1. The Activity Series
Text Reference: 3.3 (pg )

2. We have looked at several reactions: Fe + CuSO4  Cu + Fe2(SO4)3
Li + H2O  LiOH + H2
Such experiments reveal trends. The activity series ranks the relative reactivity of metals.
It allows us to predict if certain chemicals will undergo single displacement reactions when mixed: metals near the top are most reactive and will displacing metals near the bottom.
Q: Which of these will react?
Fe + CuSO4 
Ni + NaCl 
Li + ZnCO3 
Al + CuCl2  K Na Li Ca Mg Al Zn Fe Ni Sn Pb H Cu Hg Ag Au
No, Ni is below Na
Yes, Li is above Zn
Yes, Al is above Cu
Yes, Fe is above Cu
Cu + Fe2(SO4)3
NR (no reaction)
Zn + Li2CO3
Cu + AlCl3

3. A: No for cold, yes if it is hot/steam Mg + H2O  H2 + Mg(OH)2 acid
H is the only nonmetal listed. H2 may be displaced from acids or can be given off when a metal reacts with H2O (producing H2 + metal hydroxide). The reaction with H2O depends on metal reactivity & water temp.
Q: will Mg react with H2O? K Na Li Ca Mg Al Zn Fe Ni Sn Pb H Cu Hg Ag Au
cold H2O
hot H2O
steam
A: No for cold, yes if it is hot/steam
Mg + H2O 
H2 + Mg(OH)2
acid
Q: Zn + HCl 
H2 + ZnCl2
Complete these reactions:
Al + H2O(steam) 
Cu + H2O 
Ca + H2SO4 
Na + H2O 
H2 + Al(OH)3 NR
H2 + CaSO4
H2 + NaOH

4. Other Activity Series Information
All metals will have a specific place in the activity series. For simplicity, only the most common metals are shown.
The metals near the top of the activity series are more reactive because their valence electrons are more easily removed.
On tests and exams the activity series may appear as K, Na, … Ag, Au; you must remember that K is reactive, Au is not.
If the valence of a metal is not indicated in the question, use its most common valence (in bold on your periodic table) to determine the correct chemical formula.

5. Activity series lab
On the next slide, place a check in the corner of boxes where you think reactions will take place.
Get a plastic spot plate.
Combine chemicals specified in the chart. Figure out a way to keep track of the chemicals. Use a ¼ scoop for solids (the less, the better). Use 1 squeeze of an eyedropper for solutions.
Write chemical equations for chemicals that reacted. Write NR where there was no reaction.
Dump used chemicals into the large funnel at the front of the room (use a squirt bottle to rinse remaining chemicals into the funnel). Wash the spot plate and glass rod very well. Dry & return.

6.          Mg + AgNO3  Ag+ Mg(NO3)2 Cu + AgNO3  Ag+ Cu(NO3)2Zn   
Mg + AgNO3 
Ag+ Mg(NO3)2
Cu + AgNO3 
Ag+ Cu(NO3)2
Zn + AgNO3 
Ag+ Zn(NO3)2
AgNO3  
Mg + H2SO4 
H2 + MgSO4
Zn + H2SO4 
H2 + ZnSO4
H2SO4 NR  
Mg+ Fe(NO3)3 
Fe+ Mg(NO3)2
Zn+ Fe(NO3)3 
Fe+ Zn(NO3)2
Fe(NO3)3 NR  
Mg + CuCl2 
Cu + MgCl2
Zn + CuCl2 
Cu + ZnCl2
CuCl2 NR

7. Oxides K Na Li Ca Mg Al Zn Fe Ni Sn Pb H Cu Hg Ag Au
The formation and behavior of oxides can also be predicted via the activity series.
Complete these reactions:
Ca + O2 
Au + O2 
Fe2O3+ H2 
Oxides form via the addition of oxygen:
K + O2  K2O
Oxides plus H2 (with heat) will change to metal and H2O:
NiO + H2  Ni + H2O
heat
CaO
Oxides decompose with heat:
HgO  Hg + O2 NR
heat
heat
Fe + H2O