Compare the relative stability of the following species and indicate their magnetic properties;
The electronic configuration of oxygen molecule can be written as:
Here number of bonding electrons is 8 (Na) and number of antibonding electrons is 4 (Nb)
Therefore, bond order can be found out by,
=1/2(8-4)
=2
The electronic configuration of O2+ can be written as:
Nb = 8
Na = 3
Bond order is 1/2(8-3)
=2.5
The electronic configuration of O2- will be:
Nb = 8
Na = 5
Bond order is 1/2 (8-5)
=1.5
The electronic configuration of O22-will be:
Nb = 8
Na = 6
Bond order is 1/2 (8-6)
=1
Bond dissociation energy is directly proportional to bond order. Thus, the higher the bond order, the greater will be the stability. On this basis, the order of stability is:
O2+ > O2> O2- > O22-