$word_{count}$: 250

Hybridization is the mathematical mixing of atomic orbitals to form equivalent hybrid orbitals optimized for bonding. Carbon exhibits three key hybridization states: sp3 (tetrahedral, 109.5 degrees, 25% s-character), sp2 (trigonal planar, 120 degrees, 33% s-character), and sp (linear, 180 degrees, 50% s-character). The hybridization can be quickly calculated using H = $\frac{1}{2}$(V + M - C + A), where V = valence electrons, M = monovalent atoms, C = cation charge, and A = anion charge. Higher s-character means electrons are held closer to the nucleus, making bonds shorter and stronger — this is why sp C-H bonds are the shortest (1.06 Angstrom) and most acidic. Bent's rule further refines this: more electronegative substituents prefer orbitals with more p-character, while lone pairs prefer more s-character. This explains why NF3 (102 degrees) has a smaller bond angle than NH3 (107 degrees). Key JEE applications include counting sigma/pi bonds, determining molecular geometry, and predicting relative acidity based on s-character of the orbital bearing the acidic hydrogen.