Matter & Energy
States of Matter
 Solid Definite volume and shape
 Particles are tightly packed
 Slight expansion when heated
 Incompressible
Solid
Vibration
around fixed
points
States of Matter
 Liquid Has definite volume, but no definite
shape
(assumes the shape of the container)
 Particles are loosely packed
(can flow by sliding over each other)
 Easily expand when heated
 Considered incompressible
Liquid
Vibration
around
sliding
points
States of Matter
 Gas No definite shape or volume
 Expand to fill the container
 Particles are spaced far apart
 Compressible
Gas
Vibration
around
moving
points
States of Matter
 Plasma Consists of electrically charged
particles
 It’s an ionized gas
 Common in space, but very rare on
Earth
 Found in lightning, fluorescent lights
and neon signs
Plasma
When atoms
are so hot,
they lose ALL
of their
electrons.
“Super-heated
Gas”
Energy Amounts in States of Matter
 Solid- little energy, particles vibrate and
rotate
 Liquid- more energy, they move freely
by sliding over each other
 Gas- even more energy, move quickly
 Plasma- most energy, move extremely
fast
All You Really Need To Know
You Can Learn From Noah's Ark
 5. Plan ahead. It wasn't raining when
Noah built the ark.
 6. Build your future on high ground.
Solid
Made of
Atoms
Holds
its shape
Atoms move
past each
other
Liquid
Gas
Plasma
States of Matter
Changes of State
Energy
Gas
Energy
Liquid
Energy
Solid
Names of Phase Changes






Solid to Liquid
Liquid to Gas
Gas to Liquid
Liquid to Solid
Solid to Gas
Gas to Solid
=
=
=
=
=
=
Melting
Boiling/evaporation
Condensation
Freezing
Sublimation
Deposition
D
e
p
o
s
i
t
i
o
n
Boiling
Melting
Condensation
Freezing
Sublimation
When a solid
turns directly
into a gas.
Dry ice is
solid CO2
MATTER, Definition, States, and
Change of State
Lets see if you can:
1. Define matter
2. Define the various states of matter and
draw an example of each state
3. Recognize that particle motion
determines the state of matter
States of Matter
List the Location of Each
Change of State
Melting
Condensation
Boiling
Energy
Gas
Energy
Liquid
Energy
Solid
Deposition
Freezing
Sublimation
List the Location of Each
Enthapy Used to Change State
Heat of
Fusion
Heat of
Vaporization
Energy
Gas
Energy
Liquid
Energy
Solid
Endothermic 
Exothermic
Heating Curve for Water
120
T
e
m
p
.(
C)
Steam
Water and
Steam
100
80
60
Water
40
20
0
Ice
Water
and Ice
-20
0
40
120
220
Energy (calorie)
760
800
Heating Curve for Water
120
Steam
Water and
Steam
100
80
60
Water
40
20
Ice andWater
Ice Water and Ice
0
-20
0
40
120
220
760
800
Heating Curve for Water
120
BothWater
Water
and
Steam
and Steam
100
80
Steam
60
Water
40
20
0
Ice
Water
and Ice
-20
0
40
120
220
760
800
Heating Curve for Water
120
Water
and
Heat
of
Steam
Vaporization
100
80
Steam
60
Water
40
20
Heat ofWater
and Ice
Ice Fusion
0
-20
0
40
120
220
760
800
Heating Curve for Water
120
Steam
Steam
Water and
Steam
100
80
Water
60
Water
40
20
0
-20
Ice
Ice
0
40
Slope =
Specific Heat
Water
and Ice
120
220
760
800
Moisture that collects on the
outside of a cold glass results
from the process of…
1. evaporation.
2. condensation.
3. sublimation.
4. vaporization.
Matter,
Specific Heat of Matter
At the conclusion of our time
together, you should be able to:
1. Define specific heat
2. Use specific heat to determine energy
changes
Thermochemistry
 Some Definitions:
 Calorimeter – a device to measure the
energy absorbed or released as heat
in a chemical or physical change
 Temperature – measure of the
average kinetic energy of the particles
in a sample of matter
 Joule – the SI unit of heat
Thermochemistry
 Some Definitions:
 Heat – energy transferred between
samples of matter
 Specific Heat – the amount of energy
required to raise the temperature of
one gram of a substance by one
Celsius degree or one Kelvin
 1 Calorie/4.184 Joules – will do the
above with water
Thermochemistry
 Some Definitions:
 Enthalpy (Heat) of Fusion – amount of
energy gained or lost by a system as
heat during melting or freezing
 Enthalpy (Heat) of Vaporization –
amount of energy gained or lost by a
system as heat during boiling or
condensation
Specific Heat Calculations:
 q = cp x m x t:
 q
= energy lost or gained
 cp
= specific heat of the substance
at a specific pressure
 m
= mass of the sample
 t = change in temperature
(final – initial)
Practice #1
 q = cp x
 q
=
 cp
=
 m
=
 t =
59.912 J
m x t:
59.912 J
x
36.359 g
152.0 oC
= (x)(36.359 g)(152.0 oC)
= 0.01084 J/g oC
Practice #2
 q = cp x m x t:
 q
= -800. J
 cp
= 0.4210 J/g oC
 m
= 73.174 g
 t = (x – 102.0 oC)
-800. J = 0.4210 J/goC (73.174 g)(x – 102.0
oC)
-800. = 30.81x – 3142
2342 = 30.81x
= 76.0 oC
Matter,
Specific Heat of Matter
Let’s see if you can :
1. Define specific heat
2. Use specific heat to determine energy
changes
Define Specific Heat
 Specific Heat – the amount of energy
required to raise the temperature of
one gram of a substance by one
Celsius degree or one Kelvin
Practice #3
 q = cp
 q
 cp
 m
 t
-185.4
-185.4
x m x t:
= -185.4 J
= 0.440 J/g oC
=xg
= -1475 oC
J = (0.440 J/goC )(x)(-1475 oC)
J = -649 Jg
= 0.29 g
Practice #4
 q = cp x m x t:
 q
=xJ
 cp
= 0.0335 cal/goC (4.184 J/cal)
 m
= 152.00 g
 t = -51.5oC
x = (0.140164 J/goC )(152.00 g)(-51.5 oC)
= -1.10 x 103 J