7. MO Theory. Fill in the MO diagrams, determine the MO bond order, and indicate whichmolecules/ions are paramagnetic or diamagnetic110THLdlatomic0,-всLizMO diagramMO bond orderparamagneticdiamagnetic

Answered: Theory. Fill in the MO diagrams,…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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7. MO Theory. Fill in the MO diagrams, determine the MO bond order, and indicate which
molecules/ions are paramagnetic or diamagnetic110
THL
dlatomic
0,-
вс
Liz
MO diagram
MO bond order
paramagnetic
diamagnetic

Expert Solution

Step 1

According to molecular orbital theory:

Atomic orbitals will combine and form molecular orbitals.

The number of atomic orbitals combined is equal to the number of molecular orbitals.

If two atomic orbitals will combine then, two molecular orbitals will be formed and between them one molecular orbital has lower energy and the other molecular orbital has high energy.

The molecular orbital with lower energy is called bonding molecular orbital and the other with high energy is called anti bonding molecular orbital.

$B o n d o r d e r = \frac{1}{2} [n o . o f b o n d i n g e l e c t r o n s - n o . o f a n t i b o n d i n g e l e c t r o n s]$

If a molecule has unpaired electrons in its molecular orbitals then it is para magnetic.

If a molecule does not have unpaired electrons then, it is dia magnetic.

Step 2

The molecular ion diagram for the given molecules:

Step 3

Bond order of O₂²⁺:

$B o n d o r d e r = \frac{1}{2} [n o . o f b o n d i n g e l e c t r o n s - n o . o f a n t i b o n d i n g e l e c t r o n s] = \frac{1}{2} [8 - 3] = \frac{5}{2} = 2.5$

Bond order O₂:

$B o n d o r d e r = \frac{1}{2} [n o . o f b o n d i n g e l e c t r o n s - n o . o f a n t i b o n d i n g e l e c t r o n s] = \frac{1}{2} [8 - 4] = \frac{4}{2} = 2.0$

Bond order of O₂^2-:

$B o n d o r d e r = \frac{1}{2} [n o . o f b o n d i n g e l e c t r o n s - n o . o f a n t i b o n d i n g e l e c t r o n s] = \frac{1}{2} [8 - 6] = \frac{2}{2} = 1.0$

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