Post on 16-Dec-2015
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Predicting the Product in Single Replacement
ReactionsUsing the Activity Series
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)
• 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)
Introduction• In a single replacement reaction, the halide in
a salt solution is replaced by another halide.
AX(aq) + Y2 → AY(aq) + X2
• 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)
Introduction• These kinds of reactions do not occur with all
combinations of metals or halogens.
• Some metals will replace some other metal ions in solution.
• Some halogens will replace some other halogen ions in solution.
• However, not every metal will replace every other metal ion in solution.
Metals• The metals that replace other metal ions are
said to be “more active” than the metals they replace.
• For example, in the reaction
2 AgNO3(aq) + Mg(s) → Mg(NO3)2(aq) + 2 Ag(s)
•The metal Mg is more active than the Ag+ ion.
• 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.”
Metals• The most active metal is Li followed by Rb, K,
Ba, Sr, Ca, and Na.
• 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)
Metals• The most active metal is Li followed by Rb, K,
Ba, Sr, Ca, and Na.
• 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)
Metals• The next most active set of metals is Mg
followed by Al, Mn, Zn, Cr, Fe, and Cd.
• 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)
Metals• The next most active set of metals is Mg
followed by Al, Mn, Zn, Cr, Fe, and Cd.
• 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)
Metals• The next most active set of metals is Co
followed by Ni, Sn, and Pb.
• None of these metals react with H2O (hot or cold).
• 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)
Metals• The next most active set of metals is Co
followed by Ni, Sn, and Pb.
• 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)
Metals• The next most active set of metals is Sb
followed by Bi, Cu, and Hg.
• None of these metals react with water or acids.
• 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)
Metals• The least active set of metals is Ag followed by
Pt and Au.
• These metals are fairly unreactive.
• None of these metals react with water or acids.
• None of these metals react directly with O2(g) to form oxides.
• They will form oxides, but only indirectly.
Metals• The Activity Series:
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
most active
least active
incr
easi
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Halogens• The most active halogen is F2 followed by Cl2,
Br2, and I2.
• Each of these halogens are reactive with a wide variety of elements and compounds.
• The activity series just shows which is most reactive and least reactive.
Halogens• The Activity Series:
F2
Cl2
Br2
I2
most active
least active
incr
easi
ng
act
ivit
y
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.
• 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.
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.
• 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.
Using the Activity Series• For example:
• We put zinc metal in a solution of copper(II) sulfate.
Using the Activity Series• 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
Using the Activity Series• 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
Using the Activity Series• 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.
Using the Activity Series• 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).
Using the Activity Series• For example:
• We put zinc metal in a solution of copper(II) sulfate.
• 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)
Using the Activity Series• For example:
• We put magnesium metal in a solution of iron(III) chloride.
Using the Activity Series• 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
Using the Activity Series• 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
Using the Activity Series• 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.
Using the Activity Series• 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).
Using the Activity Series• For example:
• We put magnesium metal in a solution of iron(III) chloride.
• 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)
Using the Activity Series• For example:
• We put copper metal in a solution of iron(III) chloride.
Using the Activity Series• 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
Using the Activity Series• 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
Using the Activity Series• 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.
Using the Activity Series• 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).
Using the Activity Series• For example:
• We put copper metal in a solution of iron(III) chloride.
• We predict that there will be no reaction.
Cu(s) + FeCl3(aq) → no reaction
Using the Activity Series• For example:
• We add chlorine gas to a solution of iron(III) iodide.
Using the Activity Series• For example:
• We add chlorine gas to a solution of iron(III) iodide.
F2
Cl2
Br2
I2
Using the Activity Series• For example:
• We add chlorine gas to a solution of iron(III) iodide.
F2
Cl2
Br2
I2
Using the Activity Series• For example:
• We add chlorine gas to a solution of iron(III) iodide.
Cl2 is more active than I2.
F2
Cl2
Br2
I2
Using the Activity Series• For example:
• We add chlorine gas to a solution of iron(III) iodide.
Cl2 will replace I−.
F2
Cl2
Br2
I2
Cl2 is more active than I2.
Using the Activity Series• For example:
• We add chlorine gas to a solution of iron(III) iodide.
• 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)
Using the Activity Series• For example:
• We add chlorine gas to a solution of iron(III) fluoride.
Using the Activity Series• For example:
• We add chlorine gas to a solution of iron(III) fluoride.
F2
Cl2
Br2
I2
Using the Activity Series• For example:
• We add chlorine gas to a solution of iron(III) fluoride.
F2
Cl2
Br2
I2
Using the Activity Series• For example:
• We add chlorine gas to a solution of iron(III) fluoride.
F2 is more active than Cl2.
F2
Cl2
Br2
I2
Using the Activity Series• For example:
• We add chlorine gas to a solution of iron(III) fluoride.
Cl2 will not replace F−.
F2
Cl2
Br2
I2
F2 is more active than Cl2.
Using the Activity Series• For example:
• We add chlorine gas to a solution of iron(III) fluoride.
• We predict that there will be no reaction.
Cl2(g) + FeF3(aq) → no reaction
Practice ProblemsUse 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) →
Mg(NO3)2(aq) + Cu(s) 3 Fe(NO3)3(aq) + 3 Ag(s) 2 Cu(NO3)2(aq) + 2 Ag(s) no reaction
no reaction
2 3 Al2(SO4)3(aq) + 3 Sn(s) no reaction
Summary• 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.
• 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.
• 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.
• 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.
Summary