Hybridisation in Chemical Bonding

Hybridisation is a concept in chemistry that involves the mixing of atomic orbitals to form new hybrid orbitals. This process helps in explaining the shapes and properties of molecules.

Key Points:
- Hybridisation is necessary to explain the geometry of molecules that cannot be explained by the simple overlap of atomic orbitals.
- The hybrid orbitals formed have different shapes and energies compared to the original atomic orbitals.
- Hybridisation is determined by the number of sigma bonds and lone pairs around the central atom.
- The most common types of hybridisation are sp, sp2, and sp3, which involve the mixing of s and p orbitals.
- For example, in methane (CH4), the carbon atom undergoes sp3 hybridisation, resulting in four sp3 hybrid orbitals that form sigma bonds with four hydrogen atoms.

In conclusion, hybridisation is a crucial concept in understanding the molecular geometry and bonding in organic compounds. It helps in predicting the shape, bond angles, and reactivity of molecules, making it an essential tool in the study of chemical bonding.