1. The Structure of Matter
Matter – Anything that has mass and takes up space
Mass – The amount of matter in
an object

2. Molecule – The smallest particle of a substance (such as water) that can still be identified as that substance
(Latin = little mass)
Ex. – 60 million H2O – diameter of a
penny

3. Ex. All water molecules are the same
-Once a molecule is divided it is no longer that substance
H Not water
O Not water
Ex. H2O

4. Physical & Chemical Properties of Matter
Physical Properties – A characteristic of matter that can be observed by using any of your senses
Ex. Hardness, density, melting pt. /
boiling pt., State (solid, liquid, gas)
Size, shape, color, odor, taste

5. Physical & Chemical Properties of Matter
Chemical Properties – A description of how one kind of matter behaves in the presence of another kind of matter.
Ex. Vinegar & baking soda
- When vinegar is added to baking soda, CO2 is produced

6. State Definite Shape Definite Volume Solid Liquid Gas
States of Matter
State Definite Shape Definite Volume
Solid
Liquid
Gas
Yes
Yes No
Yes No No
Solid Liquid Gas

8. Solid

9. Liquid

10. Gas

11. Plasma
Plasma- State of matter where gas molecules have separated into electrically charged particles
Ex. STARS (fusion)

12. Physical & Chemical Changes
Physical Change- a change in which the form or appearance of matter changes but not its composition
Ex. Shape – crumpled paper
Dissolving – Koolaid
Change in State

13. Physical Changes Solid Liquid Gas
Freezing
Melting
Condensation
Vaporization
Solid Liquid Gas
Deposition
Sublimation
- Only the MOTION of the molecules has changed!

14. Chemical Changes
Chemical Change – a change in which the composition of a substance changes
Ex. Fireworks, Rust
- causes a new substance to form.

16. Signs of Chemical Changes
- Color Changes
Ex. Trees, apples, toast
Released – fire – heat, light
Gained – cooking/cake
- Energy

17. Signs of Chemical Changes
- Odor
Ex. Rotten food
- Bubbles formed
Ex. Vinegar + Baking soda
Antacid

18. Signs of Chemical Changes
- Solid formed - Precipitate
Ex. Sodium iodide = lead nitrate
- Not easily reversed
Ex. Ice melting vs.
Wood burning
Chemical
Physical
VS.
HARD
EASY

19. Anton Lavoisier – 18th Century
The LAW of Conservation of Mass-
- States that mass is neither created nor destroyed
(and as a result, the mass of the substance before a physical or chemical change is equal to the mass of the substances present after the change)
Ex. Apple cut up, candle burning

20. The Kinetic Theory of Matter-
Gases
The Kinetic Theory of Matter-
- The scientific principal that says that all matter is made of particles whose MOTION determines if the matter is solid, liquid, or gas

21. -Each of the 3 states of matter is called a phase
State Definite Shape Definite Volume
Solid
Liquid
Gas
Yes
Yes No
Yes No No

22. - explained by the Kinetic theory of matter
4 Properties of Gases
- explained by the Kinetic theory of matter
1. Gas molecules move VERY FAST
-A gas is mostly empty space
(large distance between gas molecules)
-Particles collide MANY times per second
(particles are NOT affected by collisions)
- No definite shape, they expand to fill all available space

23. 2.Moving gas molecules cause pressure
Pressure- The amount of force applied to a unit of area
(All that moving and colliding into things causes a force to be applied)
Ex. Balloon

24. 3.Gases have NO definite volume
-can be crowded together
-This the pressure (more collisions)
-can be allowed to expand
-This the pressure (fewer collisions)

25. 4.The temperature of a gas measures how fast molecules move
Heat = in particle movement
(particles tend to move further apart)
- volume or the pressure
Ex. Bicycle tire on a hot day
- Heat = in particle movement

26. The Temperature at which particles of matter stop moving
Absolute Zero -
The Temperature at which particles of matter stop moving
-273 oC
No Kinetic Energy at absolute zero
Kelvin (K) Temperature scale -
A temperature scale on which zero is equal to absolute zero

27. GAS LAWS!
Boyle’s Law
Pressure = Volume
No Temperature change

28. V1 . P1 = V2 . P2
Ex. The air in a balloon occupies a space of 1000mL and has a pressure of 5 N/cm2. When Gary grabs the balloon the pressure increases to 10 N/cm2. What is the new volume of the balloon?
V1= V2=
P2= P2=

29. V1= 1000mL V2= ? mL
P1= 5 N/cm2 P2=10N/cm2
= V2 . 10
V1 . P1 = V2 . P2
5000 = V2 . 10
5000 = V2 . 10
10 = 10
500 = V2
V2 = 500 mL

30. GAS LAWS! Charle’s Law Temperature = Volume Temperature= Volume
V1 . T2 = V2 . T1

31. Charle’s Law V1 . T2 = V2 . T1 V1= V2= T2= T1= 30mL ? mL 10oC 30oC

32. Charle’s Law V1 . T2 = V2 . T1 30 . 30 = V2 . 10 900 = V2 . 10 10 10
30oC
10oC
? mL
30mL
V1 . T2 = V2 . T1
V1= V2=
T2= T1=
30mL
? mL
30oC
10oC
= V2 . 10
900 = V2 . 10
V2 = 90mL
90 = V2

33. Solids- A piece of solid matter cannot change shape by itself
Solids & Liquids
Solids- A piece of solid matter cannot change shape by itself
(the molecules stay in a fixed patteren)
Ex. crystal

34. -Almost all solids are made of crystals
Crystal- A solid whose orderly arrangement of particles gives it a regular shape
-Almost all solids are made of crystals
- The shape (of the crystal) is determined by the way the particles are arranged
Ex. salt
(different crystals break in different ways)

35. -Almost all solids are made of crystals
Super cooled liquids- Solids that have been cooled soooooo quickly that they have NO crystal pattern
-Almost all solids are made of crystals
Ex. Volcanic glass

36. -Can flow (change shape)
Liquids- molecules (can move from one place to another) have NO fixed pattern.
-Can flow (change shape)
- when not moving it will have a level surface

37. -Heat is added (to a solid)
Change to a Liquid
-Heat is added (to a solid)
- Motion / Temp
- particles can’t stay in crystal pattern

38. Melting point- the temperature at which a solid becomes a liquid
Change to a Liquid
Melting point- the temperature at which a solid becomes a liquid
- each crystalline solid has its own melting point
Mercury = -39 oC
Salt = 801 oC
Sugar = 186 oC
Water = 0 oC

39. Change to a Liquid
Heat of fusion- the amount of heat required to change 1 gram of solid to a liquid
(at the same temp
no temp change)
- the energy used to break the crystalline structure

40. - Changing from a Solid Gas
Sublimation
- Changing from a Solid Gas
Ex. Dry ice

41. Change to a Gas
- In most liquids (at ordinary Temps.) Some molecules have enough energy to (escape and) become a gas
Ex. Water evaporation
Heat = evaporation

42. Boiling point –The Temp (at ordinary pressure) at which the molecules of a liquid have enough energy to become a gas

43. Exact boiling point depends on:
1. Energy needed to make particles separate
2. Pressure of the air
pressure = boiling point
pressure = boiling point
- Water (at normal pressure) will never be hotter than 100oC

44. The amount of heat required to change 1 gram of liquid to a gas
Heat of Vaporization-
The amount of heat required to change 1 gram of liquid to a gas
(No temperature change)