Chapter 3 – States of Matter

Kinetic Theory Kinetic energy = energy an object has due to its motion The faster an object is moving; the greater its kinetic energy. Kinetic theory states that all particles of matter are in constant motion.

3.1 Solids, Liquids, and Gases Definite Shape Definite Volume Particles vibrate in fixed positions Particles have low kinetic energy

Liquids Variable shape (takes the shape of the container) Definite Volume Particles can move around each other Particles have medium Kinetic Energy

Gases Variable shape Variable volume (fills all space in a container) Particles move about freely Particles have high Kinetic Energy

Other states of matter Plasma Exists only at extremely high temperatures 99% of the matter in the UNIVERSE is plasma Stars are plasma Bose-Einstein Condensate Exists only at extremely low temperatures Groups of atoms behave as a single particle

https://www.youtube.com/watch?v=KCL8zqjXbME

Day 2

3.2 The Gas Laws Pressure = the result of force distributed over an area In a closed container, gases exert pressure when the particles of the gas collide with the walls of the container. More Collisions=More Pressure Forces of attraction among gas particles so weak they can be ignored under ordinary conditions

Which shoes create the most pressure?

Factors That Affect Gas Pressure Temperature – raising temp. will increase pressure if volume of gas and # of particles are kept constant Increase in temp.  particles move faster  particles collide with walls more frequently  increased pressure

Volume – Decreasing volume of a gas causes an increase in pressure if the temp. and # of particles are constant Decrease in vol.  less space  particles collide with walls more often  increase pressure Factors That Affect Gas Pressure Cont…..

Factors That Affect Gas Pressure Cont….. Number of particles – increasing the number of particles of a gas will increase pressure if temp. and volume are constant Increase # of particles  particles collide with container more often  increase pressure

Charles’ Law The volume and absolute temperature (K) of a gas are directly related at constant mass & pressure V1 = V2 T1 T2 V T

Boyle’s Law The pressure and volume of a gas are inversely related at constant mass & temp P1V1 = P2V2

PV T V T P T PV = k P1V1 T1 = P2V2 T2 P1V1T2 = P2V2T1 Combined Gas Law PV T V T P T PV = k P1V1 T1 = P2V2 T2 P1V1T2 = P2V2T1

https://www.youtube.com/watch?v=Osq71Y82uac https://www.youtube.com/watch?v=kr1V0KtZPGw

Day 3

3.3 Phase Changes Phase change – reversible physical change that occurs when a substance changes from one state of matter to another Temperature of a substance DOES NOT CHANGE during a phase change. Energy is either absorbed or released during a phase change. Endothermic – energy is absorbed Exothermic – energy is released

Melting and Freezing Melting Solid changes to liquid Particles absorb energy (endothermic) Particles become less orderly Heat of fusion- energy a substance must absorb in order to change from solid to liquid Freezing Liquid changes to solid Particles release energy (exothermic) Particles become more orderly

Vaporization and Condensation Liquid changes into a gas Particles absorb energy (endothermic) Particles become LESS orderly and more free to move 2 types of vaporization Evaporation – takes place at the surface of a liquid Boiling – occurs when a liquid is heated to its boiling point

Condensation Gas changes to a liquid Particles release or lose energy (exothermic) Particles become MORE orderly

Sublimation and Deposition Changing from a solid directly to a gas Energy is absorbed (endothermic) Deposition Changing from a gas directly to a solid Energy is released (exothermic)

Phase Change Diagram