1. The Activity Series

2. The Theory Behind the Activity Series:
Strong reducing agents require only weak oxidizing agents to react vigorously
(eg. potassium reacts violently on contact with water.)
K (s) + H(OH) → H2 (g) + KOH (aq)
since K is higher than H on the activity series
Potassium Video

3. Weak reducing agents will not react with even strong oxidizing agents
(eg. part of the reason why gold is so precious is because it resists tarnishing.)
Au (s) + HCl (aq) –> no reaction
This is because Au is NOT higher than H on the activity series
Since it is NOT more reactive it can not displace the more reactive hydrogen from the compound

4. This is because metal atoms are by nature prone to losing electrons
This is because metal atoms are by nature prone to losing electrons. However, some metals lose electrons more easily than others. Their readiness to be oxidized makes them powerful reducing agents. We can compare the power of reducing agents in the activity series for metals.
Why do metals easily lose their electrons??
Alkali metals have a very low ionization energy and thus their electrons are easily lost.
Alkaline Earth metals also follow this trend and together they make up the top six metals on the activity series.

5. } } } } } } The Activity Series Lithium Li Potassium K Barium Ba
These metals displace hydrogen from water Ca(s) + 2H2O(l)→ Ca(OH)2 + H2 (g)
Calcium Ca These elements are very reactive and react readily to form compounds
Sodium Na
Magnesium Mg
Aluminum Al
Zinc Zn
These metals displace hydrogen from acids, but do not react with water
Chromium Cr Zn(s) + HCl(aq)→ ZnCl2 + H2(g)
Iron Fe
Cadmium Cd
Nickel Ni
Tin Sn
Lead Pb
Hydrogen H
Copper Cu These metals do not displace hydrogen from acids or water
Silver Ag These elements are more stable, and form compounds less readily than do those higher in the table.
mercury Hg
platinum Pt
Gold Au } } } } } }

6. Examples Li (s) + NaCl (aq)  SnCO3 (aq) + Mg (s) 
Au (s) + HCl (aq) 
Cu (s) + Li(OH) (aq) 
LiCl (aq) + Na (s)
MgCO3 (aq) + Sn (s)
NR (gold won’t decay in acid)
NR (pennies won’t decay in base)

7. a) Cu (s) + Ag(NO3) (aq)  b) Fe(s) + CuCl2 (aq) 
Practice: Complete the following reactions. If no reaction occurs, then please write 'NR'
a) Cu (s) + Ag(NO3) (aq) 
b) Fe(s) + CuCl2 (aq) 
c) AlCl3 (aq) + Zn (s) 
d) KCl (aq) + H2 (g) 
e) KCl (aq) + F2 (g) 
f) Br2 (g) + PbI2 (aq) 

8. g) lead + zinc acetate 
h) iron + aluminum oxide 
I) silver nitrate + nickel 
j) sodium bromide + iodine 
k) aluminum bromide + chlorine 
l) sodium iodide + bromine 
m) calcium + hydrochloric acid 
n) magnesium + nitric acid 
o) silver + sulfuric acid 
p) potassium + water 
q) sodium + water 