Understanding Hybridization Types
Hybridization is a concept in chemistry that describes the mixing of atomic orbitals to form new hybrid orbitals, which can explain the geometry of molecular bonding. Here are the main types of hybridization:
sp Hybridization
- Involves the mixing of one s and one p orbital.
- Forms two equivalent sp hybrid orbitals.
- Geometry: Linear.
- Bond angle: 180°.
- Example: Acetylene (C2H2).
sp² Hybridization
- Involves one s and two p orbitals.
- Forms three equivalent sp² hybrid orbitals.
- Geometry: Trigonal planar.
- Bond angle: 120°.
- Example: Ethylene (C2H4).
sp³ Hybridization
- Involves one s and three p orbitals.
- Forms four equivalent sp³ hybrid orbitals.
- Geometry: Tetrahedral.
- Bond angle: 109.5°.
- Example: Methane (CH4).
sp³d Hybridization
- Involves one s, three p, and one d orbital.
- Forms five equivalent sp³d hybrid orbitals.
- Geometry: Trigonal bipyramidal.
- Bond angles: 90° and 120°.
- Example: Phosphorus pentachloride (PCl5).
Summary of Hybridization
- sp: Linear, 180°
- sp²: Trigonal planar, 120°
- sp³: Tetrahedral, 109.5°
- sp³d: Trigonal bipyramidal, 90° and 120°
Understanding these hybridization types helps in predicting molecular shapes and bond angles, which are crucial for understanding chemical reactivity and properties.

By counting the no. of single bond and loan pair in a structure