In Chemical Bonding (Class 11 Chemistry), determining the hybridization and geometric shape of molecules is a very important topic. Let's analyze the Ammonia (NH₃) molecule.
Central Atom: Nitrogen (N).
Hybridization: sp³.
Electron Geometry: Tetrahedral.
Molecular Shape: Trigonal Pyramidal (due to 1 lone pair).
Bond Angle: ~ 107°.
To find the hybridization, we look at the central Nitrogen (N) atom.
Normally, an sp³ hybridized molecule (like Methane, CH₄) has a perfect Tetrahedral geometry with bond angles of 109.5°.
However, NH₃ has a Lone Pair of electrons sitting on top of the Nitrogen atom. According to the VSEPR theory, the lone pair repels the bonded pairs of electrons strongly, pushing the hydrogen atoms closer together.
Because of this repulsion:
The hybridization of the central nitrogen atom in NH3 (Ammonia) is sp3.
Although its electron geometry is tetrahedral, the presence of one lone pair on the nitrogen atom distorts the shape, making the actual molecular structure of NH3 Trigonal Pyramidal.
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