NAME:______________________________________
JHS Chemistry Dept.
Metal Activity and Reactivity
Oxidation and Reduction Reactions
Introduction:
The usefulness of metals in structural and other applications depends on their physical
and chemical properties. Although iron is the most common metal used in
manufacturing, it must be protected against corrosion because iron rust (oxidize)
easily. Copper is used in electrical wiring because it conducts electricity extremely
well and resists corrosion better than many metals. Gold is highly valuable jewelry
metal because it is essentially unreactive. How can we determine the relative reactivity
of different metals?
Ranking of metals in order of their tendency to react with acids and water is called an
activity series. Comparing the reaction of sodium, magnesium, and aluminum reveals
that sodium reacts violently with acids and water, magnesium reacts with acids and
hot water, and aluminum reacts only with acids. Based on the trend in reactivity,
sodium is more active than magnesium, which is more active than aluminum. The
activity series for these metals would be written as Na>Mg>Al.
Pre-Lab Questions:
1. According to the reading above, magnesium is more active than aluminum. Predict
which combination of reactants will show evidence of a chemical change and write out
the balanced chemical reaction below:
Mg(s) + Al(SO4)3(aq)
or Al(s) + MgSO4(aq)
Balanced Redox Reaction:
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2. Write out the following half reactions for question #1:
Oxidation half reaction: __________________________________
Reduction half reaction: __________________________________
3. Identify the following from the redox reaction in question #1:
Reducing agent: ___________
Oxidizing agent: ___________
4. Using your glossary, define the following terms:
Spontaneous Redox Reaction:
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Nonspontaneous Redox Reaction:
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Objectives:
In this experiment you will be performing the following tasks:
 Using the materials provided, initiate
a chemical reaction (REDOX) using
three different metals.
 Observe whether a chemical change
did occur and was visible.
 Compare the results to the table of
activity series (Table J).
 Differentiate between a spontaneous
REDOX reaction and a nonspontaneous REDOX reaction.
Procedure:
Obtain three test tubes and place them in a test tube rack. Into each test
tube you will perform a reaction with the amounts of the reactants as
indicated in the chart below.
Data and Observations:
Test Tube #1
Add a small piece of Al(s) in a test tube. Next, add enough copper II sulfate solution to cover
the Al(s). Observe the test-tube for three minutes and record your observations.
Observations:
Chemical Equation:
Write out the complete balanced equation for this reaction.
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Besides being a redox reaction, what type of reaction is represent by the equation above?
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Write the balanced half reactions.
Oxidation half reaction: _________________________
Reduction half reaction:__________________________
Is this reaction spontaneous or non-spontaneous? Explain why using Table J.
Test Tube #2
Add a small piece of Ca(s) in a test tube. Add enough HCl(aq) to cover the small calcium
turning.
Observations:
Chemical Equation:
Write out the complete balanced equation for this reaction.
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Besides being a redox reaction, what type of reaction is represent by the equation above?
______________________________
Write the balanced half reactions.
Oxidation half reaction: _________________________
Reduction half reaction:__________________________
Is this reaction spontaneous or non-spontaneous? Explain why using Table J.
If a piece of gold were used instead of calcium, would you expect to see signs of a
chemical reaction? Explain your prediction using Table J.
Test Tube #3
Add a small piece of Cu(s) in a test tube. Add enough hydrochloric acid solution to cover
Cu(s).
Observations:
Chemical Equation:
Write out the complete balanced equation for this reaction.
__________________________________________________________________________
Besides being a redox reaction, what type of reaction is represent by the equation above?
______________________________
Write the balanced half reactions.
Oxidation half reaction: _________________________
Reduction half reaction:__________________________
Is this reaction spontaneous or non-spontaneous? Explain why using Table J.
If a piece of zinc were used instead of copper, would you expect to see signs of a
chemical reaction? Explain your prediction using Table J.
Summary Questions:
1. Two chemistry students each combine a different metal with hydrochloric acid.
Student A uses zinc, and hydrogen gas is readily produced. Student B uses copper, and
no hydrogen gas is produced.
a. State one chemical reason for the different results of student A and B.
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b. Using Reference Table J, identify another metal that will react with hydrochloric
acid to yield hydrogen gas.
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2. Copper metal reacts with aluminum nitrate to produce aluminum metal and copper
II nitrate.
a. Write out the balanced equation.
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b. Is the reaction spontaneous or nonspontaneous? Explain your answer using
Table J.
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3. The outer structure of the Statue of Liberty is made of copper metal. The
framework is made of iron. Over time, a thin green layer (patina) forms on the
copper surface. When copper oxidized to form this patina layer, the copper atoms
became copper(II)ions (Cu2+).
a. Write a balanced half-reaction for this oxidation of copper.
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b. Where the iron framework came in contact with the copper surface, a reaction
occurred in which iron was oxidized. Using information from Reference Table J,
explain why the iron was oxidized.
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