1. Chemistry 9 - Review 1 1

2. 1. Classification Of Matter
Oxygen
Water
Salt water
Water & oil

3. 3 3

4. Name the following H2 O2 N2 NH3 CH4 H2O CO2 NaCl Hydrogen Oxygen
Nitrogen
Ammonia
Methane
Water
Carbon Dioxide
Sodium chloride 4 4

5. 2. Properties

6. a) Physical A) Qualitative: B) Quantitative State :solid, liquid, gas.
Color: colorless, black, white …
Texture: rough, smooth or bumpy
Form : crystals, cubes, powder, hexagon, wire, sheet
Odour: strong, weak, sweet, mouldy, odourless.
Lustre : shinny or dull
Clarity : transparent, translucent, opaque
Malleability : soft, pliable, hard - can bend (e.g. Al)
Ductility : ductile – can stretch (Cu)
Melting Point: high or low
(ice → 0˚ C)
Boiling Point : high or low
(water → water C )
Density = Every substance has a unique density (g/ml)
Solubility : soluble or insoluble. Capacity to dissolve in another substance
Viscosity: high or low. The measure of a substance’s resistance to flow. (e.g. maple syrup has a high viscosity)
Hardness: hard or soft. Ability to scartich another material (e.g. : icing sugar vs. table salt)
Conductivity: high or low. Ability to conduct electricity or heat.

7. b) Chemical
The ability of a substance to react with another - behaviour
Combustibility 
Reaction with acid 
Reaction with water 
Toxicity 
Stability 

8. Describe these substances
Copper (Cu)
Aluminum (Al)

9. Table (NaCl)
Icing Sugar

10. 3. The Particle Theory of Matter.
All matter is made up of tiny particles.
Particles can’t be created nor destroyed.
All particles of the same elements are identical.
Particles attract each other.
Particles are always moving.
Particles at a higher temperature move faster.

11. 4) How is density determined?
Density is mass divided by volume, or D = m/v.
Common units are g/cm3 or g/mL
Water has a density of 1 g/mL. Thus, objects with density greater than 1 g/mL will sink in water. Objects with density less than 1 g/mL float in water.
M = v • d
V= m/d 11

12. Example
A sample of aluminum metal has a mass of 8.4 g. The volume is 3.1 cm3. Find the density.
Known
Unknown
m = 8.4 g
D = ?
V = 3.1 cm3

13. 5) Gas Tests
Test
Result
Place a burning splint in the presence of the unknown gas
If you hear a « pop », and the splint goes out, it’s Hydrogen.(H2)
If the splint goes out, it’s Carbon dioxide (CO2)
Place a glowing wooden splint in the presence of the unknown gas.
If the glowing splint ignites (relights), it’s Oxygen (O2)

14. Hydrogen Gas Test

15. Carbon Dioxide Gas Test
With lime water
Burning splint

16. Oxygen Gas Test

17. 6) Modern Periodic Table
The horizontal rows are called periods
The vertical columns are called groups are labeled from 1 to 18.
Elements in the same group have similar chemical and physical properties!!

19. 7) How are elements organised today?
Elements are organised according to their atomic number.
Elements are classified in three groups:
Metals(to the left of the stairs)
Non-metals(to the right of the stairs)
Metalloids (around the stairs)

20. Must round to 11

21. Neutrons = 11-5
Boron has 6 neutrons.

22. 8) Standard Atomic Notation

23. 9) Bohr-Rutherford Atomic model
# e-= p+= atomic #
# n = atomic Mass – atomic #
Stable atom = last orbit is complete (saturated).
Ion = an atom where # p+ ≠ # e-
+ ion = an atom that has lost e-. (Mg+2)
- ion = an atom that has gained e-. (N-3) 23 23

24. 10)Valence electrons = # of electrons on the last orbit
Each group has the same # of valence e- (electrons on the last orbit)

26. Practice 26 26

27. 11) Types de compounds: 1) Ionic Compounds: Covalent Compounds
Its a molecule made of a metal and one or more non-metals.
In this type of compounds, there is a transfer of e-→ The metal loses e- and the non-metals gains e- to form an ionic bond.
Physical Properties
They are all crystals – salt.
They are hard
They are all soluble in water.
When dissolved, they are are good conductors “electrolytes”.
High melting point– it takes 800°C to melt table salt.
High boiling point.
It’s a molecule that contains 2 or more non-metals.
The two atoms share electrons to make a covalent bond.
E.g. H2O, CO2, CH4
All diatomic molecules (7 non-metals) are covalent : H2 O2 Br2 F2 I2 N2 Cl2
Physical Properties:
They can be solid, liquid or gas
If solid, they are soft.
Some are soluble in water.
They are uncharged, so they don’t conduct electricity.
Low melting point ( they melt fast, since they have weak bonds)
Low boiling point.

28. Ionic
Covalent

29. 12) How to count atoms? 1 CO2 2 NaCl 3 MgClO3 2 H2SO4 2 CaCl2
1 carbon atom
2 oxygen atoms
Total 3 atoms
1 molecule of CO2
2 NaCl
3 MgClO3
2 H2SO4
2 CaCl2 29 29