Name/Partner’s Name: ______________________________
Date: ______________ Pd. ___
Lab: Physical and Chemical Properties
Introduction:
A good understanding of material things requires an understanding of the physical and
chemical characteristics of matter. Such characteristics are familiar to you, and physical and
chemical changes are part of your everyday experience.
The physical properties of a substance can be observed and measured without changing
the composition of the substance. Physical properties include state, odor, color, magnetism,
density, solubility, boiling point, and melting point.
The chemical properties of a substance can only be observed when the substance is
undergoing a change in composition, or chemical reaction. The fact that hydrogen peroxide
decomposes to give oxygen gas and water is an example of a chemical property.
In a physical change, only the temperature, size, or physical state of a sample of matter is
changed. The melting of ice and the evaporation of gasoline are examples of physical changes. In
chemical changes, new substances, of different chemical composition are formed. Examples of
chemical change are the rusting of iron and the burning of wood. The telltale signs of a chemical
reaction or chemical change are: gas produced, formation of a precipitate (solid), color or odor
change, energy absorbed or released (shown by a change in temperature). A chemical reaction is
the process in which a chemical change takes place.
In chemical changes, the original substances are used up and new substances are produced.
Still, the total mass of the products of the reaction will always be equal to the mass of the reactants.
This is the Law of Conservation of Mass.
In this experiment, you will examine a variety of substances and describe the physical
properties of each. You will then cause changes to take place in some of the substances. Based on
your observations and the results of the tests you will conduct, you will decide whether these
changes are physical or chemical. You will also demonstrate the mass is conserved in a chemical
reaction.
Objectives:
1. To observe the physical and chemical properties of several substances.
2. To decide whether certain observed changes are physical or chemical.
3. To demonstrate that mass is conserved in a chemical reaction.
Equipment:
Goggles
Apron
Weighing dish – plastic
Weighing dish – metal
Magnet
Materials:
Iron (Fe)
Sulfur (S)
Magnesium (Mg)
Sodium bicarbonate (NaHCO3)
Spatula
Magnifying glass
Bunsen Burner
Striker
Tongs
Watch glass
Pipette
Test tube
Test tube rack
Hot plate
Acetic acid (HC2H3O2)
Sand
Salt, Sodium chlorice (NaCl)
Water
Calcium chloride (CaCl2)
Silver nitrate (AgNO3)
Phenolphthalein
Sodium hydroxide (NaOH)
Procedure:
Copy the Table 1 into your lab notebook. As you perform each experiment, record your data and
observations in this table. Note: always make as many observations as possible during an
experiment. Physical properties include state of matter, color, odor, solubility, magnetic.
Station #1: Combine the two types of matter
1. Put a pea size amount of iron (Fe) into one weighing dish and a pea size amount of sulfur (S)
into another weighing dish. Record observations in Table 1.
2. Test the effect of a magnet on each substance by passing the magnet under the weighing dish.
Do not dip the magnet directly into the material. Record your observations in Table 1.
3. Pour the iron into the dish with the sulfur. Mix the samples with a spatula. Examine the
mixture with a magnifying glass. Record your observations in Table 1. Move a magnet under
the dish below the mixture and examine it again with the magnifying glass. Record your
observations.
4. Bring this mixture to the front of the room and put it in the dish labeled Fe & S. Bring the
weighing dishes back to your station.
Station #2: Illuminate a solid
1. Write the physical properties of magnesium in your data table.
2. CAUTION: Do not look directly at the burning magnesium. Its flame is very bright and
can damage your eyes. Keep burning magnesium at arm’s length at all times and do not
inhale the fumes that are given off. Place a watch glass on the laboratory table close to the
Bunsen burner. Light the Bunsen burner. Use tongs to grasp one end of the 5-cm strip of
magnesium ribbon and hold this strip in the burner flame until the magnesium ignites. Hold
the burning magnesium over the watch glass so the ashes remaining will fall onto the watch
glass. Record your observations in the data table.
3. Throw away the ashes in the garbage. Rinse and dry the evaporating dish.
Station #3: Combine the two types of matter
1. Write the physical properties of acetic acid and sodium bicarbonate in your data table.
2. Add one dropper full of the acetic acid into a test tube followed by a pea size amount of
sodium bicarbonate. Observe the change that occurs. Touch the bottom of the test tube. Is
there a temperature change? Record data.
3. Rinse out your test tube and put it back in the test tube rack upside down to dry.
Station #4: Combine solids with liquid
1. Put a pea size amount of sand in one weighing dish and a pea size amount of salt in another
weighing dish.
2. Use the magnifying glass. Record your observations of the physical appearance of each
substance in Table 1. DO NOT taste or touch any substance with your hands.
3. Pour the salt into the dish with the sand. Mix with a spatula.
4. Put two dropper fulls of water into the test tube. Add a small amount of the mixture to the test
tube. Mix well by “flicking” the test tube as demonstrated by your teacher. CAUTION: do
not use your thumb as a cork to shake the test tube! Record observations.
5. Rinse the liquids down the drain, solid in the garbage. If there is solid in your sink, get a paper
towel and wipe it out.
6. Put both test tubes in the test tube rack upside down to dry.
Station #5: Combine the two solutions
1. Write the physical properties of the calcium chloride (CaCl2) and silver nitrate (AgNO3).
2. Caution: do not let any of the liquids get on your skin. Do not touch the droppers to the surface
of the test tube while transferring solutions. Add one dropper full of calcium chloride into a
test tube followed by one dropper full of silver nitrate. Record the change that occurs in
Table 1.
3. Rinse test tubes and put then upside down in the test tube rack to dry.
Station #6: Combine the two solutions
1. Write the physical properties of the sodium hydroxide (NaOH) and phenolphthalein in
Table 1.
2. Add one dropper full of sodium hydroxide into a test tube followed by ONE DROP of
phenolphthalein. Record observation in Table 1.
Station #7: Heat the unknown in its foil container
1. Place a pea size amount of salicylic acid on the foil dish.
2. Record physical properties of salicylic acid in Table 1.
3. Place the dish on the hot plate and turn the hot plate on medium heat (1/2 way).
4. Record observations in Table 1.
5. Use tongs to pick up the foil off the hot plate. Rinse the foil dish in the sink and dry it.
Teacher Demonstration – Law of Conservation of Mass
1. Record mass of iron and sulfur mixture.
2. Heat test tube under the fume hood.
3. Let cool and record final mass.
4. Test for magnetism.
Table 1: Physical and Chemical Properties and Changes
System
Physical Properties
During Physical or
chemical change
After physical or
chemical change
Fe and S
Mg
NaHCO3 and
HC2H3O2
Sand and NaCl
CaCl2 and Ag(NO3)
NaOH and
Phenolphthalein
Fe and S Mixture
 Heated
Initial mass:
Final mass:
Analysis:
1. Following is a list of changes you observed. Indicate whether each change was a physical
change or a chemical change. What evidence do you have to show that the change was physical or
chemical?
Station 1: Mixing iron and sulfur.
Station 2: Burning magnesium.
Station 3: Combining sodium bicarbonate with acetic acid.
Station 4: Combining sand and salt with water.
Station 5: Combining calcium chloride and silver nitrate.
Station 6: Combining sodium hydroxide with phenolphthalein.
Station 7: Putting salicylic acid on a hot plate.
Teacher demo: Heating iron and sulfur.
2. Was mass conserved in the reaction of iron and sulfur? Explain.
Conclusion:
1. How do you decide whether an observed property of matter is a physical or chemical property?
2. What criteria are used to determine if a chemical change took place?
3. State in your own words the law of conservation of mass.