Chemistry Unit 5: Covalent Bonding

Bond types, molecule shapes, polarity of covalent compounds, and IMF

Non-polar covalent bond

Difference in electronegativity < 0.4

Polar covalent bond

0.4 < Difference in electronegativity < 1.7

Ionic bond

1.7 < Difference in electronegativity

Linear

2 bonding electron groups; 0 lone pairs around central atom

Trigonal planar

3 bonding electron groups; 0 lone pairs around central atom

Tetrahedral

4 bonding electron groups; 0 lone pairs around central atom

Trigonal pyramidal

3 bonding electron groups; 1 lone pair around central atom

Bent

2 bonding electron groups; 2 lone pairs around central atom

Trigonal bipyramidal

5 bonding electron groups; 0 lone pairs around central atom

Octahedral

6 bonding electron groups; 0 lone pairs around central atom

Polar molecules

asymmetrical: not the same all around the central atom

Nonpolar molecules

symmetrical

LDF (London Dispersion Forces)

All molecules experience this IMF

Dipole-Dipole

Only polar molecules experience this IMF

Hydrogen Bons

Polar molecules with Hydrogen directly connecting to N, O or F experience this IMF