Test Review Answers
Question 1
 1a)Heterogeneous (“different kinds”)
A mechanical mixture.
2 or more substances can be seen or felt.
Homogeneous (“same kind”)
A solution
Particles of 2 or more pure substances
mix completely
Feel and look like one substance
Properties of sample always the same
Colloids
b) A mixture in which extremely small particles
are evenly distributed and are hard to see
with the unaided eye.
Example: whipped cream, fog
Suspensions
 a mixture where the particles, if left alone,
gravity will help separate.
 Example: Italian salad dressing
•
Ketchup
Classification of Matter
Mixture – Two or more pure
substances mixed together. A special
type of mixture is an alloy. See
below.
Example:
Even
though
Copper
it may
and
look
different,
Zinc
can be
it mixed
is still copper
together
and
zinc. to
Each
produce
metal
brass. its own properties
retains
like melting point.
Pure Substances
 Pure substances can also be divided into 2
categories: compounds and elements.
Compound – Two or more elements chemically
bonded together.
Examples:Carbon Dioxide (CO2) Water (H2O)
Salt (NaCl) Sucrose (C12H22O11)
Elements – Substances made up of only one type of
atom.
- Cannot be separated by any physical OR
chemical process.Examples:Carbon, Helium,Gold
Mechanical Mixture
 a substance made of more than
one kind of particle in which the
particles are not uniformly
scattered. (heterogeneous)
example: pizza
Solutions
A homogeneous mixture of 2 or
more pure substances.
Ex. Kool-Aid
Weight is the measure of
gravitational pull on matter,
measured in Newtons. Weight
can vary depending on where you
are.
Mass is the amount of matter in an
object measured in grams using a
balance scale.
A physical property describes the qualities
of matter that will not change its
composition.
Examples:color,malleability,ductile, shape
A chemical property describes the qualities
of matter that will change its composition.
Examples: combustibility, flammability,
corrosive.
Question 3
a)
b)
c)
d)
physical
physical
chemical
chemical
Question 4
Three indicators of a chemical
change are:
1. Gas is produced (bubbles, fizz)
2. Color change (cooking)
3. Burning, fire, explosives
4. Rust
Question 5
a) chemical
b) physical
c) physical
d) chemical
e) physical
f) chemical
Question 6
a) Mechanical Mixture
b) element (on periodic table)
c) Suspension (need to shake)
d) solution
e) colloid (white, cloudy)
f) mechanical mixture
g) element
h) colloid
I) alloy (solution of metals)
j) mecanical mixture
j) element
k) suspension (settle over time)
The Particle Theory
1. All matter is composed of
tiny particles.


Size and shape vary.
All particles of pure substance
are exactly the same size.
2. All particles of one
substance are the same

Salt particles are different from
pepper particles
The Particle Theory
3. There are spaces between
particles.
4. Particles are always moving –
the more energy they have, the
faster they move.
  temp the faster the particles move
5. There are forces of attraction
between particles.
The Particle Theory
Energy is transferred between
particles by moving particles
hitting each other and either
speeding up or slowing down.
Matter has particles
Moving particles
Attraction between particles
Same particles throughout
Spaces between particles
2
M ASS
Matter
Solid
Particles are close together and
locked together into a pattern.
Attractive forces are very strong.
Particles move, but only vibrate in
one place.
Matter
Liquid
Particles are slightly farther apart
Attractive forces are weaker
Particles are able to slide past
one another
Matter
Gas
Particles are far apart.
Attractive forces are weakest.
Particles are able to move in any
direction.
Classification of Matter
Any substance
or material that
has mass and
occupies space.
matter
mixtures
mechanical mixture
(heterogeneous)
pure substances
solutions
(homogeneous)
Matter can exist in 4 states: solid, liquid, gas and plasma
Law of Conservation of Matter
No matter can be created or destroyed. In a
chemical reaction, the mass of the reactants
will always equal the mass of the products.
As well, the individual atoms will not be
lost. If we start with 4 atoms of Carbon, we
will end with 4 atoms of Carbon, however in
different forms of matter.
Example: water + baking soda