Note :
(1)
Bond strength
∝ Bond order
(2)
Bond length
∝ Bondorder1
(3)
Bond order
=21 [N
b − N
a]
N
b = No of electrons in bending molecular orbital
N
a = No of electrons in anti bonding molecular orbital
(4)
upto 14 electrons, molecular orbital configuration is
Here N
a = Anti bonding electron
= 4 and N
b = 10
(5)
After 14 electrons to 20 electrons molecular orbital configuration is - - -
Here N
a = 10
and N
b = 10
(A) In O atom 8 electrons present, so in O
2, 8
× 2 = 16 electrons present.
Then in
O22− no of electrons = 18
∴ Molecular orbital configuration of O
2 (16 electrons) is
σ1s2σ1s2∗ σ2s2σ2s2∗ σ2pz2π2px2=π2py2π2px1∗=π2py1∗
∴N
a = 6
N
b = 10
∴ BO =
21[10−6]=2
Here 2 unpaired electrons are present so it is
paramagnetic.
(D) Molecular orbital configuration of O
22− (18 electrons) is
σ1s2σ1s2∗σ2s2σ2s2∗σ2pz2π2px2=π2py2π2px2∗=π2py2∗
∴ N
b = 10
N
a = 8
∴ BO =
21 [ 10
− 8] = 1
Here no unpaired electrons are present so it is
diamagnetic.
(B)
C22− has 14 electrons.
Moleculer orbital configuration of
C22− is
σ1s2σ1s2∗σ2s2σ2s2∗π2px2=π2py2σ2pz2
∴N
a = 4
N
b = 10
∴ BO =
21[10−4]=3
Here no unpaired electron present, so it is
diamagnetic.
(C)
N22− has 16 electrons.
Moleculer orbital configuration of
N22− is
σ1s2σ1s2∗σ2s2σ2s2∗π2px2=π2py2σ2pz2π2px1∗=π2py1∗
∴N
a = 6
N
b = 10
∴ BO =
21[10−6]=2
Here 2 unpaired electron present, so it is
paramagnetic.
As Bond length
∝ Bondorder1
so among two diamagnetic ions
C22− and
O22−, bond order of
C22− is more so it will have shorter bond length.