1. RedOx reactions (Single Replacement)
2 Mg (s) + O2 (g)  2 MgO (s) +2 -2
Mg = oxidized  more positive
(reducing agent)
O2 = reduced  more negative
(oxidizing agent)
LEO the lion goes GER
OIL…RIG

2. Oxidation of Metals by Acids and Salts
Zn (s) HCl (aq)  ZnCl2 (aq) + H2 (g) +1 +2
Zn = oxidized  more positive
(reducing agent)
H = reduced  more negative
(oxidizing agent)

3. Oxidation of Metals by Acids and Salts
H2SO4 (aq) + Fe (s)  FeSO4 (aq) + H2 (g) +1 +2
Fe = oxidized  more positive
(reducing agent)
H = reduced  more negative
(oxidizing agent)

4. Oxidation of Metals by Acids and Salts
Ni(NO3)2 (aq) + Fe (s)  Ni (s) + Fe(NO3)2 (aq)
Net Ionic: +2 +2
Ni+2 (aq) Fe (s)  Ni (s) + Fe+2 (aq)
Fe = oxidized  more positive
(reducing agent)
Ni = reduced  more negative
(oxidizing agent)

5. Activity Series Use to predict if a reaction will occur
Single Replacement
Any metal can be OXIDIZED by any metal below it on the series

6. Activity Series

7. Examples Cu (s) + 2AgNO3 (aq)  Cu(NO3)2 (aq) + 2 Ag (s) Net Ionic:+1 +2
Cu (s) Ag+1(aq)  Cu+2 (aq) Ag(s)
Cu = oxidized  more positive
(reducing agent)
Ag = reduced  more negative
(oxidizing agent)

8. Examples Cu (s) + 2FeNO3 (aq)  No Reaction
Based on the Activity Series Cu can’t be oxidized by Fe
Meaning that Cu is below Fe on the activity series

9. Examples Ni (s) + 2 HCl (aq)  NiCl2 (aq) + H2 (g) Net Ionic:+1 +2
Ni (s) H+1(aq)  Ni+2 (aq) + H2 (g)
Ni = oxidized  more positive
(reducing agent)
H = reduced  more negative
(oxidizing agent)

10. Types of RedOx reactions
Single replacement in acid
Mg(s) + HCl(aq) 
Single replacement in H2O
Ca(s) + H2O(l) 
Single replacement in aqueous salt
Cu(s) + AgNO3(aq) 
Single replacement of nonmetals
F2(g) + LiBr(aq) 