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Reduction/Oxidation
Notes
Redox
Oxidation:
1. A reaction in which a metal loses
electrons
2. Combining a metal with oxygen
Cu  Cu2+ + 2e-
Reduction:
1. A reaction in which a metal gains
electrons
2. Removing oxygen from a metal
Cu2+ + 2e-  Cu
But we live in an electrically-neutral world so
we can’t just have all of these electrons
(ions) hanging out. Whenever a metal loses
electrons, another must gain them. This is
why they are called REDOX reactions
Fe(s) + CuSO4(aq)  FeSO4(aq) + Cu(s)
 Which reaction is most likely to occur?
 Pb + 2LiNO3  2Li + PbNO3
 2Li + PbNO3  Pb + 2LiNO3
 Ask yourself this question:
 Is the “free metal” more active than the
“Combined metal”?
 If the answer is yes than the reaction will occur

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Ch. 4 redox

  • 2. Oxidation: 1. A reaction in which a metal loses electrons 2. Combining a metal with oxygen Cu  Cu2+ + 2e-
  • 3. Reduction: 1. A reaction in which a metal gains electrons 2. Removing oxygen from a metal Cu2+ + 2e-  Cu
  • 4. But we live in an electrically-neutral world so we can’t just have all of these electrons (ions) hanging out. Whenever a metal loses electrons, another must gain them. This is why they are called REDOX reactions Fe(s) + CuSO4(aq)  FeSO4(aq) + Cu(s)
  • 5.  Which reaction is most likely to occur?  Pb + 2LiNO3  2Li + PbNO3  2Li + PbNO3  Pb + 2LiNO3  Ask yourself this question:  Is the “free metal” more active than the “Combined metal”?  If the answer is yes than the reaction will occur