Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question
Circle the most stable resonance structure.
Transcribed Image Text:The image illustrates the resonance structures of nitrobenzene, an important organic compound in chemistry.
1. **Left Structure**:
- The benzene ring is shown with alternating double bonds.
- The nitrogen (N) is connected to the benzene ring and exhibits a positive charge.
- The oxygen (O) on the left is depicted with a single bond to the nitrogen, carrying a negative charge, and has three lone pairs.
- The oxygen (O) on the right is double-bonded to the nitrogen, with two lone pairs and no formal charge.
2. **Middle Structure**:
- Similar to the left structure but with different positioning of the bonds within the benzene ring, maintaining resonance.
- The nitrogen remains positively charged.
- The left oxygen now forms a double bond with nitrogen, with two lone pairs, while the right oxygen forms a single bond with a negative charge and three lone pairs.
3. **Right Structure**:
- Again shows the benzene ring with alternating double bonds.
- The nitrogen is bonded to the ring and positively charged.
- The right oxygen forms a double bond to the nitrogen, with two lone pairs.
- The left oxygen has a single bond to the nitrogen, carrying a negative charge and three lone pairs.
**Arrows**: Double-headed arrows between each structure indicate resonance, showing that the actual structure of nitrobenzene is a hybrid of these resonance forms. The delocalization of electrons across the molecule contributes to its stability.
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