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Intro to Electrochemistry

by: Phillip Fishbein

Intro to Electrochemistry Chem 1220(Chemistry, Dr. Clark, General Chemistry)

Phillip Fishbein
GPA 3.722

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About this Document

Revisit to redox reactions with more detail.
General Chemistry
Dr. Clark
Class Notes
25 ?




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This 2 page Class Notes was uploaded by Phillip Fishbein on Monday April 11, 2016. The Class Notes belongs to Chem 1220(Chemistry, Dr. Clark, General Chemistry) at 1 MDSS-SGSLM-Langley AFB Advanced Education in General Dentistry 12 Months taught by Dr. Clark in Winter 2016. Since its upload, it has received 10 views. For similar materials see General Chemistry in Chemistry at 1 MDSS-SGSLM-Langley AFB Advanced Education in General Dentistry 12 Months.

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Date Created: 04/11/16
Chapter 20: Electrochemistry  Electrochemistry o Study of the relationships between electricity & chemical reactions  Redox Reactions o Reactions with a change in oxidation of one or more substances o Oxidation  Loss of electrons (more positive oxidation number) o Reduction  Gain of electrons (more negative oxidation number) o Reducing Agent  Leads to reduction  Gets oxidized o Oxidizing Agent  Leads to oxidation  Gets reduced o Assigning Oxidation Numbers  Elements in elemental form have oxidation number of 0  Oxidation number of monatomic ion is its charge  Nonmetals typically have negative oxidation numbers  Fluoride is always -1  Oxygen is usually -2  Metals tend to have positive oxidation numbers  Sum of oxidation numbers of a neutral compound is 0  Sum of oxidation numbers in a polyatomic ion is the charge of the ion. o Balanced Redox Equations  Conservation of mass  Gain and loss of electrons must be balanced  Total charges balance  May include H O2l), H (aq) or OH (aq) as reactants or products o Half-reaction Method  Treat the oxidation and reduction as two separate processes  Assign oxidation numbers  Write half-reactions  Balance the half reactions  Balance all atoms other than H and O  Balance O by adding H O2  Balance H by adding H +  Balance electrons by adding electrons (balance charge)  Balance electrons between two half reactions (multiply half reactions)  Combine them to attain full reaction  Acidic conditions to basic conditions  Proceed normally -  Afterwards, add OH to both sides  Cancel water as applicable o Strengths of Oxidizing and Reducing Agents  Predicting if a redox reaction will take place Fe2+ Cu 2+ Zn 2+ Fe No reaction Reaction No reaction Cu No reaction No reaction No reaction Zn Reaction Reaction No reaction  Summarized in Table of Standard Reduction Potentials  All Reductions  Adding electrons to substance  More positive values on the table will be reduced by those below  Highest on table is strongest oxidizing agent  Lowest on table is strongest reducing agent


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