SCIENCE 1206 – UNIT 2
CHEMISTRY
November – January 2011
UNIT OUTLINE

CHEMISTRY TERMINOLOGY
◦ GENERAL TERMS
◦ PERIODIC TABLE

BOHR DIAGRAMS

ATOMS versus IONS

NAMING COMPOUNDS
◦ IONIC, MOLECULAR, ACIDS

CHEMICAL REACTIONS
◦ BALANCING CHEMICAL EQUATIONS
◦ 5 TYPES of REACTIONS
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 


LINK
LINK 2
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.
3 STATES OF MATTER

SOLID
◦ 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
WHAT IS CHEMISTRY?

DEFINITION:
◦ The study of the properties and chemical
changes/reactions of matter.

So, chemistry matters 

Examples of chemical reactions:
◦ Rusting
◦ Burning/Combustion
TWO TYPES OF CHEMISTRY

PURE 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.
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
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)
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.
 Example:
◦ Iron Rusting
4 Fe(s) +
3 O2(g)
 2 Fe2O3(s)
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.
CHEMICAL CHANGE INDICATORS

COLOUR CHANGE
CHEMICAL CHANGE INDICATORS

BUBBLES OF GAS
CHEMICAL CHANGE INDICATORS

SOLID (PRECIPITATE) FORMATION
CHEMICAL CHANGE INDICATORS

HEAT/LIGHT GIVEN OFF
HOMEWORK!!!
Identify the following as a PHYSICAL PROPERTY or
a CHEMICAL PROPERTY.
1.
1.
2.
3.
4.
5.
Burns in air when heated.
Melts at 98 degrees Celsius.
Reacts violently with water.
Can be cut with a knife.
Conducts electricity.
Identify the following as a PHYSICAL CHANGE or a
CHEMICAL CHANGE.
2.
1.
2.
3.
4.
Digesting a meal.
Butter melting in a pan.
Burning gasoline.
Wood rotting.
LINK
MATTER FLOW CHART-Draw
MATTER
PURE
SUBSTANCE
COMPOUND
ELEMENT
ATOM
MIXTURE
HOMOGENEOUS
MIXTURE
(SOLUTION)
HETEROGENEOUS
MIXTURE
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
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
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
◦ LINK
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
◦ Examples:
 Soil, soup, fruitcake
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

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)
HOMEWORK . . .
1. Name the type of pure substance that is
found on the periodic table.
2. Give an example of each of the following:
1. Pure substance
2. Heterogeneous mixture
3. Homogeneous mixture
LINK
MSDS – MATERIAL SAFETY DATA SHEET