CP Chemistry
Theodore Roosevelt High School
Lab #1-6
Reactivity of Metals Lab
Introduction
In nature, elements can occur either free (uncombined with other elements) or
chemically combined in a compound. The tendency of an element to combine with
other substances is called the reactivity of that element. The more reactive an
element is, the more likely it is to combine with other substances. In a singlereplacement reaction, one element takes the place of another element in a
compound. In general, more reactive elements replace less reactive elements. As
a result of the reaction, the less reactive element is freed from the compound.
In the reaction between zinc (Zn) and copper (II) sulfate (CuSO4), the more reactive zinc replaces
copper and combines with the sulfate ion. The less reactive copper is released from the compound and
becomes a free element. Likewise, when a metal is placed in hydrochloric acid (HCl), a single
replacement reaction can occur. If the metal is more reactive than the hydrogen in the acid, the metal
will replace the hydrogen, and bubbles of hydrogen gas (H2) will be produced. The more reactive a
metal is, the more vigorously it will react with hydrochloric acid.
In this lab, you will determine whether or not various metals undergo single-replacement reactions
when placed in hydrochloric acid. Based on your observations of these reactions, you will then rank the
metals by reactivity.
Purpose
To determine the reactivity series of common metals; to observe single replacement reactions.
Prediction
Which metal will be the most reactive? Why do you think so?
Equipment
graduated cylinder (10 mL)
marker
test tubes, 5 small
test-tube rack
Materials
aluminum [Al]
copper [Cu]
hydrochloric acid, 1M [HCl]
iron [Fe]
magnesium [Mg]
zinc [Zn]
Safety Considerations
• Hydrochloric acid is damaging to the eyes; YOU MUST WEAR GOGGLES AT ALL TIMES.
• Some of the metals may not completely react; DO NOT POUR THEM DOWN THE SINK.
Instead, pour them in the specially marked waste beakers.
Procedure
1.
Use the glass marker to label each test tube with the symbol for each metal used in the lab.
Place the test tubes in a test-tube rack.
2.
One at a time, place the appropriate metal in each test tube. Using a small graduated cylinder,
carefully measure and pour 5 mL of hydrochloric acid into each of the five test tubes.
CP Chemistry
3.
Theodore Roosevelt High School
Lab #1-6
Observe what happens to the metal in each test tube and feel each test tube as the reaction
proceeds. Record your observations.
Additional Clean-up and Disposal
1.
Pour any leftover acid or metals into the appropriately marked waste beaker, i.e. pour the “Fe” test
tube into the “Fe” waste beaker.
Data – you should create a data table in your lab write-up that looks something like this:
Metal
Observations
Reactivity Rank
Aluminum
(Al)
Copper
(Cu)
…etc. for all metals.
Questions
1.
The rate at which hydrogen gas is produced as a result of these single-replacement reactions is
an indication of the relative reactivity of the metals. List the metals in order of their reactivity from
the most reactive to the least reactive.
2.
Were these reactions endothermic or exothermic? Explain.
3.
What could you do to determine whether the gas produced by these reactions is hydrogen?
Errors
Describe two possible errors you may have committed in this lab that may have somehow affected your
results. Explain the specific steps you will take to avoid each of these errors in the future.
Conclusion
Write two or more paragraphs summarizing your results, examining the validity of your prediction, and
explaining the reactivity of each metal.
CP Chemistry
Theodore Roosevelt High School
Reactivity of Metals Lab workspace:
Lab #1-6