Forces of attraction/repulsion between molecules.

intermolecular

intramolecular

intramolecular

intermolecular forces

Forces of attraction/repulsion within a molecule.

intramolecular forces

J. Van der Waals(1837 – 1923)

Van der Waals ForcesThis is the name given to the many different weak

intermolecular forces.

Dipole-Dipole Force

Negative ends of polar molecules are attracted to positive ends of neighbouring polar molecules.

In a liquid, molecules can orient themselves to maximize attraction and minimize repulsion.

London Force

Fritz London(1900 – 1954)

(also called: London dispersion)

This force is caused by the attraction of electrons to other molecules’ nuclei.

It is caused by a brief shift in electrons from one side of an atom/molecule to another, called a momentary dipole.

The greater the number of electrons in the atoms of a molecule, the greater the dispersion forces.

Using Dipole-Dipole and London Forces to Predict Boiling Points

Boiling point is a good relative measure of intermolecular force.

The greater the number of electrons in a molecule, the greater the London forces between them, the higher the boiling point.

4 (g)CH

2 6 (g)C H

3 8 (g)C H

4 10 (g)C H

Isoelectronic molecules have the same number of electrons.

Polar molecules will have dipole-dipole forces along with London forces.

Hydrogen BondingA hydrogen bond is where a hydrogen nucleus (a proton) is shared between electrons on neighbouring molecules.

ammonia water

• The hydrogen atom must be “unshielded.” To accomplish this it must be bonded to a highly electronegative atom: nitrogen, oxygen or fluorine.

• There must be at least on lone pair of electrons on the atom bonded to the hydrogen.

+

–

Hydrogen bonding is the strongest intermolecular force.

covalent bond (intramolecular)

covalent bond (intramolecular)

hydrogen bond (intermolecular)

Some Effects of Hydrogen Bonding

Hydrogen bonding between water molecules makes water have relatively high melting and boiling points when compared to other substances.

12 22 11 (s)C H O 12 14 3 8 (s)C H O OHor

Sucrose molecules are held firmly in a crystalline structure as solid and are readily dissolved in water.

Water mixed with glycerol is called glycerine, commonly found in soaps.

Water molecules form hydrogen bonds with glycerol molecules.

sucrose

In a DNA molecule, the central bonds that holds the double helix together are hydrogen bonds.

Hydrogen bonding holds water molecules in a hexagonal lattice when it freezes.

The large spaces in the lattice makes ice less dense than water.

Physical Properties of Liquids

Surface Tension

Liquids with high intermolecular forces, especially water, have high surface tension.

Molecules right at the surface are only pulled downward and sideways.

Water’s high surface tension causes it to have a concave meniscus.

Capillary action is water being pulled up a narrow tube by the intermolecular forces between the water molecules and the tube.

rubbing alcohol

nail polish remover

gasoline

Liquids with small intermolecular forces are volatile: they tend to evaporate quickly.

Read pgs. 105 – 117

pgs. 109, 116 Practice #’s 1 – 5, 7 – 10

pg. 117 – 118 Section 3.4 Questions #’s 1 – 10