sp³ hybridization occurs when one s orbital and three p orbitals on the same atom mix together to form four equivalent hybrid orbitals. Each hybrid orbital can hold one electron pair (2 electrons). This mixing process is called hybridization and is purely a model — we use it to explain observed bond geometries.
sp³ hybridization is when one s orbital and three p orbitals from the same atom mix together to form four identical hybrid orbitals. Each hybrid orbital can hold 2 electrons. This is the most common hybridization you'll see in NEET — it appears in every saturated carbon, nitrogen, and oxygen compound. The key is understanding why these four orbitals arrange themselves at 109°28′ and how lone pairs compress this angle.
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Carbon in methane has four bonding pairs and zero lone pairs. VSEPR theory says electron pairs (bonding or lone) repel each other. The geometry that spreads four pairs farthest apart in 3D space is tetrahedral, which has bond angles of exactly 109°28′.
NH₃ has 3 bonding pairs + 1 lone pair = 4 electron pairs total. H₂O has 2 bonding pairs + 2 lone pairs = 4 electron pairs total. Lone pairs repel more strongly than bonding pairs, so they compress the bonding angles. NH₃ is ~107°, H₂O is ~104.5°.
Count electron pairs (bonding + lone) around the central atom. If total = 4, the electron geometry is tetrahedral. Then count only bonding pairs: 4 bonds = 109°28′, 3 bonds = ~107° (trigonal pyramidal), 2 bonds = ~104.5° (bent). Lone pairs always compress the angle.
Hybridization is a teaching model — it's not 'real' in the sense that orbitals don't physically mix. But the model works brilliantly to predict bond angles, bond strengths, and molecular geometry. For NEET, treat it as real and use it to explain why bonds arrange the way they do.
Visualize sp³ hybridization — neet explained with an interactive 3D simulation.
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