Electrolytes vs Non-Electrolytes

Electrolytes ( weak or strong ) are

• Aqueous solutions that CONDUCT ELECTRICITY

• All soluble ionic compounds

• very polar molecular compounds ( acids, ammonia )

Non - Electrolytes are

• Aqueous solutions that DO NOT CONDUCT ELECTRICITY

• Molecular compounds in solutions

• Insoluble ionic compounds

DISSOCIATION occurs when

IONIC COMPOUNDS break apart into their IONS when they are dissolved in an AQUEOUS SOLUTION

DISSOCIATION EQUATIONS are used

To show what happens to a substance when it is put into water.

How many situations can you have

4

1. Insoluble compounds

• Can be IONIC or MOLECULAR

• They DO NOT DISSOLVE to any great extent

• Use the SOLUBILITY TABLE for ionic compounds

Eg) AgCl (s) → AgCl (s)

2. Soluble Ionic Compounds

• Dissolve to a great extent to form IONS IN SOLUTIONS

• IONIC BONDS are broken

• Use solubility table

Eg) NaCl (s) → Na (aq) + Cl (aq)

3. Soluble Molecular Compounds

• Dissolve to form MOLECULES IN SOLUTIONS

• INTERMOLECULAR FORCES ( LD, DD, HB ) are broken

• INTRAMOLECULAR FORCES STAY INTACT

Eg) C12H22O11 (s) → C12H22O11 (aq) (sucrose)

4. Acids

• They are MOLECULAR COMPOUNDS but are VERY POLAR

• IONIZE when they dissolve in water

Eg) H2SO4 (s) → 2H (aq) + SO4 (aq)

Examples

Soluble in water:

Sucrose

CO2 (g) → CO2 (aq)

C6H12O6 (s) → C6H12O6 (aq) (glucose)

Insoluble:

Hydrocarbons like

CH4 (g) → CH4 (s) (methane)

octane

wax

oil