Question

In oxygen molecule MOT,since last electrons are going in pi orbital, then how O2 has 1 sigma and 1 pi bond?

Answer 1

Molecular orbitals (MO) are constructed from atomic orbitals. In O2 and F2, there is a crossover of the sigma and the pi ortbials: the relative energies of the sigma orbitals drop below that of the pi orbitals'. Information from the MO diagram justify O2's stability and show that it's bonding order is 2. The LUMO (lowest unoccupied molecular orbital) and HOMO (highest occupied molecular orbital) of difluoride's MO diagram help explain why the molecule is very stable - the diagram also tells us that the bond order is 1.

Answer 2

Answer:

Okay so for this molecule there is only one σ bond and one Π bond because there is a double bond between the two atoms.

The notation of : σs, σ*s, ΠPx,ΠPy,σPz,Π*Px,Π*Py, and σ*Pz are just orbitals that exist within those bonds. The notation does not indicate that each is a different σ or Π bond.

1) Energy Level:

Bonding has a lower energy than anti-bonding. When full-filled, the energy gained from having a bond and the energy lost from the anti-bond results in no net energy; as in they cancel each other out. Think of two vectors with the same magnitude but opposite directions.

Therefore, if we ignore the combination of full-filled bonding and anti-bonding and consider what's left, we have

Energy(σ2p2) = 1 sigma bond

Enery(Π2p4) + Energy(Π*2p2) (half-filled) = Energy(Π2p2) = 1 pi orbital.

1 pi and 1 sigma - this satisfies as sp hybridization.

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