2. TrueFalseStatementTrueFalse Solids have a definite shape and volume, and their particles do not move Liquids have definite shape, not volume, and their particles can move Gases do not have a definite shape or volume, and particles are free to move The Kinetic Theory states all particles of matter are in constant motion Gases can fit any size or shaped container

3. Kinetic Theory All particles of matter are in constant motion Explains the behavior of solids and liquids Kinetic Energy- an objects energy due to its motion

4. States of Matter Solid Liquid Gas Plasma

5. Solids: Matter that has Definite shape Definite volume Orderly arrangement of atomic particles. Close together

6. Behavior of Solids Particles vibrate in fixed locations Repetitive, back in forth motion Keeps solids constant shape and volume

7. Liquids: Matter that has Definite volume NO definite shape Arrangement of particles at atomic level is further apart than solids

8. Behavior of Liquids Particles can flow to new locations No definite shape Force of attraction keeps particles close together Constant volume

9. Gases: Matter that has no Definite shape Definite volume Takes the size and shape of its container

10. Behavior of Gases Particles are in constant motion Become any size or shape Kinetic Theory of Gases Particles are in constant, random motion Motion of 1 particle is unaffected by the motion of another, unless they collide Forces of attraction among particles in a gas can be ignored under ordinary conditions

11. Plasma: Gas containing Nuclei Electrons Exists in extremely hot environments Sun Stars

13. Ch. 3.3

14. TrueFalseStatementTrueFalse The temperature of a substance does not change during a phase change Energy does not change during a phase change Heat of fusion is the energy needed to melt a substance Heat of vaporization is the energy needed to turn into a gas Endothermic reactions absorb heat and become hot, exothermic give off heat becoming cold

15. Phase Changes Reversible physical changes 1 state of matter changes into another 6 Phases Melting / freezing vaporization / condensation Sublimation / deposition

16. Phase Change and Temperature Energy Temp of the substances does NOT change during a phase change Energy is either absorbed or released during a phase change

17. Energy Endothermic Exothermic Absorbs energy from surroundings Become cold Ex: Evaporation of water Releases energy into surroundings Produce heat Ex: Candle flame

18. Heat of Fusion Heat needed to melt Varies for every substance

19. Phase Changes Melting Freezing Molecules become less orderly Gain energy, vibrate more quickly to break away from fixed position Endothermic Molecules become more orderly Kinetic energy decreases, decreasing movement until a fixed arrangement is met Exothermic

20. Phase Changes: Vaporization Evaporation Liquid to gas Endothermic Heat of Vaporization- amount of heat needed Occurs on the surface & and temps BELOW boiling point Vapor Pressure the pressure of the vapor resulting from evaporation of a liquid above a sample of the liquid in a closed container Boiling Occurs below the surface at BOLING point

21. Phase Changes: Condensation Gas to liquid Exothermic

22. Phase Changes Sublimation Deposition Solid to gas, skipping liquid Endothermic Ex: Dry ice Gas to solid, skipping liquid Exothermic