MATTER
Physical and Chemical Properties of Matter
Vocabulary
1/21 – Matter
1/22 – volume
1/23 – plasma
1/26 – Boseeinstein
condensate
1/28 – density
1/29 – Regular
solid
1/30 – Irregular
solid
2/2 – Archimedes
principle
I can …….
1/21 – Explain the difference between ice
and water.
1/22 – Explain the difference between
mass and volume.
1/23 – Contrast a liquid and a solid
1/26 – Name the states of matter in order
of increasing energy!
1/28 – Name the 2 types of properties
1/29 – Calculate the volume of a regular
solid(unit?)
1/30 – Calculate the volume of an
irregular solid.
2/2 – Calculate the density of an object
WHAT DO YOU OBSERVE IN THE PICTURE
WHAT IS MATTER?
Anything that has mass and takes up space
(volume).
Examples of matter:
LAW OF CONSERVATION OF
MATTER
 MATTER
CANNOT BE CREATED
OR DESTROYED IT JUST
CHANGES FROM ONE FORM TO
ANOTHER.
(MATTER GETS RECYCLED)
THEORY OF KINETIC ENERGY
1. ATOMS ARE ALWAYS MOVING
2. THE MORE ENERGY ADDED TO
THE ATOMS, THE FASTER &
FARTHER APART THEY MOVE
ENERGY
ADDED
ENERGY
ADDED
MATTER
 Matter
can be described by using physical
and chemical properties. These are
characteristics the matter has that make
it unique.
 Physical
Properties: Are properties that
can be observed or measured. (color, mass,
length, volume, density, state, etc).
 Physical
Properties can be either:
 Observable or Measurable
OBSERVABLE PHYSICAL PROPERTIES
 Observable
Physical Properties:
Properties you can use your senses
to get information about an object.
 If you can describe the matter based
on what it looks, feels, smells or
tastes like, you are describing the
physical properties.
EXAMPLES OF OBSERVABLE PHYSICAL
PROPERTIES

State of Matter: Matter can either be a solid,
liquid, gas, or plasma. We observe this by using
our senses.
STATES OF MATTER
State of matter is a physical property!!!!
 MATTER
CAN BE FOUND IN 4 STATES
(PHASES)
 SOLID
 LIQUID
 GAS
 PLASMA
http://www.harcourtschool.com/activity/states_of_matter/
PARTICLES of a SOLID (Physical Property)
Pattern: ATOMS (PARTICLES) ARE ARRANGED
CLOSELY PACKED TOGETHER
Movement: VIBRATE
Shape/Volume: HAS FIXED SHAPE & FIXED
VOLUME
Examples – ice, rock, book

In Solids, the particles are very tightly
packed SO:
–THE OBJECT IS HARDER
– THE MORE DIFFICULT IT IS TO
BREAK THEM APART
– THE MORE ENERGY NEEDED TO
CHANGE FROM A SOLID TO A
LIQUID
The particles in a LIQUID:
Pattern: none
Movement: atoms roll or slide over each other and
move faster than a solid.
Shape: No fixed shape, takes shape of container
Volume: Fixed
Examples: water, milk, soda


The particles in a GAS:
Pattern: none
Movement:
PARTICLES MOVE
VERY FAST & AS
FAR APART AS
THEY CAN GET
Shape: NO FIXED
SHAPE, takes shape
of container
Volume: No fixed
volume
Examples – oxygen,
helium
WE ALL KNOW ABOUT:
SOLIDS
Lower
Temperatur
e
LIQUIDS
GASES
Higher
Temperatur
e
Two states of matter they didn’t teach
you about in school…
Until Now!
PLASMA
Bose-Einstein
Condensate
But what happens if you raise the
temperature to super-high levels…
between
1000°C and 1,000,000,000°C ?
Will everything
just be a gas?
NO!
If the gas is made up of particles which carry an
electric charge (“ionized particles”), but the
entire gas as a whole has no electric charge,
and if the density is not too high, then we can
get
The 4th state of matter:
PLASMA
 The
particles in PLASMA:
Pattern: none
Movement: Particles move very fast and
are therefore very HOT
Shape/Volume: NO FIXED SHAPE OR
VOLUME
Facts: Most common state of matter in
the universe.
Most Uncommon state of matter on
Earth.
Found in lightning, fluorescent lights
and stars (Sun)
Some places where plasmas are found…
1. Flames
2. Lightning
3. Aurora (Northern Lights)
4. Neon lights
5. Stars
Stars make up 99% of the total matter in the Universe.
Therefore, 99% of everything that exists in the entire
Universe is in the plasma state.
The Sun is an example of a star in its
plasma state
6. Clouds of gas and dust around stars
6
SO NOW WE KNOW ALL ABOUT
FOUR STATES OF MATTER:
SOLIDS
Lower
Temperatur
e
LIQUIDS
GASES
PLASMAS
(only for low density
ionized gases)
Higher
Temperatur
e
But now what happens if you lower the
temperature way, way, down to
100 nano degrees above
“Absolute Zero” (-273°C)
Will everything
just be a frozen
solid?
NOT NECESSARILY!
In 1924 (82 years ago), two scientists, Albert
Einstein and Satyendra Bose predicted a 5th
state of matter which would occur at very
very low temperatures.
Einstein
Bose
+
Finally, in 1995 (only 11
years ago!), Wolfgang
Ketterle and his team of
graduate students (like me)
discovered the 5th state of
matter for the first time.
Ketterle and his
students
The 5th state of matter:
Bose-Einstein Condensate
IN A BOSE-EINSTEIN CONDENSATE, ATOMS CAN NO
LONGER BOUNCE AROUND AS INDIVIDUALS.
INSTEAD THEY MUST ALL ACT IN EXACTLY THE SAME
WAY, AND YOU CAN NO LONGER TELL THEM APART!
Here is a picture a computer took of
Bose-Einstein Condensation
The big peak happens
when all the atoms
act exactly the same
way!
(We can’t see
Bose-Einstein
condensation
with our eyes
because the
atoms are too
small)
Some other computer images of Bose-Einstein Condensates…
BOSE EINSTEIN CONDENSATES
Pattern: ATOMS (PARTICLES) ARE
ARRANGED IN A PATTERN
Movement: NONE
Shape/Volume: HAS FIXED SHAPE & FIXED
VOLUME
 When temperatures get that low, you can create
a BEC with a few special elements. Cornell and
Weiman did it with rubidium (Rb).


The whole process happens at temperatures
within a few billionths of a degree, so you won't
see this at home. When the temperature becomes
that low, the atomic parts can't move at all. They
lose almost all of their energy.
Since there is no more energy to transfer (as in
solids or liquids), all of the atoms have exactly
the same levels, like twins. The result of this
clumping is the BEC. The group of rubidium
atoms sits in the same place, creating a "super
atom." There are no longer thousands of
separate atoms. They all take on the same
qualities and, for our purposes, become one blob.
EXAMPLES OF BOSE EINSTEIN
CONDENSATES
Two examples of Bose-Einstein condensates
include superfluids, such as cold liquid
helium, or superconductors, such as the
nucleons inside a neutron star. Bose-Einstein
condensates are another state of matter, similar to
solids but with less energy. They were not directly
observed until the 1990s, even though Einstein
predicted their existence in the 1920s.
TO REALLY UNDERSTAND
BOSE-EINSTEIN CONDENSATE
YOU NEED TO KNOW
Quantum Physics
In 2002, Ketterle and two other scientists
received the highest award in science for
discovering Bose-Einstein condensate:
The Nobel Prize
THE FIVE STATES OF MATTER:
BOSEEINSTEIN
SOLIDS
CONDENSATE
Lower
Temperatur
e
PLASMAS
LIQUIDS
GASES
(only for low
density ionized
gases)
Higher
Temperatur
e
OTHER OBSERVABLE
PHYSICAL PROPERTIES
EXAMPLES OF OBSERVABLE PHYSICAL
PROPERTIES


Color: The color of object can be seen and is a
physical property of matter.
Color can help identify a substance. For
example, sulfur is usually yellow in color, iodine
is usually red in color.
Sulfur
Iodine
EXAMPLES OF OBSERVABLE PHYSICAL
PROPERTIES
Smell: The smell or odor an object gives off can
also help identify a substance.
 For example, sulfur has a rotten egg smell,
vinegar has a very acidic smell, and chlorine has
a very strong bleach smell.

EXAMPLES OF OBSERVABLE PHYSICAL
PROPERTIES
 Malleability:
the ability of a substance to
be pounded into thin sheets.
EXAMPLES OF OBSERVABLE PHYSICAL
PROPERTIES
Conduction of heat or electricity: The ability for
heat and electricity to pass through an object
easily.
 Metals are usually the best conductors of heat
and electricity.

EXAMPLES OF OBSERVABLE PHYSICAL
PROPERTIES
Insulator of electricity or heat: when an object
passes heat and electricity poorly.
 Nonmetals are usually good insulators.

EXAMPLES OF OBSERVABLE PHYSICAL
PROPERTIES
Ductility: the ability to be drawn or pulled into a
wire.
 Metals usually are ductile.

EXAMPLES OF OBSERVABLE PHYSICAL
PROPERTIES
Solubility: The ability to dissolve in a nother
substance.
 Examples: sugar dissolves in water.

PHYSICAL PROPERTIES - EXAMPLES















Color
Hardness
Odor
Taste
State of matter
Texture
Luster (shine)
Flexibility
Heat conductivity
Electrical conductivity
Solubility (ability to dissolve in water.)
Shape
Viscosity
Ductility
Malleability
PHYSICAL PROPERTIES - EXAMPLES

Examples of physical
properties include:
Density
 Melting point
 Boiling point

PROPERTIES OF MATTER
Matter can be described by using physical
and chemical properties. These are
characteristics the matter has that make it
unique.
 Physical
Properties: Are properties that
can be observed or measured. (color, mass,
length, volume, density, state, etc).
 NAME
2 OBJECTS!!!!!
MEASURABLE PROPERTIES OF MATTER

Measurabe Properties: Properties that must be
measured with a tool (ruler, beaker, graduated
cylinder, scale, etc.).
Ruler
Beaker
Scale
Graduated Cylinder
Triple Beam Balance
MEASURABLE PROPERTIES OF MATTER
 Mass:
is the amount of atoms contained
in a substance.
 Calculate: Using a triple beam balance
or a scale.
 Unit: in science ALWAYS use grams (g)
or kilograms (kg).
MEASURABLE PROPERTIES OF MATTER

Weight: is the amount gravity is pulling on an
object. Different on the MOON!!! Other wise it is
measured the same as MASS!!
MEASURABLE PROPERTIES OF MATTER





Volume: the amount of space an object takes up.
Measured by: different for regular solid, irregular solid
and liquids.
Examples of Regular Solids: any solid you can measure
the length, width and height of.
Examples of Irregular Solids: any solid you cannot
measure the length, width and height of.
Examples of Liquids: any object that has no definite
shape but does have a definite volume.
Measurable Properties of Matter
Measuring the Volume of Liquids:
How to calculate: Use a graduate cylinder to find the volume
at the meniscus.
Material: graduated cylinder, beaker, flask
How to read a graduated cylinder
 Must be at eye level to read.


Must read to bottom of the curve. MENISCUS - bottom of
the curve.
Unit: mL or L
MEASURABLE PROPERTIES OF MATTER

Measuring Volume of Regular Solids: measure
the length, width and height with ruler and multiply
them together.
Length X Width X Height = Volume of Regular Solid

cm X cm X cm = cm3
 *ALWAYS USE CENTIMETERS IN SCIENCE!!!!


UNIT: cm3
MEASURABLE PROPERTIES OF MATTER
Measuring Volume of Irregular Solids: Water
displacement. Put water into a graduated cylinder
and record volume. Place irregular solid into
cylinder with water and record second volume.
Subtract the two amounts.
 Initial volume (water only) – volume with irregular
solid = volume of solid
 UNIT: measured in mL but, since it is a
solid use cm3.
1 mL = 1 cm3

MEASURABLE PROPERTIES OF MATTER

Density: the amount of matter in a given space or
volume. Density is used to describe matter
because everything has a different density.
MEASURABLE PROPERTIES OF MATTER
Measure by: dividing and objects mass by it’s
volume.
 Calculate: Density = Mass/Volume

m
D = ------V

m
D
V
Mass divided by Volume
UNIT: since mass is measured in grams and
volume is measured in cm3 or mL the unit for
density has to have those two units.
 So, the unit for density is g/mL or g/cm3.

BELLRINGER
Calculate the density for the following
objects:
2g/ml sinker
a.Mass= 10 Volume= 5
2g/cm sinker
b.Mass= 16 Volume= 8
c.Mass= 5 Volume= 10 0.5g/ml floater
d.Mass= 12 Volume= 12 1g/cm water
3
3
Which object is water? Which object will
float in water? Which objects will sink in
water?
WHICH IS GOLD?
HOW WOULD YOU KNOW?
WHO WAS ARCHIMEDES????

VIDEO!!!!!
Archimedes Principle –
measuring density with water
displacement
The
density of water is
ALWAYS 1.0 g/mL.
Anything less than 1.0 g/mL
will FLOAT.
Anything greater than 1.0
g/mL will sink.
These are two, unopened full
cans of soda. Explain why one is
floating and one has sunk.
Why are some objects less dense than other
objects?
As the molecules of a substance spread apart,
the density of the substance is lowered.
What causes molecules to spread?
Adding energy so the movement of the molecules
increases.
Objects float in other substances because
they are less dense than the substance they
are floating in.
Why does ice float in water? They are
both the same substance, right?
Notice how tightly packed the atoms are in the
liquid water vs the solid water?
The spaces between the atoms make solid water less dense.
Is this true for all solids?
NO WAY!!! This is a unique quality of water. Most solids are always
more dense than their liquid forms.
Why does this happen?
Hot air
balloon rises
Atmosphere
changes as you
climb a mountain
Basketball goes
flat in winter
Perfume can be
smelled all over the
room
DENSITY
When does an objects density change?
If heat is added or taken away!!!!
HEAT – spreads out molecules – LESS
dense
Take AWAY heat – molecules come
together – MORE dense.
Hot objects are less dense than cool
objects!!!!
CHEMICAL PROPERTIES OF MATTER
Chemical Properties- Properties that determine
whether or not a substance will react chemically.
 Flammability: the ability to burn.


Reactivity: The ability for a substance to react
with another. Simply, when two substances get
together, something can happen.
CHEMICAL PROPERTIES - EXAMPLES

Examples of chemical
properties include:







The ability to burn
Ability to tarnish
Ability to rust
Ability to decompose
Ability to react with other
chemicals
Instability
Ability to do acid/base
reactions
CHEMICAL PROPERTIES

List as many chemical
properties as you can for
this item.
Chemical and physical properties – So what?
Titanium is very strong
and doesn’t rust, so it is
often used in jet engines.
 Titanium is also
nonallergenic. This,
combined with the fact
that it is rust proof makes
it great for artificial joints
as well as piercings.

Chemical and physical properties – So what?
Tungsten is usually used
as the filament in
lightbulbs because it has
the highest melting point
of any metal.
 It glows red hot when
electricity runs through
it, and it gives off both
heat and light.

Chemical and physical properties – So what?

Vanadium is heavier and
harder than titanium, so
mixing a tiny bit of
vanadium with steel can
make cheap tools that
are still very strong.
Chemical and physical properties – So what?
Helium is almost
completely nonreactive
(inert).
 It is lighter than air, so
it’s great for floating
balloons (or making
funny voices.)
 When electricity runs
through helium, it glows
a creamy pale peach
color.

Chemical and physical properties – So what?

In 1943, all US pennies
were made of zinc plated
steel because copper was
being used in the war.
The pennies had to be
coated with zinc because
steel will rust, but zinc
won’t.
Chemical and physical properties – So what?
Sulfur smells awful.
Rotten eggs, onions, and
garlic all have sulfur in
them. Stink bombs use
sulfur to create a bad
smell.
 Sulfur is also flammable,
and it is one of the 3
main ingredients in gun
powder.

Chemical and physical properties – So what?

Chromium is famous for
its intense luster.
Chrome plated tools,
jewlery, silverware, or car
parts are very popular.
Chemical and physical properties – So what?

Most bullets are made of
lead because lead is a
very dense metal. These
bullets are required, by
international law, to be
coated with a different
metal because lead has
such a low melting point
and is so malleable.
Chemical and physical properties – So what?

The most dense elements
are Iridium and osmium
which have a density of
about 22.6 g/cm3
Physical and Chemical
Changes
7th Grade Science
Physical Changes
Matter is always changing form, size, shape,
color, etc. There are 2 types of changes
that matter undergoes.
PHYSICAL OR CHEMICAL CHANGE
I. Physical Changes: a change of matter
without changing the identity of the
substance. IN OTHER WORDS




A CHANGE IN STATE
A CHANGE IN SIZE, SHAPE, MASS
DOES NOT CHANGE THE CHEMICAL MAKE UP OF
THE MATTER
YOU HAVE WHAT YOU STARTED WITH, JUST IN A
DIFFERENT FORM
Examples of Physical Changes
-
Verbs used to describe physical changes –
grind, dissolve, erode, rip, tear, break, phase
change (melt, freeze, condense, etc)
Other Physical Change Examples
PAPER
TORN INTO PIECES
 SUGAR
DISSOLVED INTO TEA
 SALT DISSOLVED INTO WATER
 NAILS OR HAIR CUT
Chemical Changes
The other way that matter can be changed is
call a CHEMICAL CHANGE.
II.
CHEMICAL CHANGE –
occurs when 2 or more
substances are combined
into entirely new
substance with all new
properties. CANNOT
CHANGE IT BACK!!!!!
Chemical Change Verbs

Chemical Change Verbs: rusting, rotting,
curdling, burning, cooking, light sensitivity,
digesting, tarnishing.
Kinetic Theory of Matter
THEORY OF KINETIC
ENERGY
A. ATOMS ARE ALWAYS
MOVING
B. THE MORE ENERGY
ADDED TO THE ATOMS,
THE FASTER & FARTHER
APART THEY MOVE


WHEN MOLECULES MOVE FASTER, THEY
PRODUCE MORE FRICTION AND THEREFORE
MORE HEAT. THEY SPREAD FARTHER APART
& EXPAND
WHEN MOLECULES MOVE SLOWER, THEY
CAUSE LESS FRICTION AND THEREFORE
LESS HEAT & CLOSER TOGETHER &
CONTRACT

MATTER CHANGES FROM ONE STATE OF
MATTER TO ANOTHER
 WHEN
HEAT (ENERGY) IS ADDED
 WHEN HEAT (ENERGY IS TAKEN
AWAY
CHANGING STATES DOES NOT CHANGE
THE CHEMICAL MAKE UP OF THE
MATTER
 YOU HAVE WHAT YOU STARTED WITH
JUST IN A DIFFERENT FORM
 ICE 
WATER  WATER VAPOR


H 2O
H 2O
H 2O
Phase Changes are PHYSICAL
PHYSICAL!!!!!
 Types
of Phase Changes:
 1. Melting
 2. Freezing
 3. Evaporation
 4. Boiling
 5. Condensation
 6. Sublimation
 7. Deposition
 ALL phase changes are caused by
ADDING or TAKING away energy!!!
Melting
1. MELTING – matter changing FROM A
SOLID TO A LIQUID.
Energy is added
 When more heat (energy) is added to matter the
particles move faster till the bonds break.
 Decrease density except ice to water.

Evaporation/Vaporization
2. EVAPORATION
Matter changing FROM A LIQUID TO A GAS AT
THE SURFACE
 ENERGY IS ADDED TO SURFACE OF LIQUID
 THE PARTICLES AT THE SURFACE MOVE FASTER
breaking bonds.
 Decreases density.

 VAPORIZATION-
a
general term for any
substance changing to
a gas.
Boiling
3. BOILING






matter changing FROM A LIQUID TO A GAS
ALL THROUGHOUT THE LIQUID
ENERGY IS ADDED TO ALL OF LIQUID
PARTICLES MOVE FASTER ALL THROUGH THE
LIQUID
SOME PARTICLES MOVE FAST ENOUGH TO
CHANGE TO GAS WHILE THEY ARE IN THE
MIDDLE OF THE LIQUID
DENSITY DESCREASES
Water boils at 212 F, 100C.
 EX:
pan of liquid on the stove
 VAPORIZATION- a general term
for any substance changing to a gas.
VAPORIZATION!!!


Remember that vaporization is a general
word for any substance changing to a gas.
Boiling, evaporation, and sublimation are ALL
examples of vaporization!!!
Condensation
4. CONDENSATION
 Matter CHANGING FROM A GAS TO A LIQUID
 ENERGY IS REMOVED




THE PARTICLES MOVE SLOWER
THE ATTRACTION BETWEEN THE PARTICLES BEGAN
TO PULL THE PARTICLES CLOSER TOGETHER & THE
MATTER TURNS INTO A LIQUID
DENSTITY INCREASES
Ex: dew in the lawn, water running down mirror, ring on table
under glass.
Freezing
5) FREEZING


CHANGING FROM A LIQUID TO A SOLID
ENERGY IS REMOVED
THE PARTICLES MOVE EVEN SLOWER
 THE ATTRACTION BETWEEN THE PARTICLES BEGAN TO PULL
THE PARTICLES CLOSER TOGETHER & THE MATTER TURNS
INTO A SOLID
 Increase density.

Water
freezes at 32 F, 0 C
EX: water to ice, wax or chocolate hardening
SOLIDIFICATION!!!!


Solidification is a general word for any
substance changing to a solid.
Freezing and deposition are examples of
SOLIDIFICATION!
Sublimation
6) Sublimation: matter changes straight
from a solid to a gas!!!!
Heat added rapidly
Molecules speed up and spread out rapidly
decrease density
Examples
of Sublimation:
dry ice, shrinking ice in a
freezer, air freshener.
Deposition
7) Deposition- when matter changes from a gas
directly to a solid.
-Heat is taken away rapidly
-Density increases
-Molecules slow down and get closer
together.
Examples:
Snowflakes,
frost on a wind shield

WHAT HAS TO HAPPEN FOR THESE
CHANGES OF STATES TO OCCUR?
DRAW THIS DIAGRAM IN YOUR
NOTES!!!!
Let’s Sing!!!!
Phase changes are physical, physical…
 Melting is physical…. Freezing is physical.
 BOYS: Let me see some condensation.
 GIRLS: (in high pitch voice) It’s physical.
 BOYS: Let me see some sublimation.
 GIRLS: (in high pitch voice) It’s physical.
 Phase changes are physical, physical…
 Boiling is physical… Boiling is physical…
 BOYS: Let me see some deposition.
 GIRLS: (in high pitch voice) It’s physical
 BOYS: Let me see some evaporation.
 GIRLS: (in high pitch voice) It’s physical

Chemical Changes
The other way that matter can be changed is
call a CHEMICAL CHANGE.
II.
CHEMICAL CHANGE –
occurs when 2 or more
substances are combined
into entirely new
substance with all new
properties. CANNOT
CHANGE IT BACK!!!!!
Chemical Change Verbs

Chemical Change Verbs: rusting, rotting,
curdling, burning, cooking, light sensitivity,
digesting, tarnishing.
Chemical Changes

SOME SIGNS OF A CHEMICAL CHANGE
 FIZZES OR BUBBLES
 COLOR CHANGE
 HEAT GIVEN OFF
 LIGHT GIVEN OFF
 ODOR
 HEAT REQUIRED FOR REACTION
 NEW SUBSTANCE FORMED
Precipitate (solid)
 Precipitate (gas bubbles)


CHEMICAL CHANGE EXAMPLES
 BAKING
BREAD – NO
LONGER HAVE FLOUR, EGGS,
MILK, YEAST
 ALKASELTER
 BAKING SODA & VINEGAR
 RUST
 TARNISH