Orbital Hybridization: s/p Mixing into sp, sp², sp³
Step through the hybridization process and compare the resulting geometry, bond angle, and remaining unhybridized p orbitals.
About this simulation
- What
- An interactive Chemistry simulation of Orbital Hybridization: s/p Mixing into sp, sp², sp³.
- Who
- Designed for AP, IB, and A‑Level Chemistry students.
- How
- Runs in any modern browser — drag, adjust, and explore in real time.
Updated 2026-02-28
Key Concepts
Linear Combination
Hybridization forms new equivalent orbitals by combining one s orbital with one, two, or three p orbitals.
Directionality of Bonds
sp, sp², and sp³ orbitals point in specific directions to maximize separation and define molecular geometry.
Unhybridized p Orbitals
Any p orbitals not used in hybridization can overlap side-by-side to form π bonds.
Understanding Orbital Hybridization
Orbital Hybridization is a valence-bond model used to describe the mixing of pure atomic orbitals (s and p) into a new set of equivalent hybrid orbitals. This mechanism explains the bond directionality observed in molecular geometries.
The specific hybrid state—sp (linear), sp² (trigonal planar), or sp³ (tetrahedral)—is determined by the number of p-orbitals participating in the mix, directly fixing the bond angles to 180°, 120°, or 109.5° respectively.
Use our interactive visualizer to observe how wavefunction combinations generate directional hybrid lobes and learn why unhybridized p-orbitals are critical for π-bond formation and molecular reactivity.
Frequently Asked Questions
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