1. Matter & Energy Ch. 13

2. Solid Have a definite shape and volume Particles have strong attractive force, but still vibrate

3. Liquid Have a definite volume but not a definite shape Particles move fast enough to overcome forces of attraction.

4. Gas Does NOT have definite volume or shape Particles moves fast enough to break away from each other

5. Plasma Does NOT have a definite shape or volume Particle are broken apart (electrons have been stripped off) Conduct electric current Examples?

6. Energy Definition: The ability to change or move matter, or the capacity to do work Thermal Energy – the total kinetic energy of the particles that make up that object Kinetic Energy :Thermal EnergyParticle Speed :Thermal EnergyParticle Amount : Temperature is a measure of kinetic energy

7. Energy & Change of State

8. Changes of State Melting point – Temperature at which a solid changes to a liquid Freezing point – Temperature at which a liquid changes to a solid Boiling point – Temperature at which a liquid changes to a gas Condensation point – Temperature at which a gas changes to a liquid Same Temp. Same Temp.

9. Energy & Change of State Reactions/Changes can be: Endothermic – requires energy or Exothermic – produces energy

10. Phase Changes Solid Liquid Gas Melting Vaporization CondensationFreezing

11. Liquid Sublimation Melting Vaporization Deposition Condensation Solid Freezing Gas

12. Energy and Phase Change Heat/enthalpy of fusion energy required to change one gram of a substance from solid to liquid or released when changing from liquid to solid. For water 80 cal/g

13. Energy and Phase Change Heat/enthalpy of vaporization energy required to change one gram of a substance from liquid to gas or released when one gram of a substance changes from gas to liquid. For water 540 cal/g

14. Water and Ice Ice Water and Steam Steam -20 0 20 40 60 80 100 120 0 40120 220760800 Heating Curve for Water Energy (calorie) T e m p. (C)

15. Water and Ice Ice Water and Steam Steam -20 0 20 40 60 80 100 120 0 40120 220760800 Heating Curve for Water Ice and Water

16. Water and Ice Ice Water and Steam Steam -20 0 20 40 60 80 100 120 0 40120 220760800 Heating Curve for Water Both Water and Steam

17. Water and Ice Ice Water and Steam Steam -20 0 20 40 60 80 100 120 0 40120 220760800 Heating Curve for Water Heat of Fusion Heat of Vaporization

18. Water and Ice Ice Water and Steam Steam -20 0 20 40 60 80 100 120 0 40120 220760800 Heating Curve for Water Slope = Specific Heat Steam Water Ice

19. Calcualting Energy Heat = Energy = Q Three equations Heat (Q)= specific heat x mass x  T Heat (Q)= heat of fusion x mass Heat (Q)= heat of vaporization x mass

20. Numbers to Know S.H.= specific heat For ice S.H. = 2.05 J/g  C For water S.H = 4.186 J/g  C For steam S.H. = 0.50 cal/g  C Heat of vaporization= 540 cal/g Heat of fusion = 80 cal/g 1 cal=4.184 J

21. How to do Calculate The total heat = the sum of all the heats you have to use Go in order Heat Ice Below 0  C + Melt Ice At 0  C + Heat Water 0  C - 100  C + Boil Water At 100  C + Heat Steam Above 100  C

22. Examples How much heat does it take to heat 12 g of ice at -6  C to 25  C water? How much heat does it take to heat 35 g of ice at 0  C to steam at 150  C?

23. 1)Identify the state of matter: HW Quiz a.Particles vibrate but are locked in place b.c. 2)How does temperature relate to a particle’s kinetic energy 3)Energy is ___________ (absorbed or released) as solid ice turns to liquid 4)The process that refers to water vapor returning to liquid form.

24. 5)A reaction is considered to be __________ (endothermic or exothermic) if energy is released. 6)Briefly explain how a liquid thermometer measures temperature. 7)In the graph below, what “point” is represented by the letter A. (Hint: there are two possible answers). Energy change of water A

25. Changes of State