 Solid
 Liquid
 Gas
 Plasma
 Solid
 Liquid
 Gas
 Plasma
 How
are temperature and kinetic energy
related?
In other words…
 All matter is made of tiny particles (atoms) in
constant motion


How MUCH they move depends on how much energy
they have
Increased temperature will…




Increase kinetic energy= more movement
Decrease kintetic energy = less movement
So higher KE= higher temp
So lower KE = lower temp
 Almost
all matter expands as it gets hotter
and contracts when it cools.


Temperature is a measure of the average kinetic
energy of the particles in the object
Theoretically, absolute 0, (0 degrees Kelvin) has
no movement of particles

Never achieved in a lab
 Definite
Shape and
Volume

Solids are USUALLY
the most dense


There is one
IMPORTANT exceptionWATER!
How do you know?
 Usually

less dense than solids
Because they have more KE than solids and the
particles can spread out more
 Definite

Volume
Can’t normally be squeezed into a smaller space
 Indefinite

Shape
Flow and take shape of container
 Least

Because they have the most KE than and the
particles can spread out even more
 No

dense state of matter
definite shape or volume
Molecules can be squeezed together or spread
out to fill the space available

Ex. pumping up a bicycle tire
A plasma is a gaslike mixture of + and –
charged particles (ionized matter)
A plasma is a very good conductor of
electricity
ex. Fluorescent lights, stars
Plasma, like gases have an indefinite
shape and an indefinite volume.
Chumbler - Properties of Matter
13
 Energy
is RELEASED from the substance out to
its surroundings

Ex’s- each of these products have molecules with
LESS energy than they did before the phase change



Freezing (liquid water has more energy than ice)
Condensation (gas to liquid)
Deposition (gas to solid)
 Energy
is ABSORBED by the substance from its
surroundings

Ex’s- each of these products have molecules with MORE
energy than they did before the phase change



Melting (ice has less energy than water)
Evaporation (liquid gas)
Sublimation (solid gas))
 Attractive
Forces
 Kinetic Energy Forces
 The



force between two molecules
Holds them together weakly
Not as strong as “real bonds” (ionic, covalent)
Stronger in a solid than liquid, etc.
 The
more particles move, the more they will
spread out
 The
state a substance depends on which
force is greater


The kinetic energy of the particles
OR
The strength of the attractions between the
particles (attraction force)
Energy required to change a solid
at its melting point to a liquid is
equal to the energy released from
the particles when a liquid is
changed to a solid!
A
substance changes state when enough KE
has been added to break the attractive
forces and allow the molecules to spread
out.
 Explain
what is happening between the
forces when a state changes on a cooling
curve.
 (ex-
liquid to solid)
 The
heat added to the system at the melting
and boiling points goes into breaking the
attractive forces. (not to speeding up the
particles (KE))
 Therefore the temperature of the
substance does not
rise during the
phase change.
 heating
curve of water animation
 The
total energy absorbed in the
heating curve is equal to the total
energy released in the cooling curve of
water


Melting/freezing pt: occur at same temperature
Boiling/condensation pt: occur at same
temperature
 They
are EQUAL!
 Explain
what happens when a cold glass of
water “sweats”
Condensation - gas to liquid
Water particles in the air have more kinetic energy
(heat) than the glass of water. As water particles get
close to the glass, energy is transferred from the
particles to the glass. This starts the following
process…
a. Particles lose kinetic energy, slow down, and come
closer together.
b. IF’s become strong enough to make particles
merely rotate around each other.
c. The energy they lose to turn into a liquid is the heat
of vaporization.
d. Substance is releasing energy to the surroundings
(exothermic)
 Explain
what happens when liquid water
changes to ice.
Freezing - liquid to solid-.
a. Particles lose kinetic energy & slow down.
b. Substance releases energy to
surrounding (exothermic)
c. Attractive forces b/w particles become
stronger than the particles’ motion, so the
particles begin merely vibrating in place to
form a solid.
d. The amount of heat the particles must
lose to turn into a solid is called the heat of
fusion.
 Name
the process
described and then
determine if it is
exothermic or
endothermic
0%
1.
9%
2.
83%
3.
9%
4.
0%
5.
Sublimation, Exothermic
Condensation, Exothermic
Evaporation, Endothermic
Sublimation, Endothermic
Condensation, Endothermic
4%
1.
65%
2.
0%
3.
0%
4.
30%
5.
Sublimation, Exothermic
Condensation, Exothermic
Evaporation, Endothermic
Sublimation, Endothermic
Condensation, Endothermic
18%
1.
0%
2.
0%
3.
77%
4.
5%
5.
Sublimation, Exothermic
Condensation, Exothermic
Evaporation, Endothermic
Sublimation, Endothermic
Condensation, Endothermic
Heating
Cooling
Both of the above
None of the above
1.
2.
3.
4.
0%
10
Heating
Cooling
Both of the above
None of the above
1
2
3
4
5
6
7
8
21
22
23
24
25
26
27
28
9
10
11
12
13
14
15
16
17
18
19
20
IF are breaking
IF are being created
(forming)
The phase change is
increasing the temp
None of the above
0%1.
2.
0%
3.
0%
0%4.
e
T
e
m
p
p a
d
c
b
Time (min)
10
1
2
3
4
5
6
7
8
21
22
23
24
25
26
27
28
9
10
11
12
13
14
15
16
17
18
19
20
0%
1.
0%
2.
0%
3.
0%
4.
Exothermic and a chemical change
Endothermic and a physical change
endothermic and a chemical change
Exothermic and a physical change
10
1
2
3
4
5
6
7
8
21
22
23
24
25
26
27
28
9
10
11
12
13
14
15
16
17
18
19
20
0%
1.
0%
2.
0%
3.
0%
4.
Solid to liquid
Solid to gas
Liquid to gas
Gas to liquid
1
2
3
4
5
6
7
8
21
22
23
24
25
26
27
28
9
10
10
11
12
13
14
15
16
17
18
19
20
10
Gas
Liquid
Solid
plasma
0%
qu
i
2
3
4
5
6
7
8
21
22
23
24
25
26
27
28
9
10
0%
pl
Li
G
1
0%
d
as
0%
a
4.
as
m
3.
lid
2.
So
1.
11
12
13
14
15
16
17
18
19
20
Gas
Liquid
Solid
plasma
Li
G
1
2
3
4
5
6
7
8
21
22
23
24
25
26
27
28
9
10
11
0%
d
as
10
qu
i
0 of 28
0%
12
13
0%
a
0%
as
m
4.
pl
3.
ol
id
2.
S
1.
14
15
16
17
18
19
20
 Why
are there 2 portions of the phase change curve
in which the temperature is not increasing? (the
water is not removed from the heat source during
any portion of time)
0%
1.
0%
2.
0%
3.
0%
4.
Ice stage
Water + ice stage
Water stage
Water vapor stage
10
0 of 28
0%
1.
0%
2.
0%
3.
0%
4.
Thermal energy
Kinetic theory
Law of conservation of mass
Law of conservation of motion
10
0 of 28
 Contains
H bonds (which are not actually
bonds, but strong Intermolecular forces)
 Gives water special properties like…
 Surface
Tension!
 Density
special!
of ice is