How does bonding and antibonding molecular orbitals interaction stabilize molecules?

Both decrease the energy of the atomic orbitals to form the molecule by their overlap

Explanation:

Many molecules are not described correctly by Lewis theory. For example, diborane (B2H6), which is an electrodeficient compound: there are not enough valence electrons to be able to assign a Lewis structure.

The theory of binding and anti-binding orbitals describes molecular orbitals, whose atomic orbitals overlap to form them. Two atomic orbitals overlap giving a binding orbital molecular orbital. In the binder, the electrons that occupy it have a high possibility of being located between the atoms, so filling stabilizes the molecule. In an anti-binding orbital, the electrons that occupy it have a low probability of being located between the atoms, so that their filling destabilizes the molecule.

The interaction between two atomic orbitals is greater the greater their overlap and the smaller their energy difference.

the answer to this question is 3.

the answer is 1260

you spend 7 hours in school for 1 school day with 5 school days in 1 school week with 36 school weeks in a school year.

7*5*36= 1260 it's all about multiplying