Name: ____________________________________
Date: ________________________________
Chemistry Enriched
Self-Guided Activity: Properties of Matter
Per. _______
Goals:
1.
2.
3.
4.
5.
6.
To observe both Physical and Chemical Properties of Matter
To discern between elements, compounds, homogenous mixtures and heterogeneous mixtures
To describe the packing and motion of particles in solids, liquids, and gases
To recognize the different types of techniques available to separate mixtures
To recognize the evidence of a chemical change taking place
To discern between a physical change and chemical change
You will be working in a group of three or four and move around (in order) from one lab station to the next… The
purpose of which is to accomplish the aforementioned goals. Simply follow the directions (either on this handout or at
the lab station) and answer all the questions to the best of your ability.
Safety: There will be some demos and minor procedures that you will be carrying out, so you’ll need your safety googles
on, at times, and hair tied back…
Station #1: Elements, Compounds, & Mixtures
Procedure:
1. Read the definitions of elements, compounds, homogeneous mixtures and heterogeneous mixtures. Write out
“condensed” definitions for each. For example, Elements: One type of atom, identified by # of protons, cannot
be chemically broken down.
2. Examine the various substances… Then list what category each substance falls under.
3. For any element or compound, make sure to write the chemical symbol or formula of the substance. For
example: Lead, Pb or Sodium Chloride, NaCl
Station #1: Observations and further questions:
Definitions:
Elements – A pure substance in its simplest form. It cannot be broken down into simpler substances by physical
or chemical means. Elements can be identified by the number of protons in the nucleus.
Compound – consists of 2 or more atoms chemically combines. Can be broken down into simpler substances by
chemical means. Composition is uniform throughout.
Homogeneous Mixture – mixture of substances that is uniform or consistent throughout. Only one phase
present.
Heterogeneous Mixture – mixture of substances that is NOT uniform or consistent throughout. More than one
phase visible. Example: Italian Salad Dressing.
4. Classify each of the substances under the following headings (and make sure to include chemical symbols or
chemical formulas for elements and compounds):
Elements
Compounds
Homogeneous Mixtures
Heterogeneous Mixtures
Copper (Cu)
Sucrose
Maple Syrup
Lemon Juice
Food Coloring
Zinc (Zn)
Baking Powder
Copper Sulfate
Sulfur (S)
Sodium Nitrate
1.0 M Sodium Nitrate
Station #2: Solids, Liquids, and Gases.
1. If you are the first person at the station, log in to the computer and go to:
http://phet.colorado.edu/en/simulation/states-of-matter
2. Start the simulation of “States of Matter”
3. Click on Argon and lower the temperature to 20K (by putting ice underneath the container).
4. The particles are in the solid state. Describe their packing (proximity to each other, arrangement) and their
motion. They may not be moving around, but they are moving…
5. Heat up the container to 90K. You are now in the liquid state. Now describe the behavior (motion) of the
particles and their proximity to each other (close or far apart?).
6. Heat up the container to 150K. You are now in the gaseous state for Argon. Now describe the motion of the
particles AND how the distance between the particles has changed.
7. Finally, double the Kelvin temperature to 300K. How does the motion of the particles change? The formula for
kinetic energy, KE, is mass x velocity squared. What happens to their kinetic energy when the temperature
increases?
8. Return the temperature back to 20K for the next group.
9. Look at the examples 2 different types of “rocks”: Galena and Sandstone. Read the cards explaining their
differences (and refer to the model of the lattice of NaCl) and answer the follow up questions.
Station #2: Observations and further questions.
Solids
Liquids
Gases
Describe the motion
and packing of the
particles


Particles are vibrating
faster and moving past
each other.

Distance between
particles

Distance between the
particles increases
Vibration increases =
higher Kinetic Energy but
still low
Particles can slide past
each other.

Pictorial
Representation

Particles are vibrating
relatively in place.
Particles are very
close together.
Atoms vibrate but
relatively slow = very
low Kinetic Energy





Particles are vibrating
the fastest
Particles move about
through the entire
container
Distance between the
particles increases
Lots of vibration and
motion throughout the
entire container = High
Kinetic Energy
10. What is the relationship between temperature and Kinetic Energy of Particles?
As the temperature increases, the kinetic energy of the particles also increases because they are moving faster.
11. What is the difference in the arrangement of the atoms between a mineral like Galena and one like Sandstone?
Galena has a crystalline structure b/c you can see the “cubic” edges on the stone. Sandstone is NOT crystalline.
Station 3: Vocabulary Practice
1.
2.
3.
4.
Go to Quizlet.com, search “queenja”, and go to “Properties of Matter”
Click on “Scatter” and see who in the group clears the screen in the fastest time.
If you are waiting to go to the next lab station, take a practice test or try “Space Race”.
Record your fastest time for Scatter.
Station 3: Observations and further questions
What was your best time on Scatter? _____Go back and use this to study for Quiz & Test_____
Who in your group had the best time? _________________________________
Station 4: Separating Mixtures
1. There are index cards at the station explaining the various types of separation techniques.
2. Chromatography: Place one of the paper strips with the black ink dot down into the test tube that has a little
water in the bottom. You will not have time to let the strip fully develop, so one strip is already labeled what it
will look like when it is done. But at least observe initially what happens as water absorbs up the paper. Also,
you can let it develop while you are doing the crystallization and distillation parts. Answer any questions.
3. Distillation: View the You Tube Video at https://www.youtube.com/watch?v=xxNfJLMNS4E and answer any
questions.
4. Crystallization: Simply move one test tube of the warm solutions of KNO3 into the tap water beaker. The
purpose is to take advantage of the lower solubility of KNO3 in colder water so that it will crystallize “out” of
solution. Observe carefully and answer any questions.
5. Filtration: Read the instructions…Basically you are going to pour your mixture through the filter paper to
separate a heterogeneous solution (based on differences of particle size).
6. Make sure to clean up the station and leave it as you found it (the test tube of crystallized KNO3 can be placed in
the test tube rack).
Station #4: Observations and further questions.
Observations:
Crystallization – separation technique that produces pure solid particles of a substance from a solution that has the
dissolved substance. This is usually achieved by lowering the temperature of the solution.
Filtration – process used to separate solids from a liquid by interposing a filter. Separates according to particle size.
Filtration can only be used to separate heterogeneous mixtures. Example: Coffee Filter
Distillation – separation technique that can separate homogeneous mixtures according to the different boiling
points. The steam of the lower boiling point is condensed (changed back into a liquid state) and collected in a
different container.
Chromatography – technique used to separate the components of a mixture based on the tendency of each
component to travel across/through a surface.
Follow up questions:
7. Chromatography: What colors are present in black ink? yellow, red, purple, blue
8. What causes the colors to separate from each other? Some colors interact with the paper more and are unable
to travel as far staying closer to the original black dot.
9. Crystallization: What happens to the solubility of KNO3 when the temperature drops? More soluble or less
soluble? As the temperature drops, the solubility also drops. The KNO3 crystallizes when it is placed in the cold
water after it has been fully dissolved in the hot water bath.
10. Distillation: Read up on distillation and simply explain how it works. Substances have different boiling points.
When you have a mixture of two substances with different boiling points, the mixture is heated past the lower
boiling point. The substance with the lower boiling point will evaporate (go into gas state) and then be
condensed (changed back into liquid state) in the condensing tube and collected in a second container. This
successfully separates the two substances because the substance with the higher boiling point will not be able
to evaporate unless the boiling point temperature is reached.
11. Filtration: Would you separate homogeneous solutions or heterogeneous solutions by filtering? Filtration
separates according to particle size which means it can only be used for heterogeneous mixtures.
12. Ever use a colander to separate pasta from water? How is this like filtering? The colander has tiny holes (pores)
that can let the water molecules through but not the pasta. Separates according to particle size.
Station 5: Chemical vs. Physical Changes
1. Now you need your safety goggles on and hair tied back.
2. Baking Soda, NaHCO3 and Vinegar (Acetic Acid): Pour 10 mL of vinegar into a beaker. Make sure everyone feels
how warm/cool the beaker is with the solution in it. Next, add a scoop of baking soda and record your
observations. When the reaction has completed, pass the beaker around and again feel how warm/cool the
beaker is. Record your observation.
3. There are two pipets, one labeled KI, the other labeled Pb(NO3)2. Place a few drops of KI into a test tube, then
add a few drops of Pb(NO3)2 into the same test tube, and record your observation. The yellow solid that forms is
called a precipitate. Keep the test tube in the rack, do not rinse it out down the sink.
4. Let’s get a little practice lighting a Bunsen burner… Have the striker ready, turn on the gas, and create sparks
with the striker (above the burner) to light the burner.
5. Carefully hold a beaker of cold water about 8-10 inches above the flame. What forms on the outside of the
beaker? Record your observations and answer the questions.
6. Finally, there is a beaker of ice and one of boiling water. Simply observe them, write down your observations,
and answer the questions.
Station #5: Observations and further questions
Chemical property – abilitiy or inability of a substance to combine with or change into one or more other
substances. Examples: Rusting, burning, color change, bubbling, temperature change.
Physical Property – characteristic of matter that can be observed or measured without changing the sample’s
composition. Examples: density, color, odor, hardness, melting point, boiling point.
Observations of…
7. Bunsen burner activity…evidence of chemical reaction? Bunsen Burner has a flame which emits LIGHT and
HEAT.
8. Baking Soda and Vinegar…evidence of chemical reaction? The reaction gets cooler (TEMPERATURE CHANGE)
and it fizzes (PRODUCTION OF A GAS)
9. KI & Pb(NO3)2 mixing…evidence of chemical reaction? The mixture becomes yellow (COLOR CHANGE) and a solid
(grainy sand like) is formed (PRECIPITATE)
10. Ice Water & Boiling Water As water changes from ice (solid) to liquid to gas, it still keeps the same composition
of water. Phase changes are examples of physical changes and do NOT change the composition of the
substance.
11. How do you know the water is undergoing a physical change and not a chemical change? Explain The
composition of the water does not change and you are able to bring it back to any state. Ice can be melted into
liquid water, frozen into ice, melted again without ever changing the composition of the water.
Station 6: Measurements & Significant Figures
1.
2.
3.
4.
5.
Measure the volume of the blue liquid in each graduated cylinder in milliliters (mL).
Convert your recorded volumes from milliliters to centiliters, liters, and kiloliters.
Measure the length of the three objects on the station using the three meter sticks labeled A, B, and C in meters.
Convert your recorded lengths from meters to centimeters, millimeters, and kilometers.
Complete the additional practice worksheets on recording measurements with proper significant figures and
performing calculations using significant figures.
Station 6: Observations and further practice.
Record the volume in the table below (first row). Then convert each measurements to the other given units.
The number of significant
figures must be the same
as you convert from one
unit to another.
Milliliters
Graduated Cylinder A
Smallest marking is 1 mL,
must record to the tenths
of a mL
22.0 mL
Gradated Cylinder B
Smallest marking is 0.1 mL,
must record to the
hundredths of a mL
6.90 mL
Graduated Cylinder C
Smallest marking is 1 mL,
must record to the tenths
of a mL
68.0 mL
Centiliters
2.20 mL
0.690 cL
6.80 cL
Liters
0.0220 L
0.00690 L
0.0680 L
Kiloliters
0.0000220 kL
0.00000690 kL
0.0000680 kL
The number of
significant figures
must be the same
as you convert
from one unit to
another.
Meters
Meter Stick A
Smallest marking is 1 m,
must record to the tenths
of a meter
Meter Stick B
Smallest marking is 0.1 m,
must record to the
hundredths of a meter
Meter Stick C
Smallest marking is 0.001 m, must
record to the ten-thousandths of a
meter.
0.6
0.2
0.1
0.60
0.15
0.08
0.6020
0.1450
0.0750
Centimeters
60
20
10
60
15
8
60.20
14.50
7.50
Kilometers
0.0006
0.0002
0.0001
0.00060 0.00015 0.00008 0.0006020 0.0001450 0.0000750
millimeters
600
200
100
600
Test Reflection Question:
How can I improved my test grade for next time?
150
80
602.0
145.0
75.0