Orbital Hybridization & Covalent Bonding (Methane, Ethylene, Acetylene, Benzene)
See orbital hybridization theory in action: watch s and p atomic orbitals mix and overlap head-on or side-by-side to build rigid molecular skeletons.
About this simulation
- What
- An interactive Chemistry simulation of Orbital Hybridization & Covalent Bonding (Methane, Ethylene, Acetylene, Benzene).
- Who
- Designed for AP, IB, and A‑Level Chemistry students.
- How
- Runs in any modern browser — drag, adjust, and explore in real time.
Updated 2026-03-13
Key Concepts
sp³ Hybridization (Methane)
One s and three p orbitals of carbon mix to form four equivalent sp³ hybrid orbitals pointing to vertices of a tetrahedron, creating four identical C-H σ bonds.
sp² and sp Hybridization
When fewer than 3 p orbitals engage in mixing, trigonal planar (sp²) or linear (sp) frameworks emerge. The unhybridized p orbitals overlap sideways to form π bonds.
Delocalized π System (Benzene)
Six carbon atoms in benzene are sp² hybridized to form a planar hexagonal σ skeleton. Their six parallel p orbitals overlap laterally forming a continuous ring of electron density.
Peering into the Microscopic Dance of Orbitals
Orbital Hybridization is a quantum mechanical concept where atomic orbitals (s and p) mix to form new, equivalent hybrid orbitals. This process is essential for explaining molecular geometries that pure atomic orbitals cannot justify.
The spatial arrangement of a molecule is determined by its hybridization state: sp³ results in tetrahedral geometry (e.g., Methane), sp² creates trigonal planar frameworks (e.g., Ethene), and sp leads to linear configurations (e.g., Ethyne or Acetylene).
By interacting with these step-by-step 3D animations, you can observe how head-on orbital overlaps form rigid σ (sigma) bonds and how lateral overlaps of unhybridized p-orbitals create π (pi) bonds, defining the molecule's chemical reactivity.
Concept FAQ
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