P6 - Molecules And Matter Flashcards
Density
How closely packed the particles are in a solid, liquid, or gas
The amount of mass per unit volume
Density formula
Mass / volume
m / V
Solid properties
Regular pattern
Fixed position
Vibrate on the spot
Keep their shape
Liquid properties
Random arrangement
Close together
Move around
Takes the shape of a container
Gas properties
Random arrangement
Far apart
Move in all directions
Fill the shape of the container
Kinetic theory of matter - solids
Particles in a solid are held together by strong forces of attraction and vibrate at their position
At low temperatures, the vibration is small and can be considered fixed
When a solid gains energy the particles vibrate more and cause
the neighboring particles to vibrate also.
Kinetic theory of matter - liquids
The intermolecular forces within a liquid are too weak to keep particles in a fixed position so they are free to move
They move randomly and so
therefore liquids flow.
Kinetic theory of matter - gases
The particles in a gas are in constant random motion as there are very weak forces between them
The particles are spaced further apart than in liquids.
Evaporation
When particles at the surface of a liquid gain enough energy to leave as a gas
Factors increasing the rate of evaporation
Increasing the surface area of the liquid
Increasing the temperature of the liquid
Condensation
The H2O molecules in the air hit a cold surface and therefore condense, changing state from gas to a liquid
Factors increasing the rate of condensation
Increasing the surface area
Reducing surface temperature
Sublimation
The process by which a solid directly changes to a gaseous state (missing the liquid state).
E.g. dry ice
Internal energy
The combined energy of the kinetic and potential energy of the
particles in the substance
Increasing internal energy
Heating a substance will increase its kinetic energy store, and therefore an internal energy change
A change in state causes an increase in potential energy, and therefore an internal energy change