1. Separation of Matter

2. Matter is Anything that has mass and takes up space (volume)
Can it be physically separated?
(ex: filtration or evaporation)
Is it made up of only one type of atom on the periodic table?
Is the composition uniform throughout?
YES NO
Pure substance
Mixture
Heterogeneous
Compound
Element
Homogenous

3. Types of matter
Pure substances- 1. element ex: silver 2. compound ex: NaHCO3
Uniform, unchanging composition. Pure substances exist as either elements or compounds.
Found on the periodic table
cannot be separated into simpler substances by physical or chemical means
It takes a nuclear reaction to break them apart!
two or more elements that are chemically bonded.
A chemical change is required to combine elements into compounds, or to separate compounds back into elements.

4. 1. heterogeneous mixture
Mixtures
2 types
1. heterogeneous mixture
ex:
2. homogeneous mixture
Not uniform throughout. Made of very large molecules.
Uniform throughout: also called solutions: made of very small molecules.
Gas / Liquid: Soda (CO2 in H2O)
Gas / Gas: Air (Nitrogen, Oxygen, Argon, Water Vapor)
Liquid / Liquid: Gasoline (mixture of liquid hydrocarbons); Rubbing Alcohol (Isopropyl Alcohol with water); Vinegar (Acetic Acid with water)
Solid / Solid: Alloy (mixture of metals), such as brass, steel, 14-karat gold

5. Example 1 Soda Rust Iced tea Chicken soup Dirt Chlorine Sugar Gasoline
water
homogenous
compound
heterogenous
heterogenous
heterogenous
element
compound
homogenous
compound

6. Chemical and Physical Properties

7. Remember, density is tricky
Remember, density is tricky! While it’s a number, it’s always the same for a substance, no matter how much of it you have!
___Chemical____ properties describe the ability of a substance to undergo changes that transform it into different substances. Some sort of chemical reaction must be performed in order to observe these properties.
___Physical___ properties describe the substance itself. They can be observed or measured without altering the chemical identity of the substance (meaning no chemical reaction is necessary to view these properties)....

8. CHEMICAL AND PHYSICAL PROPERTY EXAMPLES

9. Types of physical properties!!! 1. Extensive physical properties
2. Intensive physical properties
DO DEPEND on the amount of matter present
DO NOT DEPEND on the amount of matter present
**Example 2: Place an I(Intensive) or E(extensive for each of the following properties:
Malleability (hammer into sheet) I Mass E
Melting point I Odor I
Ability to react with acid I Volume E
Ability to react with base I Clarity I
Ability to react with water I Color I
Ability to rust I Consistency I
Ability to tarnish I Density I
Viscosity (resistance to flow) I length E
Boiling point I Area E
Ability to conduct electricity I Luster (shine) I
Dissolves in water I Hardness I
Amount of Energy E
Ductility (ability to be molded) I
Ability to explode (combust) I
Flammability (burning) I

10. Chemical and Physical Changes

11. Changes Physical Changes Chemical Changes
Transform one or more substances into new, different substances. They involve some sort of reaction taking place!
Do not change the identity of a substance. Changes of state are all considered to be physical changes.
Just remember:
1) nothing new has formed
2) it is still the same substance
How do we know if its chemical?
heat
An unexpected change in _______ energy (hotter or colder)
A _________ is produced (bubbling)
An unexpected _________ change
A solid _____________ is produced (cloudiness)
An unexpected apparent _________
change (means that a gas was involved)
New __________ formed
_________ produced (fire)
gas
color
precipitate
mass
odor
light

12. Example 3:
All of the processes listed below are part of the digestive breakdown of food. For each of the following, classify them as a chemical or physical change, and give a reason why.
A. Chewing food
B. Breakdown of proteins
C. Breakdown of carbohydrates
D. Churning of food
E. Starch breakdown
F. food reacting with HCl
Physical
Chemical
Chemical
Physical
Chemical
Chemical

13. States of Matter and Phase Changes

14. States of Matter far Very container Definite container container
SOLID
LIQUID
GAS
Molecules _________ close
Molecules CLOSE
Molecules _____ apart
________ shape
_________ volume
Takes shape of __________
________ volume
Takes shape of ___________
Takes volume of ___________
VERY RESTRICTED motion – rotation and vibration in place only
LIMITED freedom of motion – there is some degree of fluidity
FREE TO MOVE in all directions – high degree of fluidity
HIGH density
(typically measured in g/mL)
MEDIUM-HIGH density (less than that of solid EXCEPT for water!)
LOW density (typically measured in g/L)
______ compressible (incompressible)
_________ compressible
________compressed into smaller volumes
Does NOT expand much with increases in temperature
Expands SLIGHTLY with increases in temperature
HIGHLY expansive with increases in temperature (assuming the volume of the container can change!)
Diffusion SO SLOW you can hardly notice it – must ramp temperature up really high to facilitate diffusion
Diffuses EASILY but less rapidly than the gaseous state
Diffuses EASILY and QUICKLY
far
Very
container
Definite
container
container
Definite
Definite
Not
Somewhat
Easily

15. States of Matter Very container Definite Definite Definite Somewhat
SOLID
LIQUID
GAS
Molecules _________ close
Molecules CLOSE
Molecules _____ apart
________ shape
_________ volume
Takes shape of __________
________ volume
Takes shape of ___________
Takes volume of ___________
VERY RESTRICTED motion – rotation and vibration in place only
LIMITED freedom of motion – there is some degree of fluidity
FREE TO MOVE in all directions – high degree of fluidity
HIGH density
(typically measured in g/mL)
MEDIUM-HIGH density (less than that of solid EXCEPT for water!)
LOW density (typically measured in g/L)
______ compressible (incompressible)
_________ compressible
________compressed into smaller volumes
Does NOT expand much with increases in temperature
Expands SLIGHTLY with increases in temperature
HIGHLY expansive with increases in temperature (assuming the volume of the container can change!)
Diffusion SO SLOW you can hardly notice it – must ramp temperature up really high to facilitate diffusion
Diffuses EASILY but less rapidly than the gaseous state
Diffuses EASILY and QUICKLY
Very
container
Definite
Definite
Definite
Somewhat
Not

16. States of Matter far Very shape container Definite volume Definite
SOLID
LIQUID
GAS
Molecules _________ close
Molecules CLOSE
Molecules _____ apart
________ shape
_________ volume
Takes shape of __________
________ volume
Takes ____________ of container
VERY RESTRICTED motion – rotation and vibration in place only
LIMITED freedom of motion – there is some degree of fluidity
FREE TO MOVE in all directions – high degree of fluidity
HIGH density
(typically measured in g/mL)
MEDIUM-HIGH density (less than that of solid EXCEPT for water!)
LOW density (typically measured in g/L)
______ compressible (incompressible)
_________ compressible
________compressed into smaller volumes
Does NOT expand much with increases in temperature
Expands SLIGHTLY with increases in temperature
HIGHLY expansive with increases in temperature (assuming the volume of the container can change!)
Diffusion SO SLOW you can hardly notice it – must ramp temperature up really high to facilitate diffusion
Diffuses EASILY but less rapidly than the gaseous state
Diffuses EASILY and QUICKLY
far
Very
shape
container
Definite
volume
Definite
Definite
Easily
Not
Somewhat

17. Example Problem GAS A student determined that the
SOLID
LIQUID
GAS
Molecules _________ close
Molecules CLOSE
Molecules _____ apart
________ shape
_________ volume
Takes shape of __________
________ volume
Takes shape of ___________
Takes volume of ___________
VERY RESTRICTED motion – rotation and vibration in place only
LIMITED freedom of motion – there is some degree of fluidity
FREE TO MOVE in all directions – high degree of fluidity
HIGH density
(typically measured in g/mL)
MEDIUM-HIGH density (less than that of solid EXCEPT for water!)
LOW density (typically measured in g/L)
______ compressible (incompressible)
_________ compressible
________compressed into smaller volumes
Does NOT expand much with increases in temperature
Expands SLIGHTLY with increases in temperature
HIGHLY expansive with increases in temperature (assuming the volume of the container can change!)
Diffusion SO SLOW you can hardly notice it – must ramp temperature up really high to facilitate diffusion
Diffuses EASILY but less rapidly than the gaseous state
Diffuses EASILY and QUICKLY
A student determined that the
substance he was working with took the
shape of its container, had molecules
that moved fast and were very far apart.
He also determined that the substance
was easily compressed into a smaller
container.
GAS

18. -the process of absorbing or releasing energy to
PHASE CHANGES
-the process of absorbing or releasing energy to
change from one phase to another phase
The types of phase changes include…
____________: liquid changing to vapor(boiling)
liquid + energy  vapor (gas)
______________: vapor changing to liquid
vapor  liquid + energy
___________: solid changing to liquid
solid + energy  liquid
______________: liquid changing to solid
liquid  solid + energy
_______________: solid changing directly to vapor without going through the liquid phase
solid + energy  vapor
_______________: vapor changing directly to solid without going through the liquid phase
vapor  solid + energy
Vaporization
Condensation
Melting
Freezing
Sublimation
Deposition

19. You will notice that all of the phase changes above either required an input of energy or they released energy. Each phase change is either:
Exothermic:   or
Endothermic:  
Example 3-7. Which phase changes are exothermic?   
Example 3-8. Which phase changes are endothermic?
A process that releases heat (heat exits the system)
A process that takes in heat (heat enters the system)
Condensation, Freezing, Deposition
Melting, vaporization, sublimation

20. Thank you for entering the magical world of matter!!