overlap

The term "overlap" in chemistry refers to the merging of atomic orbitals when atoms form a chemical bond. This overlap creates a region of enhanced electron density between the nuclei, which lowers the molecule's energy and strengthens the bond.1

There are different types of atomic orbitals, each with a unique shape. For example, s orbitals are spherically symmetrical, while p orbitals are double-lobed. The specific shapes and orientations of these orbitals influence how they overlap and form bonds.2

When atoms bond, their atomic orbitals can combine to form molecular orbitals, which describe the distribution of electrons in the molecule. The extent and nature of this orbital overlap are crucial for understanding bond formation, bond strength, and molecular geometry. For instance, the concept of hybridization explains how atomic orbitals can mix to form new hybrid orbitals that are better suited for bonding, as seen in molecules like methane.314