Homework SourseUsing the molecular orbital model write electronconfiguratio
Using the molecular orbital model, write electronconfigurations for the following diatomic species and calculate thebond orders. Which ones are para magnetic? Place the species inorder of increasing bond lngh and bond energy.
A. CO B.CO^+ C. CO^2+
Using the molecular orbital model, write electronconfigurations for the following diatomic species and calculate thebond orders. Which ones are para magnetic? Place the species inorder of increasing bond lngh and bond energy.
A. CO B.CO^+ C. CO^2+
Solution
According to molecualr orbital theory the electronconfigurations of the given ions are as follows.
a) CO = coantains total 14electrons,therefore theelectron configuration is
(1s2) (*1s2) (2s2) (*2s2) ( 2px2)(2py2 = 2pz2)
Bond order = Number of bondigelectrons - number of antibonding electrons / 2
= 10-4/2
=3
There is non unpaired electrons ,Hence the moleculewhole is diamagnetic.
b) CO+ = total 13 electrons
(1s2)(*1s2) (2s2) (*2s2) ( 2px2)(2py2 =2pz1)
Bond order = 9-4 /2
= 2.5
There is one unpaired electron is present ,thus themolecule is paramagnetic.
c) CO2+ = total 12 electrons
(1s2)(*1s2) (2s2) (*2s2) ( 2px2)(2py1 =2pz1)
Bond order = 8 - 4 /2
= 2
The molecule whole is paramagnetic.
The order of decreasing bond energy of the given speciesis
CO > CO+ > CO2+
