Chemistry 20.1.

Slides:

Advertisements

Similar presentations

Chemistry 21.3.

Advertisements

“Oxidation-Reduction Reactions”

7.2 Types of Reactions The walls of this cave are limestone. When hydrochloric acid is dropped on limestone, a chemical reaction occurs that produces a.

Chemistry 20.2.

OXIDATION- REDUCTION REACTIONS REDOX. Oxygen Reactions Early chemists saw oxidation only as the combination of an element with oxygen to produce an oxide.

The Finish Line is in site… Electrochemistry. “Oxidation-Reduction Reactions” LEO SAYS GER.

Year 12 Chemistry - Shipwrecks. Iron/Steel ships Iron and various forms of steel are the primary metals used in the production of ships because they:

Chemistry 21.2.

Aim: What are oxidation and reduction? Do Now: 1.Sketch the structure of an atom. Label the subatomic particles. 2.Describe the relative masses and charges.

Chemistry 17.4.

Slide 1 of 37 © Copyright Pearson Prentice Hall Describing Chemical Reactions > Writing Chemical Equations Word Equations To write a word equation, write.

Electron Transfer Reactions Electron transfer reactions are oxidation-reduction or redox reactions. Results in the generation of an electric current (electricity)

© Copyright Pearson Prentice Hall Slide 1 of 42 Types of Chemical Reactions The heat and smoke of burning charcoal are the products of a combustion reaction.

Corrosion Intermediate 2 Unit 3(c).

20.1 Oxidation/Reduction (REDOX)

20.2 Oxidation Numbers > 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Chapter 20 Oxidation-Reduction Reactions 20.1 The.

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

Chapter 20 Oxidation-Reduction Reactions 20.1 The Meaning of Oxidation

“Oxidation-Reduction Reactions”

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

Revision Quiz Corrosion 1

Chapter 20 Oxidation – Reduction Reactions. What are they? A family of reactions that are concerned with the transfer of electrons between species Redox.

“Oxidation-Reduction Reactions” LEO SAYS GER Or OIL RIG.

Slide 1 of 37 chemistry. © Copyright Pearson Prentice Hall Slide 2 of 37 Describing Chemical Reactions On May 6, 1937, the huge airship Hindenburg erupted.

Slide 1 of 42 chemistry. © Copyright Pearson Prentice Hall Slide 2 of 42 Types of Chemical Reactions The heat and smoke of burning charcoal are the products.

“Oxidation-Reduction Reactions” LEO SAYS GER Pre-AP Chemistry Charles Page High School Stephen L. Cotton.

Shipwrecks, Corrosion and Conservation

Electrochemistry Electron Transfer Reactions Electron transfer reactions are oxidation- reduction or redox reactions. Results in the generation of an.

Calderglen High School What is corrosion? A chemical reaction involving a metal changing from an element to a compound answer.

CHEMISTRY DEPARTMENT WAID ACADEMY Standard Grade Topic 12.

Chapter 11 Chemical Reactions

CHAPTER 22 “Oxidation-Reduction Reactions” LEO SAYS GER OIL REG or.

Element Elements and Compounds Structure of Atom Compounds A compound is a substance composed of two or more elements, chemically combined with one another.

Oxidation-Reduction Reactions. Oxidation and Reduction Oxidation-reduction reactions always occur simultaneoulsy. Redox Reactions Oxidation Loss of electrons.

Shipwrecks, Corrosion and Conservation Summary Slides PART 3 – Jack Dengate.

Oxidation-Reduction Reactions Redox. Iron is oxidized when it rusts.

Oxidation Reduction Reactions. Types of Reaction  Oxidation-Reduction called Redox Ionic compounds are formed through the transfer of electrons. An Oxidation-reduction.

Standard Grade Chemistry Topic 12 - Corrosion. Corrosion Corrosion is the changing of the surface of the metal from an element into a compound. This natural.

Oxidation-Reduction Reactions Part 1 Notes 11 Beginning Unit 4.

Slide 1 of 47 chemistry. © Copyright Pearson Prentice Hall Slide 2 of 47 Balancing Redox Equations When concentrated hydrochloric acid (HCl) and nitric.

© Copyright Pearson Prentice Hall Slide 1 of 47 Balancing Redox Equations When concentrated hydrochloric acid (HCl) and nitric acid (HNO 3 ) are mixed.

Types of Reactions. The Six Different Types of Reactions Synthesis Reaction Decomposition Reaction Single Replacement Reaction Double Replacement Reaction.

Rusting – Lesson Objectives Understand how salt water affects rusting. Understand that rusting is an oxidation reaction (iron reacts with oxygen forming.

Midterm Review Day 2 Do Now: HW, Calculator, and Reference Tables out.

Chapter 20 Oxidation-Reduction Reactions 20.2 Oxidation Numbers

Chapter 20.  Salt on icy roads can make driving safer, but the salt that clings to the metallic parts of cars can cause them to corrode or rust relatively.

Slide 1 of 39 © Copyright Pearson Prentice Hall Ions > Valence Electrons I. IONS A. Valence electrons: are in the highest occupied energy level of an atom.

Slide 1 of 37 chemistry. © Copyright Pearson Prentice Hall Slide 2 of 37 Describing Chemical Reactions On May 6, 1937, the huge airship Hindenburg erupted.

Batteries are voltaic cells that use spontaneous reactions to provide energy for a variety of purposes. Section 2: Batteries K What I Know W What I Want.

Section 20.1 The Meaning of Oxidation and Reduction (called “redox”) OBJECTIVES Define oxidation and reduction in terms of the loss or gain of oxygen,

Slide 1 of 42 chemistry. © Copyright Pearson Prentice Hall Slide 2 of 42 Types of Chemical Reactions The heat and smoke of burning charcoal are the products.

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

Slide 1 of 37 chemistry. © Copyright Pearson Prentice Hall Slide 2 of 37 Describing Chemical Reactions On May 6, 1937, the huge airship Hindenburg erupted.

Mrs. Howland Chemistry 10 Rev. March Learners will be able to… Define oxidation Define reduction Identify oxidation in a redox half-reaction Identify.

Standard Grade Chemistry

Chemistry 20.1.

Corrosion Intermediate 2.

Corrosion Intermediate 2 Unit 3(c).

Calderglen High School

Reactions of acids AQA Chemical Changes 1 Reactivity of metals

Section 2: Redox Reactions

Chemical Reactions Chemical reactions can be shown as chemical equations represented by words and chemical formulas. To write an equation, you must indicate.

Calderglen High School

Chemistry 20.1.

Oxidation-Reduction Reactions

Presentation transcript:

Chemistry 20.1

The Meaning of Oxidation and Reduction 20.1 The Meaning of Oxidation and Reduction Salt on icy roads can make driving safer, but the salt that clings to the metallic parts of cars can cause them to corrode or rust relatively quickly. This corrosion is one example of a chemical reaction called oxidation-reduction. You will learn about oxidation-reduction reactions.

What Are Oxidation and Reduction? 20.1 What Are Oxidation and Reduction? What Are Oxidation and Reduction? How is the gain or loss of oxygen in a chemical reaction linked to oxidation and reduction?

What Are Oxidation and Reduction? 20.1 What Are Oxidation and Reduction? The substance gaining oxygen is oxidized, while the substance losing oxygen is reduced. These reactions are called oxidation- reduction reactions and are also known as redox reactions.

What Are Oxidation and Reduction? 20.1 What Are Oxidation and Reduction? Oxygen and Redox A Bunsen burner oxidizes the methane in natural gas to carbon dioxide and water. A Bunsen burner oxidizes the methane in natural gas to carbon dioxide and water.

What Are Oxidation and Reduction? 20.1 What Are Oxidation and Reduction? Carbon is oxidized when charcoal burns. When charcoal, which is mostly carbon, is burned in air, carbon dioxide and heat are produced.

What Are Oxidation and Reduction? 20.1 What Are Oxidation and Reduction? Iron is oxidized when it rusts. When items made of iron are exposed to moist air, the Fe atoms react with O2 molecules. The iron rusts; it is oxidized to compounds such as iron(III) oxide (Fe2O3).

What Are Oxidation and Reduction? 20.1 What Are Oxidation and Reduction? Electron Shift in Redox Reactions How is the gain or loss of electrons linked to oxidation and reduction?

What Are Oxidation and Reduction? 20.1 What Are Oxidation and Reduction? Losing electrons is oxidation. Gaining electrons is reduction. Oxidation is now defined to mean complete or partial loss of electrons or gain of oxygen. Reduction is now defined to mean complete or partial gain of electrons or loss of oxygen.

What Are Oxidation and Reduction? 20.1 What Are Oxidation and Reduction? Redox Reactions That Form Ions When magnesium and sulfur are heated together, they undergo an oxidation-reduction reaction to form magnesium sulfide. Applying Concepts Where did the electrons lost by magnesium go?

What Are Oxidation and Reduction? 20.1 What Are Oxidation and Reduction? When magnesium and sulfur are heated together, they undergo an oxidation-reduction reaction to form magnesium sulfide. Applying Concepts Where did the electrons lost by magnesium go?

What Are Oxidation and Reduction? 20.1 What Are Oxidation and Reduction? The substance that loses electrons is called the reducing agent. The substance that accepts electrons is called the oxidizing agent.

for Conceptual Problem 20.1 Problem Solving 20.1 Solve Problem 1 with the help of an interactive guided tutorial.

What Are Oxidation and Reduction? 20.1 What Are Oxidation and Reduction? Redox With Covalent Compounds This welder is using an oxyhydrogen torch to cut and weld steel. When hydrogen burns in oxygen, the redox reaction generates temperatures of about 2600°C.

What Are Oxidation and Reduction? 20.1 What Are Oxidation and Reduction?

20.1 Corrosion Corrosion What happens to iron when it corrodes?

20.1 Corrosion Iron, a common construction metal often used in the form of the alloy steel, corrodes by being oxidized to ions of iron by oxygen. Bridges like this one become unsafe because of corrosion.

Resistance to Corrosion 20.1 Corrosion Resistance to Corrosion Aluminum resists corrosion because it forms a protective coating of aluminum oxide. Oxidation causes the complete corrosion of some metals. Aluminum resists such corrosion because it forms a protective coating of aluminum oxide. Applying Concepts How does the aluminum oxide on aluminum differ from the iron(III) oxide formed on corroding iron?

Controlling Corrosion 20.1 Corrosion Controlling Corrosion Painting a surface protects it from corrosion. Chromium metal also serves as a protective coating. Painting a surface (left) protects it from the effects of the environment. Chromium metal also serves as a protective coating and imparts an attractive, mirrorlike finish (right). Like aluminum, chromium forms a corrosion-resistant oxide film on its surface.

20.1 Corrosion Zinc blocks attached to the steel hull of this ship oxidize instead of the iron, preventing corrosion. Zinc blocks, the white rectangles in the photograph, are attached to the steel (iron) hull of this ship. The zinc blocks oxidize (corrode) instead of the iron, preventing the hull from corroding.

20.1 Section Quiz. 20.1.

20.1 Section Quiz. 1. Choose the correct words for the spaces. During oxidation, an element _______ electrons. During reduction, an element ________ electrons. gains, loses loses, gains gains, donates gains, accepts

20.1 Section Quiz. 2. Choose the correct words for the spaces. During reduction, a substance may _______ oxygen or ________ hydrogen. gain, lose lose, gain gain, gain lose, lose

20.1 Section Quiz.. 3. The element that donates electrons in a redox reaction is called the reducing agent. This means the reducing agent is always the more active element. the less active element. oxidized. reduced.

20.1 Section Quiz. 4. Which substance is the reducing agent in the following chemical reaction? Fe2O3 + 3CO  2Fe + 3CO2 Fe2O3 CO Fe CO2

the O2(g) in both reactions the O2(g) and H2O(l) in both reactions 20.1 Section Quiz. 5. The following equations describe the corrosion of iron to iron hydroxides in moist conditions. 2Fe(s) + O2(g) + 2H2O(l)  2Fe(OH)2(s) 4Fe(OH)2(s) + O2(g) + 2H2O(l) 4Fe(OH)3(s) What substances in the equations are being oxidized? Fe(s) and Fe(OH)2(s) the O2(g) in both reactions the O2(g) and H2O(l) in both reactions Fe(OH)2(s) and Fe(OH)3(s)

END OF SHOW