1. The document describes an experiment to determine the reactivity of metals by observing their reactions with acid and metal ion solutions. 2. Students will place pieces of copper, aluminum, iron, zinc, magnesium, and calcium in test tubes containing acid and wells containing metal ion solutions and record their observations. 3. Based on their observations, students will rank the metals from most reactive to least reactive and place them on the periodic table.

1. Name ________________________________________ Date ____________________ PAGE 1
Activity Series
Pre-Lab Discussion
Chemical elements are generally classified by their properties into three groups, called the metals, nonmetals, and
metalloids. The vast majority of the known chemical elements are metals. Metals tend to be good conductors of heat and
electricity. The also generally are shiny (high luster), are malleable (can be pounded flat without shattering), and ductile
(can be drawn out into a very thin wire). With the exception of mercury, the metals are all solids at room temperature. The
elements are found to the right and below the “stair-step” generally drawn on periodic tables starting between Boron and
Aluminum, and working down to between Polonium and Astatine.
Families, or groups, of elements consist of elements with similar chemical properties. These similar chemical
properties are caused by similar outer shell (valence) electron configurations. On the periodic table, they are placed
together in vertical columns. So, elements in a vertical column together on the periodic table have similar outer shell
electron configurations.
Many of the groups on the periodic table have names. These are:
Group 1: called the alkali metals because they react with oxygen to form bases
Group 2: called the alkaline earth metals because their presence can make soils basic (alkaline)
Groups 3-12: called the transition metals because they span the transition from metals to nonmetals
Group 15: called the pnictides, from the Greek word meaning choking suffocation
Group 16: called the chalcogens, from the Greek word meaning ore-former
Group 17: called the halogens, from the Greek cord meaning salt-former
Group 18: called the noble gases because they were thought to be unreactive
Purpose
To become familiar with the relative activities of metals in chemical reactions.
Equipment
small test tubes test tube rack well plate
Materials
6 M HCl 0.2 M
Ca(NO3)2 (labeled Ca2+
)
0.2 M Mg(NO3)2
(labeled Mg2+
)
0.2 M Zn(NO3)2 (labeled Zn2+
) 0.2 M Fe(NO3)3
(labeled Fe3+
) 0.2 M
FeSO4 (labeled Fe2+
)
0.2 M AlCl3 (labeled Al3+
) 0.5 M Cu(NO3)2 (labeled Cu2+
)
Small pieces of copper, aluminum, iron, zinc, magnesium and calcium metals
Safety
Since you will be using potentially hazardous materials, the Maryland state law requiring students to wear safety
goggles will be in effect, so they must be worn. Lab aprons are available for use should you wish to wear one. Handle all
glassware with care, especially test tubes as they are fragile and easily broken.

2. Name ________________________________________ Date ____________________ PAGE 2
Procedure
Record all observations in the table provided below on the next page. It is not necessary to rewrite these observations in
complete sentences. (“N. R.” means that no reaction occurs).
For each reaction, write down any noticeable changes that occur - color change, heat produced, precipitate forming, odor
produced, etc. Let a test tube sit for at least 5 minutes - and remember to tap test tubes to dislodge small bubbles on the
surface of a metal that might not be otherwise noticed - before you declare a “no reaction”.
1. Obtain a test tube rack and six test tubes. Fill the test tubes about 1/4 to 1/3 full with 6 M HCl solution.
2. Place a single small piece of copper metal into the first test tube. Observe for any changes. If the reaction
is slow, you may proceed to step 3 while you are waiting.
3. Repeat step 2 with the remaining test tubes, testing small pieces of Aluminum metal, iron metal, zinc
metal, magnesium metal, and calcium metal. Record your observations in the table (page 3).
4. Once your observations are complete, empty the six test tubes into the waste beaker provided by your
teacher. Place the empty test tubes into the bin of soapy water.
5. Obtain a well plate. Fill each of 6 wells about 1/3 to 1/2 full with solutions from the beakers at your lab
station labeled, in order: Ca2+
, Mg2+
, Zn2+
, Fe2+
, Fe3+
, and Al3+
.
6. Place a single small piece of copper metal into each of 6 wells from step 5. Observe for any changes. If the
reaction is slow, you may proceed to the remaining steps while you are waiting.
7. Repeat steps 5 and 6 with six new wells, using aluminum metal in solutions of Ca2+
, Mg2+
, Zn2+
, Fe2+
, Fe3+
,
and Cu2+
.
8. Repeat steps 5 and 6 with six new wells, using iron metal in solutions of Ca2+
, Mg2+
, Zn2+
, Fe3+
, Al3+
, and
Cu2+
.
9. Empty your well plate into the waste beaker. Rinse the wells and empty the rinse water into the waste
beaker. Thoroughly wash the wells, scrubbing each well with a test tube brush. Dry well plate.
10. Repeat steps 5 and 6 with six new wells, using zinc metal in solutions of Ca2+
, Mg2+
, Fe2+
, Fe3+
, Al3+
, and
Cu2+
.
11. Repeat steps 5 and 6 with six new wells, using magnesium metal in solutions of Ca2+
, Zn2+
, Fe2+
, Fe3+
, Al3+
,
and Cu2+
.
12. Repeat steps 5 and 6 with six new wells, using calcium metal in solutions of Mg2+
, Zn2+
, Fe2+
, Fe3+
, Al3+
and Cu2+
.
13. When your observations are complete, repeat step 9.

3. Observations
Metal HCl Ca2+
Mg2+
Zn2+
Fe2+
Fe3+
Al3+
Cu2+
Cu
Al
Fe
Zn
Mg
Ca

4. Questions (These should be answered in complete sentences here in the space provided or on your own paper.)
1. Which of the six metals in your observations chart (Cu, Fe, Zn, Mg, Ca, or Al) would you expect to be the most
reactive? Why did you choose this metal as your answer?
___________________________________________________________________________________________
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2. Which metal ion is more reactive: Fe2+
or Fe3+
? What makes this ion more reactive?
___________________________________________________________________________________________
___________________________________________________________________________________________
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3. Rank the six metals from your observation chart (Cu, Fe, Zn, Mg, Ca, and Al) in order from most reactive to
least reactive. This question does not need to be answered in complete sentences.
most reactive
least
reactive
1. _______ 2. _______
3.
_______
4. _______
5. _______
6. _______

5. 4. Place the 6 metals in their proper location on the periodic table below. Explain how the trend of metallic
character is arranged on the periodic table. Do any of the metals not fit this trend? Explain.

6. 4. Place the 6 metals in their proper location on the periodic table below. Explain how the trend of metallic
character is arranged on the periodic table. Do any of the metals not fit this trend? Explain.