Hybridization

Electron-geometry based

electron geometry vs molecular geometry

When lone pairs are present, the electron geometry (based on VSEPR) stays the same, but the molecular geometry changes because lone pairs aren’t visible atoms.

sp³ hybridization

4 regions of electron density = tetrahedral electron geometry

• 0 lone pairs: Tetrahedral

  • ex: (CH₄)

  • 109.5°

• 1 lone pair: Trigonal pyramidal

  • ex: (NH₃)

  • ~107°

• 2 lone pairs: Bent

  • ex: (H₂O)

  • ~104.5°

sp² hybridization

3 regions = trigonal planar electron geometry

• 0 lone pairs: Trigonal planar

  • ex: (BF₃)

  • 120°

• 1 lone pair: Bent

  • ex: (SO₂)

  • slightly <120°

sp³d hybridization

5 regions = trigonal bipyramidal

• Bond angles: 90°, 120°, 180°

• Example: PCl₅

0 lone pairs: trigonal bipyramidal

• Bond angles: 90°, 120°, 180°

• Example: PCl₅

(1 lone pair): seesaw

• ~90°, 120°, 180°

• Example: SF₄

(2 lone pairs): t-shaped

• ~90°, 180°

• Example: ClF₃

sp³d² hybridization

6 regions = octahedral

• Bond angles: 90°, 180°

• Example: SF₆

0 lone pairs: octahedral

• Example: SF₆

• Angles = 90°, 180°

(1 lone pair): square pyramidal

• ~90°

• Example: BrF₅

(2 lone pairs): square planar

• ~90°

• Example: XeF₄