Lecture 1 and 2 of Chapter 18
Lecture 1 and 2 of Chapter 18 CHEM 1312
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This 2 page Class Notes was uploaded by Lydia Notetaker on Sunday April 10, 2016. The Class Notes belongs to CHEM 1312 at University of Texas at Dallas taught by Dr. Nielsen in Spring 2016. Since its upload, it has received 10 views. For similar materials see General Chemistry II in Chemistry at University of Texas at Dallas.
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Date Created: 04/10/16
Chapter 18: Week of April 4th Balancing redox reactions: A redox reaction involves the transfer of electrons from one species to another. This results in a change in oxidation number. Oxidation (reducing agent): is the loss of electrons Reduction(oxidizing agent): is the gain of electrons Balancing redox reactions: Step 1: divide the reaction into two half reactions, and add electrons to each half reaction to balance the charge. Step 2: multiply to get the same number of electrons in each reaction Step 3: cancel the electrons to get the balanced net ionic reaction Balancing redox reactions involving hydrogen and oxygen: you will be told if the reaction occurs under acidic or basic conditions use H2O to balance oxygen use OH to make basic (under basic conditions) Step 1: write out half reaction Step 2: balance the elements on each side of the reaction Step 3: balance the Oxygens and hydrogens on either side Step 4: balance the oxygen using water Step 5: balance the hydrogen using H+ Step 6: balance charge using electrons Step 7: balance electrons in the two half reactions to add them together Step 8: add half reactions to cancel species common to both sides Step 9: check your answer for mass and charge balance Under basic conditions: Step 1: balance the reaction as though it was in an acidic solution Step 2: then add the mount of H+ in reaction to both sides Galvanic cells: Always spontaneous Ecell is always negative Electrons go from anode to cathode (a>c is in alphabetical order so easy to memorize) The reduction occurs at the cathode, and the oxidation occurs at the anode (mnemonic: An OX, and a Red Cat) When two half reactions are connected, he more positive the voltage charge of the half reaction, it becomes the reduction. The other one, goes as an oxidation, and the voltage sign becomes flipped.
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