What is Hybridization in Chemistry?

Hybridization is defined as the process where two or more atomic orbitals of similar (but slightly different) energies within the same atom mix together to form an entirely new set of identical orbitals called Hybrid Orbitals.

• These new hybrid orbitals have exactly the same energy, shape, and size, allowing them to form stronger and more stable covalent bonds.

• $sp^3$ Hybridization: One 's' orbital mixes with three 'p' orbitals. This forms 4 identical orbitals pointing to the corners of a tetrahedron. (Example: Methane, $CH_4$, with a bond angle of $109.5^\circ$).
• $sp^2$ Hybridization: One 's' orbital mixes with two 'p' orbitals. This forms 3 identical orbitals arranged in a flat triangle. (Example: Ethene, $C_2H_4$, with a bond angle of $120^\circ$).
• $sp$ Hybridization: One 's' orbital mixes with one 'p' orbital. This forms 2 identical orbitals arranged in a straight line. (Example: Ethyne/Acetylene, $C_2H_2$, with a bond angle of $180^\circ$).

The standard Valance Bond Theory failed to explain why all four Carbon-Hydrogen bonds in Methane ($CH_4$) are exactly identical in length and strength. Hybridization perfectly explains that Carbon doesn't use its pure 's' and 'p' orbitals; it hybridizes them into four equal $sp^3$ orbitals before bonding.