1. Matter, Atoms and the Periodic Table

2. Matter and Classification
Matter is anything that has mass and takes up space.
Matter
Pure Substance
Element
Compound
Mixture
Homogeneous
Solution
Heterogeneous
Mechanical
Suspension
For further terminology information, see p. 143 of textbook

3. Physical and Chemical Properties
Physical Properties of Matter
Chemical Properties of Matter
Boiling Point
Melting Point
Colour
State (solid, liquid, gas)
Malleability
Conductivity
Solubility
Ductility
Crystal Formation
Ability to burn (combust) – emission of heat, light, flame
Reaction with water
Reaction to heating
Flash point – lowest temperature in which a flammable liquid will ignite in air
Behaviour in air

4. Matter and Atoms Matter is made up of tiny units called atoms.
Atoms of one element differ from atoms of a different element (eg. physical & chemical properties).
Atoms are made up of subatomic particles:
Protons (positive charge of 1+)
Electrons (negative charge of 1-)
Neutrons (neutral, no charge)
Atoms have an inner nucleus, where protons and neutrons are held. Outside this, electrons orbit in cloud-like energy levels (shells) that surround the nucleus.
Copper and Gold

5. Periodic Table
Metalloid (semi-metal)

6. Periodic Table
Elements within the same group (columns) have similar properties because they have the same number of valence electrons (electrons in their outer shell).
Elements in the same period (rows) do NOT have similar properties. The period number indicates the number of electron shells.
Four common chemical families (groups):
Alkalis (Group 1) – silver-grey, soft, react with H2O as well as O2 (hydrogen not included in this group)
Alkalines (Group 2) – silver-grey, less reactive and a bit harder than Group 1
Halogens (Group 17) – colored, very reactive
Noble gases (Group 18) – inert (very unreactive), colorless, odorless gases

7. Elements on the Periodic Table
Atomic Number – number of protons in an atom of an element
Eg. Boron’s atomic number is 5, therefore, it has 5 protons
Atomic Mass – average mass of an atom of that element
Number of protons + number of neutrons = atomic mass
Eg. Boron’s atomic mass is 10.82
Ion Charge
An ion is an atom that has either a positive (cation) or negative (anion) charge
An atom has a charge when electrons are:
Lost (results in positive charge)
Gained (results in negative charge)
Eg. Boron can only form one ion in which it will lose 3 electrons to become 3+
Ion charge
Atomic number
Atomic mass

8. Bohr Rutherford Diagrams
Shows the arrangement and number of electrons in shells
1st shell: maximum 2 electrons
2nd shell: maximum 8 electrons
3rd shell: maximum 8 electrons
4th shell: maximum 2 electrons
Hence, “2, 8, 8, 2 rule”
To determine the number of electrons to draw, it is equivalent to the number of protons for that element!
Number of neutrons: Atomic mass – number of protons
Draw Bohr Rutherford diagrams for:
Carbon atom
Potassium atom
Fluorine ion