Electrochemistry Chapter 17 “Leo” the lion says “ger” §LEO - Lose Electrons = Oxidation GER - Gain Electrons = Reduction §What are the half reactions.

Slides:

Advertisements

Similar presentations

Inorganic chemistry Assiastance Lecturer Amjad Ahmed Jumaa  Calculating the standard (emf) of an electrochemical cell.  Spontaneity.

Advertisements

Oxidation Reduction Regents Review.

Lecture 12: Cell Potentials Reading: Zumdahl 11.2 Outline –What is a cell potential? –SHE, the electrochemical zero. –Using standard reduction potentials.

Slide 1 of 54 CHEMISTRY Ninth Edition GENERAL Principles and Modern Applications Petrucci Harwood Herring Madura Chapter 20: Electrochemistry.

Galvanic Cells What will happen if a piece of Zn metal is immersed in a CuSO 4 solution? A spontaneous redox reaction occurs: Zn (s) + Cu 2 + (aq) Zn 2.

19.2 Galvanic Cells 19.3 Standard Reduction Potentials 19.4 Spontaneity of Redox Reactions 19.5 The Effect of Concentration on Emf 19.8 Electrolysis Chapter.

Electrochemical Cells (aka – Galvanic or Voltaic Cells) AP Chemistry Unit 10 Electrochemistry Chapter 17.

Prentice Hall © 2003Chapter 20 Zn added to HCl yields the spontaneous reaction Zn(s) + 2H + (aq)  Zn 2+ (aq) + H 2 (g). The oxidation number of Zn has.

Lecture 11: Cell Potentials Reading: Zumdahl 11.2 Outline –What is a cell potential? –SHE, the electrochemical zero. –Using standard reduction potentials.

Chapter 20 Electrochemistry

Lecture 11: Electrochemistry Introduction

Lecture 10: Electrochemistry Introduction Reading: Zumdahl 4.10, 4.11, 11.1 Outline –General Nomenclature –Balancing Redox Reactions (1/2 cell method)

Oxidation and Reduction. Oxidation The chemical process by which an element or compound gains oxygen. Example: 2Mg(s) + O 2  2MgO Example: 2Mg(s) + O.

Electrochemistry. 17.1/17.2 GALVANIC CELLS AND STANDARD REDUCTION POTENTIALS Day 1.

Lecture 9. Chemistry of Oxidation-Reduction Processes Prepared by PhD Halina Falfushynska.

Electrochemistry Chapter 17.

Warmup Assign oxidation numbers to each element: NaNaClCl 2 H 2 O Ca(OH) 2 NO 3 -

Chapter 20 – Redox Reactions One of the earliest recognized chemical reactions were with oxygen. Some substances would combine with oxygen, and some would.

Chemistry 100 – Chapter 20 Electrochemistry. Voltaic Cells.

Redox Half Reactions What is the purpose of creating a half reaction? How to balance a half reaction?

Electrochemistry Experiment 12. Oxidation – Reduction Reactions Consider the reaction of Copper wire and AgNO 3 (aq) AgNO 3 (aq) Ag(s) Cu(s)

Standard Reduction Potentials Electrochem III. Balancing Oxidation-Reduction Equations Perhaps the easiest way to balance the equation of an oxidation-

Electrochemistry Applications of Redox. Review l Oxidation reduction reactions involve a transfer of electrons. l OIL- RIG l Oxidation Involves Loss l.

CHEM Pharmacy Week 9: Galvanic Cells Dr. Siegbert Schmid School of Chemistry, Rm 223 Phone:

Electrochemistry and Redox Reactions. 2Mg (s) + O 2 (g) 2MgO (s) 2Mg 2Mg e - O 2 + 4e - 2O 2- Oxidation half-reaction (lose e - ) Reduction half-reaction.

Activity Series lithiumpotassiummagnesiumaluminumzincironnickelleadHYDROGENcoppersilverplatinumgold Oxidizes easily Reduces easily Less active More active.

Electrochemistry Chapter 20 Brown-LeMay. Review of Redox Reactions Oxidation - refers to the loss of electrons by a molecule, atom or ion - LEO goes Reduction.

Electrochemistry Applications of Redox. Review l Oxidation reduction reactions involve a transfer of electrons. l OIL- RIG l Oxidation Involves Loss l.

CHM 112 Summer 2007 M. Prushan Chapter 18 Electrochemistry.

Standard Voltages Reading: Masterson 18.2 Outline –What is a standard voltage (cell potential) –SHE, the electrochemical zero. –Using standard reduction.

Tro IC.3 1.The loss of protons 2.The gain of oxygen atoms 3.The loss of hydrogen atoms 4.The gain of electrons 5.Two of the above 16.1 Which statement.

CONTENT OBJECTIVE make qualitative or quantitative predictions about galvanic (voltaic) cells based on half-cell reactions and potentials and analyze these.

Studio 13b: Activity Series. Redox Reactions 2 Fe (s) + 3 Cl 2(g)  2 FeCl 3(s) Fe 0  Fe +3 Cl 0  Cl - A species is said to undergo REDUCTION if it.

a.k.a Electrochemistry a.k.a. Oxidation-Reduction Redox!

Topic: Redox Aim: What are electrochemical cells? Do Now: Which of the following ions is most easily reduced? 1)Li+ 2) K+ 3) Ca 2+ 4) Na+ HW:

Electrochemistry Electrolysis.

Electrochemistry Chapter 5. 2Mg (s) + O 2 (g) 2MgO (s) 2Mg 2Mg e - O 2 + 4e - 2O 2- Oxidation half-reaction (lose e - ) Reduction half-reaction.

Galvanic Cell: Electrochemical cell in which chemical reactions are used to create spontaneous current (electron) flow.

Electrochemistry Chapter 19 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

Redox reactions half-reactions: Reduction 2Fe e -  2Fe 2+ oxidation Sn 2+  Sn e - 2Fe 3+ + Sn 2+  2Fe 2+ + Sn http:\asadipour.kmu.ac.ir.

Electrochemistry.  involves oxidation reduction reactions that can be brought about by electricity or used to produce electricity  it is concerned with.

Nernst Equation Walther Nernst

Chapter 19 Redox Reactions. Oxidation Numbers Rules Uncombined element = 0 Monatomic ion = charge on ion (from location of periodic table) 2 element compound.

Redox Reactions: HALF REACTIONS

Chapter 19 Redox Reactions.

Chapter 20: Electrochemistry Chemistry 1062: Principles of Chemistry II Andy Aspaas, Instructor.

Oxidation/Reduction Reactions

Galvanic Cells ELECTROCHEMISTRY/CHEMICAL REACTIONS SCH4C/SCH3U.

Chapter 19 Last Unit Electrochemistry: Voltaic Cells and Reduction Potentials.

Electrochemistry Measurement of Electrode Potential Electrode Potential of Galvanic Cell The galvanic cell has two electrode potentials; anode potential.

REDOX AND ELECTROCHEMISTRY SUROVIEC SPRING 2015 Chapter 18.

 Anything that uses batteries: › Cell phones › Game boys › Flash lights › Cars  Jewelry—electroplating.

Balancing Redox Equations – Voltaic (Galvanic) Cells.

CE Chemistry Module 8. A. Involves electron changes (can tell by change in charge) Cl NaBr 2NaCl + Br 2 B. Oxidation 1. First used.

Electrochemistry Chapter 20. oxidation: lose e- -increase oxidation number reduction: gain e- -reduces oxidation number LEO goes GER Oxidation-Reduction.

Chapter 18 Electrochemistry Lesson 1. Electrochemistry 18.1Balancing Oxidation–Reduction Reactions 18.2 Galvanic Cells 18.3 Standard Reduction Potentials.

Warm up 3/17/15 Balance the half reaction. Ch. 17 Electrochemistry.

Electrochemistry. #13 Electrochemistry and the Nernst Equation Goals: To determine reduction potentials of metals To measure the effect of concentration.

ELECTROCHEMISTRY Presentation by: P.K. CHOURASIA K.V MANDLA, Jabalpur Region.

Unit 5: Electrochemistry An AWESOME presentation by Dana and Brendan.

a.k.a. Oxidation-Reduction

Electrochemistry.

Electrochemistry Ch 13 pg 225 Princeton Review.

Chapter 19 Electrochemistry Semester 1/2009 Ref: 19.2 Galvanic Cells

Chp 17 Electrochemistry.

Harnessing the changes in oxidation and reduction

Electrochemistry.

Unit 13: Electrochemistry

Electrochemistry Chapter 20.

Electrochemistry Kenneth E. Schnobrich.

Presentation transcript:

Electrochemistry Chapter 17

“Leo” the lion says “ger” §LEO - Lose Electrons = Oxidation GER - Gain Electrons = Reduction §What are the half reactions of l Mg(s) + 2H + (aq)  Mg 2+ (aq) + H 2 (g) ? § Mg(s)  Mg 2+ (aq) + 2e - l 2H + (aq) + 2e -  H 2 (g)

Galvanic Cell §Which is the oxidation and which is the reduction? Mg(s)  Mg 2+ (aq) + 2e - 2H + (aq) + 2e -  H 2 (g) leOgeR

Galvanic Cell §Electrons flow from the anode to the cathodes Mg(s)  Mg 2+ (aq) + 2e - 2H + (aq) + 2e -  H 2 (g) cathodeanode What’s this?

Electromotive Force ( E º) §…is the combination (sum) of the potentials of two half reactions. §Reactions are listed on tables (17.1 pg 833) as reductions.  Galvanic cells require E º cell > 0. §One of the tabulated red. potentials will have to be reversed. §Sum of the redox half reactions must be > 0.

Electromotive Force (cont)  When you reverse the reaction E º gets the opposite sign.  When you multiply a reaction by a coefficient E º is NOT changed.

Practice §Which of these is galvanic? §. Mg(s) + 2H + (aq)  Mg 2+ (aq) + H 2 (g) Cu 2+ (aq) + 2Ag(s)  2Ag + (aq) + Cu(s) 2Zn 2+ (aq) + 4OH - (aq)  2 H 2 O(l) + O 2 (g) + 2Zn(s) §+2.37V, yes §-0.46V, no §-1.16V,no The more positive the E value, the more likely the species is to be reduced. (It’s a stronger oxidizing agent).