1. Aka REDOX reactions

2.  The study of chemical reactions involving the transfer of electrons between reactants.

3.  Loss of electrons  happens at the anode

4.  gain of electrons  happens at the cathode

5. LEO the Lion says GER!

6.  A substance that gains electrons in a redox reaction

7.  A substance that loses electrons in a redox reaction

8.  Either the oxidation or reduction reaction component of a redox reaction. Obtained by considering the change in oxidation states of individual substances involved

9.  Metallurgy is the science of extracting metals from their naturally occurring compounds  Since most metals are found in ores (only gold and silver are found as naturally occurring elements) we need to get them alone through chemical processes  These processes are single replacement reactions

10.  REDOX reactions involve both oxidation and reduction reactions  The overall oxidation- reduction reaction involves the transfer of electrons

11.  Show the gain and loss of electrons Net: Cu(s) + 2Ag+(aq)  Cu2+ + 2Ag(s) Cu(s)  Cu2+(aq) + 2e- (loss of e-) 2[Ag+(aq) + e-  Ag(s)] (gain of e-)

12. 1. Determine your overall reaction (just the reactants are required!) 2. Dissociate ionic compounds 3. Label whether each reactant is an oxidizing agent or a reducing agent (by looking at the chart) 4. Out of all the entities, determine your strongest agents (highest on the left, lowest on the right of the table) 5. Copy the half reaction exactly out of the booklet 6. Balance the electrons and cancel out the entities on both sides of the arrow to find the net equation

13.  Copper metal is placed in a solution of acidified potassium dichromate. Write a balanced redox reaction equation for the reaction of copper metal with postassium dichromate

14.  Leaching technology is used in mining and refining of copper ore. In the first step of the leaching process, sulfuric acid flows through a copper ore deposit. Under ideal conditions, the copper metal in the ore reacts with the concentrated sulfuric acid to form copper(II) ions. The resulting copper(II) slurry is transferred to an electrolytic cell where pure copper is produced (assume that the sulfuric acid completely ionizes to hydrogen ions and sulfate ions).  A non-spontaneous reaction may occur if the concentrations are manipulated. Demonstrate the balanced net ionic equation for the reaction of copper metal with sulfuric acid under these ideal conditions.

15.  If NO ELECTRON transfer occurs in a reaction, it is NOT a redox reaction  There must be a change in the oxidation numbers (one must decrease, one must increase)

16.  Disproportionation reactions occur when the same entity is both oxidized and reduced in a redox reaction  AKA self-oxidation-reduction  AKA auto-oxidation

17. Cr(OH) 2 (aq) reacts with CrSO 4 (aq)