The number of electrons in each of the given molecular orbital for N 2 , N 2 + , N 2 − needs to be determined. N 2 N 2 + N 2 − σ 2px * π 2py * σ 2px π 2pz σ 2s σ 2s * Concept Introduction: Molecular orbital theory explained the bonding, magnetic and spectral properties of molecule. It is based on the formation of molecular orbitals by the combination of atomic orbitals. On the basis of energy and stability these molecular orbitals can be further classified in three types: Bonding molecular orbitals (BMO): They have lesser energy than atomic orbital therefore more stable compare to atomic orbital. Antibonding molecular orbitals (ABMO): They have higher energy than atomic orbital therefore less stable compare to atomic orbital. Non-bonding molecular orbitals (NBMO): They have same energy as atomic orbital. Molecular orbital diagrams represents the distribution of electrons in different molecular orbitals in increasing order of their energy. Hence lower energy molecular orbitals occupy first then only electron moves in higher energy orbitals.

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Answer 1

Question

Chapter 14, Problem 85AE

Interpretation Introduction

Interpretation: The number of electrons in each of the given molecular orbital for N2,N2+,N2− needs to be determined.

N2 N2+ N2−
σ2px*
π2py*
σ2px
π2pz
σ2s
σ2s*

Concept Introduction: Molecular orbital theory explained the bonding, magnetic and spectral properties of molecule. It is based on the formation of molecular orbitals by the combination of atomic orbitals. On the basis of energy and stability these molecular orbitals can be further classified in three types:

Bonding molecular orbitals (BMO): They have lesser energy than atomic orbital therefore more stable compare to atomic orbital.

Antibonding molecular orbitals (ABMO): They have higher energy than atomic orbital therefore less stable compare to atomic orbital.

Non-bonding molecular orbitals (NBMO): They have same energy as atomic orbital.

Molecular orbital diagrams represents the distribution of electrons in different molecular orbitals in increasing order of their energy. Hence lower energy molecular orbitals occupy first then only electron moves in higher energy orbitals.

Expert Solution & Answer

Answer to Problem 85AE

	N2	N2+	N2−
σ2p*	0	0	0
π2p*	0	0	1
σ2p	2	1	2
π2p	4	4	4
σ2s	2	2	2
σ2s*	2	2	2

Explanation of Solution

Given information:

N2,N2+,N2− are related with each other.

The molecular orbital electronic configuration of N2,N2+,N2− can be written as:

N2 = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2

N2+ = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)1

N2− = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2(π 2py*)1

Hence number of electrons in the given molecular orbitals are:

	N2	N2+	N2−
σ2p*	0	0	0
π2p*	0	0	1
σ2p	2	1	2
π2p	4	4	4
σ2s	2	2	2
σ2s*	2	2	2

Conclusion

N2 = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2

N2+ = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)1

N2− = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2(π 2py*)1

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Answer 2

Question

Chapter 14, Problem 85AE

Interpretation Introduction

Interpretation: The number of electrons in each of the given molecular orbital for N2,N2+,N2− needs to be determined.

N2 N2+ N2−
σ2px*
π2py*
σ2px
π2pz
σ2s
σ2s*

Concept Introduction: Molecular orbital theory explained the bonding, magnetic and spectral properties of molecule. It is based on the formation of molecular orbitals by the combination of atomic orbitals. On the basis of energy and stability these molecular orbitals can be further classified in three types:

Bonding molecular orbitals (BMO): They have lesser energy than atomic orbital therefore more stable compare to atomic orbital.

Antibonding molecular orbitals (ABMO): They have higher energy than atomic orbital therefore less stable compare to atomic orbital.

Non-bonding molecular orbitals (NBMO): They have same energy as atomic orbital.

Molecular orbital diagrams represents the distribution of electrons in different molecular orbitals in increasing order of their energy. Hence lower energy molecular orbitals occupy first then only electron moves in higher energy orbitals.

Expert Solution & Answer

Answer to Problem 85AE

	N2	N2+	N2−
σ2p*	0	0	0
π2p*	0	0	1
σ2p	2	1	2
π2p	4	4	4
σ2s	2	2	2
σ2s*	2	2	2

Explanation of Solution

Given information:

N2,N2+,N2− are related with each other.

The molecular orbital electronic configuration of N2,N2+,N2− can be written as:

N2 = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2

N2+ = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)1

N2− = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2(π 2py*)1

Hence number of electrons in the given molecular orbitals are:

	N2	N2+	N2−
σ2p*	0	0	0
π2p*	0	0	1
σ2p	2	1	2
π2p	4	4	4
σ2s	2	2	2
σ2s*	2	2	2

Conclusion

N2 = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2

N2+ = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)1

N2− = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2(π 2py*)1

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Answer 3

Question

Chapter 14, Problem 85AE

Interpretation Introduction

Interpretation: The number of electrons in each of the given molecular orbital for N2,N2+,N2− needs to be determined.

N2 N2+ N2−
σ2px*
π2py*
σ2px
π2pz
σ2s
σ2s*

Concept Introduction: Molecular orbital theory explained the bonding, magnetic and spectral properties of molecule. It is based on the formation of molecular orbitals by the combination of atomic orbitals. On the basis of energy and stability these molecular orbitals can be further classified in three types:

Bonding molecular orbitals (BMO): They have lesser energy than atomic orbital therefore more stable compare to atomic orbital.

Antibonding molecular orbitals (ABMO): They have higher energy than atomic orbital therefore less stable compare to atomic orbital.

Non-bonding molecular orbitals (NBMO): They have same energy as atomic orbital.

Molecular orbital diagrams represents the distribution of electrons in different molecular orbitals in increasing order of their energy. Hence lower energy molecular orbitals occupy first then only electron moves in higher energy orbitals.

Expert Solution & Answer

Answer to Problem 85AE

	N2	N2+	N2−
σ2p*	0	0	0
π2p*	0	0	1
σ2p	2	1	2
π2p	4	4	4
σ2s	2	2	2
σ2s*	2	2	2

Explanation of Solution

Given information:

N2,N2+,N2− are related with each other.

The molecular orbital electronic configuration of N2,N2+,N2− can be written as:

N2 = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2

N2+ = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)1

N2− = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2(π 2py*)1

Hence number of electrons in the given molecular orbitals are:

	N2	N2+	N2−
σ2p*	0	0	0
π2p*	0	0	1
σ2p	2	1	2
π2p	4	4	4
σ2s	2	2	2
σ2s*	2	2	2

Conclusion

N2 = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2

N2+ = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)1

N2− = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2(π 2py*)1

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Answer 4

Question

Chapter 14, Problem 85AE

Interpretation Introduction

Interpretation: The number of electrons in each of the given molecular orbital for N2,N2+,N2− needs to be determined.

N2 N2+ N2−
σ2px*
π2py*
σ2px
π2pz
σ2s
σ2s*

Concept Introduction: Molecular orbital theory explained the bonding, magnetic and spectral properties of molecule. It is based on the formation of molecular orbitals by the combination of atomic orbitals. On the basis of energy and stability these molecular orbitals can be further classified in three types:

Bonding molecular orbitals (BMO): They have lesser energy than atomic orbital therefore more stable compare to atomic orbital.

Antibonding molecular orbitals (ABMO): They have higher energy than atomic orbital therefore less stable compare to atomic orbital.

Non-bonding molecular orbitals (NBMO): They have same energy as atomic orbital.

Molecular orbital diagrams represents the distribution of electrons in different molecular orbitals in increasing order of their energy. Hence lower energy molecular orbitals occupy first then only electron moves in higher energy orbitals.

Expert Solution & Answer

Answer to Problem 85AE

	N2	N2+	N2−
σ2p*	0	0	0
π2p*	0	0	1
σ2p	2	1	2
π2p	4	4	4
σ2s	2	2	2
σ2s*	2	2	2

Explanation of Solution

Given information:

N2,N2+,N2− are related with each other.

The molecular orbital electronic configuration of N2,N2+,N2− can be written as:

N2 = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2

N2+ = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)1

N2− = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2(π 2py*)1

Hence number of electrons in the given molecular orbitals are:

	N2	N2+	N2−
σ2p*	0	0	0
π2p*	0	0	1
σ2p	2	1	2
π2p	4	4	4
σ2s	2	2	2
σ2s*	2	2	2

Conclusion

N2 = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2

N2+ = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)1

N2− = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2(π 2py*)1

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Answer 5

Chapter 14, Problem 85AE

Interpretation Introduction

Interpretation: The number of electrons in each of the given molecular orbital for N2,N2+,N2− needs to be determined.

N2 N2+ N2−
σ2px*
π2py*
σ2px
π2pz
σ2s
σ2s*

Concept Introduction: Molecular orbital theory explained the bonding, magnetic and spectral properties of molecule. It is based on the formation of molecular orbitals by the combination of atomic orbitals. On the basis of energy and stability these molecular orbitals can be further classified in three types:

Bonding molecular orbitals (BMO): They have lesser energy than atomic orbital therefore more stable compare to atomic orbital.

Antibonding molecular orbitals (ABMO): They have higher energy than atomic orbital therefore less stable compare to atomic orbital.

Non-bonding molecular orbitals (NBMO): They have same energy as atomic orbital.

Molecular orbital diagrams represents the distribution of electrons in different molecular orbitals in increasing order of their energy. Hence lower energy molecular orbitals occupy first then only electron moves in higher energy orbitals.

Expert Solution & Answer

Answer to Problem 85AE

	N2	N2+	N2−
σ2p*	0	0	0
π2p*	0	0	1
σ2p	2	1	2
π2p	4	4	4
σ2s	2	2	2
σ2s*	2	2	2

Explanation of Solution

Given information:

N2,N2+,N2− are related with each other.

The molecular orbital electronic configuration of N2,N2+,N2− can be written as:

N2 = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2

N2+ = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)1

N2− = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2(π 2py*)1

Hence number of electrons in the given molecular orbitals are:

	N2	N2+	N2−
σ2p*	0	0	0
π2p*	0	0	1
σ2p	2	1	2
π2p	4	4	4
σ2s	2	2	2
σ2s*	2	2	2

Conclusion

N2 = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2

N2+ = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)1

N2− = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2(π 2py*)1

Answer 6

Chapter 14, Problem 85AE

Interpretation Introduction

Interpretation: The number of electrons in each of the given molecular orbital for N2,N2+,N2− needs to be determined.

N2 N2+ N2−
σ2px*
π2py*
σ2px
π2pz
σ2s
σ2s*

Concept Introduction: Molecular orbital theory explained the bonding, magnetic and spectral properties of molecule. It is based on the formation of molecular orbitals by the combination of atomic orbitals. On the basis of energy and stability these molecular orbitals can be further classified in three types:

Bonding molecular orbitals (BMO): They have lesser energy than atomic orbital therefore more stable compare to atomic orbital.

Antibonding molecular orbitals (ABMO): They have higher energy than atomic orbital therefore less stable compare to atomic orbital.

Non-bonding molecular orbitals (NBMO): They have same energy as atomic orbital.

Molecular orbital diagrams represents the distribution of electrons in different molecular orbitals in increasing order of their energy. Hence lower energy molecular orbitals occupy first then only electron moves in higher energy orbitals.

Expert Solution & Answer

Answer to Problem 85AE

	N2	N2+	N2−
σ2p*	0	0	0
π2p*	0	0	1
σ2p	2	1	2
π2p	4	4	4
σ2s	2	2	2
σ2s*	2	2	2

Explanation of Solution

Given information:

N2,N2+,N2− are related with each other.

The molecular orbital electronic configuration of N2,N2+,N2− can be written as:

N2 = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2

N2+ = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)1

N2− = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2(π 2py*)1

Hence number of electrons in the given molecular orbitals are:

	N2	N2+	N2−
σ2p*	0	0	0
π2p*	0	0	1
σ2p	2	1	2
π2p	4	4	4
σ2s	2	2	2
σ2s*	2	2	2

Conclusion

N2 = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2

N2+ = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)1

N2− = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2(π 2py*)1

Answer 7

Chapter 14, Problem 85AE

Interpretation Introduction

Interpretation: The number of electrons in each of the given molecular orbital for N2,N2+,N2− needs to be determined.

N2 N2+ N2−
σ2px*
π2py*
σ2px
π2pz
σ2s
σ2s*

Concept Introduction: Molecular orbital theory explained the bonding, magnetic and spectral properties of molecule. It is based on the formation of molecular orbitals by the combination of atomic orbitals. On the basis of energy and stability these molecular orbitals can be further classified in three types:

Bonding molecular orbitals (BMO): They have lesser energy than atomic orbital therefore more stable compare to atomic orbital.

Antibonding molecular orbitals (ABMO): They have higher energy than atomic orbital therefore less stable compare to atomic orbital.

Non-bonding molecular orbitals (NBMO): They have same energy as atomic orbital.

Molecular orbital diagrams represents the distribution of electrons in different molecular orbitals in increasing order of their energy. Hence lower energy molecular orbitals occupy first then only electron moves in higher energy orbitals.

Answer 8

Expert Solution & Answer

Answer to Problem 85AE

	N2	N2+	N2−
σ2p*	0	0	0
π2p*	0	0	1
σ2p	2	1	2
π2p	4	4	4
σ2s	2	2	2
σ2s*	2	2	2

Answer 9

Expert Solution & Answer

Answer 10

Expert Solution & Answer

Answer 11

Explanation of Solution

Given information:

N2,N2+,N2− are related with each other.

The molecular orbital electronic configuration of N2,N2+,N2− can be written as:

N2 = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2

N2+ = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)1

N2− = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2(π 2py*)1

Hence number of electrons in the given molecular orbitals are:

	N2	N2+	N2−
σ2p*	0	0	0
π2p*	0	0	1
σ2p	2	1	2
π2p	4	4	4
σ2s	2	2	2
σ2s*	2	2	2

Answer 12

Conclusion

N2 = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2

N2+ = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)1

N2− = (σ1s)2(σ 1s*)2(σ2s)2(σ 2s*)2(π2py)2(π2pz)2(σ2px)2(π 2py*)1

Answer 13

Ch. 14 - Prob. 1DQ Ch. 14 - Prob. 2DQ Ch. 14 - Prob. 3DQ Ch. 14 - Prob. 4DQ Ch. 14 - Prob. 5DQ Ch. 14 - Prob. 6DQ Ch. 14 - Compare and contrast the MO model with the LE...Ch. 14 - Prob. 8DQ Ch. 14 - Prob. 9E Ch. 14 - Prob. 10E

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