Introduction to Matter Unit
2, Cooking
(Chemistry)
EQ: What is Matter and How
Can it’s Properties be
Described?
 Helpful hints: Go online for crossword
puzzles and vocabulary flash cards:
phschool.com web code: crj-0002
 Helpful hint: Study you vocabulary
warm-up notes, or go online to my website
for the daily warm-up words regarding
matter.
 Helpful hint: If you like the videos I’ve been
showing, they can be found at
Stevespanglerscience.com
I Describing Matter
 Matter is anything that has mass and takes up
space.
 Properties of Matter
 The properties and changes of any type of
matter depend on its makeup.
 A substance is a single kind of matter that is
PURE it always has a specific composition
and a specific set of properties.

Table salt and sugar are examples. If you have a
salt shaker at home, all you have in it is salt and
nothing else—if you look into a bag of sugar, all
you have in that bag is sugar and nothing else.

These are NOT substances: Flour, baking
powder, milk, eggs, fruit.
Every form of matter has two kinds of PROPERTIES……
 Physical
 Characteristic of a pure
substance that can be
observed without changing
it into another substance.
 Examples: water freezing
into ice; hardness, texture,
color, solid, liquid, gas,
solubility (ability to dissolve)
in water , the luster
(shininess or dullness of a
metal), ability to conduct
heat/electricity, magnetic
properties, ductility (a
metal’s ability to be shaped
into useful things like wire
or tools); a physical property
of oxygen is that it is a gas at
room temperature.
 Chemical
 A characteristic of a pure
substance that describes its ability
to change into different
substances.
 Can’t be observed just by looking
at or touching a substance. To
observe chemical properties, you
must try to chnge it into another
substance.
 Examples: A chemical property of
methane (natural gas), is that it
can catch fire and burn in air.
When it burns, it combines with
oxygen in the air and forms new
substances, water and carbon
dioxide. Burning, or flammability,
is a chemical property of methane
as well as the substances in wood
or gasoline.
 More examples: A chemical
property of oxygen is that it
combines with iron to form rust.
Silver or brass reacts with sulfur in
the air to form tarnish. A
chemical property of gold is that it
does not
react easily with oxygen or sulfur.
Yeast added to bread dough causes
gas pockets in the bread;
therefore, bread rises.
Elements
Go Online to: Scilinks.org Code: scn-1111
 A pure substance that cannot be broken down into any
other substances by chemical or physical means.
Elements are the Simplest Substances. The building
blocks more complex forms of matter.
 Found on the Periodic Table (which can be found in the
back of your Agenda, on the Internet, in your
textbook, or on my wall).
 Can be identified by its specific physical and chemical
properties.
 Examples are: Aluminum (soda cans, foil, outdoor
furniture); Pennies are made from zinc, another
element, and a coating of copper. Oxygen and
Nitrogen (in the air you breathe)
 Often represented by one or two letter symbols,
such as C for carbon, and O for oxygen, and H for
hydrogen.
Elements: Atoms
 The basic particle from which all elements are made.
 Different elements (found on the periodic table only), have
different properties because their atoms are different.
 Atoms are modeled, or drawn in different ways. Below is a
picture from your book of a spherical model (the drawing with
the pencil), and the cloud model—the one with what looks like a
group of purple and blue gumballs. The cloud model shows a
drawing of the nucleus of an atom, and it’s electron cloud. We’ll
dig into this more when we get into our studies of the periodic
table.
 Atoms of most elements have the ability to combine with other
atoms. When they combine, they form a chemical bond, which is
a force of attraction between two atoms, and the product, in
many cases, forms a molecule.
Elements: Molecules
 Groups of two or more atoms held together
by chemical bonds. A molecule of water, for
example, consists of an oxygen atom
chemically bonded with two hydrogen
atoms. Two atoms of the same elements can
also combine to form a molecule. Oxygen
molecules consist of two oxygen atoms. The
picture below shows three models of
molecules.
Math in Science: Ratios
 A ratio compares two numbers. It tells you how
much you have of one item compared to how
much you have of another. For example, a
cookie recipe calls for 2 cups of flour for every
one cup of sugar. You can write the ration of
flour to sugar 2:1, or 2 to 1.
 The chemical formula for rust, a compound
made from the elements of iron (Fe), and
Oxygen (0), may be written as Fe2O3 . In this
compound, the ratio of iron atoms to oxygen
atoms is: 2:3; or 2 to 3. This compound is
different from FeO, a compound in which
the ration of iron atoms to oxygen atoms is
1:1.
 Got it? What is the ratio of nitrogen atoms
(N) to Oxygen (O) atoms in a compound
with the formula N2O5? Is it the same as the
compound NO2? Highlight Here, 2:5, to
find the answer.
Describing Matter
Compound
V.
Mixture
 Two or more substances,
 Pure substance made of two or
more elements chemically
combined in a set ratio.

When elements are chemically combined,
they form compounds having properties that
are different from those of the uncombined
elements.
Example: sulfur (AG) is a yellow solid and
silver (S) is a shiny metal. When silver and
sulfur combine, they form a compund called
silver sulfide (tarnish) (AG2S).
Table sugar (C12H22O11) is a compund
made of the elements carbon, hydrogen and
oxygen. The sweet sugar crystals do not
resemble their parent elements, Carbon
(looks like charcoal), Hydrogen (a gas), and
Oxygen (a gas).

May be represented by a chemical formula
which shows the elements in the compound
and the ratio of atoms.

Example: part of the gas you exhale is
carbon dioxide, chemical formula CO2.
There is one carbon atom, and there are two
oxygen atoms. When a symbol stands alone,
and does not show the number of atoms next
to it, like oxygen does in the formula, the
element will have one atom. The one atom in
carbon is inferred—just like a variable that
stands alone in algebra has a ‘hidden’ one in
front of it, an element that stands alone has
one ‘hidden’ atom. What is the ratio of atoms
in CO? Highlight after the colon to check
your answer: 1:1
elements, compunds or both—
that are together in the same
place but are not chemically
combined.
 Each keeps its individual
properties, and the parts of
a mixture are not in a
combined ratio.
 Examples: soil, cereal and milk,
salad.
 Each part of the mixture can be
separated; with methods like
filtration, magnetic attraction,
distillation, evaporation and
mechanical means. Compounds
cannot be separated—they’ve
been chemically combined.
 Two types of mixtures:
 Homogeneous – you can’t see
the different parts. Examples are
sugar in water (solution), bubbles
in water.
 Heterogeneous – you can see the
different parts. Examples are
salad, cereal in milk, chocolate
chip cookie dough
Measuring Matter
Weight
Mass
 Which weighs more, a  The measurement of the
amount of matter in the
pound of feathers or a
object. Mass does not
change with location, even
pound of sand?
when the force of gravity
Highlight here: They
changes. The mass of an ice
cream sandwich on the
are both the same
moon is the same as the
weight
mass of an ice cream
sandwich on earth.
 Weight is a measure of
 In science, we do not
the force of gravity on measure weight –we
measure mass.
an object (or you).!
 The units we most
commonly used in our
science work are: Kilograms
(kg), and grams (g). There
are 1,000 grams in a
kilogram. A nickel has a
mass of 5 grams, and a
baseball has a mass of 150
grams. A paper clip is about
1 gram.
Measuring Matter
Volume
 The amount of space that
matter occupies
 Units:
 Liquids: liter (L), milliliter
(ml), is 1/1000th of a liter
 Solids: cubic centimeter
(cm³)
 cm x cm x cm = cm³
 1ml = 1cm³
Volume of a solid is calculated
by multiplying the length x
width x height (l x w x h).
Measuring an irregular
object, like a piece of fruit
or rock, can be done by
submerging the object in a
graduated cylinder with
water. The water level will
rise by an amount that is
equal to the volume of the
object in milliliters (ml).
Density
 The mass of a material
in a given volume.
 Which has more
density, a cubic meter
of concrete, or a cubic
meter of feathers? Of
course, the concrete is
more dense. We have
the same volume, but
the concrete is much
heavier than the
feathers.
 Density formula:
 Density=Mass divided
by volume; or:
 D=m/v
Measuring Matter Density
(continued) Remember the
Sample Problem

A small block of wood floats on
water. It has a mass of 200 g and
a volume of 250cm³. What is the
density of the wood? Calculate
the density.

Does your answer make sense?
The density is lower than
1.0g/cm³, which makes sense
because the block can float.
Remember, the density of water is
1.0g/cm³, and the block of wood
is lighter than this.

Highlight the bullet point and
further below to see solution
 200g (mass)/250cm³
(volume) = 0.8
0 g/cm³
demonstrations I
did with common
kitchen ingredients?
 On one of them, we did
what is in the picture
below. The least dense
liquid rose to the top,
and the most dense
stayed on the bottom.
 .
Changes in Matter
Physical Change
 Any change that alters the
form or appearance of
matter but does not
make any substance
in matter into a
different substance.
 Physical changes include
a change of state, or
change of shape or form.
 Examples: crushing of
aluminum Coke cans,
mixing sugar in water, an
ice cube melting, or
water vaporizing
Chemical Change
 A change in matter that produces one
or more new substances with
properties different from those of the
original substances.
 Reactions are always happens when
chemical changes are involved.
 Examples:
Iron in metal combines with oxygen in
the air to produce rust (FeO). When
methane (CH4) burns, it makes contact
with oxygen (O) molecules in the air,
and produces carbon dioxide (CO2) gas
and water vapor (H2O). The chemical
change that occurs with burning, is
called combustion.
Other processes that result in chemical
changes include: electrolosys,
oxidation, and tarnishing.
 The Stevespanglerscience.com videos I
showed in class gave us good examples
of chemical changes. Also, when I
combined baking soda with vinegar in
class, you witnessed the result of
extreme fizzing, which was a chemical
reaction.
Changes in Matter
Conservation of Mass/Matter
 Matter is not created or destroyed
 No mass is either lost or gained during a chemical change.
 If you could collect all of the carbon dioxide (CO2) and water
produced when methane gas (CH4) burns, and you
measured the mass of all the matter collected, you
would find that it is equal to the mass of the original
methane plus the mass of the oxygen that was used in
the burning. See picture below.
 No mass is lost, because during a chemical change,
atoms are not lost or gained, only rearranged.
Changes in Matter
Matter and Thermal Energy
Energy is the ability to do work or cause change.
Every chemical or physical change in matter includes a change in
energy. Even bending a paper clip takes energy. When ice changes to
water, it absorbs energy from the surrounding matter. When candle
wax burns, it gives off energy.
Temperature is a measure of the average energy of random motion of
particles of matter.
The particles f gas in the warm outside air have greater average energy
of motion than the particles of air in the cool building.
Thermal energy is the total energy of all of the particles in an object.
Temperature and thermal energy are not the same. Thermal energy
always flows from warmer matter to cooler matter. When matter
changes, the most common form of energy released or absorbed is
thermal energy. For example, ice absorbs thermal energy from its
surroundings when it melts.
Changes in Matter
Thermal Energy (cont’d)
Endothermic
Change
Exothermic Change
 A change in which
 An exothermic
energy is taken in.
 Examples: Melting
of ice, cooling of
hot chocolate or
soup.
change releases
energy.
 Examples: burning
of a fire, burning of
a candle; or any
combustion. Also
think of how a
lightbulb gives off
heat and light.
States of Matter: Solids,
Liquids and Gases
Solids, Liquids and gases may be elements,
compounds, or mixtures. Gold is an
element, water is a compound that can be
solid, liquid or gas. Air is a mix of gases. The
states of matter are defined by whether or
not they hold their volume and shape.
http://studyjams.scholastic.com/studyjams/
Copy this link into your
jams/science/matter/solids-liquidsbrowser for an overview
gases.htm
States of Matter
*Quick overview of the 3 most common states*
Solids
Liquids
Gases
Definite shape and
volume
No shape of its own,
definite volume
No shape of it’s own
(like a liquid), no
volume of its own.
Particles packed very
close, tight and fixed.
This causes the definite
shape and volume.
Particles are free to
move around each
other, but packed
together.
Particles are spread
out, and not packed
together.
The dimensions do not
change.
Dimensions change
with container, but the
volume remains the
same.
Gases roam freely, and
can be kept in a
container like water
can
Measured in cm³ or m³
Measured in ml or L
same volume as its
container.
lxwxh
# of ml
# of ml or cm³
States of Matter Solids,
Liquids, Gases (Cont’d)
 Solids:
 Crystalline: Particles form a regular, repeating pattern which
forms crystals. Examples: salt, sugar, snow. When heated,
crystalline solids melt as a specific temperature.
 Amorphous solid: Particles are not arranged in a regular
pattern. Examples: butter, rubber, glass. Do not melt at a
distinct temperature. May become softer or change into other
substances.
 Liquids:
 Also called a fluid—substance that flows
 Fluids have certain characteristics:
Surface Tension – inward pull among the molecules of a
liquid that brings the molecules on their surface closer
together. The surface of water can act like a sort of skin.
 Viscosity – A liquid’s resistance to flowing. A liquid’s
viscosity depends on the size and shape of its particles and
the attractions between the particles. The quicker the flow,
the higher viscosity.

 *Gases: *
 Gases are actually a form of fluid. As particles move, gas
particles spread apart, filling all available space. As temperature
increases, pressure increases
*States of Matter--Changes
of State*
 Why does ice cream melt? Particles of a substance at a
warmer temperature have more thermal energy than
particles of that same substance at a cooler temperature.
Thermal energy always flows as heat from a warmer substance to a
cooler substance.
 Particles of a substance at a warmer temperature have more
thermal energy than particles of the same substance at a cooler
temperature.
 Matter changes state when thermal energy is added or removed.
Particles in a solid substance vibrate faster when energy is added.
The addition of energy causes particles of a solid to move faster
and faster until they break free from their fixed position.
 Liquid particles move more slowly as energy (heat) is removed
until they form the regular patterns of a solid.
 The point where the particles of a solid break free from
their fixed positions, is called the melting point. Different
substances have different melting points because they have
different arrangements of particles that respond
differently to added thermal energy.
Paste this link
http://articles.washingtonpost.com/2009-06into your browser 29/news/36778299_1_national-ice-cream-day-cookieto read an article: dough-large-ice-crystals
Solid to Liquid &
Liquid to Solid
Liquid to Gas & Gas to Solid to Gas & Gas
Liquid
to Solid
Called melting or freezing.
Melt at a specific temp.
called a melting point. Added
thermal energy makes liquid
molecules vibrate faster, raising
their temperature. At its
melting point, the particles
are vibrating so fast that they
break free from their fixed
positions. As ice cream
Called vaporization and
condensation. Vaporization
happens when the particles in a
liquid gain enough energy to
form a gas. The movement
States of Matter – changes of states
Changes of state at a glance
or an iceberg
melts—or anything,
for that matter,
melts, its molecules
absorb heat energy
and move further
apart.
Freezing is a change from liquid
to solid. Particles of a liquid
move so slowly that they begin to
form regular patterns. When
water freezes, its
temperature remains at
0ºC until freezing is
complete. As particles
freeze, its molecules
lose heat energy and
move slower and
closer together.
of molecules increase as
temperature stays the
same.
Condensation is the opposite of
evaporation/vaporization.
Evaporation only takes place on
the surface of the liquid.
Boiling takes place when a liquid
changes to gas below its surface
and at its surface. The
boiling point of a substance
depends on the pressure of the
air above it.
The lower the pressure, the less
energy needed to boil liquids.
In mountainous areas, the
boiling point of water is 95ºC.
In Atlanta, GA, the melting
point is 100ºC, because Atlanta
is much closer to sea level
Changes of state usually
involve transitioning from
a solid to a liquid, then a
gas (think of an ice cube
melting and evaporating).
Sometimes, though, the
transition is directly from
a solid to a gas.
Sublimation occurs when
the surface particles of a
solid gain enough energy
that they form a gas. An
example is dry ice. When
dry ice becomes a gas, it
cools water vapor in the
nearby air. The water
vapor then condenses into
a liquid forming fog
around the dry ice.
*
States of Matter – Gas Behavior
 How does a hot air balloon fly high in the sky
and come back down to earth? It’s secret is in
the gas. : ).
 The balloon is inflated using powerful air fans,
then the air is heated with propane gas burners.
Remember, air is a gas. Heating causes the air
inside the balloon to expand. Some of the
warm air leaves through the bottom of the
balloon, keeping the pressure constant. The
balloon is secured by ballasts ( anchors). When
the pilot is ready to lift off, the ballasts are
brought into the balloon’s basket, and the
balloon rises because the hot air inside the
balloon is less dense than the outside air. To
descend, the pilot slowly reduces the flame,
making the air in the balloon cooler. The air in
the balloon gradually becomes more dense
than air, so the balloon descends.
States of Matter – Gas Behavior *
 When working with gas, it is helpful to know its volume,
temperature and pressure.
 Volume: The amount of space matter fills
 Measured in cubic centimeters (cm³), milliliters (ml), and Liters
(L) and other units.
 The volume of a gas is the same as the volume of container that it’s in.
 Temperature: The average energy of the random movement of
particles of a substance. The faster the particles, the greater their energy
and the higher temperature. You might think of a thermometer as a
speedometer for molecules. Particles of a typical gas at room
temperature travel at about 500 meters per second!
 Pressure: Gas particles are constantly colliding with one another
and with the walls of their container. As a result, the gas pushes on
the walls of the container. The pressure of the gas is the force of its
outward push divided by the area of the walls of the container.
Pressure is measured in units of pascals (Pa) or kilo-pascals (kPa). The
firmness of a gas-filled object comes from the pressure of the gas. The
air inside a fully pumped basketball has a higher pressure than the air
outside. This higher pressure is due to a greater concentration of air
inside. When air leaks out of a basketball, pressure decreases. The
pressure inside drops until it equals the pressure outside of the ball.
The formula for pressure is: Pressure = Force/Area
Example:
A machine exerts a force of 252N on a piston having an area of 0.430 m². What is the pressure on
the piston in Pa?
Pressure =252N/0.430m² = 586 Pa
Watch this to 9:15 for an explanation of gas pressure:
http://www.youtube.com/watch?v=90E2jhDVCSg
States of Matter – Gas Behavior *
Pressure and
VOLUME
 When pressure of a gas at constant temperature
increases, the volume of the gas decreases. When
pressure increases, volume decreases.
Graphing Boyle’s Law*
States of Matter – Gas Behavior*
 Pressure and TEMPERATURE
 When the temperature of a gas at
constant volume is increased, the
pressure of the gas increases. When the
temperature is decreased, the pressure of
the gas decreases. (constant volume
means that the gas is in a closed, rigid
container).
States of Matter – Gas Behavior*
 VOLUME and TEMPERATURE
Graphing Charles’s Law*
Law of Conservation of
Mass/Matter
*The principle that the total amount
of matter is neither created nor
destroyed during any chemical or
physical change.
Law of Conservation of Mass/Matter*
 Suppose you could collect all of the carbon dioxide
and water produced when methane gas burns.
Methane gas is commonly used as a fuel for a kitchen
range (stove). You would find that your collection
would equal the mass of the original methane gas,
plus the amount of Oxygen that was used to burn the
methane. No mass is lost because during a chemical
change, atoms are not lost or gained, only rearranged.
(p. 53)
 Another example: In a chemical reaction, carbon (C)
and oxygen (O) combine the mass of the product is
equal to the mass of the carbon and the mass of the
oxygen.
 How does the law of conservation of mass apply to a
burning candle? When a candle burns, the mass of the
wick, candle, wax and oxygen that helped the flame
before the reaction equals the mass of the smoke, ash
and gas after the reaction. No mass is lost, it’s just
transformed into different forms of mass.
 Helpful links:
http://www.youtube.com/watch?v=dExpJAECSL8
http://www.neok12.com/php/watch.php?v=zX780d5
e7806764057657b45&t=Law-of-Conservation
Summarizing Gases
 Follow this link by using control+click:
http://www.chem.purdue.edu/gchelp/atoms
/states.html
http://www.youtube.com/watch?v=zvh9uv2
Hxx4
http://www.stevespanglerscience.com/lab/vi
deos#?video=water-balloon-in-bottle
http://www.stevespanglerscience.com/lab/vi
deos#?video=balloon-powered-car