write down the molecular configuration of N2 and NO. calculate their Bond orders.which of these two is expected to have paramagnetic Behavior?
Answers
PLS MARK AS BRAINLIEST
Answer: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})^0N
2 S
=(σ
1s
)
2
(σ
1s
∗
)
2
(σ
2s
)
2
(σ
2s
∗
)
2
(π
2px
)
2
(π
2py
)
2
(σ
2pz
)
2
(π∗
2px
)
0
(π
2py
∗
)
0
(π
2pz
∗
)
0
bond \ order=\frac{1}{2}\times(10-4)=3bond order=
2
1
×(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})^0NO=N
2
=(σ
1s
)
2
(σ
1s
∗
)
2
(σ
2s
)
2
(σ
2s
∗
)
2
(π
2px
)
2
(π
2py
)
2
(σ
2pz
)
1
(π∗
2px
)
0
(π
2py
∗
)
0
(π
2pz
∗
)
0
bond order =\frac{1}{2}\times(9-4)=2.5
2
1
×(9−4)=2.5
N_2N
2
has not any unpaired electron so it is diamagnetic whereas NO has 1 unpaired electron so it is paramagnetic.