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Chapter 9: Problem 90

The amide ion, \(\mathrm{NH}_{2}^{-}\), is a Bronsted base. Represent the reaction between the amide ion and water in terms of Lewis structures.

Short Answer

Expert verified
The reaction of the amide ion \(\mathrm{NH}_{2}^{-}\) and water can be represented using Lewis structures as follows: The amide ion, being a Bronsted base, accepts a proton (\(H^{+}\)) from water, resulting in the formation of the ammonia molecule (\(NH_{3}\)) and the hydroxide ion (\(OH^{-}\)).

Step by step solution

01

Identify the Participants

Identify the reactants in the given reaction, i.e., water (\(H_{2}O\)) and amide ion (\(NH_{2}^{-}\)).
02

Draw the Initial Lewis Structures

Draw the initial Lewis structures of the reactants. Water has the oxygen atom in center, with two single bonds to two hydrogen atoms and two lone pairs of electrons. The amide ion has the nitrogen atom in center with two single bonds to two hydrogen atoms and a lone pair of electrons, and one additional electron to get the negative charge.
03

Determine Reaction Mechanism

Since the Amide ion is a Bronsted base, it will accept a proton (\(H^{+}\)) from water molecule.
04

Draw the Final Lewis Structures

After the amide ion has accepted a proton, draw the Lewis structure of the resulting ammonia molecule (\(NH_{3}\)) and hydroxide ion (\(OH^{-}\)). For \(NH_{3}\), Nitrogen atom is in center with three single bonds to three hydrogen atoms and a lone pair of electrons. For \(OH^{-}\), Oxygen atom is in center with a single bond to a hydrogen atom and three lone pairs of electrons.

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