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Lecture 1 and 2 of Chapter 18

by: Lydia Notetaker

Lecture 1 and 2 of Chapter 18 CHEM 1312

Marketplace > University of Texas at Dallas > Chemistry > CHEM 1312 > Lecture 1 and 2 of Chapter 18
Lydia Notetaker
GPA 4.0

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These are the first topics we have reviewed regarding Chapter 18.
General Chemistry II
Dr. Nielsen
Class Notes
Chemistry II
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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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