States of Matter
3 States of Matter

Solids
Most Dense
 _____________________________________

Liquids
 ______________________________________

Gases
 ______________________________________
Least Dense
The 4th State of Matter

What happens if you raise the temperature to superhigh levels…between 1000°C and 1,000,000,000°C?
PLASMA!!



A plasma is an ionized gas.
A plasma is a very good conductor of electricity and is affected by magnetic
fields.
Plasma, like gases have an indefinite shape and an indefinite volume.
Nature of Gases


Minimal attractive forces between particles
Particles have lots of energy and move freely
Kinetic Molecular Theory:
= a model or theory used to describe the behavior of gases
1.) The particles in a gas are considered to be _________________________
__________________________________________________________
2.) The motion of the particles in a gas is ____________________________
__________________________________________________________
3.) All collisions between particles in a gas are perfectly elastic
 _________________________________________________________
_________________________________________________________
Gas Pressure

Gas pressure = _______________________________________
_______________________________________
**atmospheric pressure = ______________________
_______________________________
_______________________________
 measured with a barometer
 Units: kilopascal (kPa)
mmHg
atm
torr
1 atm = 101.3 kPa = 760 mmHg = 760 torr
Nature of Liquids

Particles are free to flow from one locations to another

BUT...
The particles are attracted to each other via intermolecular forces.
Nature of Solids



Particles are orderly and packed tightly together.
Particles vibrate in fixed positions only
Most solid substances are crystalline.
 _______________________________________________________
Phase Changes
Gas
Solid
Liquid
Temperature
Temperature = a measure of the average _________________ of particles
= _____________________
**At a given temperature, the particles of all substances, regardless of
physical state, have the same average kinetic energy.**
Kelvin Scale =_______________________________________________
 boiling point of water = ____ K
freezing pt of water = ____ K
Reference Tables:
 absolute zero = ____ K
- Table A (STP)
- Table T (degrees Celcius to Kelvin
Phase Changes: Heating Curve
***A substance will change phase from solid to liquid to gas when heat energy is added.**
Phase Changes: Cooling Curve
***A substance will change phase from gas to liquid to solid when heat energy is lost.**
Heating/Cooling Curve Combined
Vaporization

Vaporization = ___________________________________________
 Evaporation : __________________________________________
: __________________________________________
__________________________________________
: ___________________________________________

Vapor Pressure = _____________________________________________
**(Remember: gas particles collide with the walls of the sealed container)**
In a system at constant vapor pressure, a dynamic equilibrium exists
between the vapor and the liquid. The system is in equilibrium because
the rate of evaporation of liquid equals the rate of condensation of vapor.

Vapor Pressure & Temperature:
How will temperature affect vapor pressure?
______________________________________________
Why?
_______________________________________________
_______________________________________________
_______________________________________________
**The higher the vapor pressure of a substance, the
more volatile it is.
 volatility = ______________________________

Boiling Point =
______________________________________________________________
______________________________________________________________
______________________________________________________________
**Normal boiling point = boiling point of a substance at the standard
pressure of 101.3 kPa
Two factors affect the boiling point of a substance:
1.) Pressure
 ________________________________________________________
**Why does it take longer to cook food in water at high altitudes?**
2.) Intermolecular forces
 _________________________________________________________
Reference Tables: Table H