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 4.175QA
Interpretation Introduction

To draw:

a) The Lewis structures for four resonance forms of linear N5-.

b) Calculate formal charges and identify the structures that contribute the most to the bonding in N5-.

c) By comparing Lewis structures for N5- and N3-, find out the ion in which the nitrogen-nitrogen bonds have the higher average bond order.

Expert Solution & Answer
Check Mark

Answer to Problem 4.175QA

Solution:

a)

Chemistry: An Atoms-Focused Approach, Chapter 4, Problem 4.175QA , additional homework tip  1

b) The last four structures having the lowest formal charge. These structures contribute the most to the bonding in N5-.

c)

Chemistry: An Atoms-Focused Approach, Chapter 4, Problem 4.175QA , additional homework tip  2

From these resonance structures we see that each bond is predicted to be of double bond character in N3-. Therefore, in N5- there are two longer nitrogen-nitrogen bonds than in N3-. N3- has the higher average bond order.

Explanation of Solution

The ground state electronic configuration of N is 1s2 2s2 2p3.

Element Valence electrons
Symbol # of atoms In one atom Total
N 5 5 25
One electron from -1 charge 1
Valence electrons in molecule 26

Each N atom is attached with single bond.

N - N - N - N - N

Eight electrons get involved in the bond formation. Now we put remaining electrons as lone pairs on the atoms.

Chemistry: An Atoms-Focused Approach, Chapter 4, Problem 4.175QA , additional homework tip  3

The octet of terminal N atoms is get completed. The octet of remaining N is not get completed. For that we will convert some lone pairs into bond pairs.

Chemistry: An Atoms-Focused Approach, Chapter 4, Problem 4.175QA , additional homework tip  4

Now we calculate the formal charge on each atom in second structure.

Formal charge = valence electrons in atom-non bonding electrons+bonding electrons2

Formal charge on first N=5-6+ 22= -2

Formal charge on second N=5-2+ 62= 0

Formal charge on third N=5-0+ 82= +1

Formal charge on first N=5-0+ 82= +1

Formal charge on first N=5-4+ 42= -1

The Lewis structure with formal charge on N atom is as follows.

Chemistry: An Atoms-Focused Approach, Chapter 4, Problem 4.175QA , additional homework tip  5Chemistry: An Atoms-Focused Approach, Chapter 4, Problem 4.175QA , additional homework tip  6

Now we draw the resonating structures of this molecule.

Chemistry: An Atoms-Focused Approach, Chapter 4, Problem 4.175QA , additional homework tip  7

The molecules which having minimum formal charge will contribute the most to the bonding in N5-. Following structures having least formal charge and will contribute the most to the bonding in N5-.

Chemistry: An Atoms-Focused Approach, Chapter 4, Problem 4.175QA , additional homework tip  8

Chemistry: An Atoms-Focused Approach, Chapter 4, Problem 4.175QA , additional homework tip  9

Chemistry: An Atoms-Focused Approach, Chapter 4, Problem 4.175QA , additional homework tip  10

Chemistry: An Atoms-Focused Approach, Chapter 4, Problem 4.175QA , additional homework tip  11

Let’s we draw the Lewis structure of N3-.

Element Valence electrons
Symbol # of atoms In one atom Total
N 3 5 15
One electron from -1 charge 1
Valence electrons in molecule 16

Chemistry: An Atoms-Focused Approach, Chapter 4, Problem 4.175QA , additional homework tip  12

From these resonance structures we see that each bond is predicted to be of double bond character. Therefore, in N5- there are two longer nitrogen-nitrogen bonds than in N3-.

Bond order is the number of bonds between atoms. For single bond the bond order is 1. For double bond the bond order is 2. For triple bond the bond order is 3. From the resonance structure of N5- and N3-, we can say that N3- has the higher average bond order.

Conclusion:

From the electronic configuration of atoms in the molecule we can draw Lewis structure of the molecule. From the Lewis structure we can find out formal charge and bond order.

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Chapter 4 Solutions

Chemistry: An Atoms-Focused Approach

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