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Ch. 15 - Conjugated Systems, Orbital Symmetry, and Ultraviolet Spectroscopy
Wade - Organic Chemistry 9th Edition
Wade9th EditionOrganic ChemistryISBN: 9780135213728Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoWade 9th EditionCh. 15 - Conjugated Systems, Orbital Symmetry, and Ultraviolet SpectroscopyProblema 27c
Capitolo 15, Problema 27c

Draw the important resonance contributors for the following cations, anions, and radicals.
(c)

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1
Identify the structure of the given species (cation, anion, or radical) and locate any pi bonds, lone pairs, or unpaired electrons that can participate in resonance.
Determine the possible movement of electrons. For cations, look for adjacent pi bonds or lone pairs that can donate electron density. For anions, look for lone pairs or pi bonds that can delocalize the negative charge. For radicals, consider the movement of the unpaired electron in conjunction with pi bonds.
Draw the resonance structures by moving electrons appropriately. Use curved arrows to indicate the movement of electrons: a single-headed arrow for radicals and a double-headed arrow for cations and anions.
Ensure that each resonance structure follows the rules of resonance: maintain the same number of electrons, avoid exceeding the octet rule for second-row elements, and ensure that the overall charge of the molecule remains the same.
Label the resonance contributors to indicate their relative importance. Typically, structures with full octets, minimal formal charges, and charges placed on atoms with appropriate electronegativity are more significant contributors.

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Resonance Structures

Resonance structures are different Lewis structures for the same molecule that depict the same arrangement of atoms but differ in the placement of electrons. These structures help illustrate the delocalization of electrons within a molecule, which can stabilize cations, anions, and radicals. Understanding resonance is crucial for predicting the reactivity and stability of these species.
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Cation Stability

Cations are positively charged species formed by the loss of electrons. Their stability is influenced by factors such as the degree of positive charge delocalization and the presence of electron-donating groups. Recognizing how resonance can distribute the positive charge across multiple atoms is essential for evaluating the stability of cations.
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Radical Stability

Radicals are species with unpaired electrons, making them highly reactive. The stability of radicals can be enhanced through resonance, where the unpaired electron can be delocalized over adjacent atoms. Understanding the factors that contribute to radical stability, including resonance and steric effects, is vital for analyzing their behavior in chemical reactions.
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The radical stability trend.
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