The document discusses the states of matter—solid, liquid, and gas—and their properties based on the kinetic molecular theory. It explains how temperature affects the physical condition of substances, detailing phase changes such as melting, evaporation, and solidification. Key concepts include diffusion, Brownian motion, and the relationship between particle energy and state changes.

1. St
ates
of matter
and the kinetic
molecular theory

2. Matter
is anything that has mass and
takes up space. (Like you!)
3 phases:
Most of the matter in our
world can be found in
Solid
Liquid
Gas

3. of solids
Properties
Solids are in a fixed form that
can only change by denting,
breaking or bending it.
Solids are hard.
High density.
Can not be compressed.
Can not flow, except when it is
in small pieces.
Has a fixed volume.

4. of liquids
Properties
Liquids have no fixed form – it
takes the shape of the
container.
Not hard.
High density.
Cannot be visibly compressed.
Can flow.
Has a fixed volume.

5. of gases
Properties
Gases have no fixed form – it
takes the shape of the
container.
Not hard.
Low density.
Can easily be compressed.
Can flow.
Does not have a fixed volume.

6. Matter consists of
particles.
This is proven when you look at DIFFUSION.
Diffusion
The movement of particles from a high
concentration to a low concentration.
Diffusion is the result of constant motion of particles.

7. Brownian motion
Particles make strange jerky, zig-zag motions;
as if they vibrate by themselves.
However, it is caused by the collisions between
particles.

8. The physical condition of a substance
depends on the temperature, which is
measured with a thermometer in degrees
Celsius.
There are two fixed points on a
thermometer: The freezing point of water
(0 °C) and the boiling point of water
(100°C).

9. Freezing point
Melting point
Boiling point
Temperature
Temperature
Temperature
at which
at which a
at which solid
liquid is
liquid turns
is turned to liquid.
turned to solid.
to a gas.

10. Determining
the physical
Condition of a
subst
ance
If room
temperature is
more than the
boiling point, it is a
gas.
If room
temperature is less
than the melting
point, it is a solid.
If the melting point
is less than room
temperature, which
is in turn less than
the boiling point, it
is a liquid.

11. State Changes
Solid → Liquid
Melting
Solid → Gas
Sublimation
Liquid → Gas
Evaporation
Liquid → Solid
Solidification
Gas → Liquid
Condensation
Gas → Solid
Sublimation
Heating
Cooling

12. Particles are not in a
Mel
ting
fixed position, but
Melting point:
Particles vibrate strong enough to
slide over
overcome intermolecular forces.
each
For a solid to melt, E
of particles
other.
must be enough to overcome
●
●
kinetic
intermolecular forces.
Solid
On heating,
heat energy is absorbed.
●E
is converted into Ekinetic –
heat
●
particles move more violently.
Liquid

13. solidification
Liquid
When a
liquid cools, energy
of particles are
given off, particles
lose Ekinetic, and
move slower.
Solid
Intermolecular
forces at the point
of solidification
increase. The
particles do not
have enough
energy to move
around freely.
Particles can
only vibrate
around a
fixed
position,
forming a
solid.

14. Boiling
Evaporation
Only occurs at boiling
point
Occurs at a lower
temperature than boiling
point
Occurs throughout the
liquid
Only occurs on the
surface
Happens quickly
Happens slowly
Temperature remains
constant during boiling
Causes cooling because
heat is absorbed out of
the environment

15. G
as
Heating curve
Boiling
Liq
ui d
Melting point
Melting
So
lid
Temperature
Boiling point
Time

16. Slide 2:
Solid – iheartsportsgifs.tumblr.com
Liquid – aspworldtour.tumblr.com
Gas – rebloggy.com
All other diagrams drawn by author.
Slide 7:
duckingsciencebombs.wordpress.com

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