1. SCIENCE 1206 – UNIT 1 CHEMISTRY

2. UNIT OUTLINE CHEMISTRY TERMINOLOGY 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!

4. CHEMISTRY TERMINOLOGY
Matter: Anything that has mass and volume (takes up space).
What is not matter?
Energy
Mass: The amount of matter an object contains, measured in
grams, g.

5. 3 STATES OF MATTER 1. SOLID 2. LIQUID 3. GAS Chemistry Subscripts
Definite volume and shape
2. LIQUID
Definite volume, indefinite shape
3. GAS
Indefinite volume, indefinite shape
Chemistry Subscripts
(s) - solid
(l) - liquid
(g) - gas
(aq) - aqueous
(dissolved in water)

6. WHAT IS CHEMISTRY?
Chemistry is the study of the properties and chemical changes/reactions of matter.
Examples of chemical reactions:
Rusting
Burning/Combustion

7. Physical Property - quality or characteristic of a substance that can be observed WITHOUT a chemical reaction.
Examples:
State of matter
Hardness
Colour
Malleability
Ductility
Odor
Solubility
Brittleness
Conductivity
Melting and Boiling Points

8. Physical change - a change in state of matter of a substance.
Examples:
Melting/fusion (s → l)
Freezing (l → s)
Evaporation (l → g)
Condensation (g → l)
Sublimation (s → g)
Deposition (g → s)

9. Example: Magnesium ribbon burning
Chemical property - a behavior 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. They are difficult to reverse.
Example: Iron Rusting
4 Fe(s) + 3 O2(g)  2 Fe2O3(s)

10. Here are some chemical change indicators:
COLOUR CHANGE

11. BUBBLES OF GAS

12. SOLID (PRECIPITATE) FORMATION

13. HEAT/LIGHT GIVEN OFF

14. Chemists can use various tests to determine the presence of certain gases and other substances: 1. Oxygen gas is present if a glowing splint burst into flame.

15. 2. Hydrogen gas is present if a lit splint causes a “pop”.
3. Carbon dioxide is present if limewater solution turns milky when the gas is bubbled into it.

16. 4. Water vapor is present if cobalt chloride test paper changes from blue to pink. 5. Acid is present if litmus paper turns red.

17. 6. Base is present if litmus paper turns blue.
7. There is an aqueous solution of salt if it conducts electricity.

18. Reactants - 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)

19. There are 2 Types of Pure Substances: 1. Element
Pure substances - made up of only one type of atom or atom combination.
There are 2 Types of Pure Substances:
1. Element
CANNOT be broken down into a simpler substance by a chemical change.
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 - sodium
Li - lithium
Ar - argon
W - tungsten

20. 2. Compound
CAN be broken down into its elements with a chemical change..
Made up of two or more different elements are chemically joined together in fixed proportions.
Examples:
NaCl
C12H22O11
CH4
H2O

21. Counting Atoms
1. The symbol of an element represents one atom of that element.
Eg. Ba= 1 atom of barium Hg=
CO= 1 atom of carbon NaI=
1 atom of oxygen
2 atoms in total
If you don’t see a number – assume there is 1 atom!!
A subscript is a number written at the lower right hand corner behind the symbol of an element. If there is more than one atom of the same element, then a subscript number is used.
Eg. Cl2 = 2 atoms S4=
H2O3= 2 atoms of hydrogen K2CO3=
3 atoms of oxygen
5 atoms in total

22. A subscript outside a bracket multiplies all the elements inside the bracket ONLY!
Eg. Ca3(PO4)2 = 3 atoms of calcium
2 atoms of phosphorous
8 atoms of oxygen
13 atoms in total
Pb(NO3)4 =

23. 9C= 9 atoms of carbon gas 4O2 =
A coefficient is a number written in front of a chemical name and it indicates the number of elements or molecules present. (if 2 – double everything, if 7 multiply every atom by 7 in that molecule)
9C= 9 atoms of carbon gas 4O2 =
3NaSO4= 3 formula units of NaSO4 5ZnPO4 =
3 atoms of sodium
3 atoms of sulfur
12 atoms of oxygen
18 atoms in total
How to Count Atoms - worksheet
How to Count atoms video

24. Remember - Diatomic Molecules
There are 7 elements that are diatomic, or found in pairs, in their natural state.
These are: Meaning if you are counting atoms – you need to remember if these molecules are mentioned you have to remember there are 2, 4 or 8!!
H2,
O2,
F2,
Br2,
I2,
N2,
Cl2,
Also P4 and S8
Memory tool: P S H O F Br I N Cl

25. Worksheet Counting atoms
Quiz # 1 – all chem notes, worksheets, homework questions up to this point!