# Write the MO configuration of the following species-O2 , O2+ , O2- , O22-Arrange them in order of their decreasing stabilities?

The electronic configuration for O is given as:

• O-atom : 1s 2s 2p 4
The molecular orbital configuration for O2 molecule can be given as:

• O2 : (σ1s)2 (σ*1s)(σ2s)2 (σ*2s)2 (σ2pz )2 ($\mathrm{\pi }$2px2 = 2py2)($\mathrm{\pi }*$2px1=$\mathrm{\pi }*$2py1)

• Bond order
O2+ will form by removal of 1 electron from O2.The electron will be removed from $\mathrm{\pi }*$2px or $\mathrm{\pi }*$2py orbital.

Bond order in O2 = 10-5/2= 2.5
Bond order in O2 - = 10-7/2 = 1.5
Bond order in O22- = 10-8/2 = 1

So Order of bond order in all four species will be in order : O22-< O2<O2 < O2+

Maximum the bond order, maximum will be stability.
So the stability order of given species will be O2+ > O> O2 - >O22-

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