I. Classification of Matter
MATTER
(anything that has
mass & takes up space)
MATTER
PURE SUBSTANCE
(matter with a
definite composition)
Ex- water, helium,
carbon dioxide,
sodium
MATTER
MIXTURE
(2 or more pure
substances combined in
ANY ratio)
Ex- lemonade, concrete,
shaving cream
Pure Substances
COMPOUND
(2 or more elements
chemically bonded
together)
Ex- sodium chloride,
water, glucose,
CLUE- chemical formulas
have 2 capital letters; it is
NOT on the periodic table
Pure Substances
ELEMENT
(cannot be broken down
any further)
Ex- carbon, oxygen, lithium,
hydrogen
CLUE- It is any substance
written on the periodic table
Mixtures
SOLUTION
(a homogeneous mixture
that cannot be filtered & will
NEVER settle upon
standing)
Ex- saline solution, grape
juice
CLUE- It is clear (might be
clear & colored)
Mixtures
COLLOIDAL SUSPENSION
(a homogeneous mixture
that cannot be filtered & will
EVENTUALLY settle upon
standing)
Ex- mayo, milk, fog, cool
whip
CLUE- it creates the Tyndall
Effect
Mixtures
COURSE SUSPENSION
(a heterogeneous mixture
that can be filtered & will
QUICKLY settle upon
standing)
Ex- Italian Dressing, OJ
CLUE- it has
distinguishable “pieces” in
it.
SOLUTION
ALLOY
(a special type of solution
where 2 or more METALS
mix together----a “metallic
solution”)
Ex- brass (zinc & copper);
pewter (tin & lead); steel
(iron & carbon)
CLUE- It is NOT on the
periodic table
II. Physical Properties of matter that we will use to
help us separate a solution?
Magnetism
A. ___________________________
Demonstration – Magnetism:
Density
B. ___________________________
Phase Changes
C. ____________________________
1. Lab techniques that uses phase change separation.
Distillation – uses different boiling
a. ____________________________
points of the pure substances
____________________________
involved to separate and CAPTURE
____________________________
all of the substances of the mixture
___________________________
Distillation Demo:
b. ______________________
Crystallization – separation
technique that uses the boiling
point to capture ONLY the
substance with the HIGHEST
boiling point
Particle Size
D. ___________________________
1. Lab techniques that use particle size
separation.
– using a screen or paper
a. Filtering
____________________________
to help retain the larger items,
____________________________
while the smaller pass through
____________________________
E.__________________________________
Can dissolve in water (Soluble in water)
III. Characteristics of Solutions
A. Parts of a Solution
Solvent – the
substance doing
the dissolving
Solute – the
substance being
dissolved
B. Terms related to solutions:
Able to dissolve in each other
1. Soluble -___________________________
_________________________________
ex – Salt is soluble in water
NOT able to dissolve in each
2. Insoluble - _________________________
other
__________________________________
ex - Water is insoluble in water
3. concentration - _________________________
the amount of solute in a
solution
_____________________________________
you add more solvent
4. Diluted solution - when
_______________________
to a solution in order to decrease the overall
______________________________________
concentration
when you remove
5. Concentrated solution - __________________
solvent from a solution in order INCREASE
______________________________________
the overall concentration
C. Rate of solution:
1. Definition: ________________________
the speed at which a
solvent
is able to dissolve a solute
________________________________
2. Ways to increase the speed at which the
solvent dissolves the solute.
Increase temperature
a. _____________________________
Demo:
b. Increase
_____________________________
surface area
Demo:
c. _____________________________
Stir or Shake
Demo:
D. How do You Describe The Amount of Solute in
a Solution?
1. Definition of each:
a. Unsaturated- _____________________
Does not have all of the
solute
that it could at a given
________________________________
temperature
solute
i. if you add one more piece of _____________
to
an unsaturated solution, it will
dissolve
_______________
into the beaker of solution.
Has all of the solute that it can at a
b. Saturated - ____________________________
given
temperature
_____________________________________
i. if you add one more piece of
solute
_____________
to a saturated
Stay as a crystal
solution, it will __________________
in the
beaker.
Has more solute
c. supersaturated - _______________________
than
it
SHOULD
at
a
given
temperature
____________________________________
i. if you add one more piece of
solute
_____________
to a super-saturated
solution, it will __________________
in the
crystalize
beaker.
Demonstration – Super Saturated Solution:
E. Solubility and Solubility Curves
The total amount of
1. Solubility - __________________________
solute necessary to make a saturated
___________________________________
solution at a GIVEN TEMPERATURE
a graph that illustrates
2. Solubility Curve – __________________________
the solubility of given solutes in certain
________________________________________
solvents
________________________________________
1. What is the title of this
graph?
2. What is the x-axis label?
3. What is the x-axis unit
of measurement?
4. What is the y-axis label?
5. What is the y-axis unit
of measurement?
6. What is the general
trend expressed by this
graph?
SUPERSATURATEDanything above the
line
UNSATURATEDanything under the line
1. What is the
temperature of a
saturated solution of 36
g / 100 g of water?
2. What is the solubility of
BaCl2 at 60 C?
3. If a solution has 40 g of
BaCl2 dissolved in 100 g
of water and it is at 70
C, how would you
characterize it?
4. How would you create a
supersaturated
solution?
c. Common trend between temperature and heat
i. as temperature __________________,
increases
increases
solubility _________________.
1. Which salt is the
most soluble at
70 C?
2. Which salt’s
solubility is least
affected by
temperature?
3. Which salt’s
solubility is most
affected by
temperature?