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The oxyanion of nitrogen in which it has the highest oxidation state is the nitrate ion (NO 3 − ). The corresponding oxyanion of phosphorus is PO 4 3− . The NO 4 3− ion is known but not very stable. The PO 3 − ion is not known. Account for these differences in terms of the bonding in the four anions.

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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

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BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 19, Problem 41E
Textbook Problem
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The oxyanion of nitrogen in which it has the highest oxidation state is the nitrate ion (NO3). The corresponding oxyanion of phosphorus is PO43−. The NO43− ion is known but not very stable. The PO3 ion is not known. Account for these differences in terms of the bonding in the four anions.

Interpretation Introduction

Interpretation: The differences in terms of the bonding in the four given anions are to be accounted for.

Concept introduction: Nitrogen cannot hold more than eight electrons due to absence of d orbitals whereas phosphorus can expand its valence shell to hold more than eight electrons. Due to difference in their size, their corresponding oxyanion also exhibits different properties.

To determine: The differences in terms of the bonding in the four given anions.

Explanation of Solution

Explanation

The oxyanion of nitrogen in which it has the highest oxidation state is nitrate ion (NO3-) . The orthonitrate ion (NO43-) is known. Nitrogen has to provide sufficient space for four oxygen atoms around it, but it has small size and accommodation of four oxygen atoms is not possible. Therefore, it is unstable. In the phosphate ion (PO43-) , the size of phosphorous is larger than nitrogen. Thus it can accommodate four oxygen atoms. Hence it is stable in comparison to NO43- ion

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Chapter 19 Solutions

Chemistry: An Atoms First Approach
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