Compare the bond length of
N2 & N2+
Answers
By MOT, the bond orders of both are 2.5. Now acc to MOT only, the compound having more electrons in antibonding orbitals will form a weaker bond and a longer bond., IF their bond orders are equal. N2- has 5e- in antibonding while N2+ has 4. So, N2+ will make a stronger bond and will have a shorter bond length.
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Answer:
By MOT, the bond orders of both are 2.5. Now acc to MOT only, the compound having more electrons in antibonding orbitals will form a weaker bond and a longer bond., IF their bond orders are equal. N2- has 5e- in antibonding while N2+ has 4. So, N2+ will make a stronger bond and will have a shorter bond length.
Step-by-step explanation:
Which has more bond length out of N2- and N2+?
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Which has more bond length out of N2- and N2+?
By MOT, the bond orders of both are 2.5. Now acc to MOT only, the compound having more electrons in antibonding orbitals will form a weaker bond and a longer bond., IF their bond orders are equal. N2- has 5e- in antibonding while N2+ has 4. So, N2+ will make a stronger bond and will have a shorter bond length.
What is the net bond order on N2, N2+, and N2-?
Why is the bond length of N2+ greater than N2 according to the MO theory?
The bond order of n2- and n2+ is same, but do they have the same bond length, or is n2+ shorter?
What is the bond order of N2-?
Between N2 and N2+, which has less bond energy and why?
What is the net bond order on N2, N2+, and N2-?
Bond order for N2 is 3; bond order for N2- is 2.5 and bond order for N2+ is 2.5. Need to understand molecular orbitals to see why this is the case. When the nitrogen atoms combine they form both S and P bonding and anti-bonding molecular orbitals. The anti-bonding orbitals “detract” from the bonding orbitals (i.e. the bond order). The diatomic nitrogen has 10 valence electrons to fill these molecular orbitals. Two electrons occupy the S bonding orbital; two electrons occupy the S anti-bonding orbital (no contribution to bond order). There are three P bonding orbitals and three P anti-bonding orbitals. The remaining six valence electrons for the neutral N2 occupy the three bonding P orbitals hence the bond order of 3. For the N2- molecule there is an additional electron but the only orbital available to occupy is a P anti-bonding orbital therefore decreasing the bond order by 0.5 yielding a 2.5 bond order. For the N2+ molecule this has one less electron than the neutral N2 and this must come from one of the P bonding orbitals therefore reducing the bond order by 0.5 therefore yielding a bond order of 2.5. Therefore this helps us understand why the neutral N2 molecule is a more stable molecule compared to the other two. ( I have not included pictures of the MO diagrams that show the orbital energies. Electrons occupy lowest energy orbitals first. With a little searching one can find such examples