MATTER
the stuff of the universe
Matter
• Matter: ______________________________
_____________________________________
• Mass: the amount of ____________________
• Weight: ______________________________
– on Earth, this is the same as mass
• Law of Conservation of Matter: “__________
________________________________”…but
it can be rearranged (via chemical or physical
reactions)
Atoms
Matter is composed of _________
• Atoms: ___________________________
_________________________________
_________________________________
• can not be further divided and still have
_________ ___________
– Are composed of _________, ___________, and
___________
Pure Substance
• A substance with
– Ex:___________________
_______________________
• __________ and
______________are both
considered to be pure
substances
States of Matter
Solid
Liquid
Gas
Condensed States: Solids
• Solids
–Have a ___________________
__________________________
–Molecules are
• Tightly ________
• Moving _________________________
____________________
• ________________attracted to each
other
• Not _________________
Condensed States: Liquids
• Liquids

Have NO set__________but definite
__________
–Molecules are
• ____________than in a solid at the
same temperature
• _________________________
• _________ attracted to each other
• Not _______________
Expanded States: Gas
• Gas (vapor)
– Have no ________________
• Depends on the container
– Have ________________
• Varies depending on _______________ and ___________
– Molecules are
• ______________________attracted to each other
• ________________than those in a liquid at the same
temperature
• As a result are
– _________________as far as possible
– __________________past each other
– _____________________
Expanded States: Plasma
• Plasmas
– Occur at extremely ____________________
– Are ________________
• May be some atoms or molecules but mostly
– ________________ floating around not attached
– Usually are __________________________
– Most ________________ form of matter in the
universe
• ______________
– Here on Earth: _______________________________
___________________________________________
What is a non-Newtonian fluid?
You have to pull the trigger on a water pistol to get the water to squirt out. To make the
water to come out faster, you have to pull the trigger harder. Fluids resist flow. The
resistance to flow arises because of the friction between these layers. This
phenomenon is known as viscosity.
Newton devised a simple model for fluid flow that could be used to relate how hard you
have to pull the trigger to how fast the liquid will squirt out of the pistol. Picture a
flowing liquid as a series of layers of liquid sliding past each other. The slower one
layer slides over another, the less resistance there is, so that if there was no
difference between the speeds the layers were moving, there would be no
resistance.
Fluids like water and gasoline behave according to Newton's model, and are called
Newtonian fluids.
But ketchup, blood, yogurt, gravy, pie fillings, mud, and cornstarch paste DON'T follow
the model. They're non-Newtonian fluids because doubling the speed that the layers
slide past each other does not double the resisting force. It may less than double
(like ketchup), or it may more than double (as in the case of quicksand and gravy).
That's why stirring gravy thickens it, and why struggling in quicksand will make it
even harder to escape.
For some fluids (like mud, or snow) you can push and get no flow at all- until you push
hard enough, and the substance begins to flow like a normal liquid. This is what
causes mudslides and avalanches.
Physical and Chemical Properties
and Changes
Physical Property
• Characteristic of a •
substance that can
be observed
________________
________________
________________
________________
________________
Examples:
– ______________
– ______________
– ______________
– ______________
– ______________
– ______________
Chemical Property
• Ability of a substance to _____________
_________________________________
• You must change the identity _________
_________________________________
_________________________________
• Examples:
– ______________
– ______________ with acids and bases
Intrinsic v. Extrinsic Properties
• Intrinsic (intensive) Property: A
property that _______________
__________________________ of
substance changes
–_____________
–_____________
–_____________
–_____________
Intrinsic v. Extrinsic Properties
• Extrinsic (extensive) property: A
property that ___________________
______________________________
______________________________
–_____________
–_____________
–_____________
–_____________
Density…Intrinsic or Extrinsic?
Density data for a sample of gold.
 Density= mass/ volume
 Units are g/mL or g/cm3

Mass (g)
Volume (mL)
46.71
2.42
297.80
15.43
662.76
34.34
147.07
7.62
431.162
22.34
85.69
4.44
Density
Physical Change
• Change in the _________________substance, not
in its chemical nature
– No chemical bonds ___________________________
• The chemical formula is the same before and after the
change
– ________________________________are made or broken, not the
molecules themselves
– Examples:
•
•
•
•
__________________
__________________
__________________
__________________
Chemical Change (___________)
• Change_____________________________
_____________________________
 Atoms are __________________
– Bonds are ______________________ in
new ways
• Examples:
– __________________
– __________________
– _______________
– __________________
Signs of Chemical Change
• Change in:
– ___________________
• Forming a _______________ (solid made from liquids)
• ___________________________
– __________
– ________________
• _________ (exothermic)
• _________ (endothermic)
– _____________
• giving off ___________
What is an element?
• Element:
– A substance made up of only one type of
atom is an _____________________
How do we represent elements?
– Represented by symbols on the periodic table
• Usually comes from the ___________, a
_____________, or a _____________
• One or two letters for those with official names
–___________________________________
–___________________________________
• Unofficially named elements have three letters,
starting with a capital ____
Elements in Nature
• ____90 naturally occurring
– Of the __________on the Periodic Table, only ___
and ____ are not naturally occurring
• Some elements are _________________
__________________, but commonly are
found in compounds
– ex: ______________is virtually non-existent in
pure form, but is found in common_______, a
compound we call table salt.
Elements
When elements were discovered
Allotropes
•Allotropes are ___________________
__________________________
• Shown here are allotropes of carbon
•______________,
______________, and
______________
•Difference is how the atoms are
__________________________
Molecules
• Two (2) or more _______________
_____________________
– O2
– H2
– H2O
– C6H12O6
Compounds
• Two (2) or more ___________________
________________________________
_________________________________
– Has own, unique:
• ________ (law of__________________)
• properties
– ___________________________________
– Need a ___________________to separate them
into the elements it is made from
• 2 H2O -> 2H2 and O2
Law of Definite Proportions
• In samples of any chemical compound, the
________________________________
_________________________________
• ________________________________
– H2O is always H2O, and never H2O2
– Once the formula is different, the materials and
the properties are different
What is the difference between
compounds and molecules?
Molecules: two or
more atoms
bonded
Compounds:
two or more
atoms of
_______
________
bonded
•The term molecule is
more _________,
compound is more
_________.
•Molecules can be
_______________ like
___________
•Compounds by
definition ________
_______________
Separation of compounds into their
elements
• Compounds can be
broken into their
elements by
_______________,
such as
• ______________.
This is the
decomposition of a
substance (here,
water) into it’s
elements by an
______________.
Mixture
• A blend of 2 or more____________
• Have __________ compositions
–No _____________________
• Examples:
Air: A Mixture
Types of Mixtures
• Homogeneous
– ________________
– __________________
– cannot see ________________
– Examples
•
•
•
•
___________
___________
___________
___________
Types of mixture, con’t
• Heterogeneous
–______________
–not __________________
–can see ______________
–Examples:
• _________________
• _________________
• _________________
• _________________
Subtypes of mixtures...
• Solutions: one thing dissolved in another;
they do not ___________________or when
filtered (particles are molecules)
– Two parts:
• Solvent-______________________________
• Solute- _______________________________
Ex: Salt water – water is the ________, salt the _______
– Can be any state of matter
• Alloys are _____________________(a solid solution)
Subtypes of mixtures...
• Suspensions:
– Heterogeneous mixture of two or more
substances
– may look like a solution but can
____________________________
____________________________
– particles are not dissolved
• particles are larger than molecules;
sometimes they can be seen by the naked
eye
Subtypes of mixtures...
• Colloid- microscopically mixed homogeneous solutions
that will _______________ (____________)
– They will ________________out upon standing
– Emulsion- a type of colloid made from of two liquids that
normally will not mix (are_________________________)
Tyndall Effect
• Twenty-four-karat gold is an _____________
• Eighteen-karat gold is an ________.
• Fourteen-karat gold is an ___________.
– (Alloys are homogeneous mixtures- specifically
solutions- of metals)
– What is the solvent in 18K and 14K gold?
– What is/ are the solute(s) in 18K and 14K gold?
Classification of Matter
Separating Mixtures
• Mixtures can be separated by
_________________________
– No chemical reactions or changes needed
– 5 main methods are based on physical properties
•
•
•
•
•
_________________
_________________
_________________
_________________
_________________
Separating Mixtures
• Evaporation: ____________________
________________________________
• Crystallization: ___________________
_____________________________________
_____________________
•
•
•
•
– Usually paired
_____________
_____________
_____________
_____________
Chromatography: “color writing”
• Using how ______________________to
separate them
– Use specific ratios of movement through a medium
(paper, water, column) based on how some molecules
move through the medium
– Phases:
• Stationary phase
– _____________________(paper, the column)
– ____________________of the mixture _________________
• Mobile phase
– moves over the stationary phase
– _________________________of the mixture
– Rf values constant for component of a mixture
• Ratio of ________________________________________
_______________________________________________
• Ex: running colors in ink when wet
chromatograms
Gas and Column
Chromotography
Filtration
• Use a funnel
and ________
_____________
• Separates a
_____________
_____________
• Based on
_____________
• Separates _______
________________
Distillation
• One liquid has to
have a lower _____
________________
– Heat both; the one
with the lower BP is
boiled out first
– Can use
_______________ to
collect materials as
they boil out
• Used with crude oil
(______________) to
isolate separate
products
Distillation of Crude Oil:
Cracking
Other methods…
• Use ____________ (____________)
– _____________________
• Use _____________
– For solids: Mixture of pieces is placed in a
solution
• Some float and can be skimmed off
• Some sink
• Used in recycling plants to separate plastics
– For liquids that are immiscible (will not mix,
like oil and water): use a separatory funnel
Separatory Funnel
Used for
liquids that are
___________
(will not mix,
like oil and
water)
End of Chapter