Ppt on oxidation and reduction reactions

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

Electrochemistry  involves oxidation reduction reactions that can be brought about by electricity or used to produce electricity  it is concerned with the conversion of chemical energy to electrical energy, and vise versa An electrochemical cell is a system which produces electrical energy. Electrochemistry in Everyday Life  The rusting of iron, the photosynthesis that takes place in the leaves of green plants, and the conversion of foods/


Common Types of Chemical Reactions. Decomposition.

Single Displacement Combustion OxidationReduction Reactions A chemical reaction in which an atom or ion loses electrons to another atom or ion. Fe (s) + Al(NO 3 ) 3 (aq)  Fe(NO 3 ) 3 (aq) + Al (s) charges 003+ Fe: 0  +3 Oxidation Al: +3  0 Reduction Electrons Lost 3 Gained 3 “Redox” Reactions Leo the Lion says, “Ger” OSEOSE LECTRONLECTRON XIDATIONXIDATION AINAIN LECTRONLECTRON EDUCTIONEDUCTION Oxidation numbers (oxidation state) are/


Monday, April 14, 2008 1.Chapter 17 Quiz 2. Notes Section 18.1 – Oxidation-Reduction 3. Homework – Reading Analysis – Section 18.1.

Oxidation-Reduction Reactions Reactions in which one or more electrons are transferred Reactions in which one or more electrons are transferred Also called Redox reactions Also called Redox reactions Oxidation is defined as the loss of electrons Oxidation is defined as the loss of electrons Reduction is defined as the gain of electrons Reduction is defined as the gain of electrons Oxidation / Reduction OIL RIG – Oxid/ and Mg gain them to become Mg? –Which metal wants to get rid of e- more? Will a Reaction /


Electrochemistry Lesson 1 Introduction. Electrochemistry Is the study of reactions that gain or lose electrons.

Electrochemistry Lesson 1 Introduction Electrochemistry Is the study of reactions that gain or lose electrons. Electrochemistry Is the study of reactions that gain or lose electrons. In this unit we will study: Battery Reactions- oxidation and reduction Corrosion- oxidation Preventing Corrosion Oxidation Electroplating- reduction Refining Metals- reduction Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons metalion Balance charge Add/


OxidationReduction Mr. Chan Northwestern University To insert your company logo on this slid From the Insert Menu Select “Picture” Locate your logo.

key before using the resize handles, you will maintain the proportions of the object you wish to resize. Defining Redox Oxidation - reduction  Originally combining with oxygen  Reduction – originally meant loss of oxygen Oxidation – loss of electrons Reduction – gain of electrons  OILRIG Oxidizing and Reducing Agents  Red. Agent – loses electrons, gets oxidized  Ox. Agent – gains electrons, gets reduced Practice 1-2 Corrosion – some metals corrode faster than others Determining/


1 4.9 Oxidation-Reduction Reactions lRedox reactions- reactions in which one or more electrons is transferred.

1 4.9 Oxidation-Reduction Reactions lRedox reactions- reactions in which one or more electrons is transferred 2 4.9 Oxidation-Reduction Reactions Oxidation and Reduction lWhen a metal undergoes corrosion it loses electrons to form cations: Ca(s) +2H + (aq)  Ca 2 + (aq) + H 2 (g) lOxidized: atom, molecule, or ion becomes more positively charged. /


RedOx Chapter 18. Oxidation- Reduction Reactions Redox or oxidation-reduction reactions are reactions that involve a transfer of electrons. Oxidation.

must have lost 2 electrons 2 Na → 2Na + + 2 e - And Hydrogen gained two electrons 2 H 2 O +2 e - → 2 OH - + H 2 Sodium is oxidized, hydrogen is reduced in this reaction Oxidation is an increase in oxidation state Reduction is a decrease in oxidation state Balancing Redox Equations by Half Reactions Method Balancing Equations Redox reactions don’t follow normal rules for balancing equations because we/


Oxidation-Reduction Reactions “Redox”

Reducing Agents and Oxidizing Agents The substance reduced is the oxidizing agent The substance oxidized is the reducing agent Sodium is oxidized – it is the reducing agent Chlorine is reduced – it is the oxidizing agent Trends in Oxidation and Reduction Active metals: Lose electrons easily Are easily oxidized Are strong reducing agents Active nonmetals: Gain electrons easily Are easily reduced Are strong oxidizing agents Redox Reaction Prediction #1 Important Oxidizers Formed in reaction MnO4/


Electro Chemistry Unit 5 Chemistry 12.

+ ions Base donates OH- ions Bronstead-Lowery : Acid proton donor Base proton accepter Lewis : Acid is an electron pair accepter Base an electron pair donor Electro Chemical Reactions 2 types (oxidation and reduction) Oxidation 1/2 reaction in which the reacting species looses an electro Reduction 1/2 reaction in which the reacting species gains an electron Memory Trick “LEO the lion says GER” LEO: loss of electrons/


Chapter 20. Calculating Oxidation Numbers Each oxide ion has a charge of -2 7 oxide ions have a subtotal charge of -2 x 7 = -14 Since the formula has.

= +7 This compound is manganese(VII) oxide Work oxidation numbers of Cr and S in Cr 2 (SO 4 ) 3 (Hint: treat SO 4 2- as a single particle) Oxidation -Reduction Reactions I Play Video On YouTube Oxidation - Reduction Reactions II Play Video On YouTube Common Oxidation States Play Video On YouTube Cu 2+ + Fe 0 Redox Reaction Play Video In YouTube CuO + C Redox Reaction Play Video On YouTube Mercury (II/


Energy. Laws of Thermodynamics Flow of Energy in Living Things –Oxidation & Reduction Free Energy: Endergonic & Exergonic Rxs. Activation Energy Enzymes.

Things Oxidation - Reduction Oxidation atom/molecule loses an electron. Reduction atom or molecule gains an electron. Redox reactions - electron lost must be gained Fig. 8.4 (TEArt) Gain of electron  reduction Low energy e–e– AB High energy Loss of electron (oxidation)/GlucoseFructose Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Enzyme Structure and Function What do enzymes do? Bring molecules together Orients molecules in correct position Strains (bends) /


Electrochemistry. It deals with reactions involving a transfer of electrons: 1. Oxidation-reduction phenomena 2. Voltaic or galvanic cell Chemical reactions.

to produce eletrical energy: 3.Electrolytic cells Electrical energy can be used to bring about chemical transformations:electrolysis Oxidation and reduction Zn (s) + Cu 2+ (aq)  Zn 2+ (aq) + Cu (s) Zn (s)  Zn 2+ (aq) + 2e - Oxidation half-reaction Cu 2+ (aq) + 2e -  Cu (s) Reduction half-reaction Galvanic /voltaic/ cells Electrode: e.g. a metal strip which can funcion as a cathode or an anode/


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.

the electrode platinum foil Galvanic Cells Zn (s) + 2 H + (aq) Zn 2+ (aq) + H 2 (g) Oxidation half-reaction: Zn (s) Zn 2+ (aq) + 2 e - Reduction half-reaction: 2 H + (aq) + 2 e - H 2 (g) In this case a standard hydrogen electrode is used as the cathode/ reduction half- reactions, identify the metal at the anode, the balanced reaction for the galvanic cell, and the E o cell. Al 3+ (aq) + 3 e - Al (s) E o red = -1.66 V Fe 2+ (aq) + 2 e - Fe (s) E o red = -0.440 V Galvanic Cells Oxidizing Agent (oxidant):/


Selective Oxidation of hydrocarbons Part-1 Dr.K.R.Krishnamurthy National Centre for Catalysis Research (NCCR) Indian Institute of Technology Chennai-600036INDIA.

/Ammoxidation of Propylene Proceed through Mars- Krevelen mechanism Cyclic reduction- re-oxidation of the catalyst Catalyst systems contain binary/multi compoent metal oxides Bismuth molybdates ( α-β-γ- phases ) most active & selective Facile reduction- re-oxidation capability Hydrocarbon gets activated and not oxygen Redox Cycle for the catalyst Surface reactions in selective oxidation/ Ammoxidation of propylene Mechanism of Oxidation/Ammoxidation of Propylene Experiments labeled with 14 C Labeling in/


Balancing Oxidation- Reduction Reactions Any reaction involving the transfer of electrons is an oxidation-reduction (or redox) reaction.

- + C 2 O 4 2-  Cr 3+ + CO 2 2[Cr +6 + 3e -  Cr +3 ] 2[C +3  C +4 + 1e - ] Balancing Oxidation-Reduction Reactions: Balancing Oxidation-Reduction Reactions: 3. Take into account any subscripts in the formulas of reactants and products, and multiply the half reactions accordingly. Cr 2 O 7 2- + C 2 O 4 2-  Cr 3+ + CO 2 2Cr +6 + 6e -  2 Cr +3 2C/


Oxidation-Reduction Reactions

Oxidation-Reduction Reactions (Redox Reactions) Oxidationreduction reactions (REDOX) - The chemical changes that occur when electrons are transferred between reactants. Assigning Oxidation Numbers Ox# of element is zero. Sum of ox#’s is zero. If covalent, more EN element is negative. Oxygen is usually a -2, except peroxides where it is -1 or when it is electropositive and a +2 Ex: Fe0 Cu0 O20 Ex: CaBr2 +2 -1(2) = 0/


Lecture 11: Electrochemistry Introduction

: electrons are neither created or destroyed during a redox reaction. They are transferred from the species being oxidized to that being reduced. Example Identify the species being oxidized and reduced in the following (unbalanced) reactions: ClO3- + I- I2 + Cl- reduction +5 -1 0 -1 oxidation NO3- + Sb Sb4O6 + NO reduction +5 0 +3 +2 oxidation Balancing Redox Reactions One method of half reactions Key idea….make sure e- are neither created/


CHE-300Review nomenclature syntheses reactions mechanisms.

Syntheses 1. reduction of alkene (addition of hydrogen) 2. reduction of an alkyl halide a) hydrolysis of a Grignard reagent b) with an active metal and acid 3. Corey-House Synthesis Reactions 1. halogenation 2. combustion (oxidation) 3. pyrolysis/alkyl halide 2. dehydration of an alcohol 3. dehalogenation of a vicinal dihalide 4. reduction of an alkyne reactions 1. addition of hydrogen10. hydroboration-oxidation 2. addition of halogens11. addition of free radicals 3. addition of hydrogen halides12. /


Dry cells. Simple chemical cell Zinc Simple chemical cell Overall equation (Redox reaction): Zn(s) + CuSO 4 (aq)  ZnSO 4 (aq) + Cu(s) Ionic equation:

short. There is a slow direct reaction between the zinc electrode and ammonium ions. After some time, the zinc case becomes thinner and the paste leaks out. The leakage problem can be solved by enclosing the whole cell in a steel or plastic case. Alkaline manganese cell Anode (oxidation / -ve electrode): zinc powder Cathode (reduction / +ve electrode): manganese(IV) oxide Electrolyte: potassium hydroxide Alkaline manganese cell/


OXIDATION- REDUCTION REACTION REVIEW. Oxidation-Reduction (“Redox”) Reactions Most common reaction Process often written as two “half-reactions”—separating.

of electrons in element Compound becomes more NEGATIVE DECREASE in oxidation number 2) Oxidation LOSS of electrons Compound becomes more POSITIVE INCREASE in oxidation number Oxidation and Reduction MUST happen together—can’t have one without the other. electrons gained = electrons lost Example 1: 2Na + Cl 2  2Na + Cl - Practice Which equations are reduction half-reactions and which are oxidation half-reactions. 1) Zn +2 + 2e -  Zn 2) Ag  Ag + + e/


Lecture 16 The Redox Reactions Oxidation State Half-Reactions Balanced Oxidation-Reduction reactions Predicted Sequence of Redox Reactions Tracers for.

an electron acceptor. Thus: Ox1 + Red2 = Red1 + Ox2 In this case Red2 is the electron donor, passing electrons to Ox1 which is the electron acceptor. Thus Red2 is oxidized to Ox2 and Ox1 is reduced to Red1. The equilibrium constant for an oxidation-reduction reaction can be determined by combining the constants from Table 1 as follows for O 2 with glucose The two half/


CHE-300Review nomenclature syntheses reactions mechanisms.

Syntheses 1. reduction of alkene (addition of hydrogen) 2. reduction of an alkyl halide a) hydrolysis of a Grignard reagent b) with an active metal and acid 3. Corey-House Synthesis Reactions 1. halogenation 2. combustion (oxidation) 3. pyrolysis/alkyl halide 2. dehydration of an alcohol 3. dehalogenation of a vicinal dihalide 4. reduction of an alkyne reactions 1. addition of hydrogen8. hydroboration-oxidation 2. addition of halogens9. addition of free radicals 3. addition of hydrogen halides10. /


Ch. 20 Oxidation-Reduction Reactions. Types of Reactions There are many different types of reactions: 1.Redox 2.Acid-Base 3.Precipitation.

Ch. 20 Oxidation-Reduction Reactions Types of Reactions There are many different types of reactions: 1.Redox 2.Acid-Base 3.Precipitation 20.1 Oxidation and Reduction Oxidation- Reduction Reaction: reaction in which electrons are transferred from one atom to another AKA- Redox Reaction Oxidation The roaring fire shown to the right is an example of the rapid oxidization of the hydrocarbons making up the wood and the reduction of the Oxygen gas from the air. The, very/


Redox Reactions Or How Batteries Work REDOX Reactions The simultaneous transfer of electrons between chemical species. – Actually 2 different reactions.

is more active than copper. Cu + ZnSO 4 No Reaction Copper cannot replace zinc Oxidation is on top Reduction is on bottom Review of Terms oxidation-reduction (redox) reaction: – involves a transfer of electrons from the reducing agent to the oxidizing agent. oxidation: loss of electrons reduction: gain of electrons Half-Reactions The overall reaction is split into two half-reactions, one involving oxidation and one reduction. 8H + + Mn +7 O 4  + 5Fe 2+  Mn/


Carboxylic Acids Carboxylic Acids  Nomenclature  Properties  Preparation reactions  Typical reactions  Spectroscopy.

u From Primary Alcohols u From Aldehydes u From Substituted Aromatics Carbonation of Grignard Reagents Hydrolysis of Acid Derivatives and Nitriles Haloform Reaction Cleavage of methyl carbinols Cleavage of methyl carbonyls Periodic Acid Cleavage of Vicinal Dials/Diketones Oxidative Cleavage Reactions Oxidative Cleavage Reactions  Alkene Cleavage  Hot Potassium Permanganate  Alkyne Cleavage  Hot Potassium Permanganate  Ozonolysis  Alkene Cleavage  Hot Potassium Permanganate  Alkyne Cleavage  Hot/


Redox Reactions This is a oxidation-reduction reaction where the transfer of electrons from a reductant to an oxidant occur. Oxidation- is the loss of.

Reactions This is a oxidation-reduction reaction where the transfer of electrons from a reductant to an oxidant occur. Oxidation- is the loss of electrons therefore this element is being reduced. (reductant) Reduction- is the gain of electrons therefore this element is being oxidised. (oxidant) Oxidation Like acid-base reactions, redox reactions are a matched set - you dont have an oxidation reaction without a reduction reaction happening at the same time. So we call these half cell reactions/


Aqueous Reactions CHAPTER 20 “Oxidation-Reduction Reactions” LEO SAYS GER.

Aqueous Reactions CHAPTER 20 “Oxidation-Reduction Reactions” LEO SAYS GER Aqueous Reactions Oxidation-Reduction Reactions An oxidation occurs when an atom or ion loses electrons. A reduction occurs when an atom or ion gains electrons. Aqueous Reactions Oxidation and Reduction (Redox) Redox currently says that electrons are transferred between reactants Mg + S → Mg 2+ + S 2- The magnesium atom (which has zero charge) changes to a magnesium ion by losing 2 electrons, and is oxidized to Mg/


Oxidation & Reduction IB Topics 9 & 19 AP Chapters 4.9-4.10; 17.

Cr 3+ 4+ 14H 2 O28H + +12e - + Redox Balancing Practice Balance the following redox rxn that takes place in acidic sol’n: Now add the oxidation and reduction reactions together: C 2 H 5 OH  CO 2 2 3H 2 O + + 12H + + 12e - Cr 2 O 7 2-  Cr 3+ 4+/- (aq) + 2H 2 O (l) =4H 2 O (l) + 4e - Redox Balancing Practice Balance the following redox rxn that takes place in acidic sol’n: Now add the oxidation and reduction reactions together: CN - (aq) + 4Ag (s)  4Ag(CN) 2 - (aq) 8 O 2 (g)  2H 2 O (l) 4H + (aq) +4e - + /


Understand Redox reactions involve a transfer of electrons. Develop a metals activity series experimentally. Predict spontaneous reactions using an activity.

. Develop a metals activity series experimentally. Predict spontaneous reactions using an activity series. Burning and corrosion needs oxygen – oxidation. Oxidation-reduction reactions – (redox) Chemical changes when electrons are transferred from one reactant to another. Oxidation - an atom loses one or more electrons. Reduction - an atom gains one or more electrons. "LEO says GER” Losing Electrons is Oxidation, Gaining Electrons is Reduction Atoms fight for electrons. The strongest takes electrons from/


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

with oxygen in the air at high temperatures to form lead (II) oxide and sulfur dioxide. Which substance is a reluctant (reducing agent) and which is an oxidant (oxidizing agent)? A. PbS, reductant; O 2, oxidant B. PbS, reductant; SO 2, oxidant C. Pb 2+, reductant; S 2-, oxidant D. PbS, reductant; no oxidant E. PbS, oxidant; SO 2, reductant Balancing Redox Reactions by ½ Reactions –Acidic Potassium dichromate is a bright orange compound that can be reduced/


Electron-transfer reactions are called oxidation-reduction reactions or redox reactions. Oxidation – loss of electrons by one reactant. Reduction – gain.

Electron-transfer reactions are called oxidation-reduction reactions or redox reactions. Oxidation – loss of electrons by one reactant. Reduction – gain of electrons by another reactant. Oxidation and reduction always occur together. Na → Na + + e - (oxidation) Cl 2 + 2e - → 2Cl - (reduction) The substance that is oxidized is the reducing agent. The substance that is reduced is the oxidizing agent. Oxidation Is Losing e - Reduction Is Gaining e - =OIL RIG Oxidation numbers provide a way to keep tabs on /


Reduction- Oxidation Reactions (1) 213 PHC 9 th lecture Dr. mona alshehri (1) Gary D. Christian, Analytical Chemistry, 6 th edition. 1.

electrochemical cells. 4 electrochemical cells Galvanic cells Electrolytic cells ◦ Galvanic cells  A spontaneous reaction occurs and produce electrical energy. ◦ Electrolytic cells  Electrical energy is used to force a non- spontaneous reaction to occur. 5 Both cells contain electrodes where the oxidation and reduction reactions occur:electrodes Oxidation occurs at the electrode called the anode. Reduction occurs at the electrode called the cathode. Electrons flow from the anode to the/


REDOX Reactions. Redox means… OxidationReduction Reactions Redox Rxns involve the… Complete or partial transfer of electrons Change in Oxidation Numbers.

super complex, so we have a special way to balance them… How?? Use HALF REACTIONS!! What is a half reaction you say?? The idea behind using half reactions is simple:  They are reactions that show oxidation and reduction separately. Then, they can be combined (or added together) to give the overall, BALANCED, redox reaction But…prepare yourself, there are a lot of rules & it can be confusing….you/


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

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/


CVEN 5424 Environmental Organic Chemistry Lecture 24 – Redox Reactions: Reduction.

—SH  R—SO 3 - Generally, the reverse of the reduction reactions Oxidation ReactionsOxidation requires electron acceptors  natural waters  oxygen O 2 (actually, the superoxide radical)  radicals (hydroxy OH  -, peroxide, peroxy)  nitrate NO 3 -  Fe(III) and Mn(IV) (aqueous and mineral)  sulfate SO 4 2-  disinfection  hypochlorous acid HOCl, chloramine H 2 NCl, ozone O 3  “wet” oxidation  persulfate (S 2 O 8 2- ), S(VI)  permanganate/


CVEN 5424 Environmental Organic Chemistry Lecture 24 – Redox Reactions: Reduction.

1,2-diiodoethane0.42.66216 << slowestfastest Reduction Reactions  Predicting kinetics – one example Reductive dehalogenation k R  bond strength and electron withdrawal BS: C—X bond strength/reduction of organic contaminants oxidation of reductants Reduction Reactions  Zero-valent iron  permeable reactive barrier remediation  other metals also (Sn, Zn, etc.)  iron metal is oxidized  “rusting”  corrosion  Fe 0 = Fe 2+ + 2 e -  E H 0 (W) ~ -0.6 V  Promotes reductive dechlorination Reduction Reactions/


Reactions of aldehydes and ketones : oxidation reduction nucleophilic addition 1)Aldehydes are easily oxidized, ketones are not. 2)Aldehydes are more reactive.

Reactions of aldehydes and ketones : oxidation reduction nucleophilic addition 1)Aldehydes are easily oxidized, ketones are not. 2)Aldehydes are more reactive in nucleophilic additions than ketones. Aldehydes & ketones, reactions: 1)Oxidation 2)Reduction 3)Addition of cyanide 4)Addition of derivatives of ammonia 5)Addition of alcohols 6)Cannizzaro reaction 7)Addition of Grignard reagents 8) (Alpha-halogenation of ketones) 9) (Addition of carbanions) 1) Oxidation Aldehydes (very easily oxidized!) CH/


Chapter 21 - Oxidation-Reduction Reactions 2: 38.40/49 = 78.37% 3: 40.36/49 = 82.37%

shared But H-O-H, oxygen pulls electrons towards it So the oxygen partially gains electrons, making it reduced And the hydrogens partially lose electrons, making them oxidized Summary Processes Leading to Oxidation and Reduction OxidationReduction Complete loss of electrons (ionic reactions) Complete gain of electrons (ionic reactions) Shift of electrons away from an atom in a covalent bond Shift of electrons towards an atom in a/


Introduction to Oxidation-Reduction Reactions

: Acid/Base Precipitation/Solubility Complex Formation/Complex Dissociation Oxidation/Reduction Any chemical reaction consists of one (or more) of these basic categories. Oxidation/Reduction Reactions Acid/Base reactions involve a donation /acceptance of protons Precipitation/ Solubility reactions involve a donation/ acceptance of negative charge what is being donated and accepted in a redox reaction? Oxidation/Reduction Reactions Electrons! Consider the reaction taking place in a disposable battery: 2Zn/


Chapter 18 Electrochemistry.

5Fe3+ + 4H2O Half–Reactions The overall reaction is split into two half–reactions, one involving oxidation and one reduction. 8H+ + MnO4- + 5Fe2+  Mn2+ + 5Fe3+ + 4H2O Reduction: 8H+ + MnO4- + 5e-  Mn2+ + 4H2O Oxidation: 5Fe2+  5Fe3+ + 5e- Copyright © Cengage Learning. All rights reserved For each half–reaction: The Half–Reaction Method for Balancing Equations for OxidationReduction Reactions Write separate equations for the oxidation and reduction half–reactions. For each half–reaction: Balance all the/


Electrochemistry Lesson 1 Introduction. Electrochemistry Is the study of reactions that gain or lose electrons.

It is simpler to write the net ionic equation. 1.Al+Zn(NO 3 ) 2 Al Al 3+ +3e - oxidation Redox Reactions Both oxidation and reduction must occur. The number of electrons gained must be equal to the number of electrons lost. It is simpler to write the/write the net ionic equation. 1.Al+Zn(NO 3 ) 2 2(Al Al 3+ +3e - )oxidation 3(Zn 2+ +2e - Zn)reduction Balance electrons Redox Reactions Both oxidation and reduction must occur. The number of electrons gained must be equal to the number of electrons lost. It is /


Oxidation-Reduction Oxidation literally means to react with oxygen. Oxidation literally means to react with oxygen. Example:2Mg + O 2 2MgO Example:2Mg.

: Example: 2Fe 2 O 3 + 3C 4Fe + 3CO 2 Oxidation-Reduction Rapid oxidation is called combustion. Rapid oxidation is called combustion. Slow oxidation is called corrosion. Slow oxidation is called corrosion. Oxidation-Reduction In addition, the terms oxidation and reduction are applied to any reaction in which there is a gain or loss of electrons. In addition, the terms oxidation and reduction are applied to any reaction in which there is a gain or loss of/


ELECTROCHEMISTRY Chapter 20

) LEO (the lion) goes GER Losing Electrons Oxidation, Gaining Electrons Reduction OLE- Oxidation Losing Electrons But now feeling positive Oxidized is cool! Oxidation Haiku! Lost an electron But now feeling positive Oxidized is cool! OXIDATION-REDUCTION REACTIONS Direct Redox Reaction Oxidizing and reducing agents in direct contact. Cu(s) + 2 Ag+(aq) ---> Cu2+(aq) + 2 Ag(s) Copper + Silver Ion OXIDATION-REDUCTION REACTIONS Indirect Redox Reaction A battery functions by transferring electrons through an/


Redox Reactions Oxidation Numbers & Oxidation-Reduction

’s the “agent” that oxidizes Hydrogen, so it’s the Oxidizing agent. Problem: for the following Reaction C(s) + Cl2(g)  CCl4 (l) A) What is reduced? B) What gets oxidized? C) What is the reducing agent? D) What is the oxidizing agent? Problem: for the following Reaction 2 MgO  2 Mg + O2 What is the oxidizing agent? Write the Oxidation and Reduction Half cell reactions. Cl0 C0 Mg+2 O/


Chemical Reactions: An Introduction 4.1 Solutions & Solubility Rules 4.2 Molecular and Ionic Equations 4.3 Precipitation Reactions 4.4 Acid Base Reactions.

Analysis Copyright © Houghton Mifflin Company.All rights reserved. Presentation of Lecture Outlines, 4–45 Types of Chemical Reactions Oxidation-Reduction ReactionsOxidation-reduction reactions involve the transfer of electrons from one species to another. –Oxidation is defined as the loss of electrons. –Reduction is defined as the gain of electrons. –Oxidation and reduction always occur simultaneously. OIL RIG Copyright © Houghton Mifflin Company.All rights reserved. Presentation of Lecture Outlines, 4/


Chem II: Block 10.14.14 Infinite Campus: Chemical Reactions Exam Replacement Labs (30pts.) Objectives: I can predict and simplify double replacement reactions.

reaction. c.Identify and explain which element was oxidized in this reaction. Redox Reactions: Half Reactions Ex. 2Ca + O 2 -----> 2CaO Half-Reactions: Separates/identifies the oxidized and reduced reactions that occur simultaneously in nature-why called Redox reactions. Oxidized Reaction: Reduced Reaction: Chem II: Block 10.16.14 Due: Redox Reaction Worksheet Objectives: I can distinguish between oxidation and reduction reactions using oxidations numbers. I can balance oxidation-reduction (Redox) reactions/


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

SAYS GER Oxidation and Reduction (Redox)  Electrons are transferred  Spontaneous redox rxns can transfer energy  Electrons (electricity)  Heat  Non-spontaneous redox rxns can be made to happen with electricity Oxidation Reduction Reactions (Redox) Each sodium atom loses one electron: Each chlorine atom gains one electron: LEO says GER : LEO says GER : Lose Electrons = Oxidation Sodium is oxidized Gain Electrons = Reduction Chlorine is reduced Not All Reactions are Redox Reactions Reactions in which/


1 REDOX REACTIONS Day 1 Review Oxidation numbers REACTIONS BatteriesBatteries.

7 > Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. A substance that undergoes oxidation gains oxygen. A substance that undergoes reduction loses oxygen. Reactions that involve the processes of oxidation and reduction are called oxidation-reduction reactions. Oxidation-reduction reactions are also known as redox reactions. Original definition 20.1 The Meaning of Oxidation and Reduction 8 > Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. What Are/


Aqueous Reactions Precipitation Reactions When one mixes ions that form compounds that are insoluble (as could be predicted by the solubility guidelines),

4 (aq)  Na 2 SO 4 (aq) + H 2 S (g) Aqueous Reactions Oxidation-Reduction Reactions An oxidation occurs when an atom or ion loses electrons. A reduction occurs when an atom or ion gains electrons. Aqueous Reactions Oxidation-Reduction Reactions One cannot occur without the other. Aqueous Reactions Oxidation Numbers To determine if an oxidation-reduction reaction has occurred, we assign an oxidation number to each element in a neutral compound or charged entity. Aqueous/


Lecture 233/12/06. What is a REDOX reaction? OXIDATION: Ca(s)  Ca 2+ REDUCTION: 2H +  H 2 (g) OIL RIG Combined (net): REDOX REACTIONS Oxidation-Reduction.

: Zn (s) + HBr (aq)  ZnBr 2 (aq) + H 2 (g) Apparatus with oxidation and reduction reactions in different compartments Apparatus with oxidation and reduction reactions in different compartments redox reaction occurs by transferring electrons through an external connector redox reaction occurs by transferring electrons through an external connector voltaic or galvanic cell product favored reaction product favored reaction produces electric current produces electric current electrolytic cell reactant favored/


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