Lab #2 Chapter 11: Reactivity of Metals Lab
Name ____________________________
Introduction:
The following experiment is designed to demonstrate the relative reactivity of various metals through the
combination of solid metals and metal ions in solution. Through observation and recorded findings, the
initiation of a single displacement reaction or the lack of reaction will indicate the reactivity of the metals
involved. Given the metal activity series, it is possible to predict which combinations will result in a
single displacement reaction and which will not react. Relative reactivity observed in this experiment is
expected to be consistent with existing metal activity information available. More reactive metals will
replace less reactive metals in solution forming a precipitate and metals that show more reactivity than
hydrogen will replace hydrogen in an acid to form an ionic solution with the evolution of hydrogen gas.
Equipment:

10 medium test tubes

1 test tube rack
Reagents and materials:

3 mL Pb(NO3)2 (aq)

3 mL Cu(NO3)2(aq)

3 mL AgNO3 (aq)

3 mL ZnCl2(aq)

3 mL KI(aq)

3 mL NaCl(aq)
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
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3 mL MgCl2(aq)
3 mL HNO3(aq)
Copper wire
Magnesium chunks/ribbon
Zinc chunks/ribbon
Put on lab apron and safety goggles.
a. Solutions of lead and copper are toxic
b. Silver nitrate is toxic and will leave dark brown stains on skin and clothing
Label 10 test tubes # 1-10 and place in the test tube rack.
To tube #1 add 3 mL lead (II) nitrate solution and a piece of copper wire.
To tube #2 add 3 mL silver nitrate solution and a piece of copper wire.
To tube #3 add 3 mL copper (II) nitrate solution and a strip of zinc ribbon
To tube #4 add 3 mL lead (II) nitrate and a strip of zinc ribbon.
To tube #5 add 3 mL magnesium chloride solution and a strip of zinc ribbon
To tube #6 add 3 mL zinc chloride and a chunk of magnesium
To tube #7 add 3 mL sodium chloride and a chunk of magnesium
To tube #8 add 3 mL potassium iodide and a chunk of magnesium
To tube #9 add 3 mL nitric acid and a chunk of magnesium
To tube #10 add 3 mL nitric acid and a piece of copper wire.
Observe each trial and record observations in table. Record whether or not a reaction
occurred based on the formation of a precipitate, evolution or gas, color change of
solution etc. Some combinations will not produce a reaction (record as NR).
Write complete, balanced chemical equations for each reaction observed.
Table 1 Observations of metal activity
Tube # Solid metal
Metal ion in
Solution
Observations
Write complete, balanced formula equations for each reaction observed.
1._________________________________________________________________________________
2._________________________________________________________________________________
3._________________________________________________________________________________
4._________________________________________________________________________________
5._________________________________________________________________________________
Analyze data collected and arrange the metals (both solid and in solution) according to their
reactivity. List the metals below, from most reactive to least reactive.
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