Solids

• Solid is a state of matter in which materials have a definite shape and a definite volume.

• Molecules/Atoms are tightly packed in a pattern and vibrate.

• Can not be compressed.

Liquid• Liquid is the state of

matter in which a material has a definite volume but not a definite shape (Takes the shape of its container).

• Molecules/Atoms are tightly packed but can slide past each other.

• Liquids can not be compressed.

Gases• Gas is the state of

matter in which the material has no definite shape and no definite volume (Takes the shape and volume of its container).

• Molecules/Atoms are spread apart and can be compressed.

Other States/Phases• Plasma is the most

common state of matter in the universe (99%).

• It is a highly charged (ionized) gas.

• Present in stars.

• Bose-Einstein Condensate – at very low temperatures (near -273°C) atoms behave as though they were a single particle.

• Check it out

http://www.colorado.edu/physics/2000/bec/what_is_it.html

Kinetic Theory

• Kinetic Energy is the energy an object has due to its motion. The faster an object moves the more energy it possesses.

http://www.harcourtschool.com/activity/states_of_matter/

• The Kinetic Theory says that all particles of matter are in constant motion.

Most Energy

Gas

Liquid

Solid

Least Energy

Kinetic Theory of Gas• Gas

– Particles in a gas are in constant, random motion.

– The motion of one particle in unaffected by the motion of other particles unless the particles collide.

– Forces of attraction among particles in a gas can be ignored under ordinary conditions.

Kinetic Theory for Liquids and Solids

• Liquids take the shape of the container because particles in a liquid can flow to new locations. The volume of a liquid is constant because the force of attraction keep the particles close together.

• Solids have a definite volume and shape because particles in a solid vibrate around a fixed point.

Gas Laws• Pressure is the result of a force (Push)

distributed over an area.– Unit pascal (Pa) or Newton/meter2 (N/m2)

• Collisions between particles of a gas and the walls of the container cause the pressure in a closed container of gas.

• Raising the temperature of a gas will increase its pressure if the volume and the number of particles are constant.

• Reducing the volume of a gas will increase the pressure if the volume and the number of particles are constant.

Charles’s Law V1/T1=V2/T2

• Charles’s Law states that a volume of gas is directly proportional to its temperature in kelvins if the pressure and the number of particles remains constant.

• V = Volume• T = Temperature• 1 = before the change• 2 = after the change

• Absolute Zero (0 K) is the temperature at which the atoms/molecules of matter stop moving.

• 0 K = -273°C• 273 K = 0°C• 373 K = 100°C

Boyle’s Law P1V1=P2V2

• Boyle’s Law states that the volume of a gas is inversely proportional to its pressure if the temperature and the number of particles are constant.

• P = Pressure

• V = Volume

• Combination of the two laws.

P1V1 = P2V2

T1 T2

Phase Change

• A Phase Change is the reversible physical change that occurs when a substance changes from one state of matter to another.

• The temperature of a substance does not change during a phase change.

• Energy is either absorbed or released during a phase change.

http://Atoms Family•http://Weather Related News

Energy

• Endothermic – Energy taken in

• Exothermic – Energy given off

• Heat of Fusion – amount of energy absorbed by a substance as it changes from a solid to a liquid.

• Heat of Vaporization – amount of energy absorbed by a substance as it goes from a liquid to a gas.

Phase Changes• Melting – Solid to a

liquid.

• Freezing – Liquid to a solid.

• Vaporization – Liquid to a gas.

• Condensation – Gas to a liquid

• Sublimation – Solid to a gas.

• Deposition – Gas to a solid.

• Vapor Pressure – the pressure caused by the collisions of particles in a vapor with the walls of a container.