1. 1 Ch 10-12 Kinetic Molecular Theory

2. 2 States of Matter State of matter is another physical properties. State of matter is another physical properties. The four states of matter are: The four states of matter are: Solid Solid Liquid Liquid Gas Gas Plasma Plasma

3. 3 Kinetic Molecular Theory The kinetic theory of matter states that all particles are in constant motion. The kinetic theory of matter states that all particles are in constant motion.kinetic theory kinetic theory Solid’s particles are tightly bound together and barely vibrate. Solid’s particles are tightly bound together and barely vibrate. Liquid’s particles are loosely bound and have the ability to flow. Liquid’s particles are loosely bound and have the ability to flow. Gas’s particles are not bound at all and free to move in random motion unless a collision occurs. Gas’s particles are not bound at all and free to move in random motion unless a collision occurs.

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5. 5 Plasma Plasma is a state of matter that exists only at extremely high temperatures. It makes up 99% of our universe. Plasma is a state of matter that exists only at extremely high temperatures. It makes up 99% of our universe.

6. 6 Solid State Solids have a definite shape Solids have a definite shape Solids and definite volume. Solids are highly dense and have zero compressibility. Solids are highly dense and have zero compressibility. Atoms can arrange to make organized patterns called crystals or remain amorphous. Atoms can arrange to make organized patterns called crystals or remain amorphous.

7. 7 Fluids Liquids and gases are considered fluids because of their ability to flow. Liquids and gases are considered fluids because of their ability to flow. Gases and liquids also have an amorphous structure allowing them to take the shape of any container. Gases and liquids also have an amorphous structure allowing them to take the shape of any container.

8. 8 Liquid State Liquids have an indefinite shape but a definite volume. Liquids have an indefinite shape but a definite volume. Liquids Liquids are also highly dense and have little compressibility. Liquids are also highly dense and have little compressibility. Properties of liquids include… Properties of liquids include… Surface tension Surface tension Capillary action Capillary action Diffusion Diffusion

9. 9 Liquid Properties They experience surface tension which is the ability of molecules at the surface to bond tightly with one another. They experience surface tension which is the ability of molecules at the surface to bond tightly with one another. They also undergo capillary action. This is the attraction between liquids and the surface of a solid. They also undergo capillary action. This is the attraction between liquids and the surface of a solid. Liquids are able to mix through a process called diffusion. Liquids are able to mix through a process called diffusion.diffusion

10. 10 Capillary action Surface tension Diffusion

11. 11 Gas State Gases have indefinite shape and indefinite volume. Gases have indefinite shape and indefinite volume. They are highly compressible because of their low density. They are highly compressible because of their low density.

12. 12 Gases experience mixing through diffusion.Gases experience mixing through diffusion. Gases have the ability of effusion. This is the passing of a gas through a very small hole from areas of high pressure to low pressure.Gases have the ability of effusion. This is the passing of a gas through a very small hole from areas of high pressure to low pressure. Gas Properties

13. 13 Effusion Diffusion

14. 14 Gas State Pressure, volume, temperature, and number of molecules are the four measurable quantities needed to fully describe a gas. Pressure, volume, temperature, and number of molecules are the four measurable quantities needed to fully describe a gas. The gas laws are the simple mathematical relationships between these four quantities. The gas laws are the simple mathematical relationships between these four quantities.

15. 15 STP STP stands for standard temperature and pressure. STP stands for standard temperature and pressure. The standard temperature and pressure for a gas is equal to 1atm and 0oC (absolute zero). The standard temperature and pressure for a gas is equal to 1atm and 0oC (absolute zero). Some common conversions are: Some common conversions are: Volume 1000mL = 1L Volume 1000mL = 1L Pressure 1atm = 760 torr = 101.325 kPa Pressure 1atm = 760 torr = 101.325 kPa Temperature 1K = 273 o Temperature 1K = 273 o

16. 16 Ideal vs Real gas Ideal vs Real gas Under ordinary conditions, gases exhibit behavior that is nearly ideal of what a gas is supposed to do. Under ordinary conditions, gases exhibit behavior that is nearly ideal of what a gas is supposed to do. However, under extreme temperatures and pressures gases sometimes break their ideal rules. However, under extreme temperatures and pressures gases sometimes break their ideal rules.

17. 17 Combined Gas Law Combined gas law relates how pressure, volume, and temperature of a gas are related. Combined gas law relates how pressure, volume, and temperature of a gas are related. Combined gas law Combined gas law PV/T=PV/T PV/T=PV/T

18. 18 Boyle’s Law Boyle’s law states that volume and pressure are inversely proportional. Boyle’s law states that volume and pressure are inversely proportional. Boyle’s PV=PV PV=PV

19. 19 Charles’ Law Charles’s law states that volume and temperature are directly proportional. Charles’s law states that volume and temperature are directly proportional. Charles’s V/T = V/T V/T = V/T

20. 20 Gay-Lussac’s Law Gay-Lussac’s Law states that pressure and temperature are directly proportional. Gay-Lussac’s Law states that pressure and temperature are directly proportional. Gay-Lussac’s P/T=P/T P/T=P/T

21. 21 Charles’s Boyle’s Gay-Lussac’s

22. 22 Law of Partial Pressures Dalton’s law of partial pressures states that the total pressure of a mixture of gases is equal to the sum of the partial pressure of the component gases. Dalton’s law of partial pressures states that the total pressure of a mixture of gases is equal to the sum of the partial pressure of the component gases.law of partial pressures law of partial pressures P total = P + P + P +….. P total = P + P + P +…..

23. 23 Avogadro's Law Avogadro's law states that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules. Avogadro's law states that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules. Avogadro's law Avogadro's law It also indicates that gas volume is directly proportional to the number of molecules of gas. It also indicates that gas volume is directly proportional to the number of molecules of gas.

24. 24 Ideal Gas Equation Ideal gases following the equation PV=nRT Ideal gases following the equation PV=nRT n is the number of moles and R is a gas constant equal to 0.0821atm, 8.314kPa, or 62.4 mmHg. n is the number of moles and R is a gas constant equal to 0.0821atm, 8.314kPa, or 62.4 mmHg. This equation can be used to find any of the four variables, the molar mass, or the density of a gas. This equation can be used to find any of the four variables, the molar mass, or the density of a gas. This equation This equation Density of a gas can be found using D=MP/RT Density of a gas can be found using D=MP/RT Molar mass can be found using M=mRT/PV Molar mass can be found using M=mRT/PV

25. 25 State Changes By the addition or removal of heat energy, states of matter can change from one to another. By the addition or removal of heat energy, states of matter can change from one to another. The six types of state change process are: The six types of state change process are: Melting Melting Freezing Freezing Vaporization Vaporization Condensation Condensation Sublimation Sublimation Deposition Deposition

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27. 27 Solid/Liquid With the addition of heat energy a solid can change to a liquid through melting. With the addition of heat energy a solid can change to a liquid through melting. During this process, the bonds of the solid are loosened. During this process, the bonds of the solid are loosened. With the removal of heat energy a liquid can become a solid through freezing. With the removal of heat energy a liquid can become a solid through freezing. During this process, the bonds of the liquid tighten. During this process, the bonds of the liquid tighten.

28. 28 Liquid/Gas With the addition of heat energy a liquid can change to a gas through vaporization. With the addition of heat energy a liquid can change to a gas through vaporization. During this process, the bonds of the liquid are broken. During this process, the bonds of the liquid are broken. With the removal of heat energy a gas can become a liquid through condensation. With the removal of heat energy a gas can become a liquid through condensation. During this process, the gas forms loose bonds. During this process, the gas forms loose bonds.

29. 29 Solid/Gas With the addition of a lot of heat energy a solid can change directly to a gas through sublimation. With the addition of a lot of heat energy a solid can change directly to a gas through sublimation. During this process, the bonds of the solid are completely broken. During this process, the bonds of the solid are completely broken. With the removal of a lot of heat energy a gas can become a solid through deposition. With the removal of a lot of heat energy a gas can become a solid through deposition. During this process, new binds are formed. During this process, new binds are formed.

30. 30 Heats of Fusion and Vaporization Heat of fusion is the amount of heat energy that must be absorbed or released when changing between solid and liquid states. Heat of fusion is the amount of heat energy that must be absorbed or released when changing between solid and liquid states. Heat of vaporization is the amount of heat energy that must be absorbed or released when changing between the liquid and gas state. Heat of vaporization is the amount of heat energy that must be absorbed or released when changing between the liquid and gas state.

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32. 32 Phase Diagram A phase diagram is a graph of pressure versus temperature that shows the conditions under which the phases of a substance exist. A phase diagram is a graph of pressure versus temperature that shows the conditions under which the phases of a substance exist.phase diagram phase diagram The melting/freezing point and vaporization/condensation point can be found at 1atm of pressure. The melting/freezing point and vaporization/condensation point can be found at 1atm of pressure. The triple point is the temperature and pressure at which the substance could coexist in equilibrium at any of the states. The triple point is the temperature and pressure at which the substance could coexist in equilibrium at any of the states. The critical point is the temperature and pressure at which the substance can exist only in the gas state. The critical point is the temperature and pressure at which the substance can exist only in the gas state.

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