2.B Earth’s Mineral Resources. Smartboard File Earth’s Atomsphere.

Slides:

Advertisements

Similar presentations

Chemistry Chemical Reactions Single and Double Replacement Reactions PERIODIC TABLES REQUIRED CALCULATORS OPTIONAL.

Advertisements

Metals and their Properties Metals have distinctive properties such as: 1. Electrical Conductivity 2. Good Thermal Conductivity 3. Strength 4. Malleability.

Electrolysis Electrolysis breaks down ionic substances into simpler substances by using electricity!

Topic 9 Oxidation and Reduction Introduction Oxidation numbers Redox equations Reactivity Voltaic cells Electrolytic cells.

Single Displacement and Redox. Single Displacement and Redox: At the conclusion of our time together, you should be able to: 1.Identify a basic single.

Displacement Reactions By the end of this lesson I should be able to: 1.Use the Electrochemical series to explain why displacement reactions occur and.

1 Chapter 5 Chemical Reactions 5.3 Oxidation-Reduction Reactions.

Oxidation-Reduction Dr. Ron Rusay Balancing Oxidation-Reduction Reactions.

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.

Oxidation and Reduction. Historically.... Oxidation was defined as the addition of oxygen to a substance Eg. when coal was burned C + O 2 CO 2 or the.

2.B: Earth’s Mineral Resources. Objectives 1) Describe the chemicals in the Earth’s atmosphere, hydrosphere and lithosphere. 2) Describe and recognize.

Jeopardy Valence Electrons Ionic Compounds Trends Reactivity Lab REDOX Q $100 Q $200 Q $300 Q $400 Q $500 Q $100 Q $200 Q $300 Q $400 Q $500 Final Jeopardy.

Redox: Oxidation and Reduction Definitions Oxidation: loss of e- in an atom increase in oxidation number (ex: -1  0 or +1  +2)  Reduction: gain of.

Objectives Describe the chemicals in the Earth’s atmosphere, hydrosphere and lithosphere. Describe and recognize factors that determine the feasibility.

Electrochemistry Electrons in Chemical Reactions.

Corrosion The Chemical Process.

Redox Chemistry and Corrosion Chapter 16. Oxidation and Reduction ► So far we have looked at precipitation reactions and acid-base reactions. ► Now we.

Warm up: Answer 1-3 on Ch. 8.4 Notes

Chapter 20 Oxidation-Reduction Reactions (Redox Reactions)

 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.

TOPIC 10 Making Electricity Making Electricity. A cell is an apparatus which generates electricity from a chemical reaction. A Battery is when two or.

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

Redox Reactions Learning Goal: I will understand what a ‘REDOX’ reaction is, and be able to illustrate half reactions, and identify what is being oxidized.

Metals, Making Electricity and Corrosion. Metals The job that a metal is used for is determined by its physical and chemical properties. Physical properties.

OXIDATION AND REDUCTION. Oxidation Losing electrons The higher positive oxidation number the more the atom has loss control over the electrons, therefore.

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.

CHAPTER 5 ANALYSING OXIDANTS AND REDUCTANTS. REDOX REACTIONS Redox reactions involve complementary processes of oxidation and reduction, and can be identified.

Metals. Learning Objectives Use reactivity data to determine a reactivity series Relate extraction method to reactivity of metals Write word/symbol equations.

Earth’s Mineral Resources Unit 2 Sect B Environmental Chemistry.

Chapter 20 – Oxidation and Reduction Oxidation-Reduction reactions called redox reactions.

Types of Reactions Including reaction prediction.

Redox Reactions. Chemical Reactions There are 3 major classes of chemical reaction: There are 3 major classes of chemical reaction: 1. Precipitation 2.

REACTIONS. Reactions  Chemical equation: equation that shows the rearrangement of atoms that occurs in a chemical reaction  Reactants: original substances.

Oxidation and Reduction By the end of this lesson, you should be able to: 1.State that a metal element reacting to form a compound is an example of oxidation.

Copyright © McGraw-Hill Education. Permission required for reproduction or display Chapter 14: Oxidation- Reduction Reactions.

 Magnesium  Aluminium  Zinc  Iron  Copper Magnesium can displace copper from copper oxide – WHY? Mg (s) + CuO (s) → MgO + Cu.

Oxidation/Reduction Reactions

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 1 Chapter 15 Oxidation- Reduction: Transfer of Electrons 15.1 Oxidation and Reduction Rust forms.

Aqueous Reactions © 2015 Pearson Education, Inc. Compilation Presentation Chapter 4 [4.5] Reactions in Aqueous Solution James F. Kirby Quinnipiac University.

Chemical Reactions. Describing Chemical Change Chemical reactions take place around you everyday Chemical reactions are expressed on paper as chemical.

Who wants to be a millionaire?. 2 Ag + (aq) + Hg (l) > 2 Ag (s) + Hg 2+ (aq) 1. For the given reaction, What is being oxidized?

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.

Electrochemistry Redox Reactions June 13 th 2012 Mr. Dvorsky.

Chapter 11: Chemical Reactions

U4 S1 L1 Defining Oxidation and reduction Textbook Readings MHR page 712: Oxidation-Reduction Reactions pages : Defining Oxidation and Reduction.

1 Chapter 20 Oxidation-Reduction Reactions (Redox Reactions)

21-3 Classifying Chemical Reactions You will be learning: 1.How to identify the four general types of chemical reactions. 2.How to predict which metals.

Single Displacement and Redox. Septic Tank Humor.

2.B Earth’s Mineral Resources. Earth’s Composition Atmosphere: (gases) Nitrogen, Oxygen, Neon, Argon Hydrosphere: (water) Comes from water and dissolved.

3.17 Uses of electrolysis Purification of copper:

Displacement reactions

Starter Write the word equation for the following reactions.

The Activity Series.

Redox 4 The Activity Series.

Redox Chemistry and Corrosion

Redox: Oxidation and Reduction

5.9 – NOTES Metal Reactivity Trends

Redox Reactions and Electrolysis

Unit 13: More Chemical Reactions

5.11 – Notes Oxidation and Reduction

Sources and Uses of Metals

Redox Chemistry and Corrosion

Reactions of acids AQA Chemical Changes 1 Reactivity of metals

Unit 8 Redox Reactions Chapter 9.

6.8 – NOTES Metal Reactivity Trends

Electrochemistry Lesson 2

C4 – Chemical changes Key Concepts.

Presentation transcript:

2.B Earth’s Mineral Resources

Smartboard File Earth’s Atomsphere

2.B Earth’s Mineral Resources Use Table 2.3 (pg. 136) to answer these: 1. What metal might Australia wish to obtain from the US? 2. What metal could Australia trade to the US to obtain the metal in the previous question? 3. From which nation would you expect the US to obtain nickel? Why? 4. Give examples of two trade agreements by which China could obtain iron ore in exchange for a metal it has in abundance. 5. What metals might Canada seek to obtain through trade?

Challenges faced in mining: 1. Use of supplies 2. Where should mining occur 3. The quantity of useful ore found at the site 4. The percent of metal in the ore 5. The type of mining and processing needed to extract the metal from its ore 6. The distance between the mine and metal-refining facilities and markets 7. The metal’s supply vs. demand status 8. The environmental impact of the mining and metal processing. 9. Can you think of any others?

Mining Copper Ores

B.2 Production vs. Use Follow the guidelines on page to research the metal you selected for your coin. If you chose to create an alloy make sure to research all the metals involved.

B.4 Metal Reactivity 2 Cu(s) + O 2 (g)  2 CuO (s) a. Identify the reactant(s). b. Identify the product(s). c. What do the letters in parentheses represent?

Symbols used in chemical equations: (s) = solid (l) = liquid, typically H 2 O, Hg and Br (g) = gas (aq) = aqueous solutions, the solvent has to be water. Ex. Salt water solution

Activity Series The ranking of elements according to their chemical reactivity. For example, Au (gold), does not react with any components of air such as oxygen. This is one reason why it is used in jewelry. Therefore it is ranked low on the Metal Activity Series Au, also used for gold plating electrical contacts used in air bags. They are dependable because oxides do not form on gold-plated surfaces.

Metal Activity Series Reactive metals are more difficult to release from their compounds. Ex. Can zinc (Zn) replace Magnesium in Mg(NO 3 ) 2 ? Can Zn ever replace copper (Cu) in a chemical reaction?

Mining and Refining Reduction: Gain of electrons – there are electrons in the reactants Ex. Cu e -  Cu The copper cation was reduced, lost its charge by gaining electrons

Mining and Refining Oxidation: Loss of electrons – there are electrons in the products Ex. Fe  Fe e - Iron is oxidized to an iron (III) ion by losing 3 electrons

Remember… OIL RIG OIL – Oxidation Is Loss (of electrons) RIG – Reductions Is Gain (of electrons)

Oxidation – Reduction Reaction Oxidation and reduction reactions occur together and are called redox reactions. Cu 2+ (aq) + Mg(s)  Cu(s) + Mg 2+ (aq) - Which reactant (Cu 2+ or Mg(s)) is reduced? - Which is oxidized?