Physical Science CHS 2013-14

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Physical Science CHS 2013-14. Unit 3 Properties of Matter. 12/2/13 Week of 12/2 to 12/6. Entry Task Find a definition for ATOMS and ELEMENT in the textbook. . Today’s Agenda. Get out your Newton Movie Questions. Read through them together so that you know what you are listening for.

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### Physical Science CHS 2013-14

Unit 3

Properties of Matter

12/2/13Week of 12/2 to 12/6
• Find a definition for ATOMS and ELEMENT in the textbook.
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.
12/2/13
• Describe some themes in Newton’s life.
12/3/13
• 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.
C-notes on pages 178-182 and 190-194

Vocabulary (left) – meanings (right)

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.

• Element
• Compound
• Atom
• Molecule
• Mixture
• Pure Substance
• Solid
• Liquid
• Gas
• Plasma
• Intermolecular Forces
• Melting Point
• Boiling Point
C-notes on pages 178-182 and 190-194

Vocabulary (left) – meanings (right)

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.

• Element
• Compound
• Atom
• Molecule
• Mixture
• Pure Substance
• Solid
• Liquid
• Gas
• Plasma
• Intermolecular Forces
• Melting Point
• Boiling Point
12/3/13
• Explain the difference between an element and a compound.
12/4/13
• 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.
Today’s Agenda – Learn about Bunsen Burners
• What is a Bunsen Burner - history
• Video Tutorial – the one minute version
• Slow down! – How 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?
Label the parts
• air intake
• combustion nozzle
• barrel/body tube
• gas jet (point to inside)
• base
• gas valve/dial
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
Steps to Light and Turn Off
• Wear safety goggles, tie back long hair, no loose clothing.
• Check striker for sparks.
• Attach hose to burner and gas line .
• Turn barrel clockwise to close and then open slightly to let a small amount of air flow.
• Turn gas valve/dial counter clockwise to close.
• turn on gas by rotating valve parallel to hose.
• Open gas valve/dial slightly – should hear faint hissing.
• Hold striker at 45 degree angle and light.
• For a taller flame – open gas valve/dial more to allow more gas. For a shorter flame – turn gas valve/dial back counter clockwise.
• For a hotter flame – turn barrel counter clockwise (increases air flow). Flame should turn blue.
• For a cooler flame – turn barrel clockwise (decreases air flow). Flame should turn orange.
• The ideal flame is pale blue with a darker blue core. Draw a picture of the flame.
• To turn off: turn barrel clockwise for a cooler, orange flame. Completely turn off the gas valve/dial. Turn off gas line.
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.
12/4/13
• What part of the Bunsen Burner flame is the hottest? Draw a picture or explain
12/5/13
• Fill in the blanks:
• Attach hose to _______ and ________ .
• Turn barrel _________ to close and then open slightly to let a small amount of air flow.
• Turn __________ _______-_______ to close.
• turn on gas by rotating valve _________ to hose.
• Open gas valve/dial slightly – should hear __________.
• Hold _________ at 45 degree angle and light.
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.
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 _________.
12/6/13
• Say Something Nice
Today’s Agenda
• Unit2 MC tests will be returned to you.
• 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.
12/6/13
12/9/13Week of 12/9 to 12/13
• 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.
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.
12/9/13
• 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.
12/10/13
• 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!!
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
• Flame Test Lab – using colors to determine chemical elements. NEVER LEAVE FLAME UNATTENDED.
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
• Flame Test Lab – using colors to determine chemical elements. NEVER LEAVE FLAME UNATTENDED.
12/10/13
• CANCELLED DUE TO PERFORMANCE ASSESSMENTS.
12/11/13
• 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
Today’s Agenda
• Finish Performance Assessments and Bunsen Burner Licenses.
• 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!!!
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!
12/11/13
• CANCELLED DUE TO PERFORMANCE ASSESSMENTS.
• IF TIME – What colors did the flame tests show?
• Cobalt –
• Magnesium –
• Calcium –
• Barium –
• Potassium –
12/12/13
• Discuss yesterday’s flame test results.
• Give a definition of DENSITY.
• Get out homework. Calculate percent and QUICK review!

### The Nature of Matter

Classifying Matter

Matter

Are all the particles alike?

YES

NO

Pure Substance

Mixture

Are the particles one kind of atom?

Are the particles well-mixed and mixed evenly?

YES

NO

YES

NO

Homogeneous Mixture

Heterogeneous Mixture

Compounds

or Molecules

Element

Pure Substances

• 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…..
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 C6H12O6
• made up of carbon, hydrogen, and oxygen
• looks nothing like C, H, O by themselves
• can be broken down when burned

Mixtures

• 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
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®

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
Density

v

D = m/v

D = density

m= mass

v= volume

Example problem

• A piece of lead has a mass of 56.4 g and a volume of 5 mL.Calculate its density.

Density

D = 56.4 g/ 5 mL

D = 11.28 g/mL

Same as…

D = 11.28 g/cm3

Mass = 56.4 g

Volume = 5 mL

D = m/v

ml is same as cm3 so sometimes see g/cm3

12/12/13
• 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?
12/13/13
• Say Something Nice
• REMEMBER – Be nice about someone’s character, effort, behavior, respect or integrity.
Today’s Agenda
• Finish Notes
• If time: start Density Lab
12/13/13
• Post It Notes inside comp book if other labs still need to be graded:
• Speed Lab?
• Egg Drop?
12/16/13
• Look at the following chart. What is the densest material? How can you tell? What are the units?
• Collect your comp book. Tomorrow we will revise the pendulum lab.
Density of Substances
• Purpose
• Determine the densities of four solids, two liquids, and then compare to the actual answers.
• Materials
• balance, graduated cylinder, ruler, calculator
• 6 substances
• little stopper, big stopper, yellow liquid, green liquid, Cu cube, Cu wire,

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

(100)

12/16/13
• Would you expect the copper wire and copper cube to have the same density? Why or why not?
12/17/13
• 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!
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.
12/17/13
• 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.
12/18/13
• 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?

### Solutions

Identification of dissolved Solids and a metallic solid

What is a solution?
• Solution: A mixture that is homogeneous down to the molecular level

Example:

think Koolaid…

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
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.
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.
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
Name … Partners…Separation and Identification of Two Solids in Water
• Question
• What are the two solids (one soluble, one insoluble) mixed in the water?
• Materials
• Beakers – small, large
• balance/scale
• Solution with dissolved solids and a metallic solid
• hot plate
• Lab scoop
• safety goggles
• Tweezers
• Tongs
• Plastic dish
• 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
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
12/18/13
• 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?
12/19/13
• 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!!
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.
Melting point

Temp (C)

1100

1000

900

800

700

600

500

300

200

Odor Test
• Some substances have a characteristic odor – think about ammonia!
• Be sure to waft when doing an odor test.
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.
Per 1 - Procedure
• Goggles on and hair tied back.
• Use tweezers to remove the insoluble solid and place on paper towel.
• Pour 50 mL of solution into smaller beaker and place on hotplate at low temp (2-4)
• Check mass and volume and calculated density of insoluble solid while waiting.
• Write down physical properties of insoluble solid.
• Conduct odor test.
• Conduct flame test wearing gloves at bunsen burner.
• Conduct melting point test in bunsen burner flame moving solid from cool to hot to record range.
• Take to Ms. Maring for acid test in fume hood.
• Before leaving lab, use tongs to lift smaller beaker off hot plate and pour concentrated solution into plastic dish. Turn off hotplate. Team number on dish and place on shelf.
• Complete these tests for separated soluble solid AFTER XMAS BREAK!!!!!
Per 2 - Procedure
• Goggles on and hair tied back.
• Take insoluble solid out of solution with tweezers and place on paper towel.
• Find mass and volume and calculate density of insoluble solid. Record.
• Pour 50 mL of solution into small beaker, place on hotplate (2-4).
• While waiting you can conduct other tests.
• Conduct flame test on solution. Record color of flame.
• Observe and record physical characteristics, conduct odor test, is it soluble.
• Conduct a flame test and a melting point test on insoluble solid. Place hot solid in beaker with water to cool.
• Conduct acid test – take to Ms. Maring at fume hood.
Per 3 - Procedure
• Safety gear – goggles and pull back hair
• Get the insoluble solid out with tweezers and place it on paper towel.
• Pour 50 mL of solution into small beaker, plug in and turn on hotplate (2-4).
• Observe and record physical properties of insoluble solid, odor test, find mass/volume and calculate density, answer: is it soluble?
• Conduct flame test on solution and insoluble solid.
• Conduct melting point test on insoluble solid. Put hot solid in beaker of cold water.
• Take insoluble solid to Ms. Maring. She will conduct acid test at fume hood.
• RECORD ALL DATA!
• Use tongs to lift hot beaker and pour into plastic dish. Scrape any solids with scoopula. Team # on dish, dish on shelf. Turn off hotplate.
• Conduct all the above tests on separated soluble solid after XMAS BREAK
Per 4 - Procedure

1. Put on goggles and tie hair back

• Use tweezers to remove insoluble solid from solution and place on paper towels.
• Pour 50 mL of solution into small beaker, place beaker on hotplate, plug in, turn on to 2-4.
• Conduct solubility test, odor test, find mass and volume and caculate density, record physical properties.
• Conduct flame test and melting point test in bunsen burner flame. Use gloves and tongs. Drop hot solid into beaker of water to cool.
• Take solid to Ms. M at fume hood for acid test.
• Use tongs to take small beaker off hotplate. Pour and scrape concentrated solution into dish. Team # on bottom and place dish on shelf. Let beaker cool before placing on counter. Turn off hotplate.
• Conduct all the above tests on soluble solid after XMAS BREAK!!
Per 6 - Procedure
• Goggles and hair tied back.
• Use tweezers to pull insoluble solid out of solution.
• Pour 50 mL of solution into small beaker, place on hotplate, turn on to 2-4.
• Conduct odor test, say if soluble in water, calculate density, record physical properties, of the insoluble solid.
• Conduct flame test on solution with paperclip.
• Conduct flame test on insoluble solid.
• Conduct melting point test on insoluble solid.
• Take solid to Ms. M at the fume hood for acid test.
• Use tongs and pour concentrated solution into dish, scrape with scoopula. Team # and place on shelf. Turn off hotplate.
• Conduct all the above tests on the soluble solid AFTER XMAS BREAK!!!!

10. Use tongs to pour concentrated solution into plastic dish. Turn off hotplate. Let beaker cool to set on counter. Put team # on dish, place on shelf.

• 11. CONDUCT ALL THE ABOVE TESTS on soluble solid after XMAS BREAK!
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.

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.
12/19/13
• What methods would allow you to determine these characteristics:
• Physical properties
• Odor
• Solubility
• Density
• Flame test
• Melting point
12/20/13
• 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.
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.
12/20/13
• HAPPY HOLIDAYS
1/6/14Week of 1/6 to 1/10
• Recall and describe the lab we were working on before winter break. What is our goal? What methods were we using?
• Homework: Read pages 536-544. Answer questions 1-7 on page 545. Due Thursday 1/9/14.
Possible Sludge Materials
• Look through chart – individually
• Discuss – how could you use this chart in your current lab?
• Resume lab activities: COMPLETE ALL TESTS ON INSOLUBLE SOLID
• Conduct acid test, flame test, and melting point test, density on the insoluble solid.
• Refer to chart and guess what the insoluble solid is.
• Write your conclusion based on evidence for the insoluble solid.
1/6/14
• What substance do you think the insoluble solid is?
• List 2 pieces of evidence in support of this conclusion using your data table.
1/7/14
• Based on the solubility and physical properties (appearance) of the recrystallized solid, list the materials from the chart that it might be.
• REMINDER Homework: Read pages 536-544. Answer questions 1-7 on page 545. Due Thursday 1/9/13.
• Set new HW goals!
Today’s Agenda
• Complete evaporation and testing on soluble solid.
• DATA TO COLLECT for SOLUBLE SOLID:
• Physical properties
• Odor
• Solubility
• Flame test
• Melting point
• AT THE LAST: find mass of remaining soluble solid. Bring that up to fume hood to find volume IN ALCOHOL (discuss why we won’t find volume in water!)
• Finished early? Start your conclusion using evidence!!
Melting point

Temp (C)

1100

1000

900

800

700

600

500

300

200

1/7/14
• What do you guess the soluble solid is?
• Use at least 2 pieces of evidence to support your answer.
1/8/14
• EXPLAIN HOW YOUR CONCLUSION will be “logical, based on evidence, and consistent with prior established knowledge.”?
• REMINDER Homework DUE TOMORROW: Read pages 536-544. Answer questions 1-7 on page 545. Due Thursday 1/9/13.
• Watch demonstration of finding density of insoluble solid. Do you need to revise your density?
Today’s Agenda
• Write and Refine conclusions – you may discuss this in teams but each person will write the conclusion in their lab books. Your conclusion should summarize ALL DATA COLLECTED and COMPARE TO REFERENCE SHEET!
• 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.
• Identify at least TWO weaknesses or errors, then suggest specific and realistic improvements to the lab based on the two weaknesses identified
1/8/14
• Explain the 2 weaknesses of your lab and how you could improve those areas.
1/9/14
• Can you think of any ways to separate a solution of 2 liquids?
• 15 minutes to finish CONCLUSIONS – turn in.
• HAND BACK PAPERS – place in binder
Today’s Agenda
• Notes on Last Practice Lab before Sludge: Fractional Distillation.
Fractional Distillation
• Question
• How can a mixture of two liquids be separated and identified?
• Materials
• fractional distillation apparatus
• liquid mixture
• Bunsen burner and striker
• 1 large and 2 medium test tubes and stoppers
• Test tube rack
• Triple beam balance and graduated cylinder (day 2)

Procedure

• Hair back and goggles on entire lab.
• Get 15 ml of the liquid mixture (never fill the test tube you are heating more than 1/3 full).
• Make sure there are about 10 boiling chips in the test tube you will be heating.
• Heat with Bunsen burner on the lowest heat possible in order to maintain a mild, rapid boil. Flame should be orange and gas very low.
• Carefully watch the temperature.
• Keep the rubber tube out of the liquid you are “making”.
• AFTER the temperature has leveled off for a while and then begins to rise again– carefully switch test tubes to “catch” the second liquid.

Data Collection/Observations

• Record the boiling point temperature for first and second liquid (place where temperature levels off)
• Complete physical properties, density, and odor tests.
• Come to the front to complete flammability test and acid test.
• Conclusion
• State your two liquids and give ALL THE EVIDENCE for ONE of them.
• Based on evidence, our first liquid was propanol.
• Our second liquid was hydrogen disulfide. It had a slight yellow color and hydrogen disulfide is a yellow oil. Our calculated density was 1.4 g/ml and hydrogen disulfide’s density is 1.3 g/ml. That is only a 0.1 g/ml difference Like hydrogen disulfide, our liquid is not flammable………..
1/10/14
• Say Something Nice
Today’s Agenda
• Day 1 - Fractional Distillation Lab – separate liquids.
• VERY LOW HEAT ORANGE FLAMES ONLY!!!!!!
• Once separated, stopper the test tubes. Label test tube rack with your names. Place on class shelf.
1/10/14
1/13/14Week of 1/13 to 1/17/14
• Based on the physical properties (and appearance) and boiling points of the two liquids, what do you predict they are?
• Complete notes for end of lab…

Data Collection/Observations

• Record the boiling point temperature for first and second liquid (place where temperature levels off)
• Complete physical properties, density, and odor tests.
• Come to the front to complete flammability test and acid test.
• Conclusion
• State your two liquids and give ALL THE EVIDENCE for ONE of them.
• Based on evidence, our first liquid was propanol.
• Our second liquid was hydrogen disulfide. It had a slight yellow color and hydrogen disulfide is a yellow oil. Our calculated density was 1.4 g/ml and hydrogen disulfide’s density is 1.3 g/ml. That is only a 0.1 g/ml difference Like hydrogen disulfide, our liquid is not flammable………..
Today’s Agenda
• Complete tests on the two liquids: Liquid A and B
• Tests to complete:
• Physical Properties
• Density
• Odor Test
• Flammable? Watch demo!!! Come to the front desk for this.
• React with acid?
• Write your conclusion in your comp book: State the 2 liquids; write evidence for ONE!
1/13/14
• State the 2 liquids and explain which two pieces of evidence were most helpful.
1/14/14
• WRITE THIS DOWN:
• End of Semester is January 31st.
• ANY missing work for this unit due by next Friday, January 24th!!
Today’s Agenda
• Hand back papers and organize binders
• Write down work you may be missing.
• DURING FIRST 15 minutes – you can work on YOUR CONCLUSION for the fractional distillation lab – IN YOUR COMP BOOK!
• SLUDGE QUIZ – you must pass – Sludge starts tomorrow.
1/14/14
• None – taking Sludge Quiz
1/15/14
• Today you will be given a sludge mixture with 8 unknown substances, including insoluble solids, a soluble solid, and two liquids. What might you most easily separate first?
• TURN IN COMP BOOKS TO SHELF.
Today’s Agenda
• New seats and team mates
• Discuss
• Fix Answers – you’ll need 13/15 correct to proceed.
• Handout Data Table, Points Sheet
• Review Lab
• 3 grades – Participation, Lab, Written (Final)
• Create Daily Log Sheet
• RECORD SLUDGE MIXTURE NUMBER!!!!!
• Separate and test a metal
• Last 5 - Clean Up
1/15/14
• What is your goal for tomorrow’s Sludge Lab?
• What will your first steps be?
1/16/14
• Which strengths do you bring to group work?
• Application Standard: “I can work collaboratively with other students to generate ideas for solving a problem.”
• http://www.uvm.edu/~wfox/CollaborativeSkills.html
Today’s Agenda
• Take notes in your daily log.
• Separate at least 1 insoluble solid.
• You have been given 5 plastic dishes.
• DELEGATE! Everyone should be working.
• Do not WANDER from station. You will lose participation points.
• Complete all tests per substance!
• Draw a conclusion?
• Start tests on next substance.
• CLEAN-UP! Sludge left out = points lost
1/16/14
• Use 2 pieces of evidence from your tests and compare to the reference chart, to suggest the name of one substance.
Melting point

Temp (C)

1100

1000

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800

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600

500

300

200

1/17/14