Chemistry
Chemistry
4th Edition
ISBN: 9780393919370
Author: Thomas R. Gilbert
Publisher: NORTON
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Chapter 8, Problem 8.119QP

(a)

Interpretation Introduction

Interpretation: The given ions are to be ranked in order of increasing nitrogen-oxygen bond lengths and increasing bond energies.

Concept introduction: The bond length is the distance between the nuclei of atoms and bond order is defined as the total number of bonds present in a molecule. When the bond order is high, the bond length is shorter because of the stronger attraction between the atoms. Bond length shows inverse relation with the bond energy.

To determine: The order of increasing nitrogen-oxygen bond lengths for the given ions.

(a)

Expert Solution
Check Mark

Answer to Problem 8.119QP

Solution

The order of increasing nitrogen-oxygen bond lengths for the given ions is NO+<NO2<NO3 .

Explanation of Solution

Explanation

The order of nitrogen-oxygen bond lengths is predicted by calculating the bond order of the given ions. The bond order is inversely proportional to the bond length in a given ion or a molecule. So, more is the bond order value less is the bond strength.

The given ions are NO2 , NO+ and NO3 . Nitrogen and oxygen belongs to 15 and 16 groups of the periodic table and has five and six valence electrons respectively. Therefore, NO molecule has 5+6=11 total valence electrons.

By losing one electron it forms NO+ ion having 10 valence electrons. It consists of three electron pair and one NO bond. The structure of NO+ ion is,

Chemistry, Chapter 8, Problem 8.119QP , additional homework tip  1

Figure 1

The average bond order of NO bond in NO+ ion is calculated by using the formula,

Averagebondorder=TotalnumberofelectronpairinNObondsTotalnumberofNObonds

Substitute the values of number of electron pair and NO bonds in the above formula to calculate the bond order of NO+ ion.

Averagebondorder=31=3

The bond order of NO bond in NO+ ion is 3 .

The NO2 ion has one nitrogen and two oxygen atoms.

Nitrogen and oxygen belongs to 15 and 16 groups of the periodic table and has five and six valence electrons respectively. The total valence electrons in NO2 ion is calculated as,

1N+2O+chargeonion=1(5)+2(6)+1=5+12+1=18

The structure of NO2 ion is,

Chemistry, Chapter 8, Problem 8.119QP , additional homework tip  2

Figure 2

The NO2 ion has three electron pair and two NO bonds. The average bond order of NO bond in NO2 ion is calculated by using the formula,

Averagebondorder=TotalnumberofelectronpairinNObondsTotalnumberofNObonds

Substitute the values of number of electron pair and NO bonds in the above formula to calculate the bond order of NO2 ion.

Averagebondorder=32=1.5

The bond order of NO bond in NO2 ion is 1.5 .

The NO3 ion has one nitrogen and three oxygen atoms.

Nitrogen and oxygen belongs to 15 and 16 groups of the periodic table and has five and six valence electrons respectively. The total valence electrons in NO3 ion is calculated as,

1N+3O+chargeonion=1(5)+3(6)+1=5+18+1=24

The structure of NO3 ion is,

Chemistry, Chapter 8, Problem 8.119QP , additional homework tip  3

Figure 3

The NO3 ion has four electron pair and three NO bonds. The average bond order of NO bond in NO3 ion is calculated by using the formula,

Averagebondorder=TotalnumberofelectronpairinNObondsTotalnumberofNObonds

Substitute the values of number of electron pair and NO bonds in the above formula to calculate the bond order of NO3 ion.

Averagebondorder=43=1.3

The bond order of NO bond in NO3 ion is 1.3 .

The increasing order of bond order for the given ions is NO3<NO2<NO+ . As the bond order is inversely proportional to the bond length, the increasing order of bond lengths for the given ions is NO+<NO2<NO3 .

(b)

Interpretation Introduction

To determine: The order of increasing bond energies for the given ions.

(b)

Expert Solution
Check Mark

Answer to Problem 8.119QP

Solution

The order of increasing bond energies for the given ions is NO3<NO2<NO+ .

Explanation of Solution

Explanation

The bond energy shows inverse relation to the bond length that is more is the bond length lesser is the amount of energy required to break the bond. Bond energy is directly proportional to the bond order in a given molecule or ion.

Hence, the increasing order of bond energies for the given ions is NO3<NO2<NO+ .

Conclusion

  1. a. The order of increasing NO bond lengths for the given ions is NO+<NO2<NO3 .
  2. b. The order of increasing bond energies for the given ions is NO3<NO2<NO+ .

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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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