Answer: [tex]N_2[/tex] has strongest bond as the bond order is highest.
Explanation: [tex]N_2[/tex] has 14 electrons, [tex]N_2^-[/tex] has 15 electrons and [tex]N_2^-[/tex] has 13 electrons.
According to molecular orbitl theory the electrons are filled as shown below
[tex]N_2^[/tex] is [tex]\sigma1s^2\sigma^*1s^2\sigma2s^2\sigma ^*2s^2\pi 2px^2=\pi 2py^2\sigma2pz^2 [/tex]
[tex]\text{bond order} =\frac{\text{no of bonding electrons - no of antibonding electrons}}{2}[/tex]
[tex]\text{bond order} =\frac{\text{ 10 - 4 }}{2} = 3[/tex]
[tex]N_2^-[/tex] is [tex]\sigma1s^2\sigma^*1s^2\sigma2s^2\sigma ^*2s^2\sigma 2pz^2\pi2px^2=\pi2py^2\pi^*2px^1=\pi^*2py^0[/tex]
[tex]\text{bond order} =\frac{\text{no of bonding electrons - no of antibonding electrons}}{2}[/tex]
[tex]\text{bond order} =\frac{\text{ 10 - 5 }}{2} = 2.5[/tex]
[tex]N_2^+[/tex] is [tex]\sigma1s^2\sigma^*1s^2\sigma2s^2\sigma ^*2s^2\pi 2px^2=\pi 2py^2 \sigma 2pz^1[/tex]
[tex]\text{bond order} =\frac{\text{no of bonding electrons - no of antibonding electrons}}{2}[/tex]
[tex]\text{bond order} =\frac{\text{ 9 - 4 }}{2} = 2.5[/tex]
as Bond Order is the measure of bond strength thus we can say [tex]N_2[/tex] with Bond order of 3 has the strongest bond.
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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