Question

 5. What is the bond order in O₂⁺? _______ 

 6. Draw the molecular orbital diagram for B2. The number of unpaired electrons in the B2 molecule is _______ 

 7. Which one of the following statements is false?

 (a) Valence bond theory and molecular orbital theory can be described as two different views of the same thing.

 (b) When one considers the molecular orbitals resulting from the overlap of any two specific atomic orbitals, the bonding orbitals are always lower in energy than the antibonding

 orbitals.

 (c) Molecular orbitals are generally described as being more delocalized than hybridized

 atomic orbitals.

 (d) One of the shortcomings of molecular orbital theory is its inability to account for a triple bond in the nitrogen molecule, Nz.

 (e) One of the shortcomings of valence bond theory is its inability to account for the paramagnetism of the oxygen molecule, O2.

Answer 1

5)

Atomic number of O = 8

Hence, O₂⁺ has 15 electrons.

The electronic configuration of O₂⁺ is

σ1s² < σ^∗1s² < σ2s² < σ^∗2s² < π2px² = π2py² < σ_2pz² < π^∗2px¹ = π^∗2py⁰

[* = anti bonding orbital]

Bond order = [no of bonding electrons - no of anti-bonding electrons]/ 2

= [10-5]/2

= 2.5

Therefore,

bond order of O₂⁺ = 2.5