State 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
• 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)-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 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)