1. Warm Up
How do the arrangement and behavior of particles of matter differ in solids, liquids, and gases?

2. Classification of Matter
Unit 3 Matter/Change
Classification of Matter

3. What is matter?
Has a mass
Takes up space

4. States of Matter Solid Has a rigid, definite shape
The atoms, ions, or molecules that make up a solid are fixed in place

5. States of Matter Liquid Has an indefinite shape
Is flowing matter with definite volume
Takes the shape of its container
Particles of a liquid can move and easily glide over each other

6. States of Matter Gas Has no definite shape Has no definite volume
Is compressible matter
Particles of gas are much farther apart and are easily pushed together

7. Matter Pure Substance Mixtures Compound Homogeneous Heterogeneous
Uniform/Definite composition
One Chemical Formula
2 or more substances physically combined
Compound
Homogeneous
Heterogeneous
Element
Not uniform through out.
One type of atom
Found on Period Table
2 or more elements
chemically combined
Solutions
Uniform throughout

8. Physical/Chemical Changes
Matter/Change
Physical/Chemical Changes

9. Physical Property
Characteristics that a sample of matter exhibits WITHOUT any change to its identity.

10. New Substance Physical Change
A change that does not produce a new substance!
New
Substance

11. Examples: Solubility Melting/Boiling Point Phase Change
Size/Shape Change
It’s Color (not change in)
Density
Electrical Conductivity
Physical State (solid, Liquid, or gas)

12. Physical Property Extensive Intensive
Depends on amount of matter present
Mass
Volume
Intensive
Does not depend on the amount of matter present
Color
Phase
Density (mass/volume)

13. Chemical Property
Only observed when there is a change in the composition of the substance
Ability of a substance to react with other substances or to decompose.

14. Chemical Change
A change that does produce a new substance (chemical reaction)

15. Physical vs. Chemical Changes
“Can the change be reversed?”
If yes: probably physical.
If no, probably chemical.
Example: Milk goes sour.
Can the change be reversed? NO.
You cannot get the milk to taste good again. So it is a chemical change. Note that a new substance (lactic acid) has been produced. This acid is formed when bacteria break down the lactose in the milk.
Example: An ice cube melts.
Can the change be reversed? YES.
Just put the water back in the freezer. Note that no new substance is produced. Phase changes (changes between states of matter—solid, liquid, gas) are NOT chemical changes!
This rule is not perfect; it is just meant as a guide.

16. Chemical Change-Look for:
Formation of a gas (odor)
Light produced
Formation of precipitate
Change in temperature
(gets hot—exothermic* or cold—endothermic**)
Permanent Change in color

17. Energy Law of Conservation of Matter
Matter/Change
Energy
Law of Conservation of Matter

18. Law of Conservation of Mass (Matter)
Matter can be neither created nor destroyed.
Original atoms in reactants may move around, but will be found on the product side.

19. How many atoms of carbon are on the reactant side?
Don’t need to write!
How many atoms of carbon are on the reactant side?
On the product side?
How many H on the reactant side?
How many O on the reactant side? 6 6 12 12 18 18

20. The mass of the reactants must equal the mass of the products!!
Reactants = Products
372g = g

21. Exothermic
The chemical reaction releases heat energy to the surroundings.

22. Endothermic
The chemical reaction absorbs heat energy from the surroundings.

23. Energy Changes
What is energy?
The capacity to do work.

24. Two Types of Energy Potential Energy of position.
Stored energy in bonds of molecules.

25. Example
Gasoline stored at a gas station

26. Two types of energy
Kinetic
Energy in motion

27. Example
Moving cars as they go down the road. As the gasoline is burned, energy is released from the bonds and is used to power the car’s engine.

28. Energy Conversions Law of Conservation of Energy
Energy can be converted from one form to another, but it is not created or destroyed.

29. Energy can exist in these forms:
Radiant: light energy
sunlight
Chemical: stored in bonds of molecules
Fuels, food
Nuclear: stored within the nucleus of atoms
Electrical: Flowing electrons in a current.

30. Energy can exist in these forms:
Mechanical: moving machine parts or body
(you can think of your
body as a machine too)
Thermal: heat
Friction causes machine parts to heat up

31. Thermal Energy
Can be transported via 3 possible pathways

32. Convection
The transfer of heat energy in a gas or liquid (not in solids) by movement of currents.
The heat move with the fluid.
Example
The beach – hot air rises, cooler air from the ocean comes into replace it, and then the cool breeze cools your body.

33. Conduction
The transfer of heat energy through matter from particle to particle.
Material are actually touching!
Most effective in solids, but can happen in fluids.
Example
Beaker on a hot plate becomes warmer because the heat from the hot plate is conducted along the beaker.

34. Radiation The transfer of heat energy by electromagnetic waves Example
Only form that can occur in empty space without the aid of Solids, Liquids, or Gases
Example
Sunlight –travels through space via radiation.

35. What is the way that thermal energy is transported in the following?
Your leg becomes warn when you place a heating pad on it.
Conduction

36. What is the way that thermal energy is transported in the following?
The pilot light in your car illuminates a map.
Radiation

37. What is the way that thermal energy is transported in the following?
Hot soup transfers heat to the air above it.
Convection

38. The various forms of energy can be converted into one another
Radiant E: Sunlight
Chemical E: glucose produced in plants via photosynthesis
Mechanical E: rabbit eats plant and metabolizes them to release energy for hopping.

39. Try this one:
Trace the conversion of energy from sunlight to a person riding a bicycle.
radiant E:
chemical E:
mechanical E: