Hybridization is a concept in chemistry that refers to the process of mixing atomic orbitals to form new hybrid orbitals with different shapes and energies. This phenomenon occurs when atoms combine to form molecules, and it helps explain the geometry and bonding behavior of molecules.

Key points about hybridization:

1. Orbital Mixing: Hybridization involves the mixing of different types of atomic orbitals, such as s (spherical) and p (dumbbell-shaped) orbitals, to create hybrid orbitals with unique shapes and energies.
2. Formation of Bonds: The hybrid orbitals are used by atoms to overlap and form covalent bonds in molecules. They provide a more accurate description of the electron distribution around atoms participating in bonding.
3. Geometry: Hybridization influences the geometry of molecules. For example, in methane (CH4), carbon undergoes hybridization to form four sp³ hybrid orbitals, resulting in a tetrahedral molecular geometry.
4. Stability: Hybridization helps in achieving the most stable arrangement of electrons, reducing the repulsion between them and optimizing bond angles.
5. Common Types: Common hybridization states include sp³, sp², and sp hybridizations, depending on the number and type of atomic orbitals involved.

In summary, hybridization is a fundamental concept in chemistry that explains how atomic orbitals combine to form hybrid orbitals, influencing molecular geometry and the nature of chemical bonds in molecules.