Lab: Metal Activity Series – Single Replacement Reactions
Purpose
To determine the more reactive metal from each pair tested using single replacement reactions
To determine the activity series for the set of metals investigated
Theory
In single replacement reactions an elemental form is combined with an ionic compound in solution
(aqueous). By being dissolved in water, the ions are free to bind to other ions and react with the
elemental reactant.
The most active elements are the most reactive and form compounds rather than remain in elemental
forms. For non-metals, atoms that attract and hold onto valence (bonding) electrons the strongest form
ionic compounds with available cations. Of the halogens, fluorine has valence electrons in the lowest
energy level so they are attracted the strongest to the positively charged nucleus. The other halogens,
chlorine, bromine, and iodine, have increasingly higher valence energy levels and reduced attraction to
the nucleus.
Each metal can be compared to another metal using a pair of single replacement reactions. Each metal
will be placed in a solution of the other metal. Only one “metal–metal solution” pair should result in a
reaction. The most reactive metal will be the elemental metal that reacts with the solution.
Variables
Chemicals
Materials
Dependent
Observed evidence of reaction
Independent
metal pairs (Cu-Mg, Cu-Zn, Mg-Zn)
Constants
soluble metal salts used → sufficient ions for visible reaction
same solutions were used throughout → no contamination
test tubes were cleaned thoroughly before using → no contamination
copper, Cu, ribbon
copper (II) sulfate, CuSO4 (aq), solution
magnesium, Mg, turnings
magnesium nitrate, Mg(NO3)2 (aq), solution
zinc, Zn, mossy
zinc nitrate, , Zn(NO3)2 (aq), solution
test tubes (6 large)
spatula
test tube brush
Procedure
Preparation
The six (6) large test tubes were cleaned thoroughly to remove any residue
Two small samples of each metal were obtained and observed.
The three solutions were obtained and observed.
Reactions
Copper – Magnesium
2 mL of copper (II) sulfate was placed in test tube A and a sample of magnesium was added.
2 mL of magnesium nitrate was placed in test tube B and a sample of copper was added.
This was repeated for copper and zinc and for magnesium and zinc.
All observations of the reaction mixtures were recorded.
• All observations for evidence of reaction were made and recorded.
• Any evidence that a reaction did not happen were also recorded.
Conclusions
Deduce the most reactive metal in each pair.
• Provide support for your deduction
• Write a balanced chemical equation with states for each reaction
Deduce the order of activity (activity series) for this set of metals
• Compare your conclusions to published information (cite source).
Results: Raw Data
Table 1.Description of reactants (before reactions).
Chemical
Description
copper metal
magnesium metal
zinc metal
copper solution
magnesium solution
zinc solution
Table 2.Observations of reaction mixtures. This is what was observed not conclusions about whether a reaction happened or not.
Copper – Magnesium
A
copper solution + Mg
B
magnesium solution + Cu
Copper – Zinc
C
copper solution + Zn
D
zinc solution + Cu
Magnesium - Zinc
E
magnesium solution + Zn
F
magnesium solution + Mg