States of matter

2. Solid Liquid Gas
Melting Point Boiling Point

3.  Melting Point
The TEMPERATURE where a solid
changes to a liquid
 Boiling Point
The TEMPERATURE where a liquid
changes to a gas

4.  Dew Point
• The TEMPERATURE where a gas
changes to a liquid
• Dew Point = Boiling Point
 Freezing Point
• The TEMPERATURE where a
liquid turns to a solid
• Freezing Point = Melting Point

5. Liquid
Melting Point
-117°C
Boiling Point
78°C
By 35°C?
Determine the physical state of Ethanol

6. Melting Point
27°C
Boiling Point
677°C
By 25°C?
Solid
Determine the physical state of Francium

7. Melting Point
17°C
Boiling Point
37°C
By 40°C?
Determine the physical state of substance C
Gas

8.  Fixed Form
 Hard
 High Density
 Incompressible
 Cannot Flow
 Fixed Volume
 Melting point is higher
than room temperature

9.  Takes shape of container(does
not have a fixed form)
 Not hard
 High Density
 Mostly Incompressible
 Can flow
 Fixed Volume
 Melting point is higher
than room temperature

10.  Takes shape of container (do
not have a fixed form)
 Not hard
 Low Density
 Compressible
 Can flow
 Not a fixed volume (fills
entire container)
 Boiling point is lower than
room temperature

11. Gas
SolidLiquid

12. 1) All substances consists of small particles
2) Particles are continuously moving
3) There are spaces between particles
4) Particles collide with each other continuously
5) Kinetic energy of the particles is proportional
to the temperature of the substances
• Hotter is Faster
6) There exists attractive and repulsive forces
between particles
7) Phase changes takes place when particles gain
or loose enough energy to overcome
intermolecular forces
• Particles rearrange

13.  Small spaces between
particles
 Particles have little
kinetic energy
 Particles only vibrate in
one place
 Strong attractive forces
between particles

14.  Bigger spaces between
particles than in solids
 Particles have moderate
energy
 Particles move freely in
various directions
 Moderate attraction forces
between particles

15.  Big spaces between
particles
 Particles have lots of energy
 Particles move fast and
freely in all directions
 Weak forces between
particles
 Repulsive forces increase
with compression

16. The spontaneous movement of liquids and gasses
from a high concentration to a low concentration
 Spontaneous
 Spaces between
particles
 Particles move into the
open spaces because
they are always moving

17. The random motion of bigger partcles caused by
collisions with the smaller particles of the
substance in which it is suspended

18. Solid
Liquid
 Upon heating particle absorb
energy
• Particles move faster and
further apart
 At the melting point particles
have enough energy to overcome
intermolecular forces
• Particles “break loose”,
rearrange and forms a liquid

19. Solid
Liquid
 Upon cooling particles loose energy
• Particles move slower and further
apart
 Attraction forces between particles
increase
 At freeze point particles do not have
enough energy to resist
intermolecular forces
• Particles can no longer move
around freely and forms a solid

20. Liquid
Gas
 Upon heating particles absorb
energy
• Particles move faster and
further apart
 At boiling point the particles have
enough energy to overcome
intermolecular forces
• Particles start to rearrange,
moving fast in all diractions
and forming a gas.

21. Liquid
Gas
 Change from a liquid to a gas ate
temperatures other than the
boiling point
 Some particles have enough
energy to overcome
intermolecular forces
• Particles move away from the
other particles and forms a gas
 Volatile substances
• Substances that evaporate
spontaneously at room
temperature

22. Boiling Evaporation
Boiling point Any temperature
Throughout liquid
Only at the top layer of
the liquid
Fast Takes a long time
Temperature remains
constant
Temperature decrease:
particles absorb energy
from rest of liquid

23. Gas
Solid
 Change of a solid directly to a gas,
without first changing to a liquid
 Particles in a solid has enough
energy to change directly to a gas
 Substances that sublimate:
• Iodine, Carbon dioxide
 Change of a gas directly to a solid
is called DEPOSITION

24. Temperature
Time
Melting
Boiling
Condensation
Freezing

25.  During Heating
• Particles absorb energy
• Particles start to move faster and further apart
(average kinetic energy increases)
 During a Phase Change
• Particles have enough kinetic energy for a phase
change to occur
• The average kinetic energy (and therefore also
the temperature) remains constant
• All additional heat energy is used do overcome
intermolecular forces (average potential energy
increases)

26.  During Cooling
• Partilcles loose energy
• Particles start to move slower and closer together
• Intermolecular forces increase
 During Phase Change
• Intermolecular forces are strong enough to cause
a phase change to occur
• The average kinetic energy (and therefore also
the temperature) remains constant
• Average potential energy decrease