States of matter

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

3. EXAMPLES OF SOLID
ARRANGEMENT
• Crystalline – orderly 3 dimensional arranged particles in
repeating patterns of rows
• Ex; ice, diamonds, iron
• 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
• Ex. Corn syrup in our last lab

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)-units psi
• **Compression – a property unique to a gas, the ability
to squeeze or compress a gas into a smaller space

8. PLASMA
• Hot ionized (charged electrons) gas that can conduct
electricity
• Lightening is plasma, stars are plasma

9. NEED ENERGY TO CHANGE 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
(endothermic) or remove (exothermic) ENERGY

10. 1. melting - (solid to liquid) molecules speed
up(endothermic – add energy)
2. freezing (liquid to a solid) the particles of
matter begin to lock in place (exothermic -
Removing energy )
3. evaporation – (liquid to gas) at the surface
below the matters boiling point energy must
be added - endothermic

11. 4. condensation – (gas to liquid) particles must
clump together energy must be removed -
exothermic
5. sublimation – (solid directly to gas)
attraction must be completely overcome,
energy is added
•Boiling (not a change of state)– (liquid to
vapor or gas) pressure inside the bubble is
equal to the pressure on the outside of the
bubble – boiling point is same position as
evaporation and condensation points on
graph

12. • When substances lose or gain energy either
the temperature changes or the state
changes
• temperature is the speed the particles are
moving: average kinetic energy
• 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/evaporation/condensation point
• 100 °C , 212 °F or 373 K
• Freezing/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)