Download - Shauna Webb, AMSTI Adapted by Ashlynn Frith PROPERTIES OF MATTER STUDY PPT FOR LESSONS 1-11
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Shauna Webb, AMSTI Adapted by Ashlynn Frith
PROPERTIES OF MATTERSTUDY PPT FOR
LESSONS 1-11
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LESSON 1 – OUR IDEAS ABOUT MATTER
You will perform a circuit of eight inquiries to observe how matter
behaves. The inquiries involve the following: different states of matter, changes of state, mass and volume,
floating and sinking, thermal expansion, mixtures, solubility and insolubility, and
chemical reactions.
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LESSON 1 – QUESTION
What is matter?
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LESSON 1 – CONCLUSION
oMatter - the physical material that has mass and occupies space.oAir is a gas.oAir and gases are forms of matter even though they are invisible.oThe shape of an object does not affect its mass.oSome matter is soluble in water.oAll liquids are not water or do not contain water.oTemperature change affects the volume of air.oSome liquids do not mix = Immiscible
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LESSON 1 – VOCABULARY (1-4)
1. matter - the physical material that has mass and occupies space
2. expansion - the increase in the volume of matter that occurs when matter is heated.
3. contraction - decrease in volume of matter when matter is cooled.
4. dissolving - the process that takes place when a solvent is mixed with a solute to make a solution.
5. immiscible - liquids that are unable to dissolve in one another.
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LESSON 1 – VOCABULARY (2-4)
6. miscible - liquids are able to dissolve in one another.
7. density - the mass of a known volume of a substance; measured in g/cm3
8. chemical reaction - any change that involves the formation of a new substance; has reactants and products.
9. mass - the amount of matter in an object; measured in g or kg.
10. volume - the amount of space occupied by matter; measured in L, mL, cm3, or m3.
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LESSON 1 – VOCABULARY (3-4)
11. burning - a rapid chemical reaction between a substance and a gas that produces heat and light. Most burning or combustion takes place in the air and has oxygen as one of its reactants.
12. solid - a phase or state of matter in which a substance has definite shape and volume.
13. liquid - a state or phase of matter in which a substance has a definite volume but no definite shape. Liquids take the shape of the container they occupy.
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LESSON 1 – VOCABULARY (4-4)
14. mixture - two or more elements or compounds that are mixed together but are not chemically combined.
15. physical property - all the characteristic properties of a substance except those that determine how it behaves in a chemical reaction
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LESSON 2 – DETERMINING DENSITY
You will use mass and volume measurements to calculate
the densities of water, regular shaped objects, and irregular
shaped objects.
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YES NO STATEMENT YES NO1. An object floats/sinks based solely on its mass
2. Mass and volume are interchangeable terms3. Mass is affected by
changes in shape4. Density and weight are
the same5. Mass and weight are the
same
ANTICIPATION/REACTION GUIDE (INQUIRY 2.1-2.3)
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LESSON 2 – QUESTION
How will the densities of 25mL & 50 mL of water
compare?
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LESSON 2- HYPOTHESIS
Take 2 minutes to create your own hypothesis:
If…….. then….. because……..
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LESSON 2- HYPOTHESIS
If you measure the density of 25mL and 50 mL of H2O, then
it will be different because there are different amounts of
water being measured.
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LESSON 2- PROCEDURE
Step 1- Take the mass of the empty graduated cylinder.
Step 2- Add 25mL of H2O to one graduated cylinder and 50 mL of H2O to the other graduated cylinder.
Step 3- Measure mass of each graduated cylinder with the water.
Step 4- Subtract the mass of the empty graduated cylinder from the new measurement for the graduated cylinder containing 25mL of H2O and repeat for the 50mL of H2O
Step 5- Calculate the density of water (mass/volume) Round your answer to the nearest tenth.
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LESSON 2.1- RESULTS
Volume of
Water (cm3)
Mass of emptyGradua
tedCylinde
r (g)
Mass of Graduat
ed Cylinder and Water
(g)
Mass of
Water(g)
Density of water
g/cm3
2550
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LESSON 2.1-CONCLUSION
Does changing the vol. of water change the density of water? Does changing the mass of water change the density of water? What is the density of water in grams/cm3?
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LESSON 2.1- LESSON 2.1- VARIABLESVARIABLES
Independent variable:
Amount of water
Dependent variable:
The density
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INQUIRY 2.2 QUESTION
Will all of the blocks have the same density?
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LESSON 2.2- LESSON 2.2- HYPOTHESISHYPOTHESIS
If we compare the densities of the blocks, then the aluminum will have a larger density because it is a metal.
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LESSON 2.2- PROCEDURE
Step 1- measure the length x width x height Step 2- mass each item on the balance Step 3-divide the mass by volume to get density
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Comparing the Densities of Comparing the Densities of Different SubstancesDifferent Substances
Substance
Length (l)(cm)
Width (w)(cm)
Height (h)
(cm)
Volume (v)
(cm3)(v=l x w
x h)
Mass(m)(g)
Density
(g/cm3)
(m/v)
WAXTRANSPA
RENTWHITE PLASTICALUMINU
M
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LESSON 2.2- LESSON 2.2- CONCLUSIONCONCLUSION
Are the densities of the different substances the same or different? DifferentHow could this information be used to identify the substance from which an object is made? YOU COULD IDENTIFY THE OBJECTS BY CALCULATING THE DENSITY AND COMPARING IT TO A DENSITY CHART
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NEXT STEPNEXT STEP
Measure objects with IRREGULAR shape
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INQUIRY 2.3 QUESTION
How do you measure the density of irregular objects?
Or Which of the irregular objects will have the
greatest density?
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LESSON 2.3- LESSON 2.3- HYPOTHESISHYPOTHESIS If we measure all of the objects, then the copper
cylinder will have the greatest density because it
has more mass than the steel bolt and nylon
spacer.
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STEP 1: MEASURE MASS OF OBJECT
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STEP 2: ADD H2O TO THE GRADUATED CYLINDER
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STEP 3: ADD OBJECT TO THE GRADUATED CYLINDER
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STEP 4: CALCULATE DENSITY
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LESSON 2.3- LESSON 2.3- PROCEDUREPROCEDURE
STEP 1- Measure the mass of the objects using the balance STEP 2- Fill the graduated cylinder with enough water to cover the objects and record the volume STEP 3- Insert the object into the graduated cylinder STEP 4- Subtract the two volumes and record the volume of the object STEP 5- Calculate density
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ObjectObject MassMass(g)(g)
Volume of Volume of water water
without without object (mL)object (mL)
Volume of Volume of water and water and
object (mL)object (mL)
Volume of Volume of object (mL)object (mL)
DensityDensity(g/mL)(g/mL)
COPPERCOPPERCYLINDERCYLINDER
STEELSTEELBOLTBOLT
NYLONNYLONSPACERSPACER
INQUIRY 2.3: COMPARING THE COMPARING THE DENSITIES OF DIFFERENT DENSITIES OF DIFFERENT SUBSTANCESSUBSTANCES
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LESSON 2.3- LESSON 2.3- CONCLUSIONCONCLUSION
1. Are any of the blocks from inquiry 2.2 or objects from this inquiry made from the same substance?
2. What evidence do you have for your answer?
3. How do the densities of these objects compare with water?
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REFLECTING QUESTIONSREFLECTING QUESTIONS
A. What is the difference between mass and volume?
Mass is the amount of matter in an object
Volume is how much space it takes up
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REFLECTING QUESTIONS REFLECTING QUESTIONS CONT…CONT…
B. What units did you use to measure mass/volume?
g or kg/ ml and cm3.
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REFLECTING QUESTIONS REFLECTING QUESTIONS CONT…CONT…
C. How did you calculate the density of an object?
D=m/v
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REFLECTING QUESTIONS REFLECTING QUESTIONS CONT…CONT…
D. What units did you use for density?
g/cm3 or g/ml
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REFLECTING QUESTIONS REFLECTING QUESTIONS CONT…CONT…
E. Does changing the amount of a substance change its density?
no
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CONCLUSION QUESTION CONCLUSION QUESTION CONT…CONT…
F. If two objects are made of the same substance, will they have
the same density?
Yes
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LESSON 2.3- ERROR LESSON 2.3- ERROR ANALYSISANALYSIS
Not completely submerging the object
Spilling water/splashing some water
Incorrect calculationsNot using the volume of the
object
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LESSON 2- CONCLUSIONoDensity is calculated by dividing the mass
by the volume; measured in grams per cubic centimeter (g/cm3).
oMass is the amount of matter in an object; measured in grams.
oVolume is the amount of space taken up by an object; measured in ml or cm3.
oDifferent objects made of the same material will have the same density.
(characteristic property)
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LESSON 2 – CONCLUSION CONT.
oChanging the amount of a substance does not change the
density of the substance.oMass is not affected by shape.
oDensity is a characteristic property of matter.
oCharacteristic property - property that is independent of mass, volume,
and shape.
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LESSON 3 – DENSITY PREDICTIONS
You will predict whether the blocks you investigated in Inquiry 2.2 will
float or sink. After finding the density of three liquids, you will predict the order in which the
liquids will layer when you build a density column. You will calculate and predict whether objects will
float or sink in the density column.
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ANTICIPATION/REACTION ANTICIPATION/REACTION GUIDE - INQUIRY 3GUIDE - INQUIRY 3
Yes No Statement Yes No
1. All objects that float are hollow or contain air.
2. density indicates thickness
3. viscous liquids are denser than thin liquids
Before After
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LESSON 3 - QUESTION
If we mix the syrup, oil, and water how will they
behave?
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LESSON 3 - HYPOTHESIS
If… then… because…
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LESSON 3- HYPOTHESISLESSON 3- HYPOTHESIS
If we add all 3 ingredients together, then the corn syrup
will sink because it has the greatest density
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LESSON 3- RESULTS OF FLOATING & SINKING OBSERVATIONS
SubstanceDensity (g/cm3)
Floats or sinks?
Prediction Results
wax block
white plastic block
transparent plastic block
aluminum block
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LESSON 3- PROCEDURE
Step 1- Take the mass of graduated cylinder A & B
Step 2- Add 25ml of corn syrup to graduated cylinder A / 25ml of oil to B
Step 3- Take the mass of both again
Step 4- Subtract to get the mass of the liquids
Step 5- Calculate using mass/volume
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CALCULATING DENSITY – LESSON 3
LiquidVolume
(cm3)
Mass of graduated cylinder
only
(g)
Mass of graduated cylinder
plus water
(g)
Mass of liquid
(g)
Density
(g/cm3)
Vegetable oil
Corn syrup
Water __ ___
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CONCLUSIONCONCLUSION
Do the liquids mix (miscible) or not (immiscible)?
ImmiscibleWhat is the relationship between the density of a liquid and its position?
A higher density liquid is on bottomA lower density liquid is on top
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REAL LIFE APPLICATION
Oil is less dense than water. It can be applied
to cleaning up a spill from an oil tanker.
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HOW COULD YOU CLEAN UP 11 MILLION GALLONS
OF OIL?
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ANSWERS
Dilute the oil using chemicals.Breaks down oil into small particles so that it can spread throughout the ocean. Then bacteria break it down further.
Set the oil on fireDrawback: causes a lot of pollution
Suction the oil with a vacuum, skimmers
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INQUIRY 3.1
Independent variable25ml of liquidThe type of liquid
Dependent variableThe position of the objects in the liquid due to the density
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INQUIRY 4.1: GETTING STARTED
Step 1- the air occupied all of the space and prevented the liquid from passing through. Step 2- The other syringe is pushed out Step 3- Air has mass and volume or density
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LESSON 4 – DO GASES HAVE DENSITY
You will determine the mass, volume, and density
of a bottle of air.
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LESSON 4 - QUESTION
If air has mass & volume, what is
the density of air?
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LESSON 4- HYPOTHESIS
If air has density, then it should be less than 1g/cm3 because air floats and is less dense than water.
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LESSON 4- PROCEDURE
(1-2)
Step 1- measure the entire apparatus with air Step 2- suction the air out using the pump Step 3- re-measure the entire apparatus with out air Step 4- subtract the 2 masses
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LESSON 4- PROCEDURE
(2-2)
Step 5-fill the container with water and add valve until water overflows Step 6- measure water with grad. cylinder Step 7- divide the mass by volume in step 6
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LESSON 4- FINDING THE DENSITY OF AIR
Mass of bottle,
washer, & rubber valve, pump
(g)
Mass of bottle,
washer, & rubber valve
after removing
air, pump (g)
Mass of air
(g)Volume of
air
(cm3)
Density of air
(m/v)
(g/cm3)
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LESSON 4- CONCLUSIONCONCLUSION
How does the density of air compare with the density of solids and liquids? The density of air is much smaller than the density of solids and liquids
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LESSON 4- CONCLUSIONCONCLUSION
Are the results the same? No
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LESSON 4- CONCLUSIONCONCLUSION
Why do some things float in air?
Because their overall density is less
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CONVERSIONS
STANDARD FORM
0.00082g/cm3
0.00094g/cm3
SCIENTIFIC NOTATION
8.2 x 10-4 g/cm3
9.4 x 10 –4 g/cm3
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NEXT STEP/NEW QUESTION
The water is pumped into the ballast to sinkTo rise air is pumped in pushing the water out
How is density used to control the floating and sinking of a submarine?
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ERROR ANALYSIS
Different amounts of air was removedDifferent number of pumps at each groupMeasured the water incorrectlyAir may have seeped back into the bottle
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REAL-LIFE APPLICATION Bony fish have a swim bladder
It is filled with gases produced in the fish’s blood
Swim bladder fills with gas= floats
Swim bladder empties gas= sinks
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VARIABLES
INDEPENDENT The amount
of air evacuated or
removed
DEPENDENT The density of
air
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HIGH DENSITY VS. LOW DENSITY
Brick wall Are the
particles close together or far
apart? High density or
low density?
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HIGH DENSITY OR LOW HIGH DENSITY OR LOW DENSITYDENSITY
What gas do cows give off?
Methane helps replace carbon in our environment
Are the gas particles close together or far
apart?
High density or low density?
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DEADLY DENSITY PG. 44
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STUDY TIME! TEST ON LESSONS
1-4
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DON’T FORGET…
Independent variable- The variable you control/the one you change on purpose Dependent variable- The variable that is controlled by the independent variable/the one you measure
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BE ABLE TO LIST 6 SIGNS OF A CHEMICAL REACTION:
Gas/bubblesExpandedChange in temperatureChange in formChange in colorChange in texture( from soft to hard)
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How do you find density?Mass/ Volume
Define massThe amount of matter in an object
Define volumeThe amount of space an object takes up
QUICK REVIEW:
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WHAT 2 PIECES OF EQUIPMENT MEASURE VOLUME?
Graduated cylinder
Ruler
L x W x H
Look at the numbers on the side.
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CHARACTERISTIC PROPERTY
Density is a characteristic property.
This means it is used to identify different objects because it never changes!
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DENSITY NEVER CHANGES!
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Know the density of water1g/cm3
MassGrams (g)Volumeml, cm3
Density g/cm3
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EQUIPMENT
BALANCE-MEASURES MASS
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A graduated cylinder is used when:A liquid is being measuredAn irregular object is being measured
A ruler is used when: A regular object is being measuredblock
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SINKING AND FLOATING
Know the relationship between sinking and floating
If the density of an object is higher than the liquid it is in-sinks
If the density of an object is lower than the liquid it is in-floats
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IMMISCIBLE OR MISCIBLE?
If 2 liquids do not mix, then they are called__________.
Immiscible
If 2 liquids do mix, then they are _______.
miscible
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Oil and water do not mix.
Oil is less dense than water
Oil is non-polar
Water is polar
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LESSON 5 – TEMPERATURE & DENSITY
You will investigate the effect of temperature on the volume of
matter by building and calibrating a thermometer filled with water. After constructing the liquid-filled thermometer, you will replace the
water with air. You will also observe the effect of heat on a
bimetal strip.
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LESSON 5 – GETTING GETTING STARTEDSTARTED 2a. Temperature 2b. The bulb 2c. The bulb 2d. -20 to 110, 1 degree Celsius 2d. Top of the red liquid 2f. They are the same
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LESSON 5 – GETTING GETTING STARTED CONT…STARTED CONT…
3a. The liquid in the thermometer rises if the room temperature is below body temp.3b. Body temperature will appear to be about 37 degrees celsius3c. Liquid contracts as temp goes down3d. Because the bulb is in the air, they are measuring air temp3f. Liquid expands when heated
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ANTICIPATION/REACTION GUIDE INQUIRY 5.1
Before After
YES NO STATEMENT YES NO
Temperature is a measure of the heat of an object.
Thermometers measure heat.
“Heat” refers to objects that are hot compared with the reference point of
body temperature.
Heat is a fluid-like substance that flows from one place to another.
“Cold” can move into an object.Ex) “cold” from ice water moves into
thermometers, pushing the liquid down
Liquid in a thermometer goes up the tube because hot substances-such as
hot air in a balloon- rise.
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LESSON 5 – QUESTION
What is the relationship between temperature
and density?
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LESSON 5 – HYPOTHESIS
If the temperature increases, then
density will decrease because the particles
are moving farther apart.
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LESSON 5 – PROCEDURE
oDraw your design for a thermometer.
oFill test tube with water
oInsert tubing with stopper into the test tube
oPlace in cold water bath and mark the line (5 min)omeasure the temp._____ ** before removing
oPlace in hot water bath and mark the line (5 min)omeasure the temp._____ ** before removing
oMeasure the distance between the two lines in mm
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LESSON 5 – PROCEDURES CONT…PROCEDURES CONT…
To get equal increments:Divide (distance in mm) = every 1 degree
(temp. difference)Celsius
Next, multiply by 5 to get 5 degree increments
Finally, mark off the temp. scale in 5 degree increments
Test your thermometer by measuring room temperature and comparing it to the lab thermometer
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LESSON 5 – RESULTSRESULTS
Temp. of Cold water
bath (oC)
Temp. of Hot water
bath (oC)
Temperature difference
(oC)
Distance between
markings (mm)
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LESSON 5 – CONCLUSIONCONCLUSION
1. What reading did your thermometer give for room
temperature? What reading did the lab thermometer give?
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LESSON 5 – CONCLUSIONCONCLUSION
2. How accurate is your thermometer?
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LESSON 5 – CONCLUSIONCONCLUSION
3. How quickly does your thermometer respond to temperature changes?
Student thermometers respond more slowly than alcohol
thermometer
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LESSON 5 – CONCLUSIONCONCLUSION
4. When the temperature increases, what happens to the volume of
water?
An increase in volume with an increase in temp
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5. when the temperature increases, do you think the total
mass of water changes?
No change in mass.
LESSON 5 – CONCLUSIONCONCLUSION
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6. If you decreased the size of the bulb, how would the
accuracy and response time change?
Smaller bulbs would be quicker to respond but would be less
accurate
LESSON 5 – CONCLUSIONCONCLUSION
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7. How could you improve the design of the thermometer?
Using different liquids, thinner tubes
LESSON 5 – CONCLUSIONCONCLUSION
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LESSON 5 – VARIABLESVARIABLES
Independent Variable
Type of tubing (plastic)
Type of liquidTemp. of water
Amount of time in bath
Size of bulbAmt. Of tubing
inserted
Dependent Variable
Distance between markings
Temperature readings
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LESSON 5 – ERROR ANALYSIS
1. Incorrectly calibrating thermometer
2. Incorrectly measuring temp
3. Waiting too long to mark the plastic tubing
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LESSON 5.2- GETTING 5.2- GETTING STARTEDSTARTED
1a. By adding a small water column 1b. By the distance the water column moves
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What effect will replacing the liquid-filled thermometer
with air have on density?
INQUIRY 5.2
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LESSON 5.2 – HYPOTHESISHYPOTHESIS
If we place the air-filled thermometer in the hot water bath, then it will be less dense because
the particles are expanding.
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LESSON 5.2 – CONCLUSIONCONCLUSION
3a. What problems did you encounter when calibrating your air-filled thermometer?
3b. How did the sensitivity of your air-filled thermometer compare with that of your liquid-filled one?The sensitivity is much greater for the air-filled thermometer
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REAL-LIFE APPLICATIONREAL-LIFE APPLICATION
Gases expand when heated-density decreases Gases contract when cooled-density increasesDuring winter= over inflate your tiresDuring summer= under inflate your tires
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REAL LIFE APPLICATION REAL LIFE APPLICATION CONT..CONT..
When heated -water expands
When cooled -water expandsIf the temp. is going to be below freezing, then you want to run water through your pipes because your pipes will freeze and expand and the pipes will burst
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INQUIRY 5.3-QUESTIONINQUIRY 5.3-QUESTION
How will the metals react when heated?
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LESSON 5.3– HYPOTHESISHYPOTHESIS
If we heat the bimetal strip, then the strip will
expand and the density will decrease because the particles are moving apart as it
gains energy
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LESSON 5.3– RESULTSRESULTS
1. What do you think will happen when the metal strip
is heated?(sample answer) It should
curve or bend
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RESULTSRESULTS
2. What did you observe when the strip was heated?
One side of the strip expands faster causing the metal to curve because the heat is causing one
metal to gain kinetic energy faster
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RESULTSRESULTS
3. What happens after the strip is cooled?
It returns to normal after the flame is removed by
contracting
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LESSON 5.3– RESULTS RESULTS CONT…CONT…
4. What did you observe when the strip was heated on the
other side? The metal still curved in only
one direction
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LESSON 5.3– RESULTS RESULTS CONT…CONT…
5. Why do you think the strip behaves this way?
One metal is expanding more because it is gaining kinetic
energy faster
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LESSON 5.3– REFLECTING QUESTIONS
A. What do these 3 inquiries tell you about how the volume of matter is affected by temp.?Matter usually increases in
volume when heated/ decreases when cooled
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LESSON 5.3– REFLECTING QUESTIONS
B. How does the change in volume of air differ from the change in volume of liquid? Air expands more rapidly
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LESSON 5.3– REFLECTING QUESTIONS
C. How does this change in volume affect the density of solids, liquids, and gases?
Increase in volume = decrease in density, particles expand more
rapidly
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LESSON 5.3– REFLECTING QUESTIONS
D. When measuring the density of a substance why is
it important to record the temperature of the substance?
Because of fluctuations
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LESSON 5.3– REFLECTING QUESTIONS
E. Are there any other uses for the expansion and contraction
of matter?
Yes
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LESSON 5.3– REFLECTING QUESTIONS
F. Could expansion or contraction cause problems?
yes
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REAL-LIFE APPLICATION REAL-LIFE APPLICATION
When metal is heated= expansion
When metal cools= contraction
Examples: bridges, bldg., railroads
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ANTICIPATION/REACTION EXPLANATION
Temperature is a measure of the
kinetic energy of particles.
Thermometers measure
temperature.
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Density changes with temperature:
As temperature increases, density will decrease and
volume will increase (mass stays the same).expansion
LESSON 5- CONCLUSION
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Heat is a form of energy that can move from a hot place to a cooler
place (measured in joules). Temperature is a measure of kinetic energy of particles of
matter (measured by a thermometer in degrees Celsius).
LESSON 5- CONCLUSION
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Density changes with temperature:
As temperature decreases, density will increase and volume
will decrease (mass stays the same).
contraction
LESSON 5- CONCLUSION
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LESSON 5 – VOCABULARY (1-3)
32. heat - a form of energy that can move from a hot place to a cooler place; the transfer of energy from one body to another.
33. temperature - a measure of the kinetic energy of the particles that make up matter; the measurement of how hot something is.
34. Celsius - a temperature scale with the melting point of ice at 0 degrees and the boiling point of water at 100 degrees.
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LESSON 5 – VOCABULARY (2-3)
35. Fahrenheit - a temperature scale with the melting point of ice at 32 degrees and the boiling point of water at 212 degrees.
36. Kelvin - a temperature scale with the lowest possible temperature at the zero point, which is called absolute zero; ice melts at 273 K.
37. calibrate - set; measure to scale
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LESSON 5 – VOCABULARY (3-3)
38. expansion - the increase in the volume of matter that occurs when matter is heated.
39. freeze - the change in state in which a liquid turns into a solid.
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LESSON 6- ANTICIPATION/REACTION GUIDE
Yes
No
StatementYes
No
Matter is destroyed during chemical reactions.
Reactants disappear.
Gases produced during a chemical reaction is a phase
change.
A phase change is a chemical reaction.
Before
After
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LESSON 6 – APPLYING THE HEAT
You will heat pure substances and
observe and classify changes
that occur.
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LESSON 6 – QUESTION
How will the pure substances react when we
apply heat?
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LESSON 6- HYPOTHESIS
If… then… because…
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LESSON 6- HYPOTHESIS
If we heat the chemicals, then we will
notice chemical changes because each
one has different chemical properties.
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LESSON 6- PROCEDURE(1-2)
Step 1-Place one lab scoop of the first substance into a test tube.Step 2- record the appearance before heating in the tableStep 3- attach the test tube clamp near the mouth of the test tube
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LESSON 6- PROCEDURE(2-2)
Step 4- heat the bottom of the test tube for 1-2 min. while it is in constant motion from side to side at an angleStep 5- observe any changes and record in the tableStep 6- place the test tube in a 250-ml beaker and allow to cool for 1 min.Step 7- Repeat procedure for the other substances
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LESSON 6- RESULTS
Substance
Appearance
before heating
Changes
observed
during heatin
g
Appearance
after cooling
Ammonium chloride
Copper (II) sulfateSodium chloride
Zinc oxideSulfur
Copper carbonate
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LESSON 6- CONCLUSION(1-3)
1. Which substances (if any) showed no change when heated?
NaCl
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LESSON 6- CONCLUSION(2-3)
2. Which of the substances produced a new substance when
they were heated?
Ammonium chloride, sulfur, copper carbonate, copper sulfate
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LESSON 6- CONCLUSION(3-3)
3. How can heating a substance help you identify it?
It shows you its characteristic properties
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NEXT STEP, NEW QUESTION
1) What happens to copper sulfate when water is added after it has been heated?
2) The test tube gets hot3) It turns blue again
A. EXOTHERMIC REACTION4) Sound given off
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LESSON 6- ERROR ANALYSIS
Heating the substance too long or not long enough
Adding too much substanceHeating incorrectly
Cross contamination
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REAL LIFE APPLICATION
1. When cooking, food changes from one form to another. This is a chemical change.
2. Burning chemicals to get rid of pests
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Independent variables
Substance: Amount and Type
Heating timeAngle of heating
Dependent variables
Appearance/odor/sound of substance
state of matter
Lesson 6- VARIABLES
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CHARACTERISTIC PROPERTIESCharacteristic Property: An attribute that can be used to help identify a substance. A characteristic property is not affected by the amount or shape of a substance.
Density The way a substance behaves when it is heated
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LESSON 6 – CONCLUSION
Physical and chemical changes result from the application of heat. The way a substance behaves when it is heated is a characteristic property of that substance. Sublimation, evaporation, and condensation are caused when heat energy overcomes the forces that hold a solid together or keep a liquid in a fluid state.
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LESSON 6 – CONCLUSION
Heating may cause a chemical change, phase change, or no change at all. When cooling occurs after heating, changes in substances may be reversible or irreversible. If a chemical reaction occurs, new substances with different observable properties are formed. Chemical reactions have reactants and products………..
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LESSON 6 – VOCABULARY (1-3)
chemical reaction - a change in which new substances are formed; has reactants and products.
reactant - the starting substances in a chemical reaction.
product - a substance formed by a chemical reaction.
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LESSON 6 – VOCABULARY (2-3)
physical change - reversible through physical means and do not involve the formation of new substances; no change in chemical properties.
chemical change - not readily reversible and do involve the formation of new substances with different properties.
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LESSON 6 – VOCABULARY (3-3)
sublimation - physical change in which a substance goes directly from a solid to a gas and then back to a solid.
evaporation - the change of a substance from a liquid to a gas
condensation - the change of state from a gas to a liquid
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Yes
No StatementYes
No
Increasing the heat input when boiling a substance raises the melting or
boiling point
Water always boils at 100 o Celsius
Changes of state are related to temperature.
Substances that boil are always hot
A phase change is a chemical reaction
When matter changes state, there is no loss of mass.
Melting and dissolving are the same.
Freezing points are lower than melting points.
Before
After
ANTICIPATION/REACTION GUIDE (INQUIRY 7.1)
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LESSON 7 – JUST A PHASE
As ice is heated, you will observe the phase
changes that occur. You will also observe melting
and boiling points.
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LESSON 7 – GETTING GETTING STARTED STARTED
A. increase the pressure or decrease the pressure in a vacuumB. the ice absorbs heat energy from the surrounding environment. Heat flows from a high concentration to an area of low concentration. KE increases and the ice melts (melting and freezing point are the same)
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LESSON 7 – GETTING GETTING STARTED STARTED
C. Not enough energy to change to the liquid phase because the specific heat is so highD. The energy transfer is not quick/ surface area is a factor (crushed vs. chunks)E. no. During a phase change the surface tension is broken, but has not acquired enough energy to burn. Frozen just means a phase change
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LESSON 7 – QUESTION
What will happen when we add heat energy to a sample
of ice?
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LESSON 7 – HYPOTHESIS
If we add heat energy to the sample of ice,
then it will melt because the particles
are gaining kinetic energy
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LESSON 7 – PROCEDUREPROCEDURE
Step1- fill beaker with ice (50 ml)Step 2- add a small amount of waterStep 3- heat ice and record changesContinue to heat the ice 3 min. after it has begun to boil vigorouslyRemember : Do not stop the stop watch to check the time
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Time(min. and
sec.)
Temperature of water (C degrees)
Observations
0
30 s
1 min
1 min, 30 sec
2 min
2 min, 30 sec
3 min
3 min, 30 sec
4 min
4 min, 30 sec
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GRAPHING TIME!!!GRAPHING TIME!!!
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LESSON 7 – REFLECTING QUESTIONS (1-2)
A. How does the shape of your curve compare to those produced by other groups? Different temp. reading for the different phase changes B. Do any changes in the direction of your curve match the point at which the ice melted or the water boiled? The plateau indicates a phase change taking place/the diagonal line indicates that the substance is gaining energy
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LESSON 7 – REFLECTING QUESTIONS (1-2) C. How can you use the curve on your graph to determine the temp. at which ice melted and water boiled? Match the observation to the corresponding temperature reading D. Are these temps. what you expect? No, I expected that water would boil at 100 degrees Celsius
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LESSON 7 – ERROR ANALYSIS (1-2)
Not centering the flameAlcohol burners giving off different amt. Of energyMoving the thermometerAccuracy of timing using the stopwatchRead the thermometer incorrectly
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LESSON 7 – ERROR ANALYSIS (2-2)
The flame going outDifferent quantities of iceThe thermometer touching the beakerDue to changing water levels, the thermometer reads water and air temps. simultaneously
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LESSON 7 – VARIABLES
INDEPENDENT VARIABLE
Amount of Ice
Flame
Time
Amount of water
DEPENDENT VARIABLE
Temperature
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CHARACTERISTIC CHARACTERISTIC PROPERTIESPROPERTIES
1. DENSITY
2. THE WAY A SUBSTANCE BEHAVES WHEN HEATED
3. MELTING POINT/ FREEZING POINT
4. BOILING POINT
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LESSON 7 – CONCLUSION (1-4)
•Phase changes are dependent on temperature and pressure.•Three phases or states of matter: solid, liquid, gas•Phase changes take place when molecules lose or gain kinetic energy (heat energy) and can be related to a change in temperature.
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LESSON 7 – CONCLUSION (2-4)
Lose kinetic energy – molecules move
closer – (gas > liquid > solid).Gain kinetic energy – molecules move
apart – (solid > liquid > gas)A change of state is not the result of a chemical reaction.
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•The melting point and boiling point of a substance is a characteristic property of the substance.•Freezing and melting points are the same.
LESSON 7 – CONCLUSION (3-4)
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•An increased input of heat has no effect on the boiling point of a substance, although it will make a fixed mass of matter change state faster.•Substances that boil are not always hot. Many substances melt and boil below 0 degrees C
LESSON 7 – CONCLUSION (3-4)
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LESSON 7 – VOCABULARY (1-2)
melting - the phase change in which a solid turns into a liquid.
melting point - the temperature at which a solid turns into a liquid; the same temperature as freezing point; altered by changes in pressure.
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LESSON 7 – VOCABULARY (2-2)
boiling - the process by which a liquid changes into a gas at its boiling point.
boiling point - the temperature at which a liquid changes into a gas; boiling point depends on air pressure.
condense - changing from a gas to a liquid
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Mass is conserved due to the LAW OF CONSERVATION OF
MASS: Mass is neither created or
destroyed; the total mass of all substances remains the same
regardless of any changes in phase or chemical reactions that occur.
LESSON 8- CONCLUSION
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LESSON 10WHAT HAPPENS WHEN
SUBSTANCES ARE MIXED WITH WATER?
You will mix several pure substances with water
and observe what happens.
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ANTICIPATION/REACTION GUIDE (INQUIRY 10.1)
Yes
No StatementYe
sNo
Solutes disappear when added to water
The solute becomes water when it dissolves
Solute particles can be removed by filtration or settle out of solution
over timeThe solute and solvent become a
single substanceThe addition of solute does not add
any volume to the solution
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LESSON 10.1- GETTING STARTED
oIt is liquidoIt looks uniform throughoutoTranslucentoAble to see through colored substance*note: substances in solution are the
most finely divided and dispersed mixtures that exist
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LESSON 10 - QUESTION
What will happen when we mix the substances with
water?
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LESSON 10.1- HYPOTHESIS
If we mix the solutes with water, then they
will dissolve and form a mixture because they
now have different chemical and physical
properties.
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•Homogeneous- looks evenly distributed•Heterogeneous- looks like more than one substance
LESSON 10.1- VOCABULARY
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LESSON 10.1- PROCEDURE (1-2)
•Step 1- Put one lab scoop of copper (II) sulfate into a test tube•Step 2- Add water to a depth of 5cm•Step 3- Seal the test tube with a rubber stopper•Step 4- Shake the mixture 20 times
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LESSON 10.1- PROCEDURE (2-2)
•Step 5- observe and fill in the table•Step 6-label the plastic cup with your group/period and pour the 2 test tubes of copper (II) sulfate solution into them
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LESSON 10- RESULTS
Name of substance added to water
Appearance after being shaken 20
times
Does it dissolve
?(Yes or
No)
Sodium chloride (NaCl)
Copper (II) sulfate (CuSO4)
Zinc Oxide (ZnO)
Sulfur (S)
Powdered Sugar
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LESSON 10- CONCLUSION QUESTIONS (1-4)
1. Explain what happens to solutes when they mix
with water?
Some dissolve and others do not
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LESSON 10- CONCLUSION QUESTIONS (2-4)
2. Do they disappear?
If they dissolve they do not disappear they evenly spread out within the
solvent
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LESSON 10- CONCLUSION QUESTIONS (3-4)
3. Does the solute become water?
No, still 2 different substances that are well
mixed.
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LESSON 10- CONCLUSION QUESTIONS (4-4)
4. Can solute particles be removed by filtration or over time settle out of
solution? No. evaporation must occur.
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LESSON 10- DEFINITIONS LESSON 10- DEFINITIONS (1-5)(1-5)
Soluble- Able to dissolve
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LESSON 10- DEFINITIONS LESSON 10- DEFINITIONS (2-5)(2-5)
Insoluble- Unable to dissolve
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LESSON 10- DEFINITIONS LESSON 10- DEFINITIONS (3-5)(3-5)
Solvent- Substance that
dissolves the solute in a solution
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LESSON 10- DEFINITIONS LESSON 10- DEFINITIONS (4-5)(4-5)
Solute- Substance added to
the solvent and is dissolved
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LESSON 10- DEFINITIONS LESSON 10- DEFINITIONS (5-5)(5-5)
Solution- Homogeneous
mixture of solute(s) and solvent
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LESSON 10- ERROR ANALYSIS
1)Adding incorrect amount of solute
2)Adding incorrect amount of water
3)Different amount of energy added by shaking
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REAL LIFE APPLICATIONREAL LIFE APPLICATION
Liquids dissolved in liquidsrubbing alcohol in water
Solids dissolved in liquidsSalt dissolved in water
Gases dissolved in liquidsOxygen dissolved in water (fish tank)Sulfur dioxide dissolved in water = acid rain
Solids dissolved in solidsBrass (zinc in copper)
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LESSON 10- VARIABLES
Independent variable
Type of substance
Amt. of energy added
Amt. of water
Amt. of substance
Dependent variable
Solubility
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CHARACTERISTIC PROPERTIES
1.Density
2.The way a substance behaves when heated
3.Melting/ freezing point
4.Boiling point
5.Solubility
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CHEMICAL EQUATIONS/SOLUBILITY
NaCl (s) Na+ (aq) + Cl- (aq)
CuSO4 (s) Cu+2 (aq) + SO4-2
(aq)
S (s) S (s)
Reactants Yield Products
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LESSON 10- DEFINITIONSLESSON 10- DEFINITIONS
mixture - two or more elements or compounds that are mixed together but are not chemically combined
pure substance - either an element or a compound; has definite chemical and physical properties
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LESSON 11 –HOW MUCH SOLUTE
DISSOLVES IN A SOLVENT?
You will make a saturated copper sulfate solution. You will also conduct an investigation to determine the solubility of two
different chemicals.
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GETTING STARTED
The liquid is blue and translucent
Blue crystals are at the bottom
Liquid is probably a solution or a pure blue liquid rather than a solution
The solute in the solution is probably blue
The crystals at the bottom could be un-dissolved solute
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LESSON 11 – QUESTION
Which of the two substances will
have the greatest solubility?
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LESSON 11 - HYPOTHESIS
If we add NaCl & NaNO3
to water, then the NaCl should have the highest solubility because the water should dissolve
more.
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LESSON 11- HINTS/ TIPS LESSON 11- HINTS/ TIPS 1. What will you need to measure?
a. The mass of the jar without the lid
2. How will you know when you have a saturated solution?
a. No more substance will dissolve so the substance will begin to collect at the bottom of the tube
3. How will you calculate the amount dissolved?
a. By measuring the mass before and after, then subtract
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PROCEDURE(1-3)
Step1- Fill test tube with 10mL of water Step 2- Mass the jar of NaCl without lid Step 3- Add one level lab scoop of sodium chloride to the test tube
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PROCEDURE(2-3)
Step 4- Shake the test tube using the stopper for 30 sec. *Be sure to not hit the test tube on the table*
Step 5- If it completely dissolves, keep adding more salt until you see it collecting at the bottom Step 6- Count the number of scoops added and then subtract one
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PROCEDURE(3-3)
Step 7- Re-mass the jar Step 8- Repeat steps 1-7 for sodium nitrate
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LESSON 11- RESULTS
• ____ scoops of NaCl dissolved in 10mL of water
• ____ scoops of NaNO3 dissolved in 10mL of water
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LESSON 11-CONCLUSIONLESSON 11-CONCLUSION1. How do you know that no more
solute would dissolve? a) The substance started collecting
at the bottom of the test tube
2. What is your definition of a saturated solution?
a) A solution that has the maximum number of solute particles dissolved in a solvent
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LESSON 11- LESSON 11- CONCLUSIONCONCLUSION
1. Are different substances equally soluble in water?
a) No. They have different physical properties.
2. How could you use the property of solubility to help identify a type of matter?
a) You could try dissolving different unknown substances and then compare them to a solubility chart to identify them.
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Solubility is affected by temperature. Solids dissolved in water may increase in solubility with the rise in temperature or
increase with a drop in temperature.
Gases always decrease in solubility with increased temperature.
LESSON 11-CONCLUSIONLESSON 11-CONCLUSION
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NEXT STEP/NEW NEXT STEP/NEW QUESTIONQUESTION
Calculate how many grams of sodium chloride and sodium
nitrate that could dissolve in 1 liter of water. One liter is 1000
ml.
2.4 (g) = X (g)
10(ml) 1000(ml)
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LESSON 11- ERROR ANALYSIS
1. Measurement of scoop level2. Incorrect calculations3. Incorrect water amounts4. Not adding enough or too much heat
energy through shaking5. Not giving substance enough time to settle6. Loss of liquid due to shaking7. Temperature of water/room temperature8. The mass of un-dissolved solute in the
bottom of the test tube
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VARIABLES
INDEPENDENT The amount of
solute The volume of
water Temp. of water The amount of energy added by shaking the test
tubes The type of solute
DEPENDENT
solubility
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LESSON 11 – CONCLUSION
Solubility is the amount of a solute that will completely dissolve in a given amount of a solvent.Solubility is a characteristic property of matter.Different substances are not equally soluble in water.
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LESSON 11 – CONCLUSION
A saturated solution has the maximum amount of solute dissolved in it.When an unsaturated solution of a solid is cooled, it may become saturated.Recrystallization occurs when a solution of a solid is cooled and some solid solute precipitates out.
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LESSON 11 – CONCLUSION
Solubility is affected by temperature. Solids dissolved in water may increase or decrease in solubility with the rise in temperature. Gases always decrease in solubility with increased temperature.
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LESSON 11 – (1-3)
solubility - the amount of solute that will completely dissolve in a given amount of a specific solvent at a given temperature and pressure; the ability of one substance to dissolve in another
solute - the substance that dissolves in a solvent; the substance in the smaller proportion.
solvent - the substance that the solute is dissolved in; the substance present in the larger proportion.
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LESSON 11 – (2-3)
saturated solution - a solution that has the maximum amount of solute dissolved in it at a specific temperature and pressure.
exothermic reaction - heat is given off (increase in solubility with a decrease in temp.)