1. SWBAT: Define the classes of matter.
Identify the two types of mixtures.
Describe the three types of Homogeneous Mixtures.
Classification Activity.

2. Chapter 4: Mixtures, Elements and Compounds What you know about Matter. . .
What is new about matter?
There are 4 states of matter:
Solid
Liquid
Gas
Plasma
There are 4 Phase Changes of Matter
Fusion
Solidification
Condensing
Vaporization
How is matter classified?
Matter is classified into 4 Groups:
Mixtures
Solutions
Elements
Compounds

3. Mixtures
A mixture has two or more substances that are not chemically combined with each other and can be separated by physical means.
The substances in a mixture retain their individual properties.
Two Types of Mixtures:
Homogeneous Mixture
Heterogeneous Mixture

4. Homogeneous Mixture How can you tell if it is a homogeneous mixture?
A mixture that appears to be the same throughout.
“well mixed”
the particles are very small and not recognizable
The particles do not settle when let to stand.
Can be separated by heat or chemical means.

5. Examples of Homogeneous Mixtures: 1. Colloids:
Particles that are mixed but not dissolved.
Toothpaste, suntan lotion
2. Solutions
Alloys:
Solids dissolved in solids meaning metals dissolved in metals:
Examples:
Brass: copper and zinc
Sterling silver: copper and silver
Stainless steal: chromium and iron

6. Types of Colloids Name Description Example Fog liquid in gas Clouds
Smoke
solid in a gas
Foam
gas in a liquid
Whipped cream
Emulsion
liquid in liquid
Mayonnaise
Sol
solid in liquid
Paint
Gel
liquid in a solid
butter

7. Solutions It is known as a homogeneous mixture.
Solutions are made of a solute and a solvent!
Two Parts:
Solute: A substance that is being dissolved.
Solvent: The substance that does the dissolving.
Solutions can be solids or liquids.

8. Types of solutions Alloys:
Solute
Solvent
Example
Gas
Liquid
Solid
Liquid
Alloys:
Metals dissolved in metals are called alloys.

9. Types of solutions Gas Air (oxygen in nitrogen) Liquid Fruit Punch
Solute
Solvent
Example
Gas
Air (oxygen in nitrogen)
Liquid
Fruit Punch
Solid
Ocean water (salt in water)
Solid
Alloys: Gold jewelry (copper in gold)

10. Alloys Stainless steel is a mixture of iron and chromium.
Brass is an alloy of copper
and zinc.

11. Air is a solution of oxygen and other gases dissolved in nitrogen.

12. Heterogeneous Mixtures
How can you tell if it is a heterogeneous mixture?
A mixture that does not appear to be the same throughout.
“least mixed”
Particles are large and can be seen.
Particles can be separated from the mixture.

13. Examples of Heterogeneous Mixtures
Salad dressing
Oil and vinegar
Salt and pepper
Sand and water
Dirt
Fruit salad

14. Solubility Soluble: A substance that can dissolve in another substance
Insoluble:
A substance that does not dissolve in water
Solubility:
A given solute can be dissolved in a given amount of solvent at a certain temperature.
As temperature increases so does the solubility of a solid
As temperature increase solubility of gas decreases

15. Factors that affect the Solubility of a solute
Particle size
Temperature
Amount of solute
Amount of solvent

16. Particle Size What did you learn from your labs you conducted?
As the particle size decreases, the dissolve time decreases.
Why?
When a particle decreases, the Volume decreases and there is more exposure to the environment to dissolve.
surface area: amount of matter exposed to the environment.

17. Temperature

18. Analyze the graph
Write down the chemical formula that dissolves at 70 degrees C with 30 grams solubility. _______
Which chemical formula express that as the temperature increases the solubility rate decreases? ___________
Which chemical formula can dissolve with 100 grams at 27 degrees C? ___________
What is the relationship between temperature and the solubility rate based on the information provided with the exception of Ce2(SO4)3?
_____________________________________

19. Elements
An element is a pure substance made of only one kind of material or substance.
Are the same throughout.
They are the simplest type of a pure element.
They cannot be broken down into a simpler form without losing their properties.

20. Compound
Compounds are pure substances that are in unions of two or more elements.
They are chemically combined.
They can be only be chemically broken down.
They are made of molecules.

21. Molecules CHEMICAL FORMULA Example: C3H2OH Rubbing Alcohol
Molecules are made of atoms
The smallest complete part of a compound having the same properties throughout.
CHEMICAL FORMULA
A chemical formula tells you the elements and number of atoms that are needed to make the molecule or compound.
Example: C3H2OH Rubbing Alcohol

22. What is a subscript?
Provides you the number of atoms of an element in the compound.
They are found to the lower right of each element’s symbol.
When there is only one atom there is no subscript written.
Subscript

23. What does the coefficient tell you?
Tells you the number of molecules there are in a reaction.
They are found in front of the compound or molecule.

24. What does a chemical equation tell you?
A chemical equation tells you the types of molecules and or compounds that are needed to complete a chemical reaction to form products.
Each side of the equation must have the same number of atoms per element!!
Practice Web Site:

25. Researching elements Go to Computer use only. Login: User
Password: User
Next click cancel and you should then be logged in properly.
Go to the following web site:

26. Fog
peanut butter
Smoke
Sea water
whipped cream
Mayonnaise
paint
tooth paste
butter

27. Salad dressing
Iced Tea
Apple Juice
Sand and water
sugar water
Taco salad
Salt and pepper
Concrete

28. MIXTURES
H O M O G E N E O U S
H E T E R O G E N E O U S

29. Concept Map: classifying matter
HETEROGENOUS
HOMOGENOUS
SOLUTION
COLLOID
ALLOY
MIXTURES