Hybridization of Ammonia (NH₃) - sp3
What is the hybridization of Ammonia (NH₃)?
The central atom in Ammonia (NH₃) is sp3 hybridized. This produces Trigonal Pyramidal geometry with bond angles of 107 degrees. It has 4 hybrid orbitals.
| Formula | NH₃ |
| Name | Ammonia |
| Hybridization | sp3 |
| Geometry | Trigonal Pyramidal |
| Bond Angle | 107° |
| Hybrid Orbitals | 4 |
| Unhybridized p Orbitals | None |
Introduction
Ammonia has a trigonal pyramidal shape. Nitrogen forms 3 bonds to hydrogen and has 1 lone pair. How does nitrogen arrange its 4 electron groups?
Electron Configuration
Nitrogen has 5 valence electrons: 2s² 2p³. All three p orbitals are half-filled. With 3 bonds and 1 lone pair, nitrogen needs 4 equivalent orbitals.
Atomic Orbitals
The 2s orbital is a sphere. The three 2p orbitals are dumbbells along x, y, and z. Nitrogen uses all four for its 3 bonds plus 1 lone pair.
Orbital Mixing
One s and three p orbitals mix to form four sp³ hybrids. Three point toward hydrogen atoms and one holds the lone pair.
Result
Four sp³ orbitals arranged roughly tetrahedrally. Three are bonding, one is a lone pair. The lone pair compresses the H–N–H angle from 109.5° to 107°.
Bonding
Three sp³ orbitals overlap with hydrogen 1s orbitals to form σ bonds. The lone pair orbital makes ammonia a Lewis base — it can donate that electron pair.
Interactive hybridization explorer with step-by-step orbital mixing animations for 8 molecules.
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