1. Into one test tube put a couple of droppersful of an aqueous solution of Cu²⁺, and into another put a couple of droppersful of an aqueous Fe³⁺.
2. Put a small piece of copper wire into the Fe³⁺ and a small piece of iron wire into the Cu²⁺.

1. What color did the iron wire turn?  Why?

 

 
 
 
 
 
 
 
 
 
 

2. Why did one of the solutions change color from bluish/green to yellow?  Why was it bluish/green in the first place?

 

 
 
 
 
 
 
 
 
 
 

3. What occured when the copper wire was place in the Fe³⁺ solution?  Why?

 

 
 
 
 
 
 
 
 
 
 

4. Arrange the copper and iron in order of decreasing chemical activity:

 

1. Into two clean small test tubes place a couple of droppersful of an aqueous Ag+.
2. Place a piece of magnesium ribbon into one test tube and a piece of copper wire into the other.
3. After the reaction has continued for a minute, feel the test tubes and note any temperature difference.
4. Finally, add a drop or two of aqueous ammonia (NH3) to the test tube with the copper wire in it.  A dark purple/blue color means there is copper dissolved in the solution.

1. What visible proof did you  have that copper went into solution?  Be as specific as possible.

 

 
 
 
 
 
 
 
 
 
 

2. Was there any difference in temperature between the two test tubes?  Why?

 

 
 
 
 
 
 
 
 
 
 

3. Which reacted faster with the Ag⁺, magnesium or copper?  (In other words, which is more active, Mg or Cu?)

 

 
 
 
 
 
 
 
 
 
 

4. In view of the above results and the results from Part I, arrange Fe, Ag, Cu, and Mg in order from most to least active:

1. Put copper wire, aluminum foil, and magnesium ribbon into three diferent test tubes containing aqueous Pb²⁺.

1. Compare the speed of the reactions, from fastest to slowest:

 

 
 
 
 
 
 
 
 
 
 

2. In view of the results above and from Parts I and II, arrange Mg, Al, Cu, Pb, Ag, and Fe in order from most to least active:

        ______xx<xx______xx<xx______xx<xx______xx<xx______xx<xx______
spacer

1. Put magnesium ribbon in a test tube with Fe³⁺ solution.
2. Clean some iron wire, and place it in a test tube with aqueous Pb²⁺.

1. Which is more active, iron or magnesium?

 

 
 
 
 
 
 
 
 
 
 

2. Did lead come out of solution and gather on the iron wire?

 

 
 
 
 
 
 
 
 

3. In view of the results above and from Parts I, II, and III, arrange Mg, Al, Cu, Pb, Ag, and Fe in order from most to least active:

        ______xx<xx______xx<xx______xx<xx______xx<xx______xx<xx______
spacer

1. Put about 1 mL (half an inch) of dilute acid (marked H ⁺ or HCl) in each of six different test tubes.
2. Add Cu wire, Al foil, Pb, Mg ribbon, Fe wire, and a small piece of Zn (one to each test tube).
3. Note the relative rates of reaction by watching the amount of H2 gas given off.  If the metal dissolves, hydrogen will be produced but it will be a transparent gas rather than a visible solid.

1. List the metals in order of decreasing rate of reaction with H ⁺ .  You may use categories like "fast," "slow," and "NR."

 

 
 
 
 
 
 
 
 
 
 
 
 
 
 

2. In view of the results above and from Parts I - IV, arrange Fe, Al, Cu, Pb, Zn, H, Mg, and Ag in order from most to least active:

        ______xx<xx______xx<xx______xx<xx______xx<xx______xx<xx______xx<xx______xx<xx______
spacer

1. The solutions with silver and copper together should be put in the receptacle for silver waste.
2. The copper and iron wires can be cleaned and returned to their dispensing beakers.
3. All other solutions should be poured into the metal waste receptacle.
4. Wash all test tubes with soapy water and rinse.  Leave them upside down in the test tube rack to dry.
5. Put your goggles away.