Question

explain molecular orbital theory with O2 and N2​

Answer 1

Answer:

When it comes to O₂ and N₂, I think there are two things to point out:

   the energies of the starting atomic orbitals are different, due to different fundamental effects (nuclear charges, electron screening, electronegativity);

   the number of electrons that occupy the as-formed molecular orbitals are different.

All in all: on moving from left to right, the effective nuclear charge increases and the outermost electrons (5 for N, 6 for O) are more strongly attracted to the nucleus (even more so when the symmetry of the subshell is spherical, in the case of an s-type AO).

These are, IMO, the reasons why the energy levels of the and π MOs are inverted on passing from N₂ to O₂ (and F₂, too).

Explanation:

Answer 2

Answer:

The molecular orbital energy level diagram of oxygen molecule is given as follows : Bond order 2Nb​−Na​​=28−4​=2. Thus, oxygen molecule has two bonds. i.e., one is bond and one p bond. The last two electrons in p2px∙​ and p2py∙​ orbitals will remain unpaired.

There are four molecular orbitals derived from the 1s and 2s orbitals. Use the buttons to display the 1s and 2p atomic orbitals that make up the molecular orbitals. The p orbitals combine to produce a sigma and two perpendicular pi bonds.

Explanation: