Structure Overview

• Ring: B–N–B–N–B–N (6-membered ring)
• Similar to Benzene
• Planar structure

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Hybridisation of Atoms

1. Boron (B)

• Hybridisation = sp²
• Forms:
  • 2 σ bonds with N
  • 1 σ bond with H
• Has empty p-orbital

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2. Nitrogen (N)

• Hybridisation = sp²
• Forms:
  • 2 σ bonds with B
  • 1 σ bond with H
• Has lone pair in p-orbital (participates in π bonding)

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π-Bonding (Important Concept)

• p-orbitals of B and N overlap → π system
• But unlike benzene:
  • π electrons are not equally distributed
  • Due to electronegativity difference (B < N)

So, borazine is:

• Partially aromatic
• Less stable than benzene

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Key Differences from Benzene

Property	Borazine	Benzene
Hybridisation	All atoms sp²	All C sp²
Bond nature	Polar (B–N)	Nonpolar
Aromaticity	Weak	Strong

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Exam Points (JEE/NEET)

✔ Both B and N are sp² hybridised
✔ Structure is planar hexagon
✔ Contains delocalised π electrons
✔ Called “inorganic benzene” due to similarity