Why N2 is more stable than O2. Explain on the basis of Molecular Orbital Theory
Molecular orbitals of nitrogen and oxygen is as below:
Nitrogen molecule has 14 electrons. So the electron distributions in molecular orbital are as below
N2 = σ1s2 σ*1s2 σ2s2 σ*2s2 σ2px2 π(2py2 2pz2)
Bond order = (No. of electrons in bonding orbitals - No. of electrons in bonding orbitals)/2
=(10-4)/2 = 3
Oxygen molecule has 16 electrons. So the electron distributions in molecular orbital are as below
O2 = σ1s2 σ*1s2 σ2s2 σ*2s2 σ2px2 π(2py2 2pz2) π*(2py1 2pz1)
Bond order= (10-6)/2 = 2
As bond order of nitrogen is more than that of oxygen, nitrogen is more stable than oxygen.
Nitrogen molecule has 14 electrons. So the electron distributions in molecular orbital are as below
N2 = σ1s2 σ*1s2 σ2s2 σ*2s2 σ2px2 π(2py2 2pz2)
Bond order = (No. of electrons in bonding orbitals - No. of electrons in bonding orbitals)/2
=(10-4)/2 = 3
Oxygen molecule has 16 electrons. So the electron distributions in molecular orbital are as below
O2 = σ1s2 σ*1s2 σ2s2 σ*2s2 σ2px2 π(2py2 2pz2) π*(2py1 2pz1)
Bond order= (10-6)/2 = 2
As bond order of nitrogen is more than that of oxygen, nitrogen is more stable than oxygen.