1. States of Matter
• States of Matter – physical forms that
substances can exist in
• Matter is composed of atoms and
molecules that are always in motion
bumping into each other, this activity
determines the state of the matter

2. Solids
• Particles of solids do not move fast
enough to over come the strong attraction
between them, therefore, they are close
together and vibrate in place
• Solids have a definite shape and volume
• Crystalline – orderly 3 dimensional
arranged particles in repeating patterns of
rows
• Ex; ice, diamonds, iron

3. • Amorphous – no special arrangement or
pattern
• Ex; rubber, wax

4. Liquids
• Particles of a liquid move fast enough to
over come some of the attraction between
the particles, therefore, the particles are
close together but can slide past each
other
• Can change shape but not volume, liquids
take the shape of the container they are in

5. Properties specific to liquids
• Surface tension – force that acts on the surface
of liquids and that tends to minimize the area of
the surface
• Different liquids have different surface tensions
• Ex: water has high surface tension and forms
spheres, gasoline has low surface tension and
forms flat drops
• Viscosity – resistance of liquids to flow because
of the attraction of the molecules in the
liquid, stronger the attraction, the greater the
viscosity

6. Gases
• Particles of a gas move fast enough to over
come almost all of the attraction between
them, therefore, the particles are far apart and
move independently of each other (empty space
between them)
• Gases change shape and volume
• Gases can expand and shrink depending on the
space they are put in
• Volume of a gas depends on the container the
gas is in

7. • Pressure - is the force exerted on a given
area of surface (the number of times the
particles of gas hit the inside of the
container)-psi units
• Compression – a property of a gas, the
ability to squeeze or compress a gas into a
smaller space

8. Plasma
• Hot ionized (atoms are positively charges
and share space with free negatively
charged electrons) gas that can conduct
electricity
• Lightening is plasma, stars are plasma

9. Changes of state
• All changes of state are physical changes
• All states of matter have energy (solids
less energy, gases more energy)
• To change the state of matter, you must
add or remove energy
• Adding energy – (solid to liquid) melting
point is the point where added energy
allows the molecules to over come their
attraction to each other (endothermic)

10. • Removing energy (liquid to a solid) freezing
point is the point where molecules being to
overcome movement and the particles of matter
lock in place (exothermic)
• Evaporation – (liquid to gas) at the surface
below the matters boiling point
• Boiling – (liquid to vapor or gas) pressure inside
the bubble is equal to the pressure on the
outside of the bubble – boiling point

11. • Condensation – (gas to liquid) particles
must clump together when the attraction
between the particles over comes
movement, energy must be removed
• Sublimation – (solid directly to gas)
attraction must be completely
overcome, energy is added

12. • When substances lose or gain energy either the
temperature changes or the state changes
• temperature is related to the speed the particles
are moving
• When temperature changes, the speed of the
particles changes, causing a change in state
• Temperature change doesn’t happen until the
change of state is complete

13. Temperature Change of H2O
• Boiling Point/evaporation/condensation
• 100 C , 212 F or 373 K
• Freezing point/melting point
• 0 C , 32 F or 273 K
• Absolute Zero – point at which all matter stops
moving and time no longer affects the matter
(0 Kelvin, -273.15 C, -459.67 F)