Matter and Phase Changes

Kinetic Energy

Motion energy; energy to move particles, increased by heat and measured by temperature

Potential Energy

Store energy due to interactions between particles or objects, measured by state of matter with particle distance

Open System

A system where matter and energy can move in and out

Closed System

A system where energy but not matter can move in and out

System

One area isolated from everything else in the universe

Surroundings

Everything else separated from the system in the universe

Boiling/Condensation Point

When matter transitions between liquid and gas remaining at 100°C until phase change is complete

Melting/Freezing Point

When matter transitions between liquid and solid remaining at 0°C until phase change is complete

Thermal Energy

Total energy in a system factoring number and type of particles, temperature, and state of matter (KE - particle motion x PE - attractive forces)

Thermal Energy vs Temperature

Thermal Energy measures total energy of particles while Temperature measures average energy of particles

Particle Behavior of Solids

Solid particles are rigidly packed and vibrate non locomotive to hold their shape. They have a definite shape and volume that don’t change when moved or placed in different containers and are hard to compress.

Particle Behavior of Liquids

Liquid particles randomly slide past and collide into each other to flow. They have definite volume but indefinite shape, change shape but not volume when moved or placed in different containers, flows between containers as a fluid, and are hard to compress.

Particle Behavior of Gases

Gas particles are freely spaced and move around randomly at high speeds to be compressed. They have no definite shape or volume, flow between containers as a fluid, changes shape and volume when moved or placed into a different container, and are easy to compress.

Melting

Solid to liquid remaining at 0°C until phase change complete: solid particles move fast and farther apart and overpower attractive forces into liquid with more speed and thermal energy

Condensation

Gas to liquid remaining at 100°C until phase change complete: gas particles move slow and closer together as attractive forces overpower them into liquid with less speed and thermal energy

Boiling

Liquid to gas remaining at 100°C until phase change complete: when liquid heated, bubbles form within and rise as faster liquid particles overpower attractive forces with higher temperatures from extra thermal energy

Faster form of vaporization

Evaporation

Liquid to gas: when liquid heated at boiling point or lower temperatures on the surface, liquid particles overpower attractive forces and break apart into gas with more thermal energy and speed

Slower form of vaporization

Freezing

Liquid to solid remaining at 0°C until phase change complete: liquid particles move close and slow as attractive forces overpower them into a solid with lower temperatures from less thermal energy and speed

Sublimation

Solid to gas: cold, low temperatures pull energy and cool down surrounding substances for that thermal energy to overpower attractive forces and weaken solid particles into gas without the liquid stage

Deposition

Gas to solid: cold, low temperatures pulls a lot of thermal energy from supercooled gas particles that immediately condenses but freezes into solid being already past freezing point

Relationship between Potential Energy and Kinetic Energy

Direct

Relationship between Attractive Forces and Kinetic Energy

Inverse