1. Starter S-137 List and describe the four states of matter.

2. States of Matter Chapter 13

3. 13.1 The Nature of Gases Chapter 13

4. Kinetic Theory – all matter consists of tiny particles that are in constant motion 1.The particles of a gas are considered to be small hard spheres with an insignificant volume 2.The motion of the particles in a gas is rapid, constant, and random 13.1 The Nature of Gases

5. 3.Collisions between particles in a gas are perfectly elastic. -no energy is lost in collisions 13.1 The Nature of Gases

6. Gas pressure is caused by the collision of particles with the container Atmospheric Pressure – caused by the collision of atoms and molecules in air with objects 13.1 The Nature of Gases PhET Gas

7. Barometer – a device to measure atmospheric pressure The pressure depends on Temperature Altitude Measured in pascal (Pa) very small unit 13.1 The Nature of Gases

8. Units must be converted for problems to work out These are equalities, so they can be used to create conversion factors 13.1 The Nature of Gases

9. The Kelvin temperature of a substance is directly proportional to the average kinetic energy of the particles of the substance 13.1 The Nature of Gases PhET Gas

10. Notice - the average shifts, but there are particles with very different temperatures - the hotter one has particles with almost no energy, just like the colder one - this is a change in kinetic energy, not speed 13.1 The Nature of Gases

11. Starter S-139 Convert each of the following to kilopascals 1.450 mmHg 2.1045 torr 3.1.29 atm 4.95,000 pa

12. 13.2 The Nature of Liquids Chapter 13

13. Fluids – substances that can flow gases liquids Unlike gases, liquids particles attracted to each other 13.2 The Nature of Liquids

14. Physical properties of a liquid are determined by 1.Motion of the particles (due to temperature) 2.Attraction among the particles 3.The particles are closer together due to these forces 13.2 The Nature of Liquids Phase Change

15. Vaporization – conversion of a liquid to a gas or vapor Evaporation – vaporization on the surface of a liquid that is not boiling 13.2 The Nature of Liquids

16. During evaporation – only molecules with a certain minimum kinetic energy escape from the liquid Evaporation takes away the hot (faster) particles and is a cooling process 13.2 The Nature of Liquids

17. Vapor Pressure – the force exerted by a gas above a liquid Because of the gas produced by evaporation Eventually particles leaving the liquid equal the particles reentering the liquid 13.2 The Nature of Liquids Vapor Pressure Equilibrium

18. The container only reaches equilibrium if it is sealed Vapor pressure depends on temperature at higher temperature the average kinetic energy is higher 13.2 The Nature of Liquids Vapor Pressure (kPa) 0oC0oC20 o C40 o C60 o C80 o C100 o C Water0.612.337.3719.9247.34101.3 Ethanol1.635.8518.0447.02108.3225.8 Diethyl ether24.7058.96122.8230.6399.1647.9

19. The vapor pressure shows of volatile a liquid is How easily it evaporates 13.2 The Nature of Liquids

20. Boiling – when the temperature is high enough, that particles throughout the liquid have the kinetic energy to vaporize Bubbles of vapor form throughout the liquid Boiling point – the point where the vapor pressure of the liquid is equal to the external pressure on the liquid 13.2 The Nature of Liquids

21. Starter S-140 1. What is A.Vaporization B.Boiling C.Evaporation D.Vapor Pressure 2. What is the relationship between vapor pressure and boiling?

22. 13.3 The Nature of Solids Chapter 13

23. Properties of solids are determined by 1.Orderly arrangement of their particles 2.Fixed locations of their particles Melting point – temperature at which a solid changes into a liquid 13.3 The Nature of Solids

24. The melting point and freezing point are the same temperature The states are at equilibrium Crystalline Solids – the particles are arranged in crystals Crystal – orderly 3D pattern 13.3 The Nature of Solids

25. Crystal Systems Defined by 6 Values 13.3 The Nature of Solids

26. Seven Basic Shapes Unit Cell – the smallest group of particles that has the geometric shape of the crystal 13.3 The Nature of Solids

27. Allotropes – two or more different molecular forms of the same element in the same physical state Carbon Diamond Graphite Soot (buckminsterfullerene) 13.3 The Nature of Solids

28. Amorphous Solid – lacks an internal structure Rubber Plastics Glass Do not have a specific melting point Shatter into random shapes 13.3 The Nature of Solids

29. Starter S-141 1. Define A.Crystalline Solid B.Amorphous Solid 2. What are the three allotropes of carbon?

30. 13.4 Changes of State Chapter 13

31. Solid – molecules vibrate in place Melting – Particles increase speed start to move Liquid – molecules move, but still attracted to each other Evaporation – particles move fast enough to that intermolecular forces do not matter 13.4 Change of State Phase Change Melting

32. Sublimation – solid goes directly to a gas Vapor pressure of the solid is greater than atmospheric pressure Carbon Dioxide (Dry Ice) Iodine 13.4 Change of State

33. Phase Diagram – shows states (solid, liquid, gas) in relation to pressure and temperature 13.4 Change of State

34. Triple Point – the point where a solid, liquid, and gas state can all exist For water that would be 0.61 kPa and 0.016 o C Notice – An increase in pressure drives most substances toward a solid An increase in temperature drives substances toward a gas 13.4 Change of State