Final answer:
The interaction of two atomic orbitals can result in the formation of a σ bonding orbital, a π bonding orbital, an antibonding orbital, or a hybridized orbital, depending on the way the orbitals overlap and the electron density is distributed.
Step-by-step explanation:
The interaction of two atomic orbitals can result in the formation of different types of molecular orbitals. When two orbitals overlap in an end-to-end fashion with the electron density concentrated between the nuclei, they form a σ (sigma) bonding orbital, which is indicative of a single covalent bond and has no nodes perpendicular to the internuclear axis. Such σ bonds can be formed from s-s overlapped orbitals, s-p overlapped orbitals, or p-p overlapped orbitals. On the other hand, a π (pi) bonding orbital is formed from the side-by-side overlap of p orbitals, with the electron density located above and below the plane of the nuclei. π bonds usually create multiple bonds along with σ bonds. In contrast, an antibonding orbital, signified by an asterisk (e.g., σ* or π*), contains one or more nodes and is higher in energy, with electron density that is less favorable for bonding. Hybridized orbitals are a result of mixing atomic orbitals to form hybrid orbitals like sp, sp2, sp3, which participate in forming σ bonds.