Download - I. Classification of Matter
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,
hydrogenCLUE- 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
juiceCLUE- 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
whipCLUE- it creates the
Tyndall Effect
Mixtures
COURSE SUSPENSION(a heterogeneous mixture that can be filtered & will
QUICKLY settle upon standing)
Ex- Italian Dressing, OJCLUE- 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?
A. ___________________________Magnetism
Demonstration – Magnetism:
B. ___________________________C. ____________________________
1. Lab techniques that uses phase change separation.
a. ____________________________ ____________________________ ____________________________ ___________________________
DensityPhase Changes
Distillation – uses different boiling points of the pure substances involved to separate and CAPTURE all of the substances of the mixture
Distillation Demo:
b. ______________________
D. ___________________________1. Lab techniques that use particle size
separation.a.
____________________________
____________________________
____________________________
Crystallization – separation technique that uses the boiling point to capture ONLY the substance with the HIGHEST boiling point
Particle Size
Filtering – using a screen or paper 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:1. Soluble -
___________________________
_________________________________ ex –
2. Insoluble - _________________________
__________________________________
ex -
Able to dissolve in each other
Salt is soluble in water
NOT able to dissolve in each other
Water is insoluble in water
3. concentration - _________________________ _____________________________________
4. Diluted solution - _______________________ ______________________________________
5. Concentrated solution - __________________ ______________________________________
the amount of solute in a solution
when you add more solvent to a solution in order to decrease the overall concentration
when you remove 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.
a. _____________________________ Demo:
b. _____________________________ Demo:
c. _____________________________ Demo:
Increase temperature
Increase surface area
Stir or Shake
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
i. if you add one more piece of _____________ to an unsaturated solution, it will _______________ into the beaker of solution.
solute
dissolve
b. Saturated - ____________________________ _____________________________________
i. if you add one more piece of _____________ to a saturated solution, it will __________________ in the beaker.
Has all of the solute that it can at a given temperature
soluteStay as a crystal
c. supersaturated - _______________________ ____________________________________
i. if you add one more piece of _____________ to a super-saturated solution, it will __________________ in the beaker.
Has more solute than it SHOULD at a given temperature
solute
crystalize
Demonstration – Super Saturated Solution:
E. Solubility and Solubility Curves 1. Solubility - __________________________
___________________________________
2. Solubility Curve – __________________________
________________________________________
________________________________________
The total amount of solute necessary to make a saturated solution at a GIVEN TEMPERATURE
a graph that illustrates 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?
UNSATURATED- anything under the line
SUPERSATURATED- anything above the line
SATURATED - anything on 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 heati. as temperature __________________, solubility _________________.
increases increases
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?