Question

Which of the following statement is not correct from the
view point of molecular orbital theory?
(a) Be₂ is not a stable molecule
(b) He₂ is not stable but He₂+ is expected to exist
(c) Bond strength of N₂ is maximum amongst the
homonuclear diatomic molecules belonging to the
second period
(d) The order of energies of molecular orbitals in N₂
molecule is
σ2s < σ*2s < σ2pz < (π2pₓ ; π2pᵧ) < (π*2pₓ ; π*2pᵧ )
< σ*2pz

Answer 1

Answer:

c) Bond strength of N₂ is maximum amongst the

homonuclear diatomic molecules belonging to the

second period✔✔✔✔✔

Answer 2

The order of energies of molecular orbitals in N₂ molecule is σ2s < σ*2s < σ2pz < (π2pₓ ; π2pᵧ) < (π*2pₓ ; π*2pᵧ ) < σ*2pz

Explanation:

• The orbital theory of the molecules explain the bonding between the atomic to form the molecules.

• The orbital theory states the bond order which also gives a Explanation to calculate the bond order.

• Bond order is calculated as the half of difference between the total number of electrons in bonding orbital and antibonding orbital.

• Bond order of Be2 is 0 because of the equal number of electrons in bonding and antibonding orbitals.

• So it cannot exist as Be2 as energy of abtibonding orbitals are more than that of bonding orbitals.

• Similarly in He2, there's same number of electrons in bonding orbital and antibonding orbital.

• But when He₂+ is formed, the last electron is ejected from antibonding orbital and bond order comes as 0.5.

• So it can exist.

• Bond order of nitrogen is 3 which is the highest among the other 2nd period elements like Lithium, beryllium, boron, carbon, oxygen, fluorine and neon.

• So it has shortest and strongest bonds.

• But the order of energies of bonding and antibonding orbitals in nitrogen is in the order of σ2s < σ* 2s < σ2pz < (π2px = π2py ) < (π* 2px = π* 2py) < σ*2pz.

• So last option is not correct.

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