Honors Chemistry
Notes for 07-09
Using the Activity Series
Page 1 of 8
Introduction

In a single replacement reaction, the metal ion in a salt solution is replaced
by another metal.
AX(aq) + B(s) → BX(aq) + A(s)
o For example:

Adding magnesium metal to a solution of silver chloride causes
the magnesium to dissolve and the silver to precipitate out.
2 AgNO3(aq) + Mg(s) → Mg(NO3)2(aq) + 2 Ag(s)

In a single replacement reaction, the halide in a salt solution is replaced by
another halide.
AX(aq) + Y2 → AY(aq) + X2
o For example:

Adding chlorine gas to a solution of sodium bromide causes the
chlorine to dissolve and the bromine to come out as a liquid.
2 NaBr(aq) + Cl2(g) → 2 NaCl(aq) + Br2(l)

These kinds of reactions do not occur with all combinations of metals or
halogens.
o Some metals will replace some other metal ions in solution.
o Some halogens will replace some other halogen ions in solution.
o However, not every metal will replace every other metal ion in
solution.
Honors Chemistry
Notes for 07-09
Using the Activity Series
Page 2 of 8
Metals

The metals that replace other metal ions are said to be “more active” than
the metals they replace.
o For example, in the reaction
2 AgNO3(aq) + Mg(s) → Mg(NO3)2(aq) + 2 Ag(s)
o Mg is more active than Ag.

By examining a series of reactions with solid metals and dissolved metal ions,
we can build a list of metals based on activity.

We call this the “Activity Series.”

The most active metal is Li followed by Rb, K, Ba, Sr, Ca, and Na.
o Each of these metals react with cold water and acids, replacing H.
2 Li(s) + H2O(l) → Li2O(s) + H2(g)
2 K(s) + HCl(aq) → 2 KCl(aq) + H2(g)
o Each of these metals react with O2(g), forming oxides.
2 Ba(s) + O2(g) → 2 BaO(s)
2 Rb(s) + O2(g) → Rb2O(s)

The next most active set of metals is Mg followed by Al, Mn, Zn, Cr, Fe, and Cd.
o Each of these metals react with H2O(g) and acids, replacing hydrogen.
Mg(s) + H2O(g) → MgO(s) + H2(g)
Zn(s) + 2 HNO3(aq) → Zn(NO3)2(aq) + H2(g)
o Each of these metals react with O2(g), forming oxides.
2 Zn(s) + O2(g) → 2 ZnO(s)
4 Fe(s) + 3 O2(g) → 2 Fe2O3(s)
Honors Chemistry

Notes for 07-09
Using the Activity Series
Page 3 of 8
The next most active set of metals is Co followed by Ni, Sn, and Pb.
o None of these metals react with H2O (hot or cold).
o They do react with acids, replacing hydrogen.
Co(s) + 2 HNO3(aq) → Co(NO3)2(aq) + H2(g)
Pb(s) + H2SO4(aq) → PbSO4(aq) + H2(g)
o Each of these metals react with O2(g), forming oxides.
2 Ni(s) + O2(g) → 2 NiO(s)
2 Sn(s) + O2(g) → 2 SnO(s)

The next most active set of metals is Sb followed by Bi, Cu, and Hg.
o None of these metals react with water or acids.
o Each of these metals react with O2(g), forming oxides.
4 Sb(s) + 3 O2(g) → 2 Sb2O3(s)
2 Cu(s) + O2(g) → 2 CuO(s)

The least active set of metals is Ag followed by Pt and Au.
o These metals are fairly unreactive.
o None of these metals react with water or acids.
o None of these metals react directly with O2(g) to form oxides.

They will form oxides, but only indirectly.
Honors Chemistry
Page 4 of 8
Ba
Mn
Zn
Sr
Cr
Ca
Fe
Na
Cd
Ni
Sn
Pb
Sb
Bi
Cu
Hg
increasing activity
K
Al
Co
increasing activity
Rb
Mg
increasing activity
Li
increasing activity
The Activity Series
most active
increasing activity

Notes for 07-09
Using the Activity Series
Ag
Pt
Au
least active
Halogens
The most active halogen is F2 followed by Cl2, Br2, and I2.
o Each of these halogens are reactive with a wide variety of elements
and compounds.
o The activity series just shows which is most reactive and least
reactive.
most active
F2
increasing activity

Cl2
Br2
I2
least active
Honors Chemistry
Notes for 07-09
Using the Activity Series
Page 5 of 8
Using the Activity Series

The activity series is used to predict whether or not a single replacement
reaction will occur.

First, we look at the ions in a solution.

Next, we look at the metal or halogen being added to the solution.
o For metals:

If the metal is higher up on the activity series list, then it goes
into solution and the metal ion in solution precipitates out.

If the metal is lower down on the activity series list, then there
is no reaction.
o For halogens:

If the halogen is higher up on the activity series list, then it
goes into solution and the halide ion in solution comes out as a
solid, liquid, or gas.

If the halogen is lower down on the activity series list, then
there is no reaction.
Honors Chemistry
Notes for 07-09
Using the Activity Series
Page 6 of 8
For example:
We put zinc metal in a solution of copper(II) sulfate.
Li
Mg
Co
Sb
Ag
Rb
Al
Ni
Bi
Pt
K
Mn
Sn
Cu
Au
Ba
Zn
Pb
Hg
Sr
Cr
Ca
Fe
Na
Cd
Zn is more active than Cu.
Zn(s) will replace Cu2+(aq).
We predict that the solid zinc will dissolve in the solution (forming Zn2+ ions)
and copper metal will precipitate out.
Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s)
For example:
We put magnesium metal in a solution of iron(III) chloride.
Li
Mg
Co
Sb
Ag
Rb
Al
Ni
Bi
Pt
K
Mn
Sn
Cu
Au
Ba
Zn
Pb
Hg
Sr
Cr
Ca
Fe
Na
Cd
Mg is more active than Fe.
Mg(s) will replace Fe3+(aq).
We predict that the solid magnesium will dissolve in the solution (forming
Mg2+ ions) and iron metal will precipitate out.
3 Mg(s) + 2 FeCl3(aq) → 3 MgCl2(aq) + 2 Fe(s)
Honors Chemistry
Notes for 07-09
Using the Activity Series
Page 7 of 8
For example:
We put copper metal in a solution of iron(III) chloride.
Li
Mg
Co
Sb
Ag
Rb
Al
Ni
Bi
Pt
K
Mn
Sn
Cu
Au
Ba
Zn
Pb
Hg
Sr
Cr
Ca
Fe
Na
Cd
Fe is more active than Cu.
Cu(s) will not replace Fe3+(aq).
We predict that there will be no reaction.
Cu(s) + 2 FeCl3(aq) → no reaction
For example:
We add chlorine gas to a solution of iron(III) iodide.
F2
Cl2
Br2
I2
Cl2 is more active than I2.
Cl2(s) will replace I–(aq).
We predict that the chlorine gas will go into solution (forming a Cl− ion) and
the iodine will come out as a solid.
3 Cl2(g) + 2 FeI3(aq) → 2 FeCl3(aq) + 3 I2(s)
Honors Chemistry
Notes for 07-09
Using the Activity Series
Page 8 of 8
For example:
We add chlorine gas to a solution of iron(III) fluoride.
F2
Cl2
Br2
I2
F2 is more active than Cl2.
Cl2(s) will not replace F–(aq).
We predict that there will be no reaction.
3 Cl2(g) + 2 FeF3(aq) → no reaction
Practice Problems:
Use the activity series to predict the products of the following reactions. Indicate if
there is no reaction.
1. Mg(s) + Cu(NO3)2(aq) →
2. Fe(s) + AgNO3(aq) →
3. Cu(s) + AgNO3(aq) →
4. Fe(s) + Na2SO4(aq) →
5. Pb(s) + Co(NO3)2(aq) →
6. Al(s) + SnSO4(aq) →
7. Zn(s) + MnCl2(aq) →