Hybridization

Definition

Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals suitable for the pairing of electrons in chemical bonds. This process helps explain molecular geometries and bond properties.

5 Must Know Facts For Your Next Test

1. Hybridization involves the combination of s, p, and sometimes d orbitals.
2. The type of hybridization determines the geometry of the molecule (e.g., sp3 hybridization results in a tetrahedral shape).
3. sp2 hybridization forms three equivalent orbitals at 120° angles, resulting in trigonal planar geometry.
4. In sp hybridization, one s orbital mixes with one p orbital, creating two linear orbitals at 180° angles.
5. Hybridized orbitals have different shapes and energy levels compared to their original atomic orbitals.

Review Questions

• What is hybridization and why is it important in understanding molecular geometry?
• How do sp3, sp2, and sp hybridizations differ in terms of orbital arrangement and molecular shape?
• Why do hybridized orbitals have different energy levels compared to unhybridized atomic orbitals?

Related terms

Atomic Orbital: A region in an atom where there is a high probability of finding electrons. Examples include s, p, d, and f orbitals.

Molecular Geometry:

The three-dimensional arrangement of atoms within a molecule that influences its physical and chemical properties.

$\sigma$ Bond: $\sigma$ bonds are single covalent bonds formed by the direct overlap of atomic orbitals along the axis connecting two nuclei.