Answer to Question #102681 in General Chemistry for sakshi

Question

Write down the molecular orbital configurations of N2 and NO. Calculate their bond orders. Which of these two is expected to have paramagnetic behavior?

Answer 1

$N_2= (\sigma_{1s})^2(\sigma^*_{1s})^2 ( σ _{2s} )^ 2 ( σ^ * _{2s} )^ 2 ( π _{2px} )^ 2 ( π _{2py} )^2 ( σ _{2pz} )^ 2 ( π *_ {2px} ) ^0 ( π^ *_{2py})^0(\pi^*_{2pz})^0$

$bond \ order=\frac{1}{2}\times(10-4)=3$

$NO=N_2=( \sigma_{1 s} )^2(\sigma^*_{1s})^2 ( σ _{2s} )^ 2 ( σ^ * _{2s} )^ 2 ( π _{2px} )^ 2 ( π _{2py} )^2 ( σ _{2pz} )^ 1 ( π *_ {2px} ) ^0 ( π^ *_{2py})^0(\pi^*_{2pz})^0$

bond order =$\frac{1}{2}\times(9-4)=2.5$

$N_2$ has not any unpaired electron so it is diamagnetic whereas NO has 1 unpaired electron so it is paramagnetic.