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Chemistry / Chemistry: The Central Science 13 / Chapter 16 / Problem 16.67

Chemistry: The Central Science | 13th Edition | ISBN: 9780321910417 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus

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Consider the base hydroxylamine, NH2OH. (a) What is the

Chapter , Problem 16.67

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QUESTION:

Consider the base hydroxylamine, NH2OH. (a) What is the conjugate acid of hydroxylamine? (b) When it acts as a base, which atom in hydroxylamine accepts a proton? (c) There are two atoms in hydroxylamine that have nonbonding electron pairs that could act as proton acceptors. Use Lewis structures and formal charges (Section 8.5) to rationalize why one of these two atoms is a much better proton acceptor than the other.

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QUESTION:

Consider the base hydroxylamine, NH2OH. (a) What is the conjugate acid of hydroxylamine? (b) When it acts as a base, which atom in hydroxylamine accepts a proton? (c) There are two atoms in hydroxylamine that have nonbonding electron pairs that could act as proton acceptors. Use Lewis structures and formal charges (Section 8.5) to rationalize why one of these two atoms is a much better proton acceptor than the other.

ANSWER:

Problem 16.67

Consider the base hydroxylamine, . (a) What is the conjugate acid of hydroxylamine? (b) When it acts as a base, which atom in hydroxylamine accepts a proton? (c) There are two atoms in hydroxylamine that have nonbonding electron pairs that could act as proton acceptors. Use Lewis structures and formal charges (Section 8.5) to rationalize why one of these two atoms is a much better proton acceptor than the other.

Step by Step Solution

Step 1 of 3

a)

The hydroxylamine is a weak base and it accepts a proton from water to forms

hydroxylammonium ion, . It is differing only one proton from hydroxylamine, so it is a

conjugate acid of hydroxylamine. The equation for the reaction of with water is as follows:

Therefore, the conjugate acid of is .

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