Chapter 19 Oxidation-Reduction Reactions Pg. 595 Oxidation- valence electrons are lost Reduction- valence electrons are gained Rules for determining the.

Slides:

Advertisements

Similar presentations

Finish up redox Demo voltaic cell, then how does a re-charging battery work? Celebrate redox with nuclear chem soon enough Draw the standard 2 beaker voltaic.

Advertisements

Chapter 20 Electrochemistry

Electricity from Chemical Reactions

Created by C. Ippolito March 2007 Updated March 2007 Chapter 22 Electrochemistry Objectives: 1.describe how an electrolytic cell works 2.describe how galvanic.

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.

Oxidation-Reduction Reactions

Oxidation-Reduction Reactions LEO SAYS GER. Oxidation and Reduction (Redox)  Electrons are transferred  Spontaneous redox rxns can transfer energy 

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

Chapter 18 Oxidation-Reduction Reactions & Electrochemistry.

Chapter 18 Oxidation–Reduction Reactions and Electrochemistry.

Solutions of Electrolytes

ELECTROCHEMISTRY REDOX REVISITED! 24-Nov-97Electrochemistry (Ch. 21) & Phosphorus and Sulfur (ch 22)1.

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

Oxidation-Reduction Reactions REDOX Reactions. Oxidation State Oxidation numbers are very similar to charge. There are some different rules for assigning.

Aim Redox 1 – Why is redox so important in your life?

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

Oxidation-Reduction Reactions (Redox Reactions) Notes (Chapter 19)

Electrochemistry is the chemistry of reactions which involve electron transfer. In spontaneous reactions electrons are released with energy which can.

Oxidation and Reduction Reactions that involve electron transfer Batteries and chemistry.

Oxidation-Reduction Reactions

Chapter 22 REDOX.

ELECTROCHEMISTRY To play the movies and simulations included, view the presentation in Slide Show Mode.

Oxidation-Reduction Reactions LEO SAYS GER. Oxidation and Reduction (Redox) Electrons are transferred Spontaneous redox rxns can transfer energy Electrons.

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

Chapter 20: Electrochemistry

 17.1 Explain how a non-spontaneous redox reaction can be driven forward during electrolysis  17.1 Relate the movement of charge through an electrolytic.

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

Section 10.3—Batteries & Redox Reactions

CHEM 163 Chapter 21 Spring minute review What is a redox reaction? 2.

1 Electron Transfer Reactions: CH 19: Oxidation-reduction or redox reactions. Results in generation of an electric current (electricity) or caused by.

1 Oxidation-Reduction AKA Redox OB: Pages

17-Nov-97Electrochemistry (Ch. 21)1 ELECTROCHEMISTRY Chapter 21 Electric automobile redox reactions electrochemical cells electrode processes construction.

Electrochemistry. Electron Transfer Reactions Electron transfer reactions are oxidation- reduction or redox reactions. Electron transfer reactions are.

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

Unit 11 Electrochemistry. What is electrochemistry? The study of the relationship between chemical change and electrical work. ◦ Investigated using redox.

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.

Unit 16 Electrochemistry Oxidation & Reduction. Oxidation verses Reduction Gain oxygen atoms 2 Mg + O 2  2 MgO Lose electrons (e - ) Mg (s)  Mg + 2.

Section 1 Introduction to Electrochemistry

Chemistry Chapter 19 D.  Defined: branch of chemistry that deals with electricity-related redox reactions  Electrochemical cell: ◦ System of electrodes.

Oxidation Reduction.

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

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

OXIDATION ANY REACTION IN WHICH A SUBSTANCE LOSES ELECTRONS

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

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

CHAPTER 17 ELECTROCHEMISTRY. Oxidation and Reduction (Redox) Electrons are transferred Spontaneous redox rxns can transfer energy Electrons (electricity)

Oxidation and Reduction Reactions Chapters 20 and 21.

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

Chemistry 1 Chapter 22 &23 Oxidation Reduction Reactions The Students will be able to describe redox reactions and assign oxidation numbers to chemical.

Assigning Oxidation Numbers RULESExamples 2Na + Cl 2  2NaCl Na = 0 or written Na 0 Cl 2 = 0 or written Cl 2 0 RULESExamples 1. Each Uncombined Element.

Science Starter 1.Oxidation is when you _______ electrons. 2.Reduction is when you _______ electrons. 3.Together, these are know as a _________ reaction.

a.k.a. Oxidation-Reduction

Oxidation-Reduction Reactions

Electrochemistry RedOx: Part Deux.

Chapter 21: Electrochemistry

Batteries and Galvanic Cells

Chp 17 Electrochemistry.

Electrochemistry RedOx: Part Deux.

Electrochemistry.

Electrochemistry.

Batteries and Galvanic Cells

Electrochemistry Chapter 17.

ELECTROCHEMISTRY Chapter 18

Electrochemistry AP Chapter 20.

Redox & Electrochemistry

A. Oxidation-Reduction Reactions

What is a redox reaction?

Presentation transcript:

Chapter 19 Oxidation-Reduction Reactions Pg. 595 Oxidation- valence electrons are lost Reduction- valence electrons are gained Rules for determining the oxidation number of an element (pg. 595) Practice assigning Oxidation numbers (pg. 612 #7 a-j) (pg.612 #6)

Oxidation-Reduction Reaction Also called-Redox Transfer of electrons One cannot happen without the other. O xidation R eduction I s I s L osing G aining Oxidation #increases Oxidation # decreases

Remember:Oil Rig Determine Oxidation or Reduction (pg. 612 #4) Pg. 599 #3 a. is an example. Try b-e on your own for practice. Practice Pg. 605 #1 Pg. 612 #2 a-i,3,5 a-c,17 a-e,18

Hon Chem Ch 20 Pg 655 Electrochemical Cells AKA batteries Pg 643 Zn is good reducing agent (gets oxidized, loses electrons, ox# goes up) Cu is good oxidizing agent (gets reduced, gains electrons, ox# goes down)

Parts and Types of Batteries Pg Zinc-Carbon Dry Cell a. big, used in flashlights, C and D batteries b. Zn container – anode, negative, becomes + as loses electron c. C rod in center – cathode, + bump on end of battery, becomes negative as gains electrons

2. Alkaline Batteries a. smaller, AA and AAA, cameras, remotes b. Zn and KOH instead of Zn and C 3.Hg Batteries a. tiny, hearing aids, watches b. Zn, KOH, Steel, HgO

Corrosion and Prevention Pg Fe is oxidized, loses electrons, forms rust Salt and acid speed up the oxidation Zn coating prevents oxidation due to Pg 643, called galvanizing Electric potential difference = volts (how hard electricity pushes thru wire)

Recharging Batteries Pg Voltaic cell – battery making electricity, anode gives electrons to cathode Electrolytic cell – battery when being recharged, storing electricity, direct current source forces cathode to give electrons back to anode DC sources - wall charger with diode to change AC to DC, car alternator, other battery (jumping a car) Can be recharged as long as enough products to act as reactants to reverse reaction, corrosion is loss of products/reactants so can’t recharge after corroded Pg 669**do redox rxn for car battery