2. RED SLIDE: These are notes that are very important and should be recorded in your science journal. Copyright © 2010 Ryan P. Murphy

3. -Nice neat notes that are legible and use indentations when appropriate. -Example of indent. -Skip a line between topics -Don’t skip pages -Make visuals clear and well drawn. Please label. Ice MeltingWater Boiling Vapor Gas TEMPTEMP Heat Added 

4. RED SLIDE: These are notes that are very important and should be recorded in your science journal. BLACK SLIDE: Pay attention, follow directions, complete projects as described and answer required questions neatly. Copyright © 2010 Ryan P. Murphy

5. Keep an eye out for “The-Owl” and raise your hand as soon as you see him. –He will be hiding somewhere in the slideshow Copyright © 2010 Ryan P. Murphy

6. Keep an eye out for “The-Owl” and raise your hand as soon as you see him. –He will be hiding somewhere in the slideshow “Hoot, Hoot” “Good Luck!” Copyright © 2010 Ryan P. Murphy

8. Bring in a clear plastic 2 liter bottle with cap. –We will be making a Squidy to take home near the end of this set of lessons.

9. New Area of Focus: Gases and Other Laws. New Area of Focus: Gases and Other Laws. Copyright © 2010 Ryan P. Murphy

10. Demonstration: Fit a balloon to the top of a bottle and place in pan with hot and cold water. –Make an observation about the volume of a gas and temperature. Switch them periodically.

11. Gay-Lussac's Law: The pressure exerted on the sides of a container by an ideal gas of fixed volume is proportional to its temperature. –Sometimes referred to as Amontons' Law

12. Charles Law: Volume of a gas increases with temperature. (Gases expand with heat). Charles Law: Volume of a gas increases with temperature. (Gases expand with heat). Copyright © 2010 Ryan P. Murphy

14. The formula for the law is: The formula for the law is:Volume ________ = K Temp Copyright © 2010 Ryan P. Murphy

15. The formula for the law is: The formula for the law is:Volume ________ = K Temp Copyright © 2010 Ryan P. Murphy

16. The formula for the law is: The formula for the law is:Volume ________ = K Temp Copyright © 2010 Ryan P. Murphy

17. Demonstration: Fit a balloon to the top of a bottle and place in pan with hot and cold water. –Make an observation about the volume of a gas and temperature. Switch them periodically.

18. Demonstration: Fit a balloon to the top of a bottle and place in pan with hot and cold water. –Make an observation about the volume of a gas and temperature. Switch them periodically.

19. Demonstration: Fit a balloon to the top of a bottle and place in pan with hot and cold water. –Make an observation about the volume of a gas and temperature. Switch them periodically.

20. V is the volume of the gas. Copyright © 2010 Ryan P. Murphy

21. V is the volume of the gas. T is the temperature of the gas (measured in Kelvin) Copyright © 2010 Ryan P. Murphy

22. V is the volume of the gas. T is the temperature of the gas (measured in Kelvin) K is a constant. Copyright © 2010 Ryan P. Murphy

23. V is the volume of the gas. T is the temperature of the gas (measured in Kelvin) K is a constant. K= The universal constant in the gas equation: pressure times volume = R times temperature; equal to 8.3143 joules per Kelvin per mole. Copyright © 2010 Ryan P. Murphy

24. V is the volume of the gas. T is the temperature of the gas (measured in Kelvin) K is a constant. K= The universal constant in the gas equation: pressure times volume = R times temperature; equal to 8.3143 joules per Kelvin per mole. Copyright © 2010 Ryan P. Murphy

25. V is the volume of the gas. T is the temperature of the gas (measured in Kelvin) K is a constant. K= The universal constant in the gas equation: pressure times volume = R times temperature; equal to 8.3143 joules per Kelvin per mole. Copyright © 2010 Ryan P. Murphy

26. This law means that when the temperature goes up, the volume of the gas goes up.

30. As the molecules heat up they move around faster and collide more often.

31. This law means that when the temperature goes up, the volume of the gas goes up. As the molecules heat up they move around faster and collide more often. Gay-Lussac's Law: The pressure exerted on the sides of a container by an ideal gas of fixed volume is proportional to its temperature.

32. This law means that when the temperature goes up, the volume of the gas goes up. As the molecules heat up they move around faster and collide more often. Gay-Lussac's Law: The pressure exerted on the sides of a container by an ideal gas of fixed volume is proportional to its temperature.

33. Matter, Energy, and the Environment Unit Link

34. Avogadro’s Law / Hypothesis. Copyright © 2010 Ryan P. Murphy

35. Avogadro’s Law / Hypothesis. “Hello ladies, I am the Italian savant named Amedo Avogadro.” Copyright © 2010 Ryan P. Murphy

36. Avogadro’s Law / Hypothesis. “Hello ladies, I am the Italian savant named Amedo Avogadro.” –“I would love to show you my gas laws, will you join me?” Copyright © 2010 Ryan P. Murphy

37. Avogadro’s Law / Hypothesis. “Hello ladies, I am the Italian savant named Amedo Avogadro.” –“I would love to show you my gas laws, will you join me?” Copyright © 2010 Ryan P. Murphy

38. Avogadro's Law: Equal volumes of gases, at the same temperature and pressure, contain the same number of particles, or molecules. Avogadro's Law: Equal volumes of gases, at the same temperature and pressure, contain the same number of particles, or molecules. Copyright © 2010 Ryan P. Murphy

39. Study a few minutes. Questions will follow. Gases are made up of molecules which are in constant random motion.. Pressure is due to collisions between the molecules and the walls of the container. All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic. –(That means that there is no loss of kinetic energy during the collision.) The temperature of the gas is proportional to the average kinetic energy of the molecules. There are no (or entirely negligible) intermolecular forces between the gas molecules. The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

41. Study a few minutes. Questions will follow. Gases are made up of molecules which are in constant random motion.. Pressure is due to collisions between the molecules and the walls of the container. All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic. –(That means that there is no loss of kinetic energy during the collision.) The temperature of the gas is proportional to the average kinetic energy of the molecules. There are no intermolecular forces between the gas molecules. The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

42. Study a few minutes. Questions will follow. Gases are made up of molecules which are in constant random motion.. Pressure is due to collisions between the molecules and the walls of the container. All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic. –(That means that there is no loss of kinetic energy during the collision.) The temperature of the gas is proportional to the average kinetic energy of the molecules. There are no intermolecular forces between the gas molecules. The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

43. Study a few minutes. Questions will follow. Gases are made up of molecules which are in constant random motion.. Pressure is due to collisions between the molecules and the walls of the container. All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic. –(That means that there is no loss of kinetic energy during the collision.) The temperature of the gas is proportional to the average kinetic energy of the molecules. There are no intermolecular forces between the gas molecules. The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

44. Study a few minutes. Questions will follow. Gases are made up of molecules which are in constant random motion.. Pressure is due to collisions between the molecules and the walls of the container. All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic. –(That means that there is no loss of kinetic energy during the collision.) The temperature of the gas is proportional to the average kinetic energy of the molecules. There are no intermolecular forces between the gas molecules. The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

45. Study a few minutes. Questions will follow. Gases are made up of molecules which are in constant random motion.. Pressure is due to collisions between the molecules and the walls of the container. All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic. –(That means that there is no loss of kinetic energy during the collision.) The temperature of the gas is proportional to the average kinetic energy of the molecules. There are no intermolecular forces between the gas molecules. The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

46. Study a few minutes. Questions will follow. Gases are made up of molecules which are in constant random motion.. Pressure is due to collisions between the molecules and the walls of the container. All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic. –(That means that there is no loss of kinetic energy during the collision.) The temperature of the gas is proportional to the average kinetic energy of the molecules. There are no intermolecular forces between the gas molecules. The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

47. Study a few minutes. Questions will follow. Gases are made up of molecules which are in constant random motion.. Pressure is due to collisions between the molecules and the walls of the container. All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic. –(That means that there is no loss of kinetic energy during the collision.) The temperature of the gas is proportional to the average kinetic energy of the molecules. There are no intermolecular forces between the gas molecules. The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

48. Study a few minutes. Questions will follow. Gases are made up of molecules which are in constant random motion.. Pressure is due to collisions between the molecules and the walls of the container. All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic. –(That means that there is no loss of kinetic energy during the collision.) The temperature of the gas is proportional to the average kinetic energy of the molecules. There are no intermolecular forces between the gas molecules. The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

49. Study a few minutes. Questions will follow. Gases are made up of molecules which are in constant random motion.. Pressure is due to collisions between the molecules and the walls of the container. All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic. –(That means that there is no loss of kinetic energy during the collision.) The temperature of the gas is proportional to the average kinetic energy of the molecules. There are no intermolecular forces between the gas molecules. The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

50. Study a few minutes. Questions will follow. Gases are made up of molecules which are in constant random motion.. Pressure is due to collisions between the molecules and the walls of the container. All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic. –(That means that there is no loss of kinetic energy during the collision.) The temperature of the gas is proportional to the average kinetic energy of the molecules. There are no intermolecular forces between the gas molecules. The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

51. Study a few minutes. Questions will follow. Gases are made up of molecules which are in constant random motion.. Pressure is due to collisions between the molecules and the walls of the container. All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic. –(That means that there is no loss of kinetic energy during the collision.) The temperature of the gas is proportional to the average kinetic energy of the molecules. There are no intermolecular forces between the gas molecules. The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

52. Study a few minutes. Questions will follow. Gases are made up of molecules which are in constant random motion.. Pressure is due to collisions between the molecules and the walls of the container. All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic. –(That means that there is no loss of kinetic energy during the collision.) The temperature of the gas is proportional to the average kinetic energy of the molecules. There are no intermolecular forces between the gas molecules. The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

53. Study a few minutes. Questions will follow. Gases are made up of molecules which are in constant random motion.. Pressure is due to collisions between the molecules and the walls of the container. All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic. –(That means that there is no loss of kinetic energy during the collision.) The temperature of the gas is proportional to the average kinetic energy of the molecules. There are no intermolecular forces between the gas molecules. The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

54. When temperatures get colder, you may need to add some more molecules to get the safe PSI for your vehicle. Copyright © 2010 Ryan P. Murphy

55. The kinetic movement of molecules causes gas particles to move to open areas. Copyright © 2010 Ryan P. Murphy

56. The kinetic movement of molecules causes gas particles to move to open areas. Copyright © 2010 Ryan P. Murphy

57. When pressure is increased on a gas it’s volume is decreased.

60. Demonstration! Marshmallow Torture –Place Marshmallow into Bell Jar vacuum. –Remove Air from Bell Jar –Record Picture of Marshmallow. –Quickly let air rush back in and observe.

61. Demonstration! Marshmallow Torture –Place Marshmallow into Bell Jar vacuum. –Remove Air from Bell Jar –Record Picture of Marshmallow. –Quickly let air rush back in and observe.

62. Demonstration! Marshmallow Torture –Place Marshmallow into Bell Jar vacuum. –Remove Air from Bell Jar –Record Picture of Marshmallow. –Quickly let air rush back in and observe.

63. Demonstration! Marshmallow Torture –Place Marshmallow into Bell Jar vacuum. –Remove Air from Bell Jar –Record Picture of Marshmallow. –Quickly let air rush back in and observe.

64. Boyle’s Law: Pressure and Volume are inversely proportional. Boyle’s Law: Pressure and Volume are inversely proportional. Copyright © 2010 Ryan P. Murphy

65. Boyle’s Law: Pressure and Volume are inversely proportional. Boyle’s Law: Pressure and Volume are inversely proportional. Copyright © 2010 Ryan P. Murphy P is the pressure of the molecules on the container, V is the volume of the container, and k is a constant. The value of k always stays the same so that P and V vary appropriately. For example, if pressure increases, k must remains constant and thus volume will decrease.

66. Matter, Energy, and the Environment Unit Link

67. Gas Laws and more available sheet.

68. Activity! Syringes

69. Activity! Syringes (Safety Goggles Needed)

70. Activity! Syringes –Depress plunger on the syringe.

71. Activity! Syringes –Depress plunger on the syringe. –Cover hole with finger.

72. Activity! Syringes –Depress plunger on the syringe. –Cover hole with finger. –Try and pull handle (gently please). Why is it difficult? Keep thumb on opening.

73. Activity! Syringes –Depress plunger on the syringe. –Cover hole with finger. –Try and pull handle (gently please). Why is it difficult? Keep thumb on opening.

74. Matter, Energy, and the Environment Unit Link

75. Temperature and Pressure Temperature and Pressure Copyright © 2010 Ryan P. Murphy

76. Temperature and Pressure Temperature and Pressure As temp rises, pressure rises As temp rises, pressure rises Copyright © 2010 Ryan P. Murphy

77. Temperature and Pressure Temperature and Pressure As temp rises, pressure rises As temp rises, pressure rises As pressure rises, temp rises As pressure rises, temp rises Copyright © 2010 Ryan P. Murphy

78. Temperature and Pressure Temperature and Pressure As temp rises, pressure rises As temp rises, pressure rises As pressure rises, temp rises As pressure rises, temp rises Copyright © 2010 Ryan P. Murphy

79. Temperature and Pressure Temperature and Pressure As temp rises, pressure rises As temp rises, pressure rises As pressure rises, temp rises As pressure rises, temp rises Copyright © 2010 Ryan P. Murphy

80. Temperature and Pressure Temperature and Pressure As temp rises, pressure rises “Watch out” As temp rises, pressure rises “Watch out” As pressure rises, temp rises As pressure rises, temp rises Copyright © 2010 Ryan P. Murphy

81. Temperature and Pressure Temperature and Pressure As temp rises, pressure rises “Watch out” As temp rises, pressure rises “Watch out” As pressure rises, temp rises As pressure rises, temp rises Copyright © 2010 Ryan P. Murphy

82. Temperature and Pressure Temperature and Pressure As temp rises, pressure rises “Watch out” As temp rises, pressure rises “Watch out” As pressure rises, temp rises “Watch out” As pressure rises, temp rises “Watch out” Copyright © 2010 Ryan P. Murphy

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95. +

97. This photoshop job might look “Funny”.

98. Caution! Graphic Images of burns / the dangers of pressure and temperature.

99. The consequences of severe burns and explosions are not “funny”. Copyright © 2010 Ryan P. Murphy

103. The ideal gas law: PV = nRT (pressure times volume equals the number of molecules times the gas constant times temperature) The ideal gas law: PV = nRT (pressure times volume equals the number of molecules times the gas constant times temperature) Copyright © 2010 Ryan P. Murphy

104. The ideal gas law: PV = nRT (pressure times volume equals the number of molecules times the gas constant times temperature) The ideal gas law: PV = nRT (pressure times volume equals the number of molecules times the gas constant times temperature) Copyright © 2010 Ryan P. Murphy

105. The ideal gas law: PV = nRT (pressure times volume equals the number of molecules times the gas constant times temperature) The ideal gas law: PV = nRT (pressure times volume equals the number of molecules times the gas constant times temperature) Copyright © 2010 Ryan P. Murphy

106. The ideal gas law: PV = nRT (pressure times volume equals the number of molecules times the gas constant times temperature) The ideal gas law: PV = nRT (pressure times volume equals the number of molecules times the gas constant times temperature) Copyright © 2010 Ryan P. Murphy

107. The ideal gas law: PV = nRT (pressure times volume equals the number of molecules times the gas constant times temperature) The ideal gas law: PV = nRT (pressure times volume equals the number of molecules times the gas constant times temperature) Copyright © 2010 Ryan P. Murphy

108. The ideal gas law: PV = nRT (pressure times volume equals the number of molecules times the gas constant times temperature) The ideal gas law: PV = nRT (pressure times volume equals the number of molecules times the gas constant times temperature) Copyright © 2010 Ryan P. Murphy

109. The ideal gas law: PV = nRT (pressure times volume equals the number of molecules times the gas constant times temperature) The ideal gas law: PV = nRT (pressure times volume equals the number of molecules times the gas constant times temperature) Copyright © 2010 Ryan P. Murphy

110. P=PressureV=Volume is equal to the.. n= Number of molecules R= Gas constant = 8.134 JK m T= Temperature Copyright © 2010 Ryan P. Murphy

111. P=PressureV=Volume is equal to the.. n= Number of molecules R= Gas constant = 8.134 JK m T= Temperature Copyright © 2010 Ryan P. Murphy

112. P=PressureV=Volume is equal to the.. n= Number of molecules R= Gas constant = 8.134 JK m T= Temperature Copyright © 2010 Ryan P. Murphy

113. P=PressureV=Volume is equal to the.. n= Number of molecules R= Gas constant = 8.134 JK m T= Temperature Copyright © 2010 Ryan P. Murphy

114. P=PressureV=Volume is equal to the.. n= Number of molecules R= Gas constant = 8.134 JK m T= Temperature Copyright © 2010 Ryan P. Murphy Mole is a unit of measurement used in chemistry to express amounts of a chemical substance.

115. P=PressureV=Volume is equal to the.. n= Number of molecules R= Gas constant = 8.134 JK m T= Temperature Copyright © 2010 Ryan P. Murphy

116. P=PressureV=Volume is equal to the.. n= Number of molecules R= Gas constant = 8.134 JK m T= Temperature Copyright © 2010 Ryan P. Murphy

117. P=PressureV=Volume is equal to the.. n= Number of molecules R= Gas constant = 8.134 JK m T= Temperature Copyright © 2010 Ryan P. Murphy

118. Video Link! (Optional) Khan Academy Ideal Gas Law (Advanced) –http://www.khanacademy.org/video/ideal-gas- equation--pv-nrt?playlist=Chemistryhttp://www.khanacademy.org/video/ideal-gas- equation--pv-nrt?playlist=Chemistry

119. Activity! Visiting Ideal Gas Law Simulator http://www.7stones.com/Homepage/Publish er/Thermo1.htmlhttp://www.7stones.com/Homepage/Publish er/Thermo1.html How you can use this gas law to find…

120. Activity! Visiting Ideal Gas Law Simulator http://www.7stones.com/Homepage/Publish er/Thermo1.htmlhttp://www.7stones.com/Homepage/Publish er/Thermo1.html How you can use this gas law to find… –Calculating Volume of Ideal Gas: V = (nRT) ÷ P

121. Activity! Visiting Ideal Gas Law Simulator http://www.7stones.com/Homepage/Publish er/Thermo1.htmlhttp://www.7stones.com/Homepage/Publish er/Thermo1.html How you can use this gas law to find… –Calculating Volume of Ideal Gas: V = (nRT) ÷ P –Calculating Pressure of Ideal Gas: P = (nRT) ÷ V

122. Activity! Visiting Ideal Gas Law Simulator http://www.7stones.com/Homepage/Publish er/Thermo1.htmlhttp://www.7stones.com/Homepage/Publish er/Thermo1.html How you can use this gas law to find… –Calculating Volume of Ideal Gas: V = (nRT) ÷ P –Calculating Pressure of Ideal Gas: P = (nRT) ÷ V –Calculating moles of gas: n = (PV) ÷ (RT)

123. Activity! Visiting Ideal Gas Law Simulator http://www.7stones.com/Homepage/Publish er/Thermo1.htmlhttp://www.7stones.com/Homepage/Publish er/Thermo1.html How you can use this gas law to find… –Calculating Volume of Ideal Gas: V = (nRT) ÷ P –Calculating Pressure of Ideal Gas: P = (nRT) ÷ V –Calculating moles of gas: n = (PV) ÷ (RT) –Calculating gas temperature: T = (PV) ÷ (nR)

124. Activity! Gas Law Simulator. http://intro.chem.okstate.edu/1314F00/Lab oratory/GLP.htmhttp://intro.chem.okstate.edu/1314F00/Lab oratory/GLP.htm What happens to molecules when… –Temperature is increased. –Pressure is increased. –Volume is decreased. Copyright © 2010 Ryan P. Murphy

125. Activity! Gas Law Simulator. http://intro.chem.okstate.edu/1314F00/Lab oratory/GLP.htmhttp://intro.chem.okstate.edu/1314F00/Lab oratory/GLP.htm What happens to molecules when… –Temperature is increased. –Pressure is increased. –Volume is decreased. Copyright © 2010 Ryan P. Murphy

126. Activity! Gas Law Simulator. http://intro.chem.okstate.edu/1314F00/Lab oratory/GLP.htmhttp://intro.chem.okstate.edu/1314F00/Lab oratory/GLP.htm What happens to molecules when… –Temperature is increased. –Pressure is increased. –Volume is decreased. Copyright © 2010 Ryan P. Murphy

127. Activity! Gas Law Simulator. http://intro.chem.okstate.edu/1314F00/Lab oratory/GLP.htmhttp://intro.chem.okstate.edu/1314F00/Lab oratory/GLP.htm What happens to molecules when… –Temperature is increased. –Pressure is increased. –Volume is decreased. Copyright © 2010 Ryan P. Murphy

128. Optional Class Quiz: The Quiz is difficult, but the correct answers are revealed which is the learning component. –Remember Kinetic Molecular Theory. –http://www.sciencegeek.net/Chemistry/taters/U nit5KMT.htmhttp://www.sciencegeek.net/Chemistry/taters/U nit5KMT.htm Copyright © 2010 Ryan P. Murphy

129. Gas Laws and more available sheet.

130. Activity / Happy Face Copyright © 2010 Ryan P. Murphy

131. Activity / Demonstration! Copyright © 2010 Ryan P. Murphy

132. Activity / Demonstration! –Blow up a balloon 1/8 of the way. Do not tie. the balloon! Copyright © 2010 Ryan P. Murphy

133. Activity / Demonstration! –Blow up a balloon 1/8 of the way. Do not tie. the balloon! Copyright © 2010 Ryan P. Murphy

134. Activity / Demonstration! –Blow up a balloon 1/8 of the way. Do not tie. the balloon! –Squeeze balloon in one hand and draw a small face on it with Sharpie marker (Works well if nose is the end of the balloon). Copyright © 2010 Ryan P. Murphy

135. Activity / Demonstration! –Blow up a balloon 1/8 of the way. Do not tie. the balloon! –Squeeze balloon in one hand and draw a small face on it with Sharpie marker (Works well if nose is the end of the balloon). Copyright © 2010 Ryan P. Murphy

136. Activity / Demonstration! –Blow up a balloon 1/8 of the way. Do not tie. the balloon! –Squeeze balloon in one hand and draw a small face on it with Sharpie marker (Works well if nose is the end of the balloon). Copyright © 2010 Ryan P. Murphy

137. Activity / Demonstration! –Blow up a balloon 1/8 of the way. Do not tie. the balloon! –Squeeze balloon in one hand and draw a small face on it with Sharpie marker (Works well if nose is the end of the balloon). –Tie off balloon and face should shrink. Copyright © 2010 Ryan P. Murphy

138. Activity / Demonstration! –Blow up a balloon 1/8 of the way. Do not tie. the balloon! –Squeeze balloon in one hand and draw a small face on it with Sharpie marker (Works well if nose is the end of the balloon). –Tie off balloon and face should shrink. –Release and then add pressure to one side of the balloon so that your face expands. Have fun for a bit! Copyright © 2010 Ryan P. Murphy

141. Matter, Energy, and the Environment Unit Link

142. Pascal's Law: If you apply pressure to fluids that are confined (or can’t flow anywhere), the fluids will then transmit (or send out) that same pressure in all directions at the same rate. Pascal's Law: If you apply pressure to fluids that are confined (or can’t flow anywhere), the fluids will then transmit (or send out) that same pressure in all directions at the same rate. Copyright © 2010 Ryan P. Murphy Cool Picture of a Gnome being squeezed and yelling something about Pascal in a different language. Cool Picture of a Gnome being squeezed and yelling something about Pascal in a different language.

143. Pascal's Law: If you apply pressure to fluids that are confined (or can’t flow anywhere), the fluids will then transmit (or send out) that same pressure in all directions at the same rate. Pascal's Law: If you apply pressure to fluids that are confined (or can’t flow anywhere), the fluids will then transmit (or send out) that same pressure in all directions at the same rate. Copyright © 2010 Ryan P. Murphy

146. Hydraulics - The branch of applied science that deals with fluids in motion.

150. Don’t forget, air is also considered a fluid.

151. Activity – Pascal’s Law and Hydraulics.

152. Activity! Making a hydraulic syringe drive. Copyright © 2010 Ryan P. Murphy

153. Activity! Making a hydraulic syringe drive. –Push syringe to bottom of tube on one side. Copyright © 2010 Ryan P. Murphy

154. Activity! Making a hydraulic syringe drive. –Push syringe to bottom of tube on one side. –Dip end of syringe in water and pull to fill tube. Copyright © 2010 Ryan P. Murphy

155. Activity! Making a hydraulic syringe drive. –Push syringe to bottom of tube on one side. –Dip end of syringe in water and pull to fill tube. –Attach hose to one side. Copyright © 2010 Ryan P. Murphy

156. Matter, Energy, and the Environment Unit Link

157. Viscosity: Resistance of liquid to flow. Copyright © 2010 Ryan P. Murphy

158. High Viscosity = Travels slow because of high resistance.

159. Low Viscosity = Travels fast because low resistance.

160. Activity! What is more viscous? –Remember, Viscosity is resistance to flow. Copyright © 2010 Ryan P. Murphy

161. Answer! The peanut butter doesn’t flow as much as the ketchup so it has more viscosity. Copyright © 2010 Ryan P. Murphy

162. Newtonian and non-Newtonian fluids. Copyright © 2010 Ryan P. Murphy

163. Newtonian and non-Newtonian fluids. –Newtonian fluid will flow the same when a great deal of force is applied as when it is left alone. Copyright © 2010 Ryan P. Murphy

164. Newtonian and non-Newtonian fluids. –Newtonian fluid will flow the same when a great deal of force is applied as when it is left alone. –Non-Newtonian fluids change their viscosity or flow under stress. Copyright © 2010 Ryan P. Murphy

165. Which one a Newtonian fluid and which one is a non-Newtonian fluid? Copyright © 2010 Ryan P. Murphy

166. Which one a Newtonian fluid and which one is a non-Newtonian fluid? Copyright © 2010 Ryan P. Murphy

167. Which one a Newtonian fluid and which one is a non-Newtonian fluid? Copyright © 2010 Ryan P. Murphy

168. Which one a Newtonian fluid and which one is a non-Newtonian fluid? Copyright © 2010 Ryan P. Murphy

169. Which one a Newtonian fluid and which one is a non-Newtonian fluid? Copyright © 2010 Ryan P. Murphy

170. Video Link! non-Newtonian fluid on a subwoofer. –http://www.youtube.com/watch?v=3zoTKXXNQIUhttp://www.youtube.com/watch?v=3zoTKXXNQIU

178. Viscosity increases with stress over time

185. Learn more about Newtonian and non-Newtonian fluids at… http://www.sciencelearn.org.nz/Science-Stories/Strange- Liquids/Non-Newtonian-fluids http://www.sciencelearn.org.nz/Science-Stories/Strange- Liquids/Non-Newtonian-fluids

186. Making Oobleck. Non-Newtonian Fluid –To create Oobleck use a box of cornstarch, some water and a mixing bowl. In general, a mixture of about 1.5 cups of cornstarch to 1 cup of water. Add food coloring if desired.

187. Matter, Energy, and the Environment Unit Link

188. Activity! The Condiment Olympics. –Official / ceremony / entrance of the condiments required. Volunteers needed to march each condiment into the classroom. –http://www.youtube.com/watch?v=EbHw8DBCXQ8http://www.youtube.com/watch?v=EbHw8DBCXQ8 Copyright © 2010 Ryan P. Murphy

189. Create the following spreadsheet in your journal. CondimentFinish Time Mustard Ketchup Jelly Maple Syrup (Fake) Chocolate Syrup Mystery Fluid Copyright © 2010 Ryan P. Murphy

190. Create the following spreadsheet in your journal. CondimentFinish Time Mustard Ketchup Jelly Maple Syrup (Fake) Chocolate Syrup Mystery Fluid Copyright © 2010 Ryan P. Murphy

191. Activity! Viscosity. –Lay tray on table.

192. Activity! Viscosity. –Lay tray on table. –Place condiments at one side along a starting line.

193. Activity! Viscosity. –Lay tray on table. –Place condiments at one side along a starting line. –Use textbooks or manually raise tray just off the vertical at start of race.

194. Activity! Viscosity. –Lay tray on table. –Place condiments at one side along a starting line. –Use textbooks or manually raise tray just off the vertical at start of race. –Record the times each condiment takes to cross the finish line. (DNF = Did Not Finish) –I needed green text here to complete the Olympic colors.

195. Activity! Viscosity. –Lay tray on table. –Place condiments at one side along a starting line. –Use textbooks or manually raise tray just off the vertical at start of race. –Record the times each condiment takes to cross the finish line. (DNF = Did Not Finish) –I needed green text here to complete the Olympic colors.

196. Visual of Set-Up Top View Side View Start Finish

197. Matter, Energy, and the Environment Unit Link

198. Archimedes Principle – Any Guesses? Archimedes Principle – Any Guesses? Copyright © 2010 Ryan P. Murphy

199. Archimedes Principle: A body that is submerged in a fluid is buoyed up by a force equal in magnitude to the weight of the fluid that is displaced. Archimedes Principle: A body that is submerged in a fluid is buoyed up by a force equal in magnitude to the weight of the fluid that is displaced. Copyright © 2010 Ryan P. Murphy

200. Archimedes Principle: A body that is submerged in a fluid is buoyed up by a force equal in magnitude to the weight of the fluid that is displaced. Archimedes Principle: A body that is submerged in a fluid is buoyed up by a force equal in magnitude to the weight of the fluid that is displaced. Copyright © 2010 Ryan P. Murphy

201. Archimedes Principle: A body that is submerged in a fluid is buoyed up by a force equal in magnitude to the weight of the fluid that is displaced. Archimedes Principle: A body that is submerged in a fluid is buoyed up by a force equal in magnitude to the weight of the fluid that is displaced. Copyright © 2010 Ryan P. Murphy

202. Archimedes Principle: A body that is submerged in a fluid is buoyed up by a force equal in magnitude to the weight of the fluid that is displaced. Archimedes Principle: A body that is submerged in a fluid is buoyed up by a force equal in magnitude to the weight of the fluid that is displaced. Copyright © 2010 Ryan P. Murphy

203. Archimedes Principle: A body that is submerged in a fluid is buoyed up by a force equal in magnitude to the weight of the fluid that is displaced. Archimedes Principle: A body that is submerged in a fluid is buoyed up by a force equal in magnitude to the weight of the fluid that is displaced. Copyright © 2010 Ryan P. Murphy Boat must weigh less than this much water to float.

204. Copyright © 2010 Ryan P. Murphy

207. Buoyancy: Buoyancy force is equal to the weight of fluid displaced by the body. Buoyancy: Buoyancy force is equal to the weight of fluid displaced by the body. Copyright © 2010 Ryan P. Murphy

208. If your boat doesn’t displace more water than it weighs, your boat will sink. Copyright © 2010 Ryan P. Murphy

215. Matter, Energy, and the Environment Unit Link

216. Activity! Creating a boat using Archimedes Principle. Copyright © 2010 Ryan P. Murphy

217. Activity! Creating a boat using Archimedes Principle. Copyright © 2010 Ryan P. Murphy

226. Part II, Gas Laws and more Review Game

228. Areas of Focus within The Matter, Energy, and the Environment Unit. There is no such thing as a free lunch, Matter, Dark Matter, Elements and Compounds, States of Matter, Solids, Liquids, Gases, Plasma, Law Conservation of Matter, Physical Change, Chemical Change, Gas Laws, Charles Law, Avogadro’s Law, Ideal Gas Law, Pascal’s Law, Viscosity, Archimedes Principle, Buoyancy, Seven Forms of Energy, Nuclear Energy, Electromagnet Spectrum, Waves / Wavelengths, Light (Visible Light), Refraction, Diffraction, Lens, Convex / Concave, Radiation, Electricity, Lightning, Static Electricity, Magnetism, Coulomb’s Law, Conductors, Insulators, Semi-conductors, AC and DC current, Amps, Watts, Resistance, Magnetism, Faraday’s Law, Compass, Relativity, Einstein, and E=MC2, Energy, First Law of Thermodynamics, Second Law of Thermodynamics, Third Law of Thermodynamics, Industrial Processes, Environmental Studies, The 4 R’s, Sustainability, Human Population Growth, Carrying Capacity, Green Design, Renewable Forms of Energy. Matter, Energy, and the Environment Unit Link

229. This PowerPoint is one small part of my Matter, Energy and the Environment Unit. This unit includes… Five Part 3,700+ Slide PowerPoint roadmap. 14 Page bundled homework package, 20 pages of units notes that chronologically follow the PowerPoint. 5 PowerPoint review games (150 slides each), video and academic links, follow along worksheets / lab sheets, rubrics, games, activity sheets, crosswords, and much more. Matter, Energy, and the Environment Unit Link

239. Please open the welcome / guide document on each unit preview. –This document will describe how to utilize these resources in your classroom and provide some curriculum possibilities.

240. Please visit the links below to learn more about each of the units in this curriculum and to see previews of each unit. –These units take me four busy years to complete with my students in grades 5-10. Earth Science UnitsExtended Tour Link and Curriculum Guide Geology Topics Unit http://sciencepowerpoint.com/Geology_Unit.html Astronomy Topics Unit http://sciencepowerpoint.com/Astronomy_Unit.html Weather and Climate Unit http://sciencepowerpoint.com/Weather_Climate_Unit.html Soil Science, Weathering, More http://sciencepowerpoint.com/Soil_and_Glaciers_Unit.html Water Unit http://sciencepowerpoint.com/Water_Molecule_Unit.html Rivers Unit http://sciencepowerpoint.com/River_and_Water_Quality_Unit.html = Easier = More Difficult = Most Difficult 5 th – 7 th grade 6 th – 8 th grade 8 th – 10 th grade

241. Physical Science UnitsExtended Tour Link and Curriculum Guide Science Skills Unit http://sciencepowerpoint.com/Science_Introduction_Lab_Safety_Metric_Methods. html Motion and Machines Unit http://sciencepowerpoint.com/Newtons_Laws_Motion_Machines_Unit.html Matter, Energy, Envs. Unit http://sciencepowerpoint.com/Energy_Topics_Unit.html Atoms and Periodic Table Unit http://sciencepowerpoint.com/Atoms_Periodic_Table_of_Elements_Unit.html Life Science UnitsExtended Tour Link and Curriculum Guide Human Body / Health Topics http://sciencepowerpoint.com/Human_Body_Systems_and_Health_Topics_Unit.html DNA and Genetics Unit http://sciencepowerpoint.com/DNA_Genetics_Unit.html Cell Biology Unit http://sciencepowerpoint.com/Cellular_Biology_Unit.html Infectious Diseases Unit http://sciencepowerpoint.com/Infectious_Diseases_Unit.html Taxonomy and Classification Unit http://sciencepowerpoint.com/Taxonomy_Classification_Unit.html Evolution / Natural Selection Unit http://sciencepowerpoint.com/Evolution_Natural_Selection_Unit.html Botany Topics Unit http://sciencepowerpoint.com/Plant_Botany_Unit.html Ecology Feeding Levels Unit http://sciencepowerpoint.com/Ecology_Feeding_Levels_Unit.htm Ecology Interactions Unit http://sciencepowerpoint.com/Ecology_Interactions_Unit.html Ecology Abiotic Factors Unit http://sciencepowerpoint.com/Ecology_Abiotic_Factors_Unit.html

242. Thank you for your time and interest in this curriculum tour. Please visit the welcome / guide on how a unit works and please link to the many unit previews to see the PowerPoint slideshows, bundled homework packages, review games, unit notes, and much more. Thank you again and please feel free to contact me with any questions you may have. Best wishes. Sincerely, Ryan Murphy M.Ed www.sciencepowerpoint@gmail.com