Chapter 2 & 3: States of
Matter
Matter
Matter is anything that has mass and
occupies space
Matter: Everything is Made of It!
There are two types of matter:
• 1. Pure Substances: Cannot be broken into simpler
compounds
Elements
Compounds
• 2. Mixtures: Made of two or more substance that
can be easily separated
Homogeneous (same all the way throughout)
Heterogeneous (different throughout)
Matter is anything that has mass and takes up space!
Mixtures
Pure substances
All pure substances are
homogeneous
Elements
Compounds
(1 – simple)
(2 or more)
Examples:
Silver (Ag)
Gold (Au)
Oxygen (O)
Examples:
Salt (NaCl)
Water (H2O)
Homogeneous
Heterogeneous
(same throughout)
(not same throughout)
Examples:
Tap water
Coffee
Air
Examples:
Hershey bar
(with almonds)
Pizza
Vegetable soup
Classify the Following Examples as
Heterogeneous or Homogeneous:
• Hershey Bar?
Homogeneous
____________________________
• Snickers Bar?
____________________________
Heterogeneous
• Pizza?
____________________________
Heterogeneous
• Italian Dressing?
____________________________
Heterogeneous
• Magnesium Bromide (MgBr2)?
Homogeneous
____________________________
Properties of Matter
What is used to describe or identify matter?
•
•
•
•
•
•
•
•
Color (red, blue)
Shape (round, square)
Texture (smooth, rough)
Size (short, big)
Melting point (high, low)
Boiling point (high, low)
Malleability (is, is not)
Density (high, low)
Density
A measurement of how much matter is in a
certain volume of a substance
• Low density = “feels light”
• High density = “feels heavy”
Determines if an object will sink or float
Density = Mass / Volume
Density Practice Problem #1
(density = mass/volume)
• If 20.0 cm3 of ice has a mass of 18.4
grams, what is the density of the ice?
–Equation:
Density = mass / volume
–Show your work: Density = ______/______
18.4 g 20.0 cm3
–Answer:
Density = _____________
0.92 g/cm3
Density Practice Problem #2
(density = mass/volume)
List items which will
float on the
particular sample of
ice from the
previous problem:
• ____________
Air
• ____________
Wood
Methanol
• ____________
Density Practice Problem #3
Find the density of the material using the
graph below:
• Pick any two points on the graph! Density
remains constant for the sample.
• Density = mass/volume
– Mass = __________
– Volume = ________
• Density = _____/_____
= ___________
How to Separate a Mixture
• Use Magnetism
– Ex) Iron filings can be removed from
a mixture with a magnet
• Add Heat (evaporation)
– Ex) Salt (sodium chloride) dissolves
easily in water and can be recovered
from the solution by slow
evaporation of the water and
re-crystallization of the sodium chloride
How to Separate a Mixture
• Use a Funnel
– Ex) Oil and water will separate into layers
and the heavier (denser) layer can be
drained out using a separatory funnel
• Filtration
– Ex) Solid removed from a liquid by using
filter paper. Pour the mixture on top of the
filter paper and catch the liquid below in a
beaker. Solid is separated and trapped on
the paper
Solutions
A solution is a homogeneous mixture composed of
only one phase.
• They can be solid, liquid or gaseous.
There are 2 Parts of a Solution
Solute – Helps make a solution, this is what
dissolves (usually solid) in the solution
• Ex) sugar
Solvent – Helps make a solution, this is what
makes the solute dissolve (usually liquid) in
the solution
Ex) the universal solvent is water
There are 3 Types of Solutions
 Saturated (contains all the
solute it can hold at a given
temperature)
 Unsaturated (can still dissolve
more solute)
 Supersaturated (contains
more solute than it would
normally at a given
temperature)
What Changes the Speed of Solubility
in a Solution?
Concentration
• The solute and solvent interact with each other until
the concentration of the two substances is equal
throughout the system
Temperature
• In general more solute dissolves in a solvent with
higher temps
• More kinetic energy to overcome the attractive forces
between bonds
Stirring
• Stirring will increase the rate of dissolving
 Particle Size
– Larger particles take longer to dissolve
Are Solutions Always Liquids?
No!
–Solutions can also
be gases dissolved in liquids, such
as carbonated water or pop!
Can You Dissolve More Solute in
Warm or Cool Water?
• The cold water can’t dissolve as much as the hot
water
• When the solution can no longer dissolve the solute
it becomes a 'saturated solution', this means that the
solute starts forming on the bottom of the container
• The reason the hot water dissolves more is because
it has faster moving molecules which are spread
further apart than the molecules in the cold water.
With bigger gaps between the molecules in the hot
water, more solute molecules can fit in between.
Matter Changes by Adding or
Removing Energy(aka heat)
Matter can NEVER be created or
destroyed…it will change forms though!
Law of Conservation of Mass
• States that matter can be changed from one form
into another, but the total amount of mass
remains constant