ELECTROCHEMISTRY CHAPTER 20. 20.1 These types of reactions involving the transfer of electrons also have changes in energy, but instead of heat it is.

Slides:

Advertisements

Similar presentations

Topic: Electrochemical Cells Do Now: 5 color pencils.

Advertisements

Aim: How do chemists use redox reactions to produce electricity? 1.How are oxidation numbers assigned? 2.How to determine if a particle is oxidized or.

DO NOW: Questions in M.C. packet. 1. An oxidation-reduction reaction involves the transfer of electrons 2. Reduction is the gain of electrons and decrease.

Electrochemical Cells

Regents Warm-Up Given the balanced equation representing a reaction: Cl 2 (g) →  Cl(g) + Cl(g) What occurs during this change? (1) Energy is absorbed.

Chapter 20 Preview Multiple Choice Short Answer Extended Response

CHAPTER 20.2 Electrochemistry. Review For the following reaction, determine which is being oxidized, which is being reduced, draw the voltaic cell, and.

Oxidation- Reduction Ms. Randall. Lesson 2: Recognizing Oxidation-Reduction Reactions Objective: To identify redox reactions based on the changes of oxidation.

Aim: What are electrochemical cells?

Chapter 18 Oxidation-Reduction Reactions & Electrochemistry.

Section 18.1 Electron Transfer Reactions 1.To learn about metal-nonmetal oxidation–reduction reactions 2.To learn to assign oxidation states Objectives.

Electrochemistry Chapter 21. Electrochemistry and Redox Oxidation-reduction:“Redox” Electrochemistry: study of the interchange between chemical change.

Electrochemistry AP Chapter 20. Electrochemistry Electrochemistry relates electricity and chemical reactions. It involves oxidation-reduction reactions.

Chapter 22 REDOX.

Electrochemistry. Electrochemical Cells  Electrons are transferred between the particles being oxidized and reduced  Two types –Spontaneous = Voltaic.

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

Electrochemistry.

Chapter 21.  Two types: ◦ Voltaic cell: electrons flow spontaneously ◦ Electrolytic cell: electrons are forced to flow.

CHM 112 Summer 2007 M. Prushan Chapter 18 Electrochemistry.

Electrochemistry. Terminology You may have noticed oxygen never gets oxidized, it always gets reduced. The reason for this is because oxygen is an oxidizing.

Electrochemistry or REDOX Unit 9. I. The Vocabulary of Electrochemistry A] Electrochemsitry is…… The field of chemistry studying reactions resulting from.

Electrochemical Cells - producing an electric current with a redox reaction.

Chapter 18 Notes1 Chapter 18 Electrochemistry 1. review of terms; balancing redox equations 2. galvanic cell notation, relationships 3. standard reduction.

 Learners must be able to define galvanic cell in terms of electrode reaction. e.g. salt bridge.(N.B. anode and cathode)  Learners must be able to do.

Electrochemistry - Section 1 Voltaic Cells

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 ZnSO4(aq) CuSO4(aq) Cu Zn Zn

Chapter 18: Introduction to Electrochemistry CHE 321: Quantitative Chemical Analysis Dr. Jerome Williams, Ph.D. Saint Leo University.

Chapter 20 Electrochemistry West Valley High School General Chemistry Mr. Mata.

Electrochemistry Ch.19 & 20 Using chemical reactions to produce electricity.

Batteries Electrochemical cells  Terms to know Anode Cathode Oxidation Reduction Salt Bridge Half cell Cell potential Electron flow Voltage.

Electrochemistry. Electrochemistry is the study of the relationship between the flow of electric current and chemical changes, including the conversion.

Electrochemical cells - batteries

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

Chem Catalyst Determine what is being oxidized and what is being reduced in the following reaction: CuO + H 2  Cu + H 2 O.

Electrochemical Reactions. Anode: Electrons are lost due to oxidation. (negative electrode) Cathode: Electrons are gained due to reduction. (positive.

ELECTROCHEMICAL CELLS. ELECTROCHEMISTRY The reason Redox reactions are so important is because they involve an exchange of electrons If we can find a.

2 Types of Electrochemical Cells 1)Voltaic Cells  Spontaneous reaction  Reaction itself creates electric current  Main concept for batteries 2)Electrolytic.

Electrolytic Cells Chemistry Chapter 19 E.

Electrochemistry Ch. 18 Electrochemistry 18.1 Voltaic Cells.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Electrochemistry The study of the interchange of chemical and electrical energy.

Electrochemistry Introduction Voltaic Cells. Electrochemical Cell  Electrochemical device with 2 half-cells with electrodes and solutions  Electrode—metal.

ELECTROCHEMISTRY Electrochemistry relates electricity and chemical reactions. It involves oxidation-reduction reactions (aka – redox) They are identified.

Electrochemical Reactions. Anode: Electrons are lost due to oxidation. (negative electrode) Cathode: Electrons are gained due to reduction. (positive.

Redox 21-3 Electrochemistry. 1.) Electrochemical Cells A.) Also called Galvanic Cells B.) Conservation of mass, charge and energy C.) Changes Chemical.

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

mr4iE. batteries containers of chemicals waiting to be converted to electricity the chemical reaction does not.

Electrochemistry Chapter 18. Electrochemistry –the branch of chemistry that studies the electricity- related application of oxidation-reduction reactions.

Electro-chemistry: Batteries and plating Electrochemistry: The study of the interchange of chemical and electrical energy Oxidation is the loss of electrons.

Electrochemistry. To obtain a useful current, we separate the oxidation and reduction half-reactions so that electron transfer occurs thru an external.

General Chemistry Unit 14. A. Involves electron changes (can tell by change in charge) Cl NaBr 2NaCl + Br 2 B. Oxidation 1. First.

ELECTROCHEMISTRY is the branch of chemistry which deals with…

ELECTROCHEMISTRY Voltaic and Electrolytic Cells

Oxidation-Reduction Reactions

17.1 Galvanic Cells (Batteries)

14.6 Electrochemistry Unit Review

10.2 Electrochemistry Objectives S2

Unit 8: Electrochemistry Applications

Electrochemistry.

Electrochemistry.

An electrolytic cell uses electricity to do a chemical reaction.

Electrochemistry i.e. This is the End!.

Introduction to Electrochemistry

Electrochemistry AP Chapter 20.

Redox & Electrochemistry

Chapter 21: Electrochemistry

Galvanic Cells Assignment # 17.1.

Chapter 15 Notes Oxidation number - number of electrons an element wants to gain or lose to become stable. Determining oxidation number: Ex. CaSO4 CCl4.

A. Oxidation-Reduction Reactions

Presentation transcript:

ELECTROCHEMISTRY CHAPTER 20

20.1 These types of reactions involving the transfer of electrons also have changes in energy, but instead of heat it is electrical energy. The study of these types of reactions is called electrochemistry.

20.1 Electrons can be transferred through wires or through aqueous solutions. As long as there is a continuous connection, the electrons always flow in the same direction.

20.1 Electrons can be transferred through wires or through aqueous solutions. As long as there is a continuous connection, the electrons always flow in the same direction. A salt bridge allows the electrons to flow from one solution to another.

20.1 The anode is where oxidation occurs electrons are lost to something electrons away The cathode is where reduction occurs electrons are gained by something electrons come

20.1 How about a typical battery you would use?

20.1 How about a typical battery you would use?

20.1 How about a car battery?

20.1 How about a car battery?

20.1 How about a fuel cell?

20.1 How about a fuel cell?

20.1 How about a fuel cell?

20.1 How about a solar cell?

20.1 How about a solar cell?

20.1 How about a solar cell?

CHAPTERS 19 AND 20 TEST NOTES 15 multiple choice (4 points each) 10 short answer (2 points each) 4 short answer (5 points each) 1 extra credit (5 points)

CHAPTERS 19 AND 20 TEST NOTES Oxidation / reduction OILRIG or LEO the lion goes GER Assigning oxidation numbers Writing half-reactions Electrochemical cells Electrodes - anode vs cathode Movement of electrons Movement of ions through salt bridge