1. Intermolecular Forces
Chemistry 11
Ms. McGrath

2. Intermolecular Forces
The forces that bond atoms to each other within a molecule are called intramolecular forces. Covalent bonds and ionic bonds are an example of intramolecular forces. In comparison, the forces that bond molecules to each other are called intermolecular forces.

3. Intermolecular Forces
Intermolecular forces are generally weaker than ionic or covalent bonds. For example, only 16 kJ/mol is required to overcome the intermolecular attractions between HCl molecules. In contrast, the energy required to break the covalent bond to dissociate HCl into H and Cl atoms is 431 kJ/mol.

4. Intermolecular Forces
Intermolecular forces were studied extensively by Johannes van der Waals (1837 – 1923) and they are therefore often referred to as van der Waals forces.

5. Intermolecular Forces Dipole – Dipole Forces
Dipole means polar molecule
Dipoles will change their direction so that their oppositely charged ends are near to one another.
The electrostatic attraction between the oppositely charged ends of the polar molecules are called
dipole -dipole forces.

6. Intermolecular Forces Dipole – Dipole Forces
As a result of these dipole – dipole forces of attraction, polar molecules will tend to attract one another more at room temperature than similarly sized non-polar molecules would.
The strength of these dipole-dipole forces and the amount of energy required to separate them is indicated by the temperature at which the substance changes phases – its melting point and its boiling point.

7. Intermolecular Forces Dispersion (London) Forces
Weakest intermolecular force between non polar molecules
It is a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles

8. Intermolecular Forces Dispersion (London) Forces
The shared pairs of electrons in a covalent bond are constantly vibrating.
The bond vibrations, which are part of the normal condition of a non-polar molecule, cause momentary, uneven distribution of charge.

9. Intermolecular Forces Dispersion (London) Forces
In other words, a non-polar molecule becomes slightly polar for an instant, and continues to do this on a random but on- going basic. At the instant that one non-polar molecule is in a slightly polar condition, it is capable of inducing a dipole in a nearby molecule.

10. Intermolecular Forces Dispersion (London) Forces
An intermolecular force of attraction results.
The degree of force is related to the number of electrons as well as the size and shape of the molecule – larger molecules tend to display stronger London dispersion forces.

11. Intermolecular Forces Hydrogen Bonding
Is a special type of intermolecular attraction that exists between the H atom in a polar bond (particularly H-F, H-O, H-N bonds) and an unshared electron pair on a nearby small electronegative ion or atom (usually a F, O or N atom on another molecule).
More lone pairs means stronger hydrogen bonds.

12. Intermolecular Forces Interesting facts…
“Hydrogen Bonding”
If a compound experiences strong intermolecular forces such as hydrogen bonding, it will have a higher melting and boiling point. This is because hydrogen bonding helps to stick the molecules together, making it harder to pull them apart.

13. Intermolecular Forces Interesting facts…
“Like Dissolves Like”
Ionic solutes dissolve in polar solvents
(ex: NaCl and H2O)
Non polar solutes dissolve in non polar solvents
(ex: solid I2 and liquid Br2)

14. For your notes Read through pages 203 and 204
Record notes for Ion – Dipole Forces and Induced Intermolecular Forces
See the table on page 209, be familiar with the strength of the bonds. Note: Intramolecular Forces are stronger than Intermolecular Forces