The most frequently tested aspect of INC-03 in NEET is molecular geometry and hybridization. Here are the definitive key points:

Ozone (O3):

• Hybridization: sp2 | Geometry: Angular | Bond angle: ~117° | Lone pairs on central O: 1

SO2 vs. SO3 Comparison:

• SO2: sp2, angular (~119°), 1 lone pair on S, reducing agent
• SO3: sp2, trigonal planar (120°), 0 lone pairs on S, powerful oxidizer/acid anhydride

Xenon Fluorides — The Most Critical Table:

• XeF2: sp3d, linear (3 lone pairs equatorial in TBP, 2 F atoms axial, 180°)
• XeF4: sp3d2, square planar (2 lone pairs trans axial in octahedral, 4 F atoms equatorial)
• XeF6: sp3d3, distorted octahedral (1 lone pair distorts regular octahedral)

Interhalogen Geometries:

• AB (ClF): sp3 (diatomic, linear) — 3 lone pairs on central atom
• AB3 (ClF3): sp3d, T-shaped — 2 lone pairs equatorial in TBP
• AB5 (BrF5, IF5): sp3d2, square pyramidal — 1 lone pair in octahedral axial position
• AB7 (IF7): sp3d3, pentagonal bipyramidal — 0 lone pairs

VSEPR Lone Pair Rules:

• In trigonal bipyramidal (5 $e^{-}$ pairs): lone pairs prefer equatorial positions (120° vs. 90° repulsions)
• In octahedral (6 $e^{-}$ pairs): lone pairs prefer opposite (trans) positions (180° — maximum separation)

Hybridization Calculation Method:

• Hybridization = ½ [valence $e^{-}$ of central atom + bonds formed + charge adjustment]
• XeF2: ½[8 + 2] = 5 → sp3d
• XeF4: ½[8 + 4] = 6 → sp3d2
• XeF6: ½[8 + 6] = 7 → sp3d3
• ClF3: ½[7 + 3] = 5 → sp3d
• IF7: ½[7 + 7] = 7 → sp3d3

Common Geometry Traps:

• XeF2 looks like it should be bent (2 bonds) but is LINEAR (3 lone pairs in equatorial)
• XeF4 looks like it should be tetrahedral (4 bonds) but is SQUARE PLANAR (2 lone pairs)
• ClF3 might seem trigonal planar but is T-SHAPED (2 lone pairs occupy equatorial positions)