1. Valence Shell Electron Repulsion Theory (VSEPR)

2. Intermolecular forces Intramolecular forces
Chemical Bonding
Intermolecular forces
Intramolecular forces

3. Polarity
Polar bonds are a result of varying electronegativities

4. Polar vs. Non-Polar
If the polar bonds of a molecule are oriented such that they are in opposite directions, the dipoles are cancelled out and the molecule is non-polar
Example CH4

5. Polar vs. Non-Polar
If the polar bonds of a molecule are oriented such that they complement each other, then the molecule is polar
Eg. Water

6. General Rule
Molecule will be polar if it has polar covalent bonds and there are one lone pair of electrons on the central atom.

7. Intramolecular Forces
Force between atoms in the molecules
Strong bonds
Eg. Covalent bond

8. Intermolecular Forces
Force holding molecules next to other molecules
Weak forces
Also called Van der Waals forces

9. 2 Types of Van der Waals Forces
dipole-dipole force
London force

10. Dipoles
Polar molecules are often referred to as dipoles (slightly positive and negative ends).
Polar molecules experience an attraction between molecules.
These are called dipole-dipole forces

11. Hydrogen Bonding Special type of dipole-dipole forces
Hydrogen bonding is particular strong dipole-dipole force

12. London Forces
The weakest of van der Waals forces and are the result of momentary dipoles.
Eg. He

13. London Forces
In general, the more electrons an atom/molecule has, the stronger the London forces.
The greater the atomic number of an atom, the stronger the London force.

14. London Forces ALWAYS PRESENT
A lot weaker than covalent or ionic bonds. Hence, London forces are important when they are the only force of attraction between 2 species.

15. London Forces Important between the following closed-shell species:
Adjacent noble gas atoms
Adjacent covalently-bonded molecules (made up of atoms having a full shell after bonding)