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Question

Compare the relative stability of the following species and indicate their magnetic properties :

O2, O+2, O2 (superoxide) and O22 (peroxide).

Solution
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(1) The electronic configuration of O2 molecule is
KK(σ2s)2(σ2s)2(σ2pz)2(π2px)2(π2py)2(π2px)1(π2py)1
Its bond order is 842=2.
It contains 2 unpaired electrons and is paramagentic.
(2) The electronic configuration of O+2 ion is
KK(σ2s)2(σ2s)2(σ2pz)2(π2px)2(π2py)2(π2px)1
Its bond order is 832=2.5.
It contains 1 unpaired electron and is paramagnetic.
(3) The electronic configuration of O2 ion is
KK(σ2s)2(σ2s)2(σ2pz)2(π2px)2(π2py)2(π2px)2(π2py)1
Its bond order is 852=1.5.
It contains 1 unpaired electron and is paramagnetic.
(4) The electronic configuration of O22 ion is
KK(σ2s)2(σ2s)2(σ2pz)2(π2px)2(π2py)2(π2px)2(π2py)2
Its bond order is 862=1.
It contains all paired electrons and is diamagnetic.
Higher is the bond order, stronger is the bond, and higher is the stability.

The decreasing order of the stability is O+2>O2>O2>O22.

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