Chemistry
Chemistry
4th Edition
ISBN: 9780393919370
Author: Thomas R. Gilbert
Publisher: NORTON
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Chapter 8, Problem 8.90QP
Interpretation Introduction

Interpretation: All the resonance forms of the sulfur-nitrogen anion, S4N are to be drawn and formal charges are to be assigned.

Concept introduction: Formal charges play an important role in choosing between the possible molecular structures. The preferred structure is the one in which formal charges are zero.

To determine: All the resonance forms of the sulfur-nitrogen anion, S4N and the formal charges.

Expert Solution & Answer
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Answer to Problem 8.90QP

Solution

All the resonance forms of the sulfur-nitrogen anion, S4N are shown in Figure 1 and formal charges have been assigned.

Explanation of Solution

Explanation

The given anion is S4N . Number of valence electrons in sulfur is 6 and number of valence electrons in nitrogen is 5 . There are four sulfur atoms and one nitrogen atom present in S4N . There is an additional charge of 1 in the anion, therefore the total valence electrons are =(4×6)+(1×5)+1=30

It is given that the atoms are arranged as SSNSS . The lone pairs of electrons on sulfur are delocalized which results in the formation of different lewis structures. The lewis structures for S4N are,

Chemistry, Chapter 8, Problem 8.90QP

Figure 1

The atoms in the resonating structures are named as a,b,c,d and e.

The formal charge on each atom of resonating structure (I) of S4N is calculated as,

Formal charge is calculated by the formula,

Formalcharge=Valenceelectrons(Lonepairelectrons+12Bondpairelectrons) (1)

Number of valence electrons in S (a) is 6 .

Number of lone pair electrons in S (a) is 6 .

Number of bond pair electrons in S (a) is 2 .

To calculate the formal charge on S (a), substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).

Formalcharge=6(6+12(2))=1

Number of valence electrons in S (b) is 6 .

Number of lone pair electrons in S (b) is 2 .

Number of bond pair electrons in S (b) is 6 .

To calculate the formal charge on S (b), substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).

Formalcharge=6(2+12(6))=1

Number of valence electrons in nitrogen (c) is 5 .

Number of lone pair electrons in nitrogen (c) is 2 .

Number of bond pair electrons in nitrogen (c) is 6 .

To calculate the formal charge on nitrogen (c), substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).

Formalcharge=5(2+12(6))=0

Number of valence electrons in S (d) is 6 .

Number of lone pair electrons in S (d) is 4 .

Number of bond pair electrons in S (d) is 4 .

To calculate the formal charge on S (d), substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).

Formalcharge=6(4+12(4))=0

Number of valence electrons in S (e) is 6 .

Number of lone pair electrons in S (e) is 6 .

Number of bond pair electrons in S (e) is 2 .

To calculate the formal charge on S (e), substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).

Formalcharge=6(6+12(2))=1

The formal charge on each atom of resonating structure (II) of S4N is calculated as,

Number of valence electrons in S (a) is 6 .

Number of lone pair electrons in S (a) is 6 .

Number of bond pair electrons in S (a) is 2 .

To calculate the formal charge on S (a), substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).

Formalcharge=6(6+12(2))=1

Number of valence electrons in S (b) is 6 .

Number of lone pair electrons in S (b) is 4 .

Number of bond pair electrons in S (b) is 4 .

To calculate the formal charge on S (b), substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).

Formalcharge=6(4+12(4))=0

Number of valence electrons in nitrogen (c) is 5 .

Number of lone pair electrons in nitrogen (c) is 2 .

Number of bond pair electrons in nitrogen (c) is 6 .

To calculate the formal charge on nitrogen (c), substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).

Formalcharge=5(2+12(6))=0

Number of valence electrons in S (d) is 6 .

Number of lone pair electrons in S (d) is 2 .

Number of bond pair electrons in S (d) is 6 .

To calculate the formal charge on S (d), substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).

Formalcharge=6(2+12(6))=1

Number of valence electrons in S (e) is 6 .

Number of lone pair electrons in S (e) is 6 .

Number of bond pair electrons in S (e) is 2 .

To calculate the formal charge on S (e), substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).

Formalcharge=6(6+12(2))=1

The formal charge on each atom of resonating structure (III) of S4N is calculated as,

Number of valence electrons in S (a) is 6 .

Number of lone pair electrons in S (a) is 4 .

Number of bond pair electrons in S (a) is 4 .

To calculate the formal charge on S (a), substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).

Formalcharge=6(4+12(4))=0

Number of valence electrons in S (b) is 6 .

Number of lone pair electrons in S (b) is 2 .

Number of bond pair electrons in S (b) is 8 .

To calculate the formal charge on S (b), substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).

Formalcharge=6(2+12(8))=0

Number of valence electrons in nitrogen (c) is 5 .

Number of lone pair electrons in nitrogen (c) is 2 .

Number of bond pair electrons in nitrogen (c) is 6 .

To calculate the formal charge on nitrogen (c), substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).

Formalcharge=5(2+12(6))=0

Number of valence electrons in S (d) is 6 .

Number of lone pair electrons in S (d) is 4 .

Number of bond pair electrons in S (d) is 4 .

To calculate the formal charge on S (d), substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).

Formalcharge=6(4+12(4))=0

Number of valence electrons in S (e) is 6 .

Number of lone pair electrons in S (e) is 6 .

Number of bond pair electrons in S (e) is 2 .

To calculate the formal charge on S (e), substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).

Formalcharge=6(6+12(2))=1

The formal charge on each atom of resonating structure (IV) of S4N is calculated as,

Number of valence electrons in S (a) is 6 .

Number of lone pair electrons in S (a) is 6 .

Number of bond pair electrons in S (a) is 2 .

To calculate the formal charge on S (a), substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).

Formalcharge=6(6+12(2))=1

Number of valence electrons in S (b) is 6 .

Number of lone pair electrons in S (b) is 4 .

Number of bond pair electrons in S (b) is 4 .

To calculate the formal charge on S (b), substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).

Formalcharge=6(4+12(4))=0

Number of valence electrons in nitrogen (c) is 5 .

Number of lone pair electrons in nitrogen (c) is 2 .

Number of bond pair electrons in nitrogen (c) is 6 .

To calculate the formal charge on nitrogen (c), substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).

Formalcharge=5(2+12(6))=0

Number of valence electrons in S (d) is 6 .

Number of lone pair electrons in S (d) is 2 .

Number of bond pair electrons in S (d) is 8 .

To calculate the formal charge on S (d), substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).

Formalcharge=6(2+12(8))=0

Number of valence electrons in S (e) is 6 .

Number of lone pair electrons in S (e) is 4 .

Number of bond pair electrons in S (e) is 4 .

To calculate the formal charge on S (e), substitute the value of valence electrons, lone pair electrons and bond pair electrons in the equation (1).

Formalcharge=6(4+12(4))=0

Conclusion

All the resonance forms of the sulfur-nitrogen anion, S4N are shown in Figure 1 and formal charges have been assigned.

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Chapter 8 Solutions

Chemistry

Ch. 8.7 - Prob. 11PECh. 8.8 - Prob. 12PECh. 8 - Prob. 8.1VPCh. 8 - Prob. 8.2VPCh. 8 - Prob. 8.3VPCh. 8 - Prob. 8.4VPCh. 8 - Prob. 8.5VPCh. 8 - Prob. 8.6VPCh. 8 - Prob. 8.7VPCh. 8 - Prob. 8.8VPCh. 8 - Prob. 8.9VPCh. 8 - Prob. 8.10VPCh. 8 - Prob. 8.11VPCh. 8 - Prob. 8.12VPCh. 8 - Prob. 8.13VPCh. 8 - Prob. 8.14VPCh. 8 - Prob. 8.15VPCh. 8 - Prob. 8.16VPCh. 8 - Prob. 8.17VPCh. 8 - Prob. 8.18VPCh. 8 - Prob. 8.19QPCh. 8 - Prob. 8.20QPCh. 8 - Prob. 8.21QPCh. 8 - Prob. 8.22QPCh. 8 - Prob. 8.23QPCh. 8 - Prob. 8.24QPCh. 8 - Prob. 8.25QPCh. 8 - Prob. 8.26QPCh. 8 - Prob. 8.27QPCh. 8 - Prob. 8.28QPCh. 8 - Prob. 8.29QPCh. 8 - Prob. 8.30QPCh. 8 - Prob. 8.31QPCh. 8 - Prob. 8.32QPCh. 8 - Prob. 8.33QPCh. 8 - Prob. 8.34QPCh. 8 - Prob. 8.35QPCh. 8 - Prob. 8.36QPCh. 8 - Prob. 8.37QPCh. 8 - Prob. 8.38QPCh. 8 - Prob. 8.39QPCh. 8 - Prob. 8.40QPCh. 8 - Prob. 8.41QPCh. 8 - Prob. 8.42QPCh. 8 - Prob. 8.43QPCh. 8 - Prob. 8.44QPCh. 8 - Prob. 8.45QPCh. 8 - Prob. 8.46QPCh. 8 - Prob. 8.47QPCh. 8 - Prob. 8.48QPCh. 8 - Prob. 8.49QPCh. 8 - Prob. 8.50QPCh. 8 - Prob. 8.51QPCh. 8 - Prob. 8.52QPCh. 8 - Prob. 8.53QPCh. 8 - Prob. 8.54QPCh. 8 - Prob. 8.55QPCh. 8 - Prob. 8.56QPCh. 8 - Prob. 8.57QPCh. 8 - Prob. 8.58QPCh. 8 - Prob. 8.59QPCh. 8 - Prob. 8.60QPCh. 8 - Prob. 8.61QPCh. 8 - Prob. 8.62QPCh. 8 - Prob. 8.63QPCh. 8 - Prob. 8.64QPCh. 8 - Prob. 8.65QPCh. 8 - Prob. 8.66QPCh. 8 - Prob. 8.67QPCh. 8 - Prob. 8.68QPCh. 8 - Prob. 8.69QPCh. 8 - Prob. 8.70QPCh. 8 - Prob. 8.71QPCh. 8 - Prob. 8.72QPCh. 8 - Prob. 8.73QPCh. 8 - Prob. 8.74QPCh. 8 - Prob. 8.75QPCh. 8 - Prob. 8.76QPCh. 8 - Prob. 8.77QPCh. 8 - Prob. 8.78QPCh. 8 - Prob. 8.79QPCh. 8 - Prob. 8.80QPCh. 8 - Prob. 8.81QPCh. 8 - Prob. 8.82QPCh. 8 - Prob. 8.83QPCh. 8 - Prob. 8.84QPCh. 8 - Prob. 8.85QPCh. 8 - Prob. 8.86QPCh. 8 - Prob. 8.87QPCh. 8 - Prob. 8.88QPCh. 8 - Prob. 8.89QPCh. 8 - Prob. 8.90QPCh. 8 - Prob. 8.91QPCh. 8 - Prob. 8.92QPCh. 8 - Prob. 8.93QPCh. 8 - Prob. 8.94QPCh. 8 - Prob. 8.95QPCh. 8 - Prob. 8.96QPCh. 8 - Prob. 8.97QPCh. 8 - Prob. 8.98QPCh. 8 - Prob. 8.99QPCh. 8 - Prob. 8.100QPCh. 8 - Prob. 8.101QPCh. 8 - Prob. 8.102QPCh. 8 - Prob. 8.103QPCh. 8 - Prob. 8.104QPCh. 8 - Prob. 8.105QPCh. 8 - Prob. 8.106QPCh. 8 - Prob. 8.107QPCh. 8 - Prob. 8.108QPCh. 8 - Prob. 8.109QPCh. 8 - Prob. 8.110QPCh. 8 - Prob. 8.111QPCh. 8 - Prob. 8.112QPCh. 8 - Prob. 8.113QPCh. 8 - Prob. 8.114QPCh. 8 - Prob. 8.115QPCh. 8 - Prob. 8.116QPCh. 8 - Prob. 8.117QPCh. 8 - Prob. 8.118QPCh. 8 - Prob. 8.119QPCh. 8 - Prob. 8.120QPCh. 8 - Prob. 8.121QPCh. 8 - Prob. 8.122QPCh. 8 - Prob. 8.123QPCh. 8 - Prob. 8.124QPCh. 8 - Prob. 8.125QPCh. 8 - Prob. 8.126QPCh. 8 - Prob. 8.127QPCh. 8 - Prob. 8.128QPCh. 8 - Prob. 8.129QPCh. 8 - Prob. 8.130QPCh. 8 - Prob. 8.131QPCh. 8 - Prob. 8.132QPCh. 8 - Prob. 8.133QPCh. 8 - Prob. 8.134QPCh. 8 - Prob. 8.135QPCh. 8 - Prob. 8.136QPCh. 8 - Prob. 8.137QPCh. 8 - Prob. 8.138QPCh. 8 - Prob. 8.139APCh. 8 - Prob. 8.140APCh. 8 - Prob. 8.141APCh. 8 - Prob. 8.142APCh. 8 - Prob. 8.143APCh. 8 - Prob. 8.144APCh. 8 - Prob. 8.145APCh. 8 - Prob. 8.146APCh. 8 - Prob. 8.147APCh. 8 - Prob. 8.148APCh. 8 - Prob. 8.149APCh. 8 - Prob. 8.150APCh. 8 - Prob. 8.151APCh. 8 - Prob. 8.152APCh. 8 - Prob. 8.153APCh. 8 - Prob. 8.154APCh. 8 - Prob. 8.155APCh. 8 - Prob. 8.156APCh. 8 - Prob. 8.157APCh. 8 - Prob. 8.158APCh. 8 - Prob. 8.159APCh. 8 - Prob. 8.160APCh. 8 - Prob. 8.161APCh. 8 - Prob. 8.162APCh. 8 - Prob. 8.163APCh. 8 - Prob. 8.164APCh. 8 - Prob. 8.165APCh. 8 - Prob. 8.166APCh. 8 - Prob. 8.167APCh. 8 - Prob. 8.168APCh. 8 - Prob. 8.169APCh. 8 - Prob. 8.170APCh. 8 - Prob. 8.171APCh. 8 - Prob. 8.172APCh. 8 - Prob. 8.173APCh. 8 - Prob. 8.174APCh. 8 - Prob. 8.175APCh. 8 - Prob. 8.176AP
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