Use molecular orbital theory to predict which species has the strongest bond n2 n2- n2+

N2 having a bond order of 3 has the strongest bond.

The molecular orbital theory enables us to fill electrons into molecular orbitals and thereby obtain the bond order in molecules. In order to predict the stability of N2, N2- and N2+, we must write down the molecular orbital configuration for each specie.

For N2;

σ1s2 σ*1s2  σ2s2 σ*2s2  π2py2 π2py2  σ2p2

Bond order =1/2 (Number of  bonding electrons - Number of antibonding electrons) = 1/2(10 - 4) = 3

For N2-;

σ1s2 σ*1s2  σ2s2 σ*2s2  π2py2 π2py2  σ2p2  π*2py1

Bond = 1/2(10 - 5) = 2.5

For N2+;

σ1s2 σ*1s2  σ2s2 σ*2s2  π2py2 π2py2  σ2p1

Bond order = 1/2(9 - 4) = 2.5

We know that the higher the bond order, the stronger the bond. Therefore, N2 having a bond order of 3 has the strongest bond.

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has strongest bond as the bond order is highest.

Explanation: has 14 electrons,   has 15 electrons and has 13 electrons.

According to molecular orbitl theory the electrons are filled as shown below

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as Bond Order is the measure of bond strength thus we can say   with Bond order of 3 has the strongest bond.

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