Organizing matter by its physical and chemical
properties.
What is “Matter”
 Anything that has mass and volume
It weighs something!
It takes up space!
So almost everything is matter!!!
What things are NOT matter?
 Thoughts, ideas, emotions, songs, energy
 Just about everything else is matter
How Matter is Classified…
 Memorize the diagram on the next slide
 Know the definitions of each term
 Know 3 examples of each class of matter
MATTER
Mixtures
Homogeneous
Mixture
Pure Substances
Heterogeneous
Mixture
Elements
Compounds
**The dashed boxes are the 4 classes of matter**
Types of Properties
 Physical- characteristics that can be observed or
measured without changing the identity of a
substance
 Ex. melting point, boiling pt
 Chemical- relates to a substances ability to undergo
changes that transform it into a different substance
 Easiest to see when a chemical is reacting
Types of Properties
Physical Changes in Matter
 change in a substance that doesn’t change the
identity of the substance
 Ex. grinding, cutting, melting, boiling
 Includes all changes of state (physical changes of a
substance from one state to another)
Solid
definite volume
 definite shape
 atoms are packed
together in fixed
positions
 strong attractive forces
between atoms
 only vibrate in place

Liquid




definite volume
indefinite shape
atoms are close
together
atoms can overcome
attractive forces to
flow
Gases
indefinite volume
 indefinite shape
 atoms move very
quickly
 atoms are far apart
 pretty weak attractive
forces

Plasma
 high temperature state in which atoms lose their
electrons
 Ex. the sun
Energy Increasing
Changes of State
Sublimation
Melting/Fusion
Freezing/Solidification
Vaporization
Condensation
Deposition
Energy Decreasing
Chemical Changes in Matter
 a change in which a substance is converted into a
different substance
 same as chemical reaction
 doesn’t change the amount of matter present
 reactants- substances that react
 products- substances that form
Energy Changes in Matter
 when any change occurs, energy is
always involved
 energy can be in different forms (light,
heat, etc.)
 energy is never destroyed or created
(law of conservation of energy)
Energy Changes in Matter
 Exothermic Reaction- reaction
that gives off energy (feels warm
on outside)

http://www.youtube.com/watch?v=rdCsbZf1_Ng&feature=related
 Endothermic Reaction-
reaction that uses up energy
(feels cold on outside)
Pure Substances vs. Mixtures
 Pure substances can NOT be separated into simpler
components by “physical” means
 Mixtures are easily separated into its component parts
by “physical” means
Pure Substances
 Contain only one thing. It can’t be
broken down into anything else
 There are 2 kinds of pure substances
 Elements
 Compounds
Elements
OMG…We
learned some of
these already!!
 Simplest form of matter
 About 115 elements exist
 Can’t be broken down into anything else
 smallest piece of an element is called an atom
 Examples:
 Carbon, nitrogen, oxygen
Elements
 Organized by properties on periodic table
 Each square shows the name and letter symbol for
each element
 Usually the symbols relate to the English names but
some come from older names (usually Latin)
 Ex: gold’s symbol is Au from aurum
 Ex: iron’s symbol is Fe from ferrum
Periodic Table
Periodic Table
 Two rows below the periodic table are the
lanthanide and actinide series
 These rows fit after #57 and #89
 They are only at the bottom to keep the width of
the chart smaller
Periodic Table
 Groups
 also called families
 vertical columns
 numbered 118
 have similar chemical properties
 Periods
 horizontal rows
 properties changes consistently across a period
Types of Elements
 Metals
 Good conductor of electricity
 At room temperature, most are




solids
Malleable- can be rolled or
hammered into sheets
Ductile- can be made into wire
High tensile strength- can resist
breakage when pulled
Most have silvery or grayish
white luster
Types of Elements
 Nonmetals
 Poor conductor of heat and electricity
 Many are gases at room temperature
 Some are solids: usually brittle, not malleable
Types of Elements
 Metalloids
 Has some characteristics of metals and nonmetals
 Appear along staircase line
 B, Si, Ge, As, Sb, Te
 All are solids at room temperature
 Less malleable than metals but less brittle than
nonmetals
 Are semiconductors
Types of Elements
 Noble Gases
 Generally unreactive gases
 Far right column of periodic table
Compounds
 2 or more elements are chemically “bonded” so it acts
like it is just one thing so we still classify it as a pure
substance
 Examples:
 Carbon dioxide (CO2)
 Sodium chloride (NaCl)
Mixtures
 2 or more substances put together in random
proportions
 Substances that make up the mixture do not “react” or
“bond” with each other
 2 kinds of mixtures
 Heterogeneous mixtures
 Homogeneous mixtures
Heterogeneous Mixture
 Can see the different parts
 Examples:



Italian salad dressing
Lucky Charms cereal
Concrete
Homogeneous Mixture
 Can’t see the different parts…it all looks like one thing
 Also called a “solution”
 Examples:
 Milk
 Tap water
 Air
What are “physical” means of
separation????
 Ways of separating things without doing a chemical
reaction!
Methods of Physical Separation
 Distillation
 Filtration
 Crystallization/Precipitation
 Chromatography
 Centrifugation
Separation Techniques
 Distillation – add heat
and the component with
the lowest boiling point
turns into a gas and leaves
the mixture
Separation Techniques
 Filtration- solid part is
trapped by filter paper and
the liquid part runs through
the paper
 Vaporization- where the
liquid portion is evaporated
off to leave solid
Separation Techniques
 Crystallization/Precipitation – cool mixture down or
react it with something so that a solid forms that can then
be filtered out or let it settle to bottom
Separation Techniques
 Decanting- when liquid is
poured off after solid has
settled to bottom
 Centrifuge- machine that
spins a sample very quickly
so that components with
different densities will
separate
Separation Techniques
 Chromatography – add
mixture to absorbing
media; the smaller
components will be
“absorbed” quicker and
will start to move away
from the larger particles
Separation Techniques
 Paper Chromatography-
used to separate mixtures
because different parts
move quicker on paper
than other
Separation Techniques
 Thin Layer Chromatography
Separation Techniques
 Column chromatography
Separation Techniques
 Gas Chromatography
Separation Techniques
 High Pressure Liquid Chromatography
Separation Techniques
 Gel Electrophoresis