Chemistry: An Atoms-Focused Approach
Chemistry: An Atoms-Focused Approach
14th Edition
ISBN: 9780393912340
Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster
Publisher: W. W. Norton & Company
Question
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Chapter 4, Problem 4.121QA
Interpretation Introduction

To find:

a) Draw Lewis structure for possible arrangement of N-O-N  in N2O.

b) Assign formal charges of each structure.

c) Give reason why structure is not stable.

Expert Solution & Answer
Check Mark

Answer to Problem 4.121QA

Solution:

a) i)  ii)

Chemistry: An Atoms-Focused Approach, Chapter 4, Problem 4.121QA , additional homework tip  1 Chemistry: An Atoms-Focused Approach, Chapter 4, Problem 4.121QA , additional homework tip  2

b) i) Formal charge on each N is -1 and on O is +2.

ii)  Formal charge on one of N is -2 and on O is +2.

c) In both structure the formal charge on oxygen is +2. Since oxygen is more electronegative than Nitrogen none of these structure is stable.

Explanation of Solution

1) Concept:

Each molecule contains two Nitrogen and one oxygen has an overall charge zero. Nitrogen and oxygen are in group 15 and 16 and have bonding capacity three and two. Nitrogen can show hypervalency.

2) Calculations:

The number of valence electrons are,

Elements Valence electrons
Symbol Number of atom In one atom Total
N 2 5 10
O 1 6 6
Valence electrons in molecule 16

First possible arrangement of N-O-N  is,

Chemistry: An Atoms-Focused Approach, Chapter 4, Problem 4.121QA , additional homework tip  3

Second possible arrangement of N-O-N  is,

Chemistry: An Atoms-Focused Approach, Chapter 4, Problem 4.121QA , additional homework tip  4

Formula:

To find formal charge we need to use following equation,

Formal charge=Number of valence electrons- Number of electrons in lone pairs+12 Number of shared electrons

Calculation:

Step 1) Calculations of formal charge on atoms in first structure,

Formal charge on N=5- 4+12 4= -1

Formal charge on O=6- 0+12 8= +2

Step 2) Calculations of formal charge on atoms in second structure,

Formal charge on N=5- 6+12 2= -2

Formal charge on O=6- 0+12 8= +2

Formal charge on N=5- 2+12 6= 0

Oxygen has electronegativity 3.5 and nitrogen has electronegativity 3.0. Thus, structures with formal negative charges on nitrogen and formal positive charges on oxygen are not preferred. Therefore none of these structures is stable.

Conclusion:

a) Lewis structure for possible arrangement of N-O-N  in N2O are,

i)  ii)

Chemistry: An Atoms-Focused Approach, Chapter 4, Problem 4.121QA , additional homework tip  5 Chemistry: An Atoms-Focused Approach, Chapter 4, Problem 4.121QA , additional homework tip  6

b) i) Formal charge on each N is -1 and on O is +2.

ii)  Formal charge on one of N is -2 and on O is 2+

c) Oxygen is more electronegative than Nitrogen and each of structure contains +2 charge on oxygen so none of these structure is likely to be stable.

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Chapter 4 Solutions

Chemistry: An Atoms-Focused Approach

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