the structure of the matter

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
Ex. H2O
H2 Not water
O Not water
O
H H

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. States of Matter
State Definite Shape Definite Volume
Solid
Liquid
Gas No
Yes
Yes Yes
No
No
Solid Liquid Gas
http://www.harcourtschool.com/activity/states_of_matter/index.html

7. http://www.juliethompson.com/science.html

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

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

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

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. 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 No
Yes
Yes Yes
No
No

22. 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
Ex. Balloon
(All that moving and colliding into
things causes a force to be applied)
Pressure- The amount of force
applied to a unit of area

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. Absolute Zero -
-The Temperature at which particles of
matter stop moving -273 o
C
-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
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
1000 .
5 = 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
http://www.delta.edu/slime/cancrush.html

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

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

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

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

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

38. 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 o
C
Salt = 801 o
C
Sugar = 186 o
C
Water = 0 o
C

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

40. 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 100o
C

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