Download physical and chemical change

PHYSICAL AND CHEMICAL CHANGE
Objective: to investigate the criteria used to distinguish between physical and
chemical changes in matter.
Background: Matter has both physical and chemical properties. A physical
property is a quality or condition of a substance that can be observed or
measured without changing the composition of the substance. Color is an
example of a physical property. During a physical change, some properties of a
sample of matter change, but the composition of the sample does not change.
Melting and dissolving are examples of physical changes. A chemical change
produces matter with a different composition that the original sample. Chemical
bonds are broken and/or reformed. A chemical property describes the ability of a
substance to undergo a specific chemical change. The ability to rust is a
chemical property of iron.
In this experiment, you will observe various materials and describe their physical
properties. You will then cause some of the materials to undergo changes.
Based upon our observations, you will determine whether the changes are
physical or chemical changes.
Safety First:
1) Wear your safety goggles.
2) Hydrochloric acid will burn skin and clothes. If you spill it on you, wash
quickly with lots of water.
3) Do not look directly at burning magnesium.
4) Hot glass looks like cold glass.
PROCEDURE:
Part A. The Physical Properties of Matter
1. Label a separate piece of paper for each of the seven substances
to be examined. Place two pieces of magnesium ribbon, one 5
cm long and one 1 cm long, on the paper labeled “magnesium.”
Your instructor will give you samples of the other substances.
2. Examine each substance with a magnifying glass. Record your
observations in Data Table 1.
3. Test the effect of a magnet on each substance by passing the
magnet under the sheet of paper.
4. In separate small test tubes, test the solubility of each substance
by mixing a small amount of each substance with ~3 ml of
distilled water. Flick each test tube to mix the contents.
5. Return the strip of magnesium ribbon in the test tube to its
paper. Follow your instructors directions for proper disposal of
the other materials.
Part B. Causing a Physical or Chemical Change
6. Mix the iron filings and sulfur on a clean piece of paper.
Examine the mixture with a magnifying glass. Test the effect of
a magnet by passing the magnet under the paper. Give this
mixture to your teacher for use in Part C.
7. Mix the sodium chloride and sand on a clean piece of paper.
Examine the mixture with a magnifying glass, and test the effect
of a magnet.
8. Transfer the salt-sand mixture to a clean 100 ml beaker. Add
about 30 ml of tap water and stir. Record your observations.
Prepare a filtration setup as shown by your instructor. Filter the
mixture and record your observations. Pour about 10 ml of the
filtrate into an evaporating dish. Convert your filtration setup
into a setup you can use to heat the liquid in the evaporating
dish. Heat the dish gently until the filtrate has completely
evaporated. Examine both the dry residue in the evaporating
dish and the wet residue on the filter paper.
9. Caution: do not look directly at the burning magnesium.
Position a watch glass near the gas burner. Using tongs, grasp
one end of the 5 cm strip of magnesium ribbon and hold it in the
burner flame. As soon as it ignites, hold it over the watch glass
in order to catch the combustion products. Compare the
appearance of this product with that of the original magnesium
ribbon.
10. Place the unburned 1 cm strip of magnesium and the combustion
product in separate test tubes. Add 10 drops of 6M hydrochloric
acid to each tube. Feel the bottom of each test tube. Record
your observations.
11. Put half of your sucrose sample into a test tube. Caution:
when heating a test tube, never point the mouth of it at
yourself or anyone else. Heat the test tube gently in a burner
flame and watch carefully for changes. Periodically remove the
tube from the flame and check for odors by fanning the fumes
toward your nose. Now, heat the residue in the test tube more
vigorously for 1 to 2 minutes. After cooling the test tube, use a spatula to
scrape some of the residue into a clean test tube. Examine the residue
and test its solubility in water.
12. Transfer the sodium hydrogen carbonate sample in a test tube. Carefully
add 5 drops of 6M hydrochloric acid. Touch the bottom of the test tube
with your hand. Record your observations.
13. Follow your instructor’s directions for proper disposal of materials.
DATA TABLE 1: PHYSICAL PROPERTIES OF MATTER
Substance
and
formula
Sulfur, S
Physical
state
Color
Odor
Dissolves
in water
Iron filings,
Fe
Sodium
hydrogen
carbonate,
NaHCO3
Sodium
chloride,
NaCl
Sucrose,
C12H22O11
Sand, SiO2
Magnesium,
Mg
DATA TABLE 2: OBSERVATIONS OF PHYSICAL AND CHEMICAL
CHANGES
SYSTEM
Fe and S mixture
-tested with magnet
NaCl and sand mixture
-mixed with water
-filtered
-filtrate evaporated
Mg
-burned in air
Mg
-reacted with 6M HCl
Mg combustion product
- reacted with 6M HCl
Sucrose
-heated
NaHCO3
- reacted with 6M HCl
OBSERVATIONS
Effect of
Magnet
Part C: Conservation of Mass (Teacher Demonstration)
14. Several samples of the iron-sulfur mixture from Part B will be combined in
a clean, dry test tube. The mass of the test tube and its contents will be
determined and recorded. The test tube is then heated gently, then
vigorously, for several minutes. After heating, the mass is remeasured
and recorded. Examine the reaction product. Test the material with a
magnet.
Fe and S mixture:
Initial mass:
Final mass:
Observations:
ANALYSES AND CONCLUSIONS
1. The following is a list of changes you observed in Parts B and C. Indicate
whether each change was a physical change or a chemical change and give
reasons for your answer.
a. Mixing iron and sulfur (Part B, Step 6)
b. Mixing salt, sand, and water (Part B, Step 8)
c. Burning magnesium (Part B, Step 9)
d. Mixing magnesium and the product of burning magnesium with
hydrochloric acid (Part B, Step 10)
e. Heating sucrose (Part B, Step 11)
f. Mixing sodium hydrogen carbonate and hydrochloric acid (Part B, Step
12)
g. Heating iron and sulfur (Part C, Step 14)
2. Was mass conserved in the reaction of iron and sulfur. Explain.
3. Except for the reaction between iron and sulfur, none of the reactions in this
experiment can be used to demonstrate the law of conservation of mass.
Explain why.
4. How do you decide whether an observed property of matter is a physical or a
chemical property?
5. What criteria are used to distinguish between a chemical change and a
physical change?
6. state in your own words the law of conservation of mass.