1. SCIENCE 1206 – UNIT 2 CHEMISTRY

2. UNIT OUTLINE CHEMISTRY TERMINOLOGY BOHR DIAGRAMS ATOMS versus IONS
GENERAL TERMS
PERIODIC TABLE
BOHR DIAGRAMS
ATOMS versus IONS
NAMING COMPOUNDS
IONIC, MOLECULAR, ACIDS
CHEMICAL REACTIONS
BALANCING CHEMICAL EQUATIONS
5 TYPES of REACTIONS

3. IMPORTANT TO KNOW . . . You will get a PERIODIC TABLE!!!
It is your best friend for this unit!
You will need it each and every day.
Take care of it, cherish it, appreciate it!
In other words, do not leave it in a crumpled mess at the base of your locker or bookbag 

4. CHEMISTRY TERMINOLOGY
MATTER
DEFINITION:
Anything that has mass and volume (takes up space).
What is not matter?
Energy
In chemistry, we often discuss microscopic matter, such as atoms, ions, elements, and compounds.
MASS
The amount of matter an object contains, measured in grams, g.

5. 3 STATES OF MATTER SOLID LIQUID GAS Chemistry Subscripts
Definite volume and shape
LIQUID
Definite volume, indefinite shape
GAS
Indefinite volume, indefinite shape
Chemistry Subscripts
(s) - solid
(l) - liquid
(g) - gas
(aq) – aqueous, dissolved in water

6. WHAT IS CHEMISTRY? DEFINITION: So, chemistry matters 
The study of the properties and chemical changes/reactions of matter.
So, chemistry matters 
Examples of chemical reactions:
Rusting
Burning/Combustion

7. TWO TYPES OF CHEMISTRY PURE CHEMISTRY APPLIED CHEMISTRY
Theoretical work that involves DESCRIBING known substances and DISCOVERING new compounds for research purposes.
APPLIED CHEMISTRY
Practical work that involves searching for USES for known substances.

8. PHYSICAL PROPERTY
A QUALITY or CHARACTERISTIC of a substance that can be observed WITHOUT a chemical reaction.
Examples of Physical Properties
State of matter
Hardness
Colour
Malleability
Ductility
Odor
Solubility
Brittleness
Conductivity
Melting Point and Boiling Point

9. PHYSICAL CHANGE A change in state of matter of a substance.
Examples of Physical Changes:
Melting/fusion – SOLID to LIQUID
Freezing – LIQUID to SOLID
Evaporation – LIQUID to GAS
Condensation – GAS to LIQUID
Sublimation – SOLID to GAS
Deposition – GAS to SOLID
Ex: H2O(s)  H2O(l)

10. CHEMICAL PROPERTY
A BEHAVIOUR of a substance that can only be observed when a CHEMICAL CHANGE is taking place.
Example:
Magnesium ribbon burning
2 Mg(s) + O2(g)  2 MgO(s) + light energy
The chemical property is that light is given off when magnesium is burned.
CHEMICAL CHANGE
A change in which ONE OR MORE NEW SUBSTANCES is formed.
Iron Rusting 4 Fe(s) + 3 O2(g)  2 Fe2O3(s)

11. INDICATORS OF A CHEMICAL CHANGE
Basically, a chemical change has occurred if the change is DIFFICULT TO REVERSE.
However, there are many good indicators of a chemical change.
Observe the following pictures, and take a guess at what is happening to indicate a CHEMICAL CHANGE.

12. CHEMICAL CHANGE INDICATORS
COLOUR CHANGE

13. CHEMICAL CHANGE INDICATORS
BUBBLES OF GAS

14. CHEMICAL CHANGE INDICATORS
SOLID (PRECIPITATE) FORMATION

15. CHEMICAL CHANGE INDICATORS
HEAT/LIGHT GIVEN OFF

16. MATTER FLOW CHART-Draw
PURE SUBSTANCE
COMPOUND
ELEMENT
ATOM
MIXTURE
HOMOGENEOUS MIXTURE
(SOLUTION)
HETEROGENEOUS MIXTURE

17. PURE SUBSTANCE Made up of only ONE TYPE OF ATOM or ATOM COMBINATION
Stays the same in response to a physical change
Example: O2
H2O
TWO TYPES:
Element
Compound

18. TYPES OF PURE SUBSTANCES
ELEMENT
A pure substance that CANNOT be broken down into a simpler substance by a CHEMICAL CHANGE.
It is made up of 1 TYPE OF ATOM.
Element SYMBOLS are always written with the first letter UPPERCASE and the second letter LOWERCASE.
Element NAMES are always written in LOWERCASE letters.
Examples: Na Li Ar W

19. TYPES OF PURE SUBSTANCES
COMPOUND
A pure substance that CAN be broken down into its elements with a CHEMICAL CHANGE.
It is made up of two or more different elements are chemically joined together in fixed proportions.
Examples:
NaCl
C6H12O6
CH4
H2O

20. MIXTURE Contains 2 or more pure substances TWO TYPES:
HOMOGENEOUS MIXTURE
AKA SOLUTION
Have only one visible phase throughout
Examples:
air, apple juice, salt water
HETEROGENEOUS MIXTURE
Contains 2 or more visible phases throughout
Soil, soup, fruitcake

21. DIATOMIC MOLECULES
There are 7 elements that are diatomic, or found in pairs, in their natural state.
These are:
H2,
O2,
F2,
Br2,
I2,
N2,
Cl2,
Also P4 and S8
Memory tool: P.S., HOFBrINCl

22. REACTANTS PRODUCTS CHEMICAL REACTION
Starting Materials in a chemical reaction
PRODUCTS
New substances formed in a chemical reaction
CHEMICAL REACTION
Reactants go to form Products
Example:
C(s) + O2(g)  CO2(g)

23. MSDS – MATERIAL SAFETY DATA SHEET