Valence Bond Theory & Hybridization

Valence bond theory describes covalent bond formation as the overlap of atomic orbitals from different atoms, where each atom donates one electron to form a shared pair, resulting in increased electron density between the nuclei. This theory is complemented by the concept of hybridization, which involves the mixing of atomic orbitals to form new hybrid orbitals with equivalent energy levels, allowing atoms like carbon to form stable bonds with specific geometries. For example, in methane (CH4​), carbon undergoes sp3 hybridization, creating four equivalent orbitals that form sigma bonds with hydrogen atoms. Understanding valence bond theory and hybridization is essential for predicting the structure and reactivity of organic molecules, as they explain the formation and orientation of bonds