In the following reactions,
(iv) provide an arrow-pushing mechanism of the proton transfer that will occur, and
(v) predict the product of the reactions. [You'll need to provide the lone pairs here.]
(c)

Guida verificata passo dopo passo

Step 1: Identify the reactants and their roles in the proton transfer. Ethanolate (CH3CH2O⁻) is a strong base due to its negatively charged oxygen atom, which has lone pairs of electrons. Acetic acid (CH3COOH) is a weak acid, capable of donating a proton (H⁺) from its hydroxyl group (-OH).

Step 2: Recognize the site of interaction. The negatively charged oxygen atom in ethanolate will act as a nucleophile and attack the hydrogen atom of the hydroxyl group (-OH) in acetic acid. This is the proton transfer step.

Step 3: Draw the arrow-pushing mechanism. Use curved arrows to show the movement of electrons: (i) A lone pair of electrons on the oxygen atom of ethanolate attacks the hydrogen atom of acetic acid, forming a bond. (ii) Simultaneously, the bond between the hydrogen and oxygen in acetic acid breaks, and the electrons move to the oxygen atom of acetic acid, creating an acetate ion (CH3COO⁻).

Step 4: Predict the products of the reaction. The proton transfer results in the formation of ethanol (CH3CH2OH) and acetate ion (CH3COO⁻). Ethanol is formed as the ethanolate gains a proton, and acetate ion is formed as acetic acid loses a proton.

Step 5: Verify the stability of the products. Ethanol is neutral and stable, while acetate ion is resonance-stabilized due to the delocalization of electrons between the two oxygen atoms in the carboxylate group. This makes the reaction thermodynamically favorable.

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Proton Transfer Mechanism

Proton transfer mechanisms involve the movement of a proton (H+) from one molecule to another, often facilitated by the presence of a base or acid. In this case, ethanolate acts as a base, accepting a proton from acetic acid. Understanding the arrow-pushing notation is crucial, as it visually represents the flow of electrons during the reaction, indicating how bonds are formed and broken.

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Acid-Base Reactions

Acid-base reactions are fundamental in organic chemistry, characterized by the transfer of protons between reactants. Acetic acid, a weak acid, donates a proton to the ethanolate ion, which is a strong base. Recognizing the strength of acids and bases helps predict the direction of the reaction and the stability of the resulting products.

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Lone Pairs and Bond Formation

Lone pairs are pairs of valence electrons that are not involved in bonding and can play a significant role in chemical reactions. In the context of the given reaction, the lone pair on the ethanolate ion is used to form a bond with the proton from acetic acid. Understanding how lone pairs participate in bond formation is essential for predicting the products of reactions and the overall mechanism.

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