1. STOICHIOMETRIC RELATIONS
Introduction To The Particulate Nature of Matter and Chemical Change

2. MATTER
Mass
Volume
Particles
Particles in constant motion

3. Contain 1 type of particles Contain different types of particles
MATTER
Pure Matters
ELEMENTS
COMPOUNDS
Mixtures
Homogeneous
(SOLUTIONS)
Heterogeneous
Suspension
Emulsion
Aerosol
Contain 1 type of particles
Contain different types of particles
Have 1 type of molecule with different atoms
Have 1 type of atom
S – L
L – L
S – G
L – G

4. MATTER Exercise 4, Test yourself pg 7 ELEMENT COMPOUND MIXTURE Pure
Not pure
Contain 1 type of atom
Contain 1 type of molecule with different atoms
Contain different types of particles
Shown by symbols
Shown by formula
No specific figures -
Constant ratio btw components
No fixed ratio btw components
Homogeneous
Homogeneous
Homogeneous or Heterogeneous
Fixed phys. properties
Fixed phys. properties
Not fixed properties -
Formed/separated by chemical methods
Formed/separated by physical methods
Exercise 4, Test yourself pg 7

5. STATES OF MATTER Solid Liquid Gas + heat + heat + heat - heat - heat
Endothermic
+ heat
Sublimation
Melting
Boiling
+ heat
+ heat
Solid
Liquid
Gas
Freezing
Condensation
- heat
- heat
- heat
Deposition
exothermic

6. STATES OF MATTER Solid Liquid Gas + heat + heat
Fixed volume
No shape
Fixed volume
Fixed shape
No fixed volume
No shape
Solid
+ heat
Liquid
+ heat
Gas
From solid to liquid
Volume generally increases
Density generally decreases
Inter-particular forces get weaker
Total energy increases.
Randomness increases.

7. CHANGES OF STATE Heating Graph of a pure substance Temperature(t, °C)
Heat (Q, j) L G t2 S L t1 t0 S I II
III IV Q1 Q2 Q3 Q4

8. Equality between reactants and products
CHEMICAL EQUATIONS
A(s) + B(l)  C(aq) + D(g)
(s): Solid
(l): Liquid
(g): Gas
(aq): Aqueous solution
Reactants
Products
Equality between reactants and products

9. CHEMICAL EQUATIONS Balancing Equations NaOH + H2SO4  Na2SO4 + H2O
Exercises 1, 2, 3, 5
Test yourself pg 6