Hybridization and its types

Hybridization

Hybridization in chemistry refers to mixing atomic orbitals to form new hybrid orbitals involved in covalent bonding. It is a concept used to explain the shape of molecule and their bonding properties.

In a covalent bond, atoms share electrons to form a stable molecule. Hybridization occurs when the atomic orbitals of the central atom in a molecule mix to create a set of hybrid orbitals. These hybrid orbitals are formed by combining different atomic orbitals, such as s, p, and d, to create a new set of orbitals with specific directional properties.

Types of hybridization:

The most common types of hybridization are sp, sp2, and sp3 hybridization.
 

Sp hybridization:

In sp hybridization, one s orbital and one p orbital of the central atom combine to form two sp hybrid orbitals. These orbitals are linearly oriented at an angle of 180 degrees to each other. Examples of molecules with sp hybridization include BeCl₂ and linear carbon dioxide (CO₂).

 

Sp2 hybridization: 

In sp2 hybridization, one s orbital and two p orbitals of the central atom combine to form three sp2 hybrid orbitals. These orbitals are arranged in a trigonal planar geometry, with an angle of 120 degrees between them. Examples of molecules with sp2 hybridization include ethene (C₂H₄) and formaldehyde (CH₂O).
 
Sp3 hybridization:

 In sp3 hybridization, one s orbital and three p orbitals of the central atom combine to form four sp3 hybrid orbitals. These orbitals are arranged in a tetrahedral geometry, with an angle of 109.5 degrees between them. Examples of molecules with sp3 hybridization include methane (CH₄) and water (H₂O).

Hybridization allows atoms to achieve a more stable and energetically favorable arrangement of electrons, leading to the observed molecular shapes and bond angles. It is an important concept in understanding the molecular geometry and properties of compounds in chemistry.