From single displacement reactions it
is easy to see some metals are more
reactive than others.
For instance when iron combines with
copper sulfate the iron "steals" the
sulfate from the copper.
This means if an activity series was
created with the more reactive metal
on top and the less reactive metal on
bottom the result would be:
Iron
Copper
You will now perform a
series of single
displacements using
metals and solutions
containing metal ions.
This will enable you to
create your own reactivity
series.
Reaction Plate
Place a small amount CuSO4 in
4 of the wells.
Repeat the same step with solutions of
Iron(II) chloride, zinc nitrate,
aluminium nitrate, magnesium chloride
CuSO4
FeCl3
ZnNO3
Al(NO3)2
MgCl2
CuSO4
FeCl2
ZnNO3
Al(NO3)2
MgCl2
Al, Mg, Cu in each
of the wells but
don’t place metals
with solutions
which are the
same.
CuSO4
FeCl3
Zn(NO3)2
Al(NO3)3
MgCl2
Fe
Zn
Al
Mg
Cu
Now observe the wells using a
dissecting microscope to detect
any evidence of chemical
change.
Construct an activity series
based on the empirical
evidence.
Fe
Zn
Al
Mg
Cu
Zn
Fe
Al
Mg
Cu
Cu
Zn
Fe
Al
Mg
Mg
Cu
Zn
Fe
Al
Al
Mg
Cu
Zn
Fe
Write a lab report.
In the conclusion include balanced chemical
equations for all observed single displacement
reactions.
There are more than 20 possible chemical
reactions. For metals with multiple oxidation
states write all possible reactions.
If no reaction occurs write the reactants with
an arrow and NR (no reaction) as the product.
If Cu doesn’t react with MgCl2(aq) write:
Cu + MgCl2 ------> NR
follow this sequence:
CuSO4
FeCl3
Zn(NO3)2
Al(NO3)3
MgCl2
Fe
Zn
Al
Mg
Cu
Products of Reactions
CuSO4
FeCl 3
Zn(NO3)2
Al(NO3)3
MgCl 2
Fe
Zn
Al
Mg
Cu
FeSO4 + Cu
Cu + ZnSO4
Cu + Al2(SO4)3
Cu + MgSO4
x
Fe + ZnCl2
Fe + AlCl3
Fe + MgCl2
Zn + Al(NO3)2
Zn + Mg(NO3)2
x
Al + Mg(NO3)2
x
x
x
Products of Reactions
CuSO4
FeCl 3
Zn(NO3)2
Al(NO3)3
MgCl 2
Fe
Zn
Al
Mg
Cu
FeSO4 + Cu
Cu + ZnSO4
Cu + Al2(SO4)3
Cu + MgSO4
x
Fe + ZnCl2
Fe + AlCl3
Fe + MgCl2
Zn + Al(NO3)2
Zn + Mg(NO3)2
x
Al + Mg(NO3)2
x
x
x
Mg
Al
Zn
Fe
Cu