In: Chemistry
Consider the species (O2)2- and (O2)2+. According to molecular orbital theory, which of these species will be diamagnetic?
(O2)2+ and (O2)2- |
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(O2)2+ |
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(O2)2- |
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neither is diamagnetic |
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The magnetic property can only be determined for molecules, not ions. |
1) for O22+
σ and σ* orbital can have maximum of 2 electrons
π and π* orbital can have maximum of 4 electrons
1 O atom have 8 electrons
Here, number of O is 2
so, total number of electrons in O2 is 16
Since charge is +2
Total number of electron = 14
So, total number of electrons to fill is 14
order of filling of orbitals is:
σ1s σ*1s σ2s σ*2s π2p σ2p π*2p σ*2p
Lets fill the orbital
the filled orbital is σ1s2 σ*1s2 σ2s2 σ*2s2 π2p4 σ2p2
The orbital σ2p2 has unpaired number of electrons
So, it is diamagnetic in nature
2) FOR O2-2
σ and σ* orbital can have maximum of 2 electrons
π and π* orbital can have maximum of 4 electrons
1 O atom have 8 electrons
Here, number of O is 2
so, total number of electrons in O2 is 16
Since charge is -2
Total number of electron = 18
So, total number of electrons to fill is 18
order of filling of orbitals is:
σ1s σ*1s σ2s σ*2s σ2p π2p π*2p σ*2p
Lets fill the orbital
the filled orbital is σ1s2 σ*1s2 σ2s2 σ*2s2 σ2p2 π2p4 π*2p4
The orbital π*2p4 has unpaired number of electrons
So, it is diamagnetic in nature
Answer: both are diamagnetic (option 1)