Hybridization Explorer — sp, sp², sp³ Orbital Mixing & Molecular Geometry

Orbital hybridization explains why carbon, nitrogen, and other atoms form bonds at angles that pure atomic s and p orbitals could never produce on their own — a core AP Chemistry Unit 2 concept and prerequisite for understanding both VSEPR geometry and organic reactivity.

Hybridization mixes atomic orbitals on a single atom into new, equivalent hybrid orbitals suited to the bonding geometry actually observed. sp hybridization mixes one s and one p orbital into two sp orbitals arranged linearly (180°), seen in molecules like BeCl2 and any carbon with two pi bonds, such as the central carbon in CO2. sp² hybridization mixes one s and two p orbitals into three orbitals in a trigonal planar arrangement (120°), leaving one unhybridized p orbital available for pi bonding — exactly the geometry of every carbon in a C=C double bond or a benzene ring.

sp³ hybridization, the most common in organic chemistry, mixes one s and three p orbitals into four equivalent orbitals pointing toward the corners of a tetrahedron (109.5°), the geometry of methane and every sp³ carbon. Expanding beyond the octet, sp³d hybridization (trigonal bipyramidal, 90°/120°) and sp³d² hybridization (octahedral, 90°) describe central atoms like phosphorus in PCl5 and sulfur in SF6, which require d-orbital involvement to accommodate five or six bonding domains.

Lone pairs occupy hybrid orbitals just like bonding pairs but exert slightly greater repulsion, compressing observed bond angles below the idealized values — this is why water's H-O-H angle is 104.5° rather than the tetrahedral 109.5°, despite oxygen being sp³ hybridized with two lone pairs.

This hybridization explorer lets you select any hybridization state from sp through sp³d², see the corresponding 3D orbital mixing diagram and geometry, and view real example molecules for each — connecting the abstract orbital math directly to the molecular shapes you're asked to predict on exams.