General Chemistry
General Chemistry
4th Edition
ISBN: 9781891389603
Author: Donald A. McQuarrie, Peter A. Rock, Ethan B. Gallogly
Publisher: University Science Books
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Chapter 9, Problem 9.9P
Interpretation Introduction

Interpretation:

The ground state configuration, bond order and the magnetic nature of the species has to be given.

Concept Introduction:

Bond order of a molecule or ion is calculated by the following formula,

Bond order =(Nb)-(Na)2

Where, Nb is number of electrons in bonding orbital.

Na is number of electrons in antibonding orbital.

Paramagnetic and diamagnetic compounds:

Paramagnetic compounds have unpaired electrons and are attracted to magnetic field whereas diamagnetic compounds have paired spins and are repelled by the magnetic field.

Expert Solution & Answer
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Explanation of Solution

The ground state electronic configuration is the arrangement of electrons around the nucleus of an atom with lower energy levels.

Ground state electronic configurations of three species are as follows,

  NF=(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2(σ2pz)2(π2px)2(π2py)2(π*2px)1(π*2py)1

  NF+=(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2(σ2pz)2(π2px)2(π2py)2(π*2px)1

  NF-=(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2(σ2pz)2(π2px)2(π2py)2(π*2px)2(π*2py)1

All the three species have lone pair electrons in their antibonding orbitals.  Thus, they get attracted by the magnetic field.  Hence, they are paramagnetic species.

Bond order calculation:

NF molecule has the same configuration as oxygen molecule thus, the bond order of NF molecule is two.

Bond order of NF can be calculated as,

  Bond order=(10)-(6)2                  =42=2

NF+ ion is formed when NF molecule loses one of its electron.

Bond order of NF+ can be calculated as,

  Bond order=(10)-(5)2                  =52=2.5

The bond order of NF+ is 2.5.

Bond order of NF- can be calculated as

  Bond order=(10)-(7)2                  =32=1.5

The bond order of NF- is 1.5.

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Chapter 9 Solutions

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