Molecular Shapes, Polar & Non-Polar Bonds, and Intermolecular Forces

Linear with 2 elements

2 atoms

No central atom

No BP or NBP

Bond Angle: 180

Linear with 3 elements

3 atoms

4 BP

0 NBP

Bond Angle: 180

Bent with Single Bond

3 atoms

2 BP

2 NBP

Bond Angle: 104.5

Bent with Double Bonds

3 atoms

3 BP

1 NBP

Bond Angle: 106

Trigonal Pyramidal

4 atoms

3 BP

1 NPB

Bond Angle: 107

Trigonal Planar

4 atoms

4 BP

0 NBP

Max Separation: 120

Trigonal Planar (Boron)

Boron only needs 6 vse-

3 BP

0 NBP

Max Separation: 120

Tetrahedral

5 atoms

4 BP

0 NBP

Bond Angle: 109.5

Non-Polar Covalent Bond

Even Sharing of Electrons

EN Diff. 0.0 — 0.4

Or Equal EN

Polar Covalent

Uneven Sharing of Electrons

EN Diff. 0.4 — 2.0

Ionic Bonds

Transfer Electrons

EN Diff. > 2

Polar Molecules

Assymetrial Shape

Non-Polar Molecules

Symmetrical Shape

Always Polar

Bent

Trigonal Planar

Because they always have lone pairs

Intermollecular

Between 2+ molecules

Intramollecular

On the inside of an atom

Dipole-Dipole

Polar Bond

Any Polar Molecule

Hydrogen Bonding

Vey strong Dipole-Dipole force

Has Hydrogen bonded to F, O, or N

Short distance between Dipoles

Unusually Strong

High EN

London Dispersion Forces (LDF)

Non-Polar Molecules

Covalent Bonds