Chemical Principles: The Quest for Insight
Chemical Principles: The Quest for Insight
7th Edition
ISBN: 9781464183959
Author: Peter Atkins, Loretta Jones, Leroy Laverman
Publisher: W. H. Freeman
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Chapter 2, Problem 2G.4E

(a)

Interpretation Introduction

Interpretation:

Valence shell electronic configuration of N2+, N22+ and N22 species has to be determined.

Concept Introduction:

Molecular orbital diagram is a linear combination of atomic orbitals of similar energy and similar symmetry. It is formed by the proper overlap of the atomic orbitals.

There are 3 types of molecular orbitals as follows:

1. Bonding molecular orbital: They are formed by the constructive interference of atomic orbitals and electrons in it stabilize the molecule and are of lesser in energy.

2. Antibonding molecular orbital: This type of orbitals increases the energy of molecule and destabilizes it and weakens the bond between the atoms.

3. Non-bonding molecular orbital: These types of orbitals have energy similar to atomic orbitals that is addition or removal of electron does not change the energy of molecule.

The order of energy in molecular orbital follows two rules as follows:

1. For atomic number less than or equal to 14 order of energy is,

  σ1s<σ1s<σ2s<σ2s<(π2px=π2py)<σ2pz<(π2px=π2py)<σ2pz

2. For atomic number more than 14 order of energy is,

  σ1s<σ1s<σ2s<σ2s<σ2pz<(π2px=π2py)<(π2px=π2py)<σ2pz

(a)

Expert Solution
Check Mark

Explanation of Solution

For N2+ molecule

The symbol for nitrogen is N with atomic number 7. Its electronic configuration is [He]2s22p3. Thus, it possesses 5 valence electrons.

One positive charge is added up in the total valence count.

Thus total valence electrons is sum of the valence electrons for each atom in N2+. It is calculated as follows:

  Total valence electrons=5(2)1=9

Hence, 9 electrons are to be arranged in each molecular orbital to obtain an electronic configuration. Since number of electrons in N2+ is less than 14 so electronic configuration is (σ2s)2(σ2s*)2(π2p)4(σ2p)1.

Hence, the electronic configuration of N2+ is (σ2s)2(σ2s*)2(π2p)4(σ2p)1.

For N22+ molecule

The symbol for nitrogen is N with atomic number 7. Its electronic configuration is [He]2s22p3. Thus, it possesses 5 valence electrons.

Two positive charges are subtracted from the total valence count.

Thus total valence electrons are sum of the valence electrons for each atom in N22+. It is calculated as follows:

  Total valence electrons=5(2)2=8

Hence, 8 electrons are to be arranged in each molecular orbital to obtain an electronic configuration. Since number of electrons in N22+ is less than 14 so electronic configuration is (σ2s2)2(σ2s*)2(π2p)4.

Hence, the electronic configuration of N22+ is (σ2s2)2(σ2s*)2(π2p)4.

For N22 molecule

The symbol for nitrogen is N with atomic number 7. Its electronic configuration is [He]2s22p3. Thus, it possesses 5 valence electrons.

Two negative charges are added up in total valence count.

Thus total valence electrons are sum of the valence electrons for each atom in N22. It is calculated as follows:

  Total valence electrons=5(2)+2=12

Hence, 12 electrons are to be arranged in each molecular orbital to obtain an electronic configuration. Since number of electrons in N22 is more than 14 so electronic configuration is (σ2s)2(σ2s*)2(σ2p)2(π2p)4(π2p*)2.

Hence, the electronic configuration of N22 is (σ2s)2(σ2s*)2(σ2p)2(π2p)4(π2p*)2.

(b)

Interpretation Introduction

Interpretation:

The bond order of N2+ N22+ and N22 species has to be determined.

Concept Introduction:

Bond order b is defined as total number of bonds between the atoms. It is calculated as follows:

  b=12[number of elctrons in bonding orbitalsnumber of electrons in antibonding orbitals]        (1)

(b)

Expert Solution
Check Mark

Explanation of Solution

For N2+ molecule

The electronic configuration of N2+ is (σ2s)2(σ2s*)2(π2p)4(σ2p)1.

Substitute 7 for number of electrons in bonding orbitals and 2 for number of electrons in antibonding orbitals in equation (1) to calculate bond order.

  b=12(72)=52=2.5

Hence, the bond order of the molecule N2+ is 2.5.

For N22+ molecule

The electronic configuration of N22+ is (σ2s2)2(σ2s*)2(π2p)4.

Substitute 6 for number of electrons in bonding orbitals and 2 for number of electrons in antibonding orbitals in equation (1) to calculate bond order.

  b=12(62)=42=2

Hence, the bond order of the molecule N22+ is 2.

For N22 molecule

The electronic configuration of N22 is (σ2s)2(σ2s*)2(σ2p)2(π2p)4(π2p*)2.

Substitute 8 for number of electrons in bonding orbitals and 4 for number of electrons in antibonding orbitals in equation (1) to calculate bond order.

  b=12(84)=2

Hence, the bond order of the molecule N22 is 2.

(c)

Interpretation Introduction

Interpretation:

Molecular orbital diagram of N2+, N22+ and N22 species have to be drawn.

Concept Introduction:

Refer to (a)

(c)

Expert Solution
Check Mark

Explanation of Solution

For N2+ molecule

The electronic configuration of N2+ is (σ2s)2(σ2s*)2(π2p)4(σ2p)1. The molecular orbital diagram of N2+ is as follows:

Chemical Principles: The Quest for Insight, Chapter 2, Problem 2G.4E , additional homework tip  1

Since N2+ has one unpaired electron, therefore it is paramagnetic.

For N22+ molecule

The electronic configuration of N22+ is (σ2s2)2(σ2s*)2(π2p)4. The molecular orbital diagram of N22+ is as follows:

Chemical Principles: The Quest for Insight, Chapter 2, Problem 2G.4E , additional homework tip  2

Since N22+ molecule has no unpaired electron, therefore it is diamagnetic.

For N22 molecule

The electronic configuration of N22 is (σ2s)2(σ2s*)2(σ2p)2(π2p)4(π2p*)2. The molecular orbital diagram of N22 molecule is as follows:

Chemical Principles: The Quest for Insight, Chapter 2, Problem 2G.4E , additional homework tip  3

Since N22 has two unpaired electrons, therefore it is paramagnetic.

(d)

Interpretation Introduction

Interpretation:

Character of highest energy orbital of N2+ , N22+ and N22 species has to be determined.

Concept Introduction:

Refer to (a)

(d)

Expert Solution
Check Mark

Explanation of Solution

For N2+ molecule:

The electronic configuration of N2+ is (σ2s)2(σ2s*)2(π2p)4(σ2p)1. The highest energy orbital electron in N2+ is present in (σ2p)1. Therefore, it contains σ character.

For N22+ molecule

The electronic configuration of N22+ is (σ2s2)2(σ2s*)2(π2p)4. The highest energy orbital electron in N22+ is present in  π2p4. Therefore, it contains π character.

For N22 molecule:

The electronic configuration of N22 is (σ2s)2(σ2s*)2(σ2p)2(π2p)4(π2p*)2. The highest energy orbital electron in N22 is present in  π2p2*. Therefore, it contains π character.

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Chapter 2 Solutions

Chemical Principles: The Quest for Insight

Ch. 2 - Prob. 2A.3ECh. 2 - Prob. 2A.4ECh. 2 - Prob. 2A.5ECh. 2 - Prob. 2A.6ECh. 2 - Prob. 2A.7ECh. 2 - Prob. 2A.8ECh. 2 - Prob. 2A.9ECh. 2 - Prob. 2A.10ECh. 2 - Prob. 2A.11ECh. 2 - Prob. 2A.12ECh. 2 - Prob. 2A.13ECh. 2 - Prob. 2A.14ECh. 2 - Prob. 2A.15ECh. 2 - Prob. 2A.16ECh. 2 - Prob. 2A.17ECh. 2 - Prob. 2A.18ECh. 2 - Prob. 2A.19ECh. 2 - Prob. 2A.20ECh. 2 - Prob. 2A.21ECh. 2 - Prob. 2A.22ECh. 2 - Prob. 2A.23ECh. 2 - Prob. 2A.24ECh. 2 - Prob. 2A.25ECh. 2 - Prob. 2A.26ECh. 2 - Prob. 2A.27ECh. 2 - Prob. 2A.28ECh. 2 - Prob. 2A.29ECh. 2 - Prob. 2A.30ECh. 2 - Prob. 2B.1ASTCh. 2 - Prob. 2B.1BSTCh. 2 - Prob. 2B.2ASTCh. 2 - Prob. 2B.2BSTCh. 2 - Prob. 2B.3ASTCh. 2 - Prob. 2B.3BSTCh. 2 - Prob. 2B.4ASTCh. 2 - Prob. 2B.4BSTCh. 2 - Prob. 2B.5ASTCh. 2 - Prob. 2B.5BSTCh. 2 - Prob. 2B.1ECh. 2 - Prob. 2B.2ECh. 2 - Prob. 2B.3ECh. 2 - Prob. 2B.4ECh. 2 - Prob. 2B.5ECh. 2 - Prob. 2B.6ECh. 2 - Prob. 2B.7ECh. 2 - Prob. 2B.8ECh. 2 - Prob. 2B.9ECh. 2 - Prob. 2B.10ECh. 2 - Prob. 2B.11ECh. 2 - Prob. 2B.12ECh. 2 - Prob. 2B.13ECh. 2 - Prob. 2B.14ECh. 2 - Prob. 2B.15ECh. 2 - Prob. 2B.16ECh. 2 - Prob. 2B.17ECh. 2 - Prob. 2B.18ECh. 2 - Prob. 2B.19ECh. 2 - Prob. 2B.20ECh. 2 - Prob. 2B.21ECh. 2 - Prob. 2B.22ECh. 2 - Prob. 2B.23ECh. 2 - Prob. 2B.24ECh. 2 - Prob. 2C.1ASTCh. 2 - Prob. 2C.1BSTCh. 2 - Prob. 2C.2ASTCh. 2 - Prob. 2C.2BSTCh. 2 - Prob. 2C.3ASTCh. 2 - Prob. 2C.3BSTCh. 2 - Prob. 2C.1ECh. 2 - Prob. 2C.2ECh. 2 - Prob. 2C.3ECh. 2 - Prob. 2C.4ECh. 2 - Prob. 2C.5ECh. 2 - Prob. 2C.6ECh. 2 - Prob. 2C.7ECh. 2 - Prob. 2C.8ECh. 2 - Prob. 2C.9ECh. 2 - Prob. 2C.10ECh. 2 - Prob. 2C.11ECh. 2 - Prob. 2C.12ECh. 2 - Prob. 2C.13ECh. 2 - Prob. 2C.14ECh. 2 - Prob. 2C.15ECh. 2 - Prob. 2C.16ECh. 2 - Prob. 2C.17ECh. 2 - Prob. 2C.18ECh. 2 - Prob. 2D.1ASTCh. 2 - Prob. 2D.1BSTCh. 2 - Prob. 2D.2ASTCh. 2 - Prob. 2D.2BSTCh. 2 - Prob. 2D.1ECh. 2 - Prob. 2D.2ECh. 2 - Prob. 2D.3ECh. 2 - Prob. 2D.4ECh. 2 - Prob. 2D.5ECh. 2 - Prob. 2D.6ECh. 2 - Prob. 2D.7ECh. 2 - Prob. 2D.8ECh. 2 - Prob. 2D.9ECh. 2 - Prob. 2D.10ECh. 2 - Prob. 2D.11ECh. 2 - Prob. 2D.12ECh. 2 - Prob. 2D.13ECh. 2 - Prob. 2D.14ECh. 2 - Prob. 2D.15ECh. 2 - Prob. 2D.16ECh. 2 - Prob. 2D.17ECh. 2 - Prob. 2D.18ECh. 2 - Prob. 2D.19ECh. 2 - Prob. 2D.20ECh. 2 - Prob. 2E.1ASTCh. 2 - Prob. 2E.1BSTCh. 2 - Prob. 2E.2ASTCh. 2 - Prob. 2E.2BSTCh. 2 - Prob. 2E.3ASTCh. 2 - Prob. 2E.3BSTCh. 2 - Prob. 2E.4ASTCh. 2 - Prob. 2E.4BSTCh. 2 - Prob. 2E.5ASTCh. 2 - Prob. 2E.5BSTCh. 2 - Prob. 2E.1ECh. 2 - Prob. 2E.2ECh. 2 - Prob. 2E.3ECh. 2 - Prob. 2E.4ECh. 2 - Prob. 2E.5ECh. 2 - Prob. 2E.6ECh. 2 - Prob. 2E.7ECh. 2 - Prob. 2E.8ECh. 2 - Prob. 2E.9ECh. 2 - Prob. 2E.10ECh. 2 - Prob. 2E.11ECh. 2 - Prob. 2E.12ECh. 2 - Prob. 2E.13ECh. 2 - Prob. 2E.14ECh. 2 - Prob. 2E.15ECh. 2 - Prob. 2E.16ECh. 2 - Prob. 2E.17ECh. 2 - Prob. 2E.18ECh. 2 - Prob. 2E.19ECh. 2 - Prob. 2E.20ECh. 2 - Prob. 2E.21ECh. 2 - Prob. 2E.22ECh. 2 - Prob. 2E.23ECh. 2 - Prob. 2E.24ECh. 2 - Prob. 2E.25ECh. 2 - Prob. 2E.26ECh. 2 - Prob. 2E.27ECh. 2 - Prob. 2E.28ECh. 2 - Prob. 2E.29ECh. 2 - Prob. 2E.30ECh. 2 - Prob. 2F.1ASTCh. 2 - Prob. 2F.1BSTCh. 2 - Prob. 2F.2ASTCh. 2 - Prob. 2F.2BSTCh. 2 - Prob. 2F.3ASTCh. 2 - Prob. 2F.3BSTCh. 2 - Prob. 2F.4ASTCh. 2 - Prob. 2F.4BSTCh. 2 - Prob. 2F.1ECh. 2 - Prob. 2F.2ECh. 2 - Prob. 2F.3ECh. 2 - Prob. 2F.4ECh. 2 - Prob. 2F.5ECh. 2 - Prob. 2F.6ECh. 2 - Prob. 2F.7ECh. 2 - Prob. 2F.8ECh. 2 - Prob. 2F.9ECh. 2 - Prob. 2F.10ECh. 2 - Prob. 2F.11ECh. 2 - Prob. 2F.12ECh. 2 - Prob. 2F.13ECh. 2 - Prob. 2F.14ECh. 2 - Prob. 2F.15ECh. 2 - Prob. 2F.16ECh. 2 - Prob. 2F.17ECh. 2 - Prob. 2F.18ECh. 2 - Prob. 2F.19ECh. 2 - Prob. 2F.20ECh. 2 - Prob. 2F.21ECh. 2 - Prob. 2G.1ASTCh. 2 - Prob. 2G.1BSTCh. 2 - Prob. 2G.2ASTCh. 2 - Prob. 2G.2BSTCh. 2 - Prob. 2G.1ECh. 2 - Prob. 2G.2ECh. 2 - Prob. 2G.3ECh. 2 - Prob. 2G.4ECh. 2 - Prob. 2G.5ECh. 2 - Prob. 2G.6ECh. 2 - Prob. 2G.7ECh. 2 - Prob. 2G.8ECh. 2 - Prob. 2G.9ECh. 2 - Prob. 2G.11ECh. 2 - Prob. 2G.12ECh. 2 - Prob. 2G.13ECh. 2 - Prob. 2G.14ECh. 2 - Prob. 2G.15ECh. 2 - Prob. 2G.16ECh. 2 - Prob. 2G.17ECh. 2 - Prob. 2G.18ECh. 2 - Prob. 2G.19ECh. 2 - Prob. 2G.20ECh. 2 - Prob. 2G.21ECh. 2 - Prob. 2G.22ECh. 2 - Prob. 2.1ECh. 2 - Prob. 2.2ECh. 2 - Prob. 2.3ECh. 2 - Prob. 2.4ECh. 2 - Prob. 2.5ECh. 2 - Prob. 2.6ECh. 2 - Prob. 2.7ECh. 2 - Prob. 2.8ECh. 2 - Prob. 2.9ECh. 2 - Prob. 2.10ECh. 2 - Prob. 2.11ECh. 2 - Prob. 2.12ECh. 2 - Prob. 2.13ECh. 2 - Prob. 2.14ECh. 2 - Prob. 2.17ECh. 2 - Prob. 2.19ECh. 2 - Prob. 2.22ECh. 2 - Prob. 2.23ECh. 2 - Prob. 2.24ECh. 2 - Prob. 2.25ECh. 2 - Prob. 2.26ECh. 2 - Prob. 2.27ECh. 2 - Prob. 2.28ECh. 2 - Prob. 2.29ECh. 2 - Prob. 2.30ECh. 2 - Prob. 2.31ECh. 2 - Prob. 2.32ECh. 2 - Prob. 2.33ECh. 2 - Prob. 2.34ECh. 2 - Prob. 2.35ECh. 2 - Prob. 2.36ECh. 2 - Prob. 2.37ECh. 2 - Prob. 2.39ECh. 2 - Prob. 2.40ECh. 2 - Prob. 2.41ECh. 2 - Prob. 2.42ECh. 2 - Prob. 2.43ECh. 2 - Prob. 2.44ECh. 2 - Prob. 2.45ECh. 2 - Prob. 2.46ECh. 2 - Prob. 2.47ECh. 2 - Prob. 2.48ECh. 2 - Prob. 2.49ECh. 2 - Prob. 2.50ECh. 2 - Prob. 2.51ECh. 2 - Prob. 2.52ECh. 2 - Prob. 2.53ECh. 2 - Prob. 2.54ECh. 2 - Prob. 2.55ECh. 2 - Prob. 2.56ECh. 2 - Prob. 2.57ECh. 2 - Prob. 2.58ECh. 2 - Prob. 2.59ECh. 2 - Prob. 2.60ECh. 2 - Prob. 2.61ECh. 2 - Prob. 2.62ECh. 2 - Prob. 2.63ECh. 2 - Prob. 2.64E
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