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Understanding Hybridisation of NH3: Ammonia

Understanding Hybridisation of NH3: Ammonia

formula

formula

 

Screenshot 2025-12-24 113935.png

Geometry of Ammonia

formula

Using the Hybridisation Formula

We can determine the hybridisation of ammonia using the simple formula:

formula

Step-by-step calculation:

  • Valence electrons of central atom (N): 5
  • Monovalent atoms (H): 3
  • Negative charge: 0
  • Positive charge: 0

formula

Interpretation:

3 σ bonds + 1 lone pair → 4 regions of electron density → sp³ hybridisation

Central Atom and Its Valence Electrons

formula

Screenshot 2025-12-24 114037.png

 Ground state and hybridised state of Nitrogen and Hydrogen

formula

For hybridisation:

  • The 2s orbital mixes with all three 2p orbitals to form four equivalent sp³ orbitals.
  • One of these sp³ orbitals holds the lone pair, and the other three overlap with H 1s orbitals.
  • Hence, the three p orbitals of nitrogen form 3 σ bonds with H atoms and keep 1 lone pair (2s) orbital.
Screenshot 2025-12-24 114100.png

 Orbital overlap in NH3

formula

Number of electron domains around nitrogen: 4 (3 bonds + 1 lone pair)

Electron domain geometry: Tetrahedral

Molecular geometry: Trigonal pyramidal

The lone pair is responsible for the pyramidal shape and bond angle (~107° instead of 109.5°).

Details At A Glance

Property NH3 Value / Feature
Central Atom Nitrogen (N)
Hybridisation sp³
Bond Formation 3 σ bonds (N–H)
Lone Pairs on Central Atom 1
Electron Domain Geometry Tetrahedral
Molecular Shape Trigonal pyramidal
Bond Angle ~107°
Polarity Yes, a Polar molecule

formula

The formal charge (FC) of an atom in a molecule is given by:

Formal Charge = Valence electrons − (Non-bonding electrons + ½ Bonding electrons)

formula

Valence electrons of nitrogen = 5

Non-bonding electrons = 2 (one lone pair)

Bonding electrons = 6 (three N–H bonds)

Half of the bonding electrons = 3

Formal Charge = 5 − (2 + 3)

Formal Charge = 0

This means nitrogen has a formal charge of 0, and the molecule is neutral overall.

formula

Valence electrons = 1

Non-bonding electrons = 0

Bonding electrons (N–H single bond) = 2

Half of the bonding electrons = 1

Formal charge = 1 − (0 + 1)

Formal Charge = 0

Each hydrogen in ammonia has a formal charge of 0 (all three H atoms are identical).

formula

Conclusion

formula

Frequently Asked Questions

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