MCGRAW: CHEMISTRY THE MOLECULAR NATURE
MCGRAW: CHEMISTRY THE MOLECULAR NATURE
8th Edition
ISBN: 9781264330430
Author: VALUE EDITION
Publisher: MCG
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Chapter 11, Problem 11.45P

(a)

Interpretation Introduction

Interpretation:

The bond orders of the given molecules and the ions are to be compared with the help of molecular orbital theory.

Concept introduction:

A molecular orbital diagram is a tool that is used to describe the chemical bonding formed between different molecules. It is used to predict the bond strength and the electronic transitions that a molecule can undergo.

The formula to calculate the bond order of any species is as follows:

  Bondorder=12(numberofelectronsinbondingorbitalsnumberofelectronsinantibondingorbitals)        (1)

(a)

Expert Solution
Check Mark

Answer to Problem 11.45P

The bond orders of NO, O2 and N2 are 2.5, 2 and 3 whereas the bond orders of NO+, O2+ and N2+ are 3, 2.5 and 2.5.

Explanation of Solution

The molecular orbital configuration of NO is (σ2s)2(σ2s*)2(π2p)2(π2p)2(σ2p)2(π2p*)1.

Substitute 8 for bonding and 3 for the antibonding orbitals in equation (1) to calculate the bond order of NO.

  Bond order of NO=12(83)=2.5

The molecular orbital configuration of O2 is

(σ2s)2(σ2s*)2(σ2p)2(π2p)2(π2p)2(π2p*)1(π2p*)1.

Substitute 8 for bonding and 4 for the antibonding orbitals in equation (1) to calculate the bond order of O2.

  Bond order of O2=12(84)=2

The molecular orbital configuration of N2 is (σ2s)2(σ2s*)2(π2p)2(π2p)2(σ2p)2.

Substitute 8 for bonding and 2 for the antibonding orbitals in equation (1) to calculate the bond order of N2.

  Bond order of N2=12(82)=3

The molecular orbital configuration of NO+ is (σ2s)2(σ2s*)2(π2p)2(π2p)2(σ2p)2.

Substitute 8 for bonding and 2 for the antibonding orbitals in equation (1) to calculate the bond order of NO+.

  Bond order of NO+=12(82)=3

The molecular orbital configuration of O2+ is (σ2s)2(σ2s*)2(σ2p)2(π2p)2(π2p)2(π2p*)1.

Substitute 8 for bonding and 3 for the antibonding orbitals in equation (1) to calculate the bond order of O2+.

  Bond order of O2+=12(83)=2.5

The molecular orbital configuration of N2+ is (σ2s)2(σ2s*)2(π2p)2(π2p)2(σ2p)1.

Substitute 7 for bonding and 2 for the antibonding orbitals in equation (1) to calculate the bond order of N2+.

  Bond order of N2+=12(72)=2.5.

Conclusion

The bond order of the species depends on the number of electrons that are present in bonding and antibonding molecular orbitals.

(b)

Interpretation Introduction

Interpretation:

Whether the magnetic behavior of all the species change or not when ions are formed is to be determined.

Concept introduction:

When a neutral atom gains electrons, it acquires a negative charge on it due to the presence of excess electrons as compared to the protons. This results in the formation of the anion. When a neutral atom loses electrons, it acquires a positive charge on it due to the presence of excess protons as compared to the electrons. This results in the formation of the cation.

Paramagnetism is the property of materials due to which they are weakly attracted by an externally applied magnetic field. It arises due to the presence of unpaired electrons in the atoms so the atoms with incompletely filled atomic orbitals are paramagnetic. The unpaired electrons have magnetic dipole moment and therefore act like tiny magnets.

Diamagnetism is the property of materials due to which they are slightly repelled by an externally applied magnetic field. It occurs due to the presence of paired electrons so the atoms with all the filled orbitals are diamagnetic.

(b)

Expert Solution
Check Mark

Answer to Problem 11.45P

The magnetic behavior of all the molecules does not change when ions are formed.

Explanation of Solution

The molecular orbital configuration of NO is (σ2s)2(σ2s*)2(π2p)2(π2p)2(σ2p)2(π2p*)1 and it is paramagnetic in nature due to the presence of an unpaired electron.

The molecular orbital configuration of O2 is (σ2s)2(σ2s*)2(σ2p)2(π2p)2(π2p)2(π2p*)1(π2p*)1 and it is paramagnetic due to the presence of two unpaired electrons.

The molecular orbital configuration of N2 is (σ2s)2(σ2s*)2(π2p)2(π2p)2(σ2p)2 and it is diamagnetic due to the absence of unpaired electrons.

The molecular orbital configuration of NO+ is (σ2s)2(σ2s*)2(π2p)2(π2p)2(σ2p)2 and it is diamagnetic in nature due to the absence of an unpaired electron.

The molecular orbital configuration of O2+ is (σ2s)2(σ2s*)2(σ2p)2(π2p)2(π2p)2(π2p*)1 and it is paramagnetic due to the presence of an unpaired electron.

The molecular orbital configuration of N2+ is (σ2s)2(σ2s*)2(π2p)2(π2p)2(σ2p)1 and it is paramagnetic due to the presence of an unpaired electron.

The magnetic behavior of NO and N2 changes when their respective ions are formed but that of O2 remains the same.

Conclusion

The magnetic behavior depends on the availability of the unpaired electrons.

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Chapter 11 Solutions

MCGRAW: CHEMISTRY THE MOLECULAR NATURE

Ch. 11 - Prob. 11.3PCh. 11 - Prob. 11.4PCh. 11 - Prob. 11.5PCh. 11 - Give the number and type of hybrid orbital that...Ch. 11 - What is the hybridization of nitrogen in each of...Ch. 11 - What is the hybridization of carbon in each of the...Ch. 11 - Prob. 11.9PCh. 11 - Prob. 11.10PCh. 11 - Prob. 11.11PCh. 11 - Prob. 11.12PCh. 11 - Phosphine (PH3) reacts with borane (BH3) as...Ch. 11 - The illustrations below depict differences in...Ch. 11 - Use partial orbital diagrams to show how the...Ch. 11 - Use partial orbital diagrams to show how the...Ch. 11 - Prob. 11.17PCh. 11 - Prob. 11.18PCh. 11 - Methyl isocyanate, , is an intermediate in the...Ch. 11 - Are these statements true or false? Correct any...Ch. 11 - Prob. 11.21PCh. 11 - Identify the hybrid orbitals used by the central...Ch. 11 - Prob. 11.23PCh. 11 - Identify the hybrid orbitals used by the central...Ch. 11 - Prob. 11.25PCh. 11 - Prob. 11.26PCh. 11 - Certain atomic orbitals on two atoms were combined...Ch. 11 - Prob. 11.28PCh. 11 - Antibonding MOs always have at least one node. Can...Ch. 11 - Prob. 11.30PCh. 11 - Prob. 11.31PCh. 11 - The molecular orbitals depicted are derived from...Ch. 11 - The molecular orbitals depicted below are derived...Ch. 11 - Prob. 11.34PCh. 11 - Use an MO diagram and the bond order you obtain...Ch. 11 - Prob. 11.36PCh. 11 - Prob. 11.37PCh. 11 - Prob. 11.38PCh. 11 - Prob. 11.39PCh. 11 - Epinephrine (or adrenaline; below) is a naturally...Ch. 11 - Prob. 11.41PCh. 11 - Isoniazid (below) is an antibacterial agent that...Ch. 11 - Prob. 11.43PCh. 11 - Prob. 11.44PCh. 11 - Prob. 11.45PCh. 11 - Prob. 11.46PCh. 11 - Tryptophan is one of the amino acids found in...Ch. 11 - Prob. 11.48PCh. 11 - Prob. 11.49PCh. 11 - Prob. 11.50PCh. 11 - Prob. 11.51PCh. 11 - Prob. 11.52PCh. 11 - Sulfur forms oxides, oxoanions, and halides. What...Ch. 11 - Prob. 11.54PCh. 11 - Use an MO diagram to find the bond order and...Ch. 11 - Acetylsalicylic acid (aspirin), the most widely...Ch. 11 - Prob. 11.57P
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INTRODUCTION TO MOLECULAR QUANTUM MECHANICS -Valence bond theory - 1; Author: AGK Chemistry;https://www.youtube.com/watch?v=U8kPBPqDIwM;License: Standard YouTube License, CC-BY