Background: In a single-replacement reaction, atoms of an element replace the atoms of a second element in a compound:
A + BC → AC + B
The reaction only takes place if the element being replaced, or displaced, is less
reactive than the yet uncombined element. The activity series for metals indicates the relative activity, or reactivity, for certain metals:
Li, K, Ba, Ca, Na, Mg, Al, Zn, Fe, Ni, Sn, Pb, H, Cu, Hg, Ag, Au
Most Reactive

Least Reactive
Decreasing Activity and Reactivity
Goal: To observe a single-replacement reaction.
Materials:
1.) Safety glasses and plastic apron
2.) Sample of Copper (II) Chloride
3.) 8 cm x 8 cm strip of aluminum foil
4.) (2) 250 mL beaker
5.) Stirring rod
6.) Scissors
7.) Thermometer
8.) Magnifying glass
Procedures:
1.) Obtain a small sample of copper (II) chloride crystals and using the magnifying lens, record some observations
2.) Fill each beaker with 150 mL of water and then add the copper (II) chloride into each beaker. Place one beaker to side (this will be your reference beaker).
3.) Place the thermometer into the beaker.
4.) Observe the changes taking place when the copper (II) Chloride is added to the water. Record your observations. Also, record the initial temperature of the solution. STIR well to make sure all the crystals have fully dissolved.
5.) Cut an 8 cm x 8 cm strip of aluminum foil and fold it so it fits into the beaker.
Do not crumple into a ball!
6.) Make some observations about the aluminum foil. Record in the table on the
following page.
7.) Add the aluminum foil to the solution. Start recording your temperature every minute.
8.) Immediately write down any observations you notice in the beaker with foil.
9.) Make observations of this beaker and record in table for each time interval.
10.) Occasionally stir the solution with the stirring rod to knock off any residue.

11.) At the end of the lab, carefully remove the foil and discard only the foil in the
trash.
12.) Compare the solutions in each beaker and record. Complete procedures #11
and #12 (below) before moving on to the analysis section of the lab.
13.) Flush unreacted solution down the sink. Pour reacted solution into the flask in
the back with the funnel and filter paper. Clean both test tubes thoroughly
with the test tube brush. Turn test tubes upside down to dry.
14.) Return all other equipment and clean your area.
Time vs. Temperature Chart:
Time: Temperature ( 0 C)

Observations:
Time
Dry Copper
(II) chloride crystals on the spoon
Copper (II) chloride in water
Foil before putting in test tube with solution
Foil immediately after putting in solution
1 minute
3 minutes
5 minutes
10 minutes
15 minutes
Comparison of solutions after 15 minutes
Observations

Analysis:
1.) What is the brownish material you see forming in the test tube?
2.) What accounts for the difference in the solutions after 15 minutes?
3.) Write, in words, the chemical reaction that took place.
4.) Now, write the equation above using formulas and balance it.
5.) The following reactants produce single-replacement reactions. Complete the
reactions using formulas and then balance the equation. Use the highest valence
for elements that have more than one valence number.
A.) Iron plus copper (II) sulfate
B.) Chlorine plus sodium bromide
C.) Oxygen plus hydrogen iodide
D.) Aluminum plus iron (II) oxide

6.) The following metals are placed into hydrochloric acid (hydrogen chloride). Use the activity series chart at the beginning of this lab to determine if a reaction will take place. Write, in words, the reactions that do take place. For those that do take place, write the equation and balance it. Use the highest valence for elements that have more than one valence number.
A.) Zinc
B.) Copper
C.) Aluminum
D.) Iron
E.) Magnesium
F.) Gold
G.) Barium
H.) Nickel
I.) Silver
7.) Of the above metals, which would react more actively when placed in the acid?
Explain.