Answer:
See explanation
Step-by-step explanation:
The question is incomplete.
However, I will discuss here the general principles of filling molecular orbitals. The filling of molecular orbitals is synonymous to the filling of atomic orbitals because the Hund's rule applies in both cases.
For simple Homonuclear molecules, the order of filling electrons in the molecule into molecular orbitals are as follows;
σ1s, σ*1s, σ2s, σ*2s,σ2px, (π2py,π2pz), (π*2py,π*2pz), σ*2px
For lighter elements, such as Boron, carbon, nitrogen, the π2py and π2pzare less in energy than the σ2px and the σ*2px is lesser in energy than the π*2py and π*2pz orbitals. For these atoms the order is;
σ1s, σ*1s, σ2s, σ*2s,(π2py,π2pz), σ2px,σ*2px, (π*2py,π*2pz).
The molecular orbital diagrams for molecules and ions are drawn from the order of increasing energies shown in the molecular orbital configuration. Always remember that the number of molecular orbitals formed must be equal to the number of atomic orbitals that were combined in the molecule.