
Resonance structures are different ways of drawing the same molecule that illustrate the delocalization of electrons. They are not distinct compounds but rather representations that help visualize the electron distribution within a molecule. The actual structure is a hybrid of these forms, which contributes to the stability and reactivity of the compound.
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03:04
Drawing Resonance Structures
Formal Charge
Formal charge is a theoretical charge assigned to an atom in a molecule, calculated based on the number of valence electrons, the number of non-bonding electrons, and half the number of bonding electrons. It helps in determining the most stable resonance structure, as structures with lower formal charges are generally more favorable. Understanding formal charge is crucial for evaluating the differences between resonance forms.
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01:34Calculating formal and net charge.
Stability of Resonance Forms
The stability of resonance forms is determined by factors such as the arrangement of charges, the presence of complete octets, and the overall energy of the structure. More stable resonance forms contribute more to the resonance hybrid, while less stable forms are less significant. Analyzing the stability of these forms is essential for understanding the behavior and properties of the compound in question.
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Related Practice
Textbook Question
1. From what you remember of electronegativities, show the direction of the dipole moments of the following bonds.
2. In each case, predict whether the dipole moment is relatively large (electronegativity difference >0.5) or small.
a. C—Cl
b. C—H
c. C—Li
d. C—N
e. C—O
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Textbook Question
Draw the important resonance forms to show the delocalization of charges in the following ions. In each case, indicate the major resonance form(s).
(j)
(k)
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Textbook Question
For each of the following structures,
1. Draw a Lewis structure; fill in any nonbonding electrons.
2. Calculate the formal charge on each atom other than hydrogen
d. [(CH3)3O]+
e. CH3NC
f. (CH3)4NBr
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Textbook Question
In the following sets of resonance forms, label the major and minor contributors and state which structures would be of equal energy. Add any missing important resonance forms.
(d)
(e)
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Textbook Question
Determine whether the following pairs of structures are actually different compounds or simply resonance forms of the same compounds.
i.
j.
k.
l.
970
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