Two resonance structures are shown for each molecule. Use the arrow-pushing formalism to represent the electron flow from the structure on the left to the one on the right.
(e)

검증된 단계별 안내

Step 1: Identify the resonance structures. The structure on the left has a positively charged nitrogen atom and a negatively charged oxygen atom, while the structure on the right has a neutral nitrogen atom and a double bond between the carbon and oxygen.

Step 2: Locate the electron-rich and electron-deficient areas. The lone pairs on the oxygen atom in the left structure are electron-rich, and the positively charged nitrogen atom is electron-deficient.

Step 3: Use the arrow-pushing formalism to show electron flow. Begin by moving one lone pair of electrons from the oxygen atom to form a double bond with the adjacent carbon atom.

Step 4: To maintain the octet rule, move the π electrons from the carbon-nitrogen double bond toward the nitrogen atom, converting the nitrogen atom into a neutral species with a lone pair.

Step 5: Verify the resulting resonance structure. The new structure should have a neutral nitrogen atom with a lone pair and a double bond between the carbon and oxygen, consistent with the structure on the right.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

53s

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주요 개념

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Resonance Structures

Resonance structures are different ways of drawing the same molecule that illustrate the delocalization of electrons. They are used to represent molecules that cannot be accurately depicted by a single Lewis structure. Each resonance structure contributes to the overall hybrid structure, which is a more accurate representation of the molecule's electron distribution.

Arrow-Pushing Formalism

Arrow-pushing formalism is a method used in organic chemistry to depict the movement of electrons during chemical reactions and resonance. Curved arrows indicate the direction of electron flow, showing how electrons are added or removed from bonds or atoms. This technique helps visualize the changes in electron density and the formation of new bonds.

Electron Delocalization

Electron delocalization refers to the spreading of electron density across multiple atoms in a molecule, rather than being localized between two specific atoms. This phenomenon is crucial in resonance structures, as it stabilizes the molecule by allowing electrons to be shared among several atoms, leading to lower energy configurations and increased stability.

Two resonance structures are shown for each molecule. Use the arrow-pushing formalism to represent the electron flow from the structure on the left to the one on the right. (e)