Hybridization of Ethene (C₂H₄) - sp2
What is the hybridization of Ethene (C₂H₄)?
The central atom in Ethene (C₂H₄) is sp2 hybridized. This produces Trigonal Planar geometry with bond angles of 120 degrees. It has 3 hybrid orbitals and 1 unhybridized p orbital (pi bond).
| Formula | C₂H₄ |
| Name | Ethene |
| Hybridization | sp2 |
| Geometry | Trigonal Planar |
| Bond Angle | 120° |
| Hybrid Orbitals | 3 |
| Unhybridized p Orbitals | 2pᵩ (pi bond) |
Introduction
Ethene (C₂H₄) has a C=C double bond. Each carbon forms 3 σ bonds in a flat plane, with 1 p orbital left over for the π bond. This is sp² hybridization.
Electron Configuration
Carbon has 4 valence electrons: 2s² 2p². For a double bond, carbon only mixes 3 of its 4 orbitals — leaving one p orbital unhybridized for the π bond.
Atomic Orbitals
The 2s orbital is spherical. Two of the three 2p orbitals (pₓ and pᵧ) participate in hybridization. The third (pᵩ) stays unhybridized, perpendicular to the molecular plane.
Orbital Mixing
One s and two p orbitals combine to form three sp² hybrids. The unhybridized pᵩ orbital remains unchanged. Watch the s and two p orbitals blend together.
Result
Three sp² orbitals lie in a plane at 120° angles (trigonal planar). The leftover p orbital sticks up and down, perpendicular to the plane.
Bonding
The sp² orbitals form σ bonds (head-on overlap). The unhybridized p orbitals on both carbons overlap side-by-side to form the π bond — completing the double bond.
Interactive hybridization explorer with step-by-step orbital mixing animations for 8 molecules.
Visualize Ethene's Orbital Mixing in 3DRelated Topics
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