Chemistry: The Science in Context (Fifth Edition)
Chemistry: The Science in Context (Fifth Edition)
5th Edition
ISBN: 9780393614046
Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster, Stacey Lowery Bretz, Geoffrey Davies
Publisher: W. W. Norton & Company
Question
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Chapter 8, Problem 8.108QP

(a)

Interpretation Introduction

Interpretation: Odd-electron molecules among the given nitrogen oxides are to be identified.

Concept introduction: A molecule is said to be an odd-electron when the sum of the valence electrons of all the atoms in a molecules is odd that is the total number of bonds formed in a molecule is a fraction.

To determine: If the given nitrogen oxide is an odd-electron molecule.

(a)

Expert Solution
Check Mark

Answer to Problem 8.108QP

Solution

The molecule NO is an odd-electron molecule.

Explanation of Solution

Explanation

The given molecule is NO . It consists of 1 nitrogen and 1 oxygen atoms. Nitrogen has 5 valence electrons and oxygen has 6 valence electrons. The total number of electrons required to complete an octet is calculated as,

1N+1O=1(8)+1(8)=8+8=16

The total number of valence electrons is calculated as,

1N+1O=1(5)+1(6)=5+6=11

The total number of valence electrons in NO is 11 . Therefore, the difference between the total number of electrons and valence electron is 1611=5 electrons.

One bond contains two electrons. Therefore, the number of bonds formed in NO is 212 bonds. Hence, the bond formed is a fraction, NO molecule is an odd-electron molecule.

(b)

Interpretation Introduction

To determine: If the given nitrogen oxide is an odd-electron molecule.

(b)

Expert Solution
Check Mark

Answer to Problem 8.108QP

Solution

The molecule NO2 is an odd-electron molecule.

Explanation of Solution

Explanation

The given molecule is NO2 . It consists of 1 nitrogen and 2 oxygen atoms. Nitrogen has 5 valence electrons and oxygen has 6 valence electrons. The total number of electrons required to complete an octet is calculated as,

1N+2O=1(8)+2(8)=8+16=24

The total number of valence electrons is calculated as,

1N+2O=1(5)+2(6)=5+12=17

The total number of valence electrons in NO2 is 17 . Therefore, the difference between the total number of electrons and valence electron is 2417=7 electrons.

One bond contains two electrons. Therefore, the number of bonds formed in NO2 is 312 bonds. Hence, the bond formed is a fraction, NO2 molecule is an odd-electron molecule.

(c)

Interpretation Introduction

To determine: If the given nitrogen oxide is an odd-electron molecule.

(c)

Expert Solution
Check Mark

Answer to Problem 8.108QP

Solution

The molecule NO3 is an odd-electron molecule.

Explanation of Solution

Explanation

The given molecule is NO3 . It consists of 1 nitrogen and 3 oxygen atoms. Nitrogen has 5 valence electrons and oxygen has 6 valence electrons. The total number of electrons required to complete an octet is calculated as,

1N+3O=1(8)+3(8)=8+24=32

The total number of valence electrons is calculated as,

1N+3O=1(5)+3(6)=5+18=23

The total number of valence electrons in NO3 is 23 . Therefore, the difference between the total number of electrons and valence electron is 3223=9 electrons.

One bond contains two electrons. Therefore, the number of bonds formed in NO3 is 412 bonds. Hence, the bond formed is a fraction, NO3 molecule is an odd-electron molecule.

(d)

Interpretation Introduction

To determine: If the given nitrogen oxide is an odd-electron molecule.

(d)

Expert Solution
Check Mark

Answer to Problem 8.108QP

Solution

The molecule N2O4 is not an odd-electron molecule.

Explanation of Solution

Explanation

The given molecule is N2O4 . It consists of 2 nitrogen and 4 oxygen atoms. Nitrogen has 5 valence electrons and oxygen has 6 valence electrons. The total number of electrons required to complete an octet is calculated as,

2N+4O=2(8)+4(8)=16+32=48

The total number of valence electrons is calculated as,

2N+4O=2(5)+4(6)=10+24=34

The total number of valence electrons in N2O4 is 34 . Therefore, the difference between the total number of electrons and valence electron is 4834=14 electrons.

One bond contains two electrons. Therefore, the number of bonds formed in N2O4 is 7 bonds. Hence, the bond formed is not a fraction, N2O4 molecule is not an odd-electron molecule.

(e)

Interpretation Introduction

To determine: If the given nitrogen oxide is an odd-electron molecule.

(e)

Expert Solution
Check Mark

Answer to Problem 8.108QP

Solution

The molecule N2O5 is not an odd-electron molecule.

Explanation of Solution

Explanation

The given molecule is N2O5 . It consists of 2 nitrogen and 5 oxygen atoms. Nitrogen has 5 valence electrons and oxygen has 6 valence electrons. The total number of electrons required to complete an octet is calculated as,

2N+5O=2(8)+5(8)=16+40=56

The total number of valence electrons is calculated as,

2N+5O=2(5)+5(6)=10+30=40

The total number of valence electrons in N2O5 is 40 . Therefore, the difference between the total number of electrons and valence electron is 5640=16 electrons.

One bond contains two electrons. Therefore, the number of bonds formed in N2O5 is 8 bonds. Hence, the bond formed is not a fraction, N2O5 molecule is not an odd-electron molecule.

Conclusion

The molecules, NO , NO2 and NO3 are odd-electron molecules.

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Chapter 8 Solutions

Chemistry: The Science in Context (Fifth Edition)

Ch. 8.6 - Prob. 11PECh. 8.7 - 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. 8.175AP
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