Chapter 3-1 Matter and Energy
Kinetic Theory Kinetic theory - an explanation of how particles in matter behave. 3 requirements
Kinetic Theory All matter is composed of small particles (atoms, molecules, and ions).
Kinetic Theory Particles are in constant, random motion.
Kinetic Theory Particles are colliding with each other and the walls of their container.
Solids Definite shape and volume Crystalline – orderly arrangement of atoms Amorphous – atoms in no particular pattern
Crystalline Solid
Amorphous Solid
Liquids Change shape but not volume Surface tension – force acting on the surface of a liquid
Surface Tension
Thermal Energy Atoms in solids – tightly packed together Thermal energy in the particles causes them to vibrate in place
Gas Particles are free to move in all directions
Plasma Plasma – state of matter that starts as a gas and then becomes ionized 99% of know matter in universe Electrons stripped off
Plasma Stars Lightning Fire Fluorescent Lights
Energy Energy – the capacity to do work
Thermal Energy Thermal Energy – Kinetic energy of a substance’s atoms Kinetic energy – energy of motion
Average Kinetic Energy Temperature - average kinetic energy of particles in the substance How fast the particles are moving.
Average Kinetic Energy On average, molecules of frozen water at 0°C will move slower.
Average Kinetic Energy On average, molecules of water at 90°C will move faster.
Change of state Endothermic change Exothermic change Requires energy Melting Sweating Exothermic change Energy released from change Freezing
Evaporation vs Boiling Boiling - occurs throughout a liquid Evaporation - occurs at the surface of a liquid
Sublimation Sublimation – process where a solid turns directly to a gas Ex. old ice cubes or dry ice
Condensation Condensation – change of a substance from a gas to a liquid Gas comes in contact with a cool surface
Conservation of Mass and Energy Mass can not be created or destroyed Amount mass and energy stays the same before and after the change
States of Matter Clip