1. Physical Science CHS 2013-14 Unit 3 Properties of Matter

2. 12/2/13 Week of 12/2 to 12/6 Entry Task Find a definition for ATOMS and ELEMENT in the textbook.

3. Today’s Agenda Get out your Newton Movie Questions. Read through them together so that you know what you are listening for. Raise your hand to share if you hear an answer to one of the questions. The movie will be paused briefly when answers are heard.

4. 12/2/13 Exit Task Describe some themes in Newton’s life.

5. 12/3/13 Entry Task What is a pure substance? What is a mixture? List physical means of separation (p. 181). 5 minute review and Turn in whatever you have for the Newton Questions.

6. C-notes on pages 178-182 and 190-194 Vocabulary (left) – meanings (right) Element Compound Atom Molecule Mixture Pure Substance Solid Liquid Gas Plasma Intermolecular Forces Melting Point Boiling Point Key Ideas (left) – answer (right) Describe the differences between pure substances and mixtures (a venn diagram may help). List the 4 phases of matter in order of increasing temperature Describe what happens at the molecular level when a substance melts. Describe what happens at the molecular level when a substance boils.

7. C-notes on pages 178-182 and 190-194 Vocabulary (left) – meanings (right) Element Compound Atom Molecule Mixture Pure Substance Solid Liquid Gas Plasma Intermolecular Forces Melting Point Boiling Point Key Ideas (left) – answer (right) Describe the differences between pure substances and mixtures (a venn diagram may help). List the 4 phases of matter in order of increasing temperature Describe what happens at the molecular level when a substance melts. Describe what happens at the molecular level when a substance boils.

8. 12/3/13 Exit Task Explain the difference between an element and a compound.

9. 12/4/13 Entry Task Look at your safety rules (Unit 1). Write down 3 safety rules for using bunsen burners or open flames in the lab. TEST MAKE-UPS: If you still need to complete a Unit 2 test YOU ARE RESPONSIBLE to schedule with me.

10. Today’s Agenda – Learn about Bunsen Burners What is a Bunsen Burner - historyhistory Video Tutorial – the one minute versionthe one minute version Slow down! – How to Light a Bunsen BurnerHow to Light a Bunsen Burner Notes – parts and steps of use Tomorrow you will take a quiz and a performance assessment on using Bunsen burners. You will have to pass the quiz and the performance assessment in order to get your bunsen burner license. What is the right sequence?

11. Label the parts air intake combustion nozzle barrel/body tube gas jet (point to inside) base gas valve/dial

13. Functions of Parts – air intake: adjustable; controls amount of oxygen; adding more air makes flame hotter – combustion nozzle: gas and air mix to ignite – barrel: turn this to adjust air intake – gas valve/dial: adjustable; controls amount of gas entering burner; adding more gas makes flame taller – base: holds up Bunsen burner – gas jet: small hole that gas goes through

14. Steps to Light and Turn Off 1.Wear safety goggles, tie back long hair, no loose clothing. 2.Check striker for sparks. 3.Attach hose to burner and gas line. 4.Turn barrel clockwise to close and then open slightly to let a small amount of air flow. 5.Turn gas valve/dial counter clockwise to close. 6.turn on gas by rotating valve parallel to hose. 7.Open gas valve/dial slightly – should hear faint hissing. 8.Hold striker at 45 degree angle and light. 9.For a taller flame – open gas valve/dial more to allow more gas. For a shorter flame – turn gas valve/dial back counter clockwise. 10.For a hotter flame – turn barrel counter clockwise (increases air flow). Flame should turn blue. 11.For a cooler flame – turn barrel clockwise (decreases air flow). Flame should turn orange. 12.The ideal flame is pale blue with a darker blue core. Draw a picture of the flame. 13.To turn off: turn barrel clockwise for a cooler, orange flame. Completely turn off the gas valve/dial. Turn off gas line.

15. Safety Precautions Wear safety goggles, tie back long hair, no loose clothing. Hold Bunsen burner at the bottom to avoid burns. Never leave open flames unattended. Know location of safety exits, emergency shut- off and fire extinguishers.

16. 12/4/13 Exit Task What part of the Bunsen Burner flame is the hottest? Draw a picture or explain

17. 12/5/13 Entry Task Fill in the blanks: 1.Attach hose to _______ and ________. 2.Turn barrel _________ to close and then open slightly to let a small amount of air flow. 3.Turn __________ _______-_______ to close. 4.turn on gas by rotating valve _________ to hose. 5.Open gas valve/dial slightly – should hear __________. 6.Hold _________ at 45 degree angle and light.

18. Today’s Agenda TURN IN HOMEWORK ASSIGNMENT. Complete notes Take written portion of quiz. Passed the quiz? Practice the steps to light the burner and turn off the burner AT YOUR TABLE WITHOUT ACTUALLY USING GAS Performance Assessment of these steps tomorrow or Monday.

19. 12/5/13 Exit Task-SKIPPED DUE TO QUIZ Fill in the blanks: To turn off: turn barrel _________ for a cooler, orange flame. Completely turn off the __________. Turn off _________.

20. 12/6/13 Entry Task Say Something Nice

21. Today’s Agenda Unit2 MC tests will be returned to you. Please get out your red sheets. Graph your post-assessment score. Did you meet your goal set towards the beginning of the unit? Unit 2 Math tests will be returned to you. REQUIRED REFLECTIONS: If your Scantron score is less than 28. Discuss Answers.

22. 12/6/13 Exit Task Trade and Grade Please turn in your Entry/Exit task sheets for this week: 12/2 – 12/6/13.

23. 12/9/13 Week of 12/9 to 12/13 Entry Task Papers handed back. Add together your Unit 2 MC test POINTS and math portion POINTS. Take the TOTAL POINTS and divide by 66. Multiply by 100 to calculate your percent. Record this percent and write down if you would like to regain some points with a reflection.

24. Today’s Agenda Review Math answers to Unit 2 test. Divide into 3 groups: Group 1 - reflecting on MC portion of UNIT 2 – retrieve your test from counter; sit down with separate sheet of paper for reflection. TESTS WILL BE RECOLLECTED AT END OF CLASS. Group 2 – reflecting on MATH portion of UNIT 2. Remember to reflect on a separate piece of paper. Group 3 – no reflection necessary. Read pages 200-210. Answer questions #1-10 on p. 211.

25. 12/9/13 Exit Task Make a connection: Consider the amount of homework you completed for Unit 2. Also consider the quality of your efforts studying. Did your effort yield results in your test scores? Explain what these results show you.

26. 12/10/13 Entry Task What kind of energy is heat? Does heat flow from hot to cold or cold to hot? Homework: Read pages 200-210. Answer questions #1-10 on p. 211. Due Thursday 12/12/13 SAFETY LECTURE!!

27. Today’s Agenda On back of quiz: Please explain WHY the steps are in the SAFEST ORDER. REVISE ANY CIRCLED items on the written Bunsen Burner. You must get 100% PRACTICE: – 1. Goggles and tie back hair. – 2. attach hoses – 3. allow a small amount of air – 4. Close gas valve/dial – 5. Turn on gas line. – 6. Turn on small amount of gas. – 7. Light with striker Performance Assessment for Bunsen Burners Once you receive your license…. Flame Test Lab – using colors to determine chemical elements. NEVER LEAVE FLAME UNATTENDED.

28. Today’s Agenda On back of quiz: Please explain WHY the steps are in the SAFEST ORDER. REVISE ANY CIRCLED items on the written Bunsen Burner. You must get 100% PRACTICE: – 1. Goggles and tie back hair. – 2. attach hoses – 3. allow a small amount of air – 4. Close gas valve/dial – 5. Turn on gas line. – 6. Turn on small amount of gas. – 7. Light with striker Performance Assessment for Bunsen Burners Once you receive your license…. Flame Test Lab – using colors to determine chemical elements. NEVER LEAVE FLAME UNATTENDED.

29. 12/10/13 Exit Task CANCELLED DUE TO PERFORMANCE ASSESSMENTS.

30. 12/11/13 Entry Task Describe the energy transfers and transformations from the gas coming through the tube to the paperclip in the flame. (Remember gas is stored chemical energy) Homework: Read pages 200-210. Answer questions #1-10 on p. 211. Due Thursday 12/12/13

31. Today’s Agenda Finish Performance Assessments and Bunsen Burner Licenses. Once you receive your license….MAKE SURE I HAVE THAT RECORDED IN GRADEBOOK BEFORE YOU LEAVE! Flame Test Lab – using colors to determine chemical elements. NEVER LEAVE FLAME UNATTENDED. Make sure a team mate is attending the burner before you retrieve the chemical. Test the chemical in the hottest part of the flame. Put the paper clip back in the appropriate beaker!!!

32. General Steps for Flame Test Make sure your flame test loop is clean. – Put it into hottest part of Bunsen Burner flame. No color change should occur if it is clean. – If it isn’t clean, dip it into acid provided, then put into flame. Repeat until there is no color change. Dip clean loop into solution. Put loop into hottest part of the Bunsen Burner flame. Observe and record the color of the flame for the particular solution. Put the paperclip back in SAME SOLUTION!

33. 12/11/13 Exit Task CANCELLED DUE TO PERFORMANCE ASSESSMENTS. IF TIME – What colors did the flame tests show? Cobalt – Magnesium – Calcium – Barium – Potassium –

34. 12/12/13 Entry Task Discuss yesterday’s flame test results. Give a definition of DENSITY. Get out homework. Calculate percent and QUICK review!

35. The Nature of Matter

36. Matter MixturePure Substance YESNO YESNO Homogeneous Mixture Heterogeneous Mixture NO Element Compounds or Molecules Are the particles one kind of atom? Are all the particles alike? Are the particles well-mixed and mixed evenly? YES Classifying Matter

37. Pure Element, Compound/Molecule, or Mixture?

39. 1.Elements – all particles are alike – the smallest particle of an element that is still recognizable is called an atom – they can’t be broken down anymore by “normal means” – they are found on the periodic table currently there are about 118 elements chemical symbols are used to represent the elements – Example: C=carbon, N=nitrogen….. Pure Substances

42. 2.Compounds and Molecules (over 10 million exist) – two or more elements chemically combined – once combined, the properties of a compound are different than the elements that make it up – can be broken down into the elements that make them up – example: Sugar is C 6 H 12 O 6 made up of carbon, hydrogen, and oxygen looks nothing like C, H, O by themselves can be broken down when burned

44. 1.Heterogeneous Mixture – different samples are not necessarily made up of exactly the same proportions of matter – can often see different particles mixed together – often can be easily separated Mixtures

45. 2.Homogeneous Mixture – is the same throughout – often can’t see different particles mixed together – often difficult to separate – examples: steel, milk, salt water, Kool Aid®

46. properties of matter are that it has: – mass: amount of matter (atoms) in an object – volume: amount of space an object takes up – density: the mass per unit volume of an object

48. – density is a property of material independent of quantity or shape

49. Density v D = density m = mass v = volume D = m/v

50. Example problem A piece of lead has a mass of 56.4 g and a volume of 5 mL. Calculate its density. ml is same as cm 3 so sometimes see g/cm 3 Looking for: Solution: Given: Formula: Density Mass = 56.4 g Volume = 5 mL D = m/v D = 56.4 g/ 5 mL D = 11.28 g/mL Same as… D = 11.28 g/cm3

51. 12/12/13 Exit Task How do you determine density of an object? What two characteristics do you need to know about the object? If time: How could you measure those for an irregular solid?

52. 12/13/13 Entry Task Say Something Nice REMEMBER – Be nice about someone’s character, effort, behavior, respect or integrity.

53. Today’s Agenda Finish Notes If time: start Density Lab

54. 12/13/13 Exit Task Post It Notes inside comp book if other labs still need to be graded: – Speed Lab? – Egg Drop? If Time: Trade and Grade

55. 12/16/13 Entry Task Look at the following chart. What is the densest material? How can you tell? What are the units? Please turn in your MATTER AND DENSITY NOTES. Collect your comp book. Tomorrow we will revise the pendulum lab.

57. Density of Substances P urpose –D–D etermine the densities of four solids, two liquids, and then compare to the actual answers. M aterials –b–b alance, graduated cylinder, ruler, calculator –6–6 substances l ittle stopper, big stopper, yellow liquid, green liquid, Cu cube, Cu wire,

58. Procedure – find the mass (using a balance) and volume (using a ruler or graduated cylinder) of each substance – calculate density using D = m/v – Optional: calculate percentage error using │your answer – actual answer│ actual answer (100)

59. 289.968 g

60. 11.5? ml

62. SubstanceMass (g)Volume (ml or cm 3 ) Calculated Density (g/ml or g/cm 3 ) Actual Density (g/ml or g/cm 3 ) Cu cube Cu wire big stopper little stopper yellow liquid green liquid Density of Different Substances

63. SubstanceMass (g)Volume (ml or cm 3 ) Calculated Density (g/ml or g/cm 3 ) Actual Density (g/ml or g/cm 3 ) Cu cube9.0 Cu wire9.0 big stopper1.3 little stopper1.3 yellow liq.?? green liq.1.0 Density of Different Substances

64. 12/16/13 Exit Task Would you expect the copper wire and copper cube to have the same density? Why or why not?

65. 12/17/13 Entry Task At the mouth of some rivers, a fresh water layer can form on top of salt water. Explain this using your understanding of density. HOMEWORK: Read pages 216-220 and 222-225. Answer # 1,2,3,6 on page 221 AND #1-8 on page 226. DUE FRIDAY 12/20/13. HOLIDAY COOKIES TO CLASS WHO MEETS THEIR HW GOAL!

66. Today’s Agenda Finish density lab. You will have 15 MINUTES for the remainder. Discuss results. Record actual densities. Return papers. Show best Labs. Fix Pendulum Labs where needed (circled items on rubric). An adult will sign off on your rubric when finished fixing circled items. If there is not time to check yours, you MUST turn back in your comp book to the shelf for re- grading WITH YOUR RUBRIC. When finished, you may begin on homework.

67. 12/17/13 Exit Task How close did you come to calculating the actual density of the 6 materials at the stations? Explain where/how/when you could have been more accurate.

68. 12/18/13 Entry Task Write down the definition of SOLUTION from the textbook. Is a solution of MIXTURE or a PURE SUBSTANCE? Can you think of a common solution you like to drink?

69. Identification of dissolved Solids and a metallic solid Solutions

70. What is a solution? Solution: A mixture that is homogeneous down to the molecular level Example: think Koolaid…

71. Types of solutions 2 solids – metal alloy like steel 2 liquids – lemon juice and water Solid and liquid – salt water Liquid and gas – carbonated drink Gas in gas – oxygen and nitrogen in atmosphere

72. Parts of a solution Solvent : the thing that does the dissolving. (the water) Solute : the thing that gets dissolved. (the Koolaid powder) Could you filter out the powder after it dissolves? No, it is homogeneous to the molecular level.

73. How do you get the dissolved solid back out of the solution? Evaporation! Remove all the liquid by turning it into a gas and the solid will recrystallize.

74. To separate a dissolved solid from a liquid… Boil off the liquid at a low temp and keep the solid before it reaches its melting point! Liquid turns to gas… solid is left behind! DEMO http://www.youtube.com/watch?v=O87PYJgi w1Y http://www.youtube.com/watch?v=O87PYJgi w1Y

75. Name … Partners… Separation and Identification of Two Solids in Water Q uestion –W–W hat are the two solids (one soluble, one insoluble) mixed in the water? M aterials –B–B eakers – small, large –b–b alance/scale –S–S olution with dissolved solids and a metallic solid –h–h ot plate –L–L ab scoop –s–s afety goggles –T–T weezers –T–T ongs –P–P lastic dish

76. Your part in the lab….. Procedure – Complete this today….what will you do to separate and identify the two solids? Numbered and detailed. Data Collection – For each substance, you will need to collect data to help you identify it. – What data? – Mass and Volume, and calculated density – Observed physical characteristics: solid, crystalline, metallic, etc

77. Analysis Conclusion – State what your two substance are and give as much supporting evidence as possible. – example The silver metal in our mixture is tin. The calculated density was 6.4 g/ml while tin’s actual density is 7.3 g/ml; a difference of only 0.9 g/ml. The metal is the same silver/grey color as tin. It is not soluble in water like tin. The metal melted around 450°C and tin melts at 231°C. Like tin, the metal has no odor nor color flame when heated. And finally, like tin, it did not react with hydrochloric acid. The solid that dissolved in water in our mixture is sugar. The… Evaluation – Evaluate how the lab went Identify at least TWO weaknesses or errors, then suggest specific and realistic improvements to the lab based on the two weaknesses identified

78. 12/18/13 Exit Task In Portugal, they allow salt water to pour into shallow pools. After a number of days in the hot sun, the sea salt can be collected from the edges of the pool. How is the solid salt separated from the sea water?

79. 12/19/13 Entry Task Based on your knowledge that flames are hotter and cooler in different regions, how might you determine the melting point of a solid? REMINDER: Homework due TOMORROW!! Cookies at stake!!

80. Melting point You can’t find melting point exactly with our equipment You can get a good range. Start with the coldest flame parts and work toward the hotter parts. The coldest part of the flame it melts in is the top of the range.

81. Melting point Temp (C  ) 1100 1000 900 800 700 600 500 300 200

82. Odor Test Some substances have a characteristic odor – think about ammonia! Be sure to waft when doing an odor test.

83. Today’s Agenda Finish Notes Think and talk and write down procedure. You may conduct the initial portion of the lab: pull out the insoluble solid and begin heating the solution. Find the density of the insoluble solid. Record physical properties. Record odor.

84. Procedure Goggles on Pull insoluble solid out of solution with tweezers and dry on paper towel. Pour 50-100 mL of the solution into the small beaker and begin warming on low heat. Find the mass and volume of the insoluble solid. Calculate its density.

85. Take solid to Ms. Maring to do an acid test. Conduct a flame test on the insoluble solid. Determine approximate melting point of insoluble solid by starting in the coolest part of the flame and moving the substance upwards until it just begins to melt. Use wafting to conduct and record odor. Complete above tests on separated dissolved solid after Holiday Break.

86. 12/19/13 Entry Task What methods would allow you to determine these characteristics: – Physical properties – Odor – Solubility – Density – Flame test – Melting point

87. 12/20/13 Entry Task Say Something Nice Tally HW percent and GET COOKIES if you meet your goal. I will hand you your cookies as you exit the classroom! Hand in HW.

88. Today’s Agenda Conduct acid test, flame test, and melting point test on the insoluble solid. Refer to chart and guess what the insoluble solid is. Write your conclusion based on evidence for the insoluble solid.

89. 12/20/13 Exit Task Trade and Grade Turn in your Entry/Exit Task Sheet for the week. HAPPY HOLIDAYS