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Chem 113 Weel 14

by: Caroline Hurlbut

Chem 113 Weel 14 Chem 113

Caroline Hurlbut
GPA 3.7

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About this Document

Introduction to electrochemistry, including rules for finding oxidation states and steps of the half reaction method to balancing redox reactions.
General Chemistry II
Ingrid Marie Laughman
Class Notes
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This 1 page Class Notes was uploaded by Caroline Hurlbut on Friday April 29, 2016. The Class Notes belongs to Chem 113 at Colorado State University taught by Ingrid Marie Laughman in Spring 2016. Since its upload, it has received 13 views. For similar materials see General Chemistry II in Chemistry at Colorado State University.


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Date Created: 04/29/16
Intro to Electrochemistry • reduction - gain of electrons • oxidation - loss of electrons • oxidizing agent - reactant that does the oxidizing (being reduced) • reducing agent - reactant that does the reducing (being oxidized) • oxidation numbers/states - number of electrons a component has vs how many it would have as a free atom • rules for oxidation states —oxidation states of pure elements = 0 —oxidation state of single ion = charge of ion —oxidation state of hydrogen = +1 —oxidation state of fluorine = -1 —oxidation state of oxygen = -2 except when bonded with F or another O atom —ex. oxidation state of P in PO4 3-: -3 = x + 4(-2)—>x = +5 half reaction method for balancing redox reactions • —identify what is being oxidized/reduced A. use oxidation states —balance each half reaction A. balance elements other than H and O B. balance O atoms by adding H2O C. balance H atoms by adding H+ D. if in basic solution, add OH- to both sides so all H+ becomes H2O E. balance charge by adding electrons —add up half reactions A. need same # of electrons in each half reaction B. add reactions C. check that elements and charge balance • ex. Cu+(aq) + Fe(s) →Fe 3+(aq) + Cu(s) Step 1: Cu from +1 to 0—> reduced Fe from +3 to 0—>oxidized Step 2: Cu+ + e-→Cu Fe→Fe 3+ + 3e- Step 3: 3Cu+ + 3e-→3Cu Fe→Fe 3+ + 3e- 3Cu+ + Fe→3Cu + Fe 3+ elements balance ✓ charge balances ✓


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