Unit 9 (Molecular Geometry, Polarity, Hybridization)

Electron geometry of 2 e domains

Linear

Electron domain geometry of 3 domains

Trigonal planar

Electron domain geometry of 4 domains

Tetrahedral

Electron domain geometry of 5 domains

Trigonal Bipyramidal

Electron domain geometry of 6 domains

Octahedral

Molecular geometry of 3 domains, one lone pair

Bent

Molecular geometry of four domains one lone pair

Trigonal pyramidal

Molecular geometry of four domains two lone pairs

Bent

Molecular geometry of five domains one lone pair

Seesaw

Molecular geometry of 5 domains two lone pairs

T-shape

Molecular geometry of five domains, three lone pairs

Linear

Molecular geometry of six domains, one lone pair

Square pyramid

Molecular geometry of six domains, 2 lone pairs

Square planar

Molecular geometry of 6 domains, 3 lone pairs

T-shape

Molecular geometry of 5 domains, 4 lone pairs

Linear

Bond angle of linear

180

Bond angle of Trigonal planar (electron domain geom)

120

Bond angle of tetrahedral

109.5

Bond angle of Trigonal bipyramidal

90/120

Bond angle of octahedral

90

Two distinct electron domain positions in a Trigonal bipyramidal electron domain

• axial (top/bottom)

• Equatorial (sides)

Bond angle of bent, three domains

120

Bond angle of Trigonal planar, four domains

109

Bond angle of bent, four domains (two lone pairs)

109

Bond angle of seesaw

90 axial, 120 equatorial

Bond angle of T-shape

90

Bond angle of square pyramid

90

Bond angle of square planar

90

What does it mean for a molecule to be nonpolar

If the bond dipoles within the molecules cancel out by being in equal and opposite directions, look at the direction of electronegativity arrows

What do lone pairs do to polarity?

Push polarity

What is the valence-bond theory

Electrons of two atoms begin to occupy the same space (“overlap” of orbitals)

Hybridization of ED# 2

Sp

Hybridization ED#3

Sp2

Hybridization ED#4

Sp3

Hybridization ED#5

Sp3d

Hybridization ED#6

Sp3d2

Order the bonds by size

Single>Double>Triple