The bond between two fluorine atoms in \(\mathrm{F}_{2}\) can be viewed as resulting from the end-on interaction between the \(2 p_{y}\) orbital on each fluorine. Sketch the molecular orbitals produced through the interaction of two fluorine \(2 p_{y}\) atomic orbitals.

Atomic orbitals are regions around a nucleus where electrons are likely to be found.
Each fluorine atom in the \(\mathrm{F}_{2}\) molecule has three 2p orbitals: 2p_x, 2p_y, and 2p_z.
These orbitals are essential because they participate in forming molecular bonds.
In fluorine's case, the bond forms specifically through the interaction of the 2p_y orbitals from each atom.

When these orbitals overlap, they change, combining to form new molecular orbitals.
These interactions can either lower the system's energy, creating a stable bond,
or increase the energy, making the bonding less stable. The magic lies in how the wave functions of these orbitals interfere with each other.

A bonding molecular orbital results from the constructive interference of atomic orbitals.
When the 2p_y orbitals from each fluorine atom align and overlap end-on, they combine to form a bonding molecular orbital.
This combination leads to increased electron density between the fluorine nuclei.
As a result, the bonding molecular orbital has lower energy compared to the original atomic orbitals.
One key feature of a bonding molecular orbital is that it stabilizes the molecule.
It forms because the electron wave functions of the fluorine atoms interfere constructively.
This constructive interference creates a region with a higher probability of finding electrons between the two nuclei.
This, in turn, pulls the nuclei together, forming a strong covalent bond.

Antibonding molecular orbitals form through destructive interference of atomic orbitals.
In the case of fluorine's 2p_y orbitals, this means that when they overlap, they also produce an antibonding molecular orbital.
This antibonding orbital has higher energy compared to the bonding molecular orbital.
Here's why: the wave functions of the 2p_y orbitals interfere destructively.
This interference creates a node between the nuclei, a region with no electron density.
Without electron density in between, there's no force pulling the nuclei together.
Therefore, these orbitals destabilize the molecule and, if occupied, can weaken the bond.
This concept is crucial in understanding why not all orbital interactions lead to stable molecules.