1 / 30

Electron Transfer in Chemical Reactions

Electron Transfer in Chemical Reactions. Redox Part II: Including batteries. Chapter 10. Redox Reactions in Our World. Batteries. Corrosion. Fuels. Manufacturing metals. Examples of Redox Reactions. Metal + halogen 2 Al + 3 Br 2  Al 2 Br 6. e . e .

nuru
Download Presentation

Electron Transfer in Chemical Reactions

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript


  1. Electron Transfer in Chemical Reactions Redox Part II: Including batteries Chapter 10

  2. Redox Reactions in Our World Batteries Corrosion Fuels Manufacturing metals

  3. Examples of Redox Reactions Metal + halogen 2 Al + 3 Br2 Al2Br6

  4. e e Electron Transfer in a Redox Reaction 2Ag+(aq) + 2Ag(s) + Cu(s)  Cu2+(aq) • Two electrons leave copper. • The silver ions accept them. • The copper metal is oxidized to copper (II) ion. • The silver ion is reduced to solid silver metal.

  5. 10.3 Recognizing Electron-Transfer Reactions (Continued) • Reduction • The gaining of electrons • Decrease in the overall oxidation state

  6. 10.3 Recognizing Electron-Transfer Reactions (Continued) • Oxidation • The loss of electrons • Increase in the overall oxidation state

  7. 10.3 Recognizing Electron-Transfer Reactions (Continued) • Oxidizing agent • Substance that oxidizes something else • Reducing agent • Substance that reduces something else

  8. 10.3 Recognizing Electron-Transfer Reactions (Continued) Which substance is the oxidizing agentand which is the reducing agent in the following: P4 + 6 Br2 4 PBr3

  9. 10.3 Recognizing Electron-Transfer Reactions (Continued) Which substance is the oxidizing agent and which is the reducing agentin the following: P4 + 6 Br2 4 PBr3

  10. 10.1 What Is Electricity? • Electricity is the flow of electrons. • Voltage is the push of the electrons.

  11. 10.1 What Is Electricity? (Continued) • Production of electricity • Occurs at power plants • Mechanically produced by generator • Wound copper wire spinning between magnets • Occurs in chemical reactions • Electrons released by atoms/compounds • Batteries are an example of a chemical-based release of electrons.

  12. 10.4 Electricity from Redox Reactions • Galvanic cell • Also known as a battery • Wire allows path for the flow of electrons

  13. 10.4 Electricity from Redox Reactions (Continued) • Salt bridge • Conductive component completing cell • Maintain charge balance between sides • Spectator ions • Ions not directly involved in the redox reaction • Electrodes • Metal strips submerged in the solutions

  14. 10.4 Electricity from Redox Reactions (Continued)

  15. 10.4 Electricity from Redox Reactions (Continued)

  16. 10.4 Electricity from Redox Reactions (Continued) • Standard cell battery • Redox reaction in a can • Reactants are MnO2 and Zn. • A semimoist paste containing NH4Cl acts as the salt bridge.

  17. 10.4 Electricity from Redox Reactions (Continued) Standard Cell Battery

  18. 10.4 Electricity from Redox Reactions (Continued) • A wire connecting terminals allows electron flow.

  19. 10.4 Electricity from Redox Reactions (Continued) • Cathode • Positive electrode • MnO2 in standard cell battery • Anode • Negative electrode • Zn in standard cell battery

  20. 10.4 Electricity from Redox Reactions (Continued) • Lithium ion battery • Made of Co+4 (cathode) • Li atoms in graphite sheets (anode) • Separator membrane

  21. 10.4 Electricity from Redox Reactions (Continued) • During discharge: • Li ions give up electrons. • Co+4 is reduced to Co+3. • LiCoO2 is formed.

  22. 10.4 Electricity from Redox Reactions (Continued) • Fuel cell • Battery in which one reactant is a combustible fuel and the other is oxygen.

  23. 10.5 Which Way Do Electrons Flow?—The EMF Series • Electron flow • Electrons flow from active metals to less active metals. • Electrons flow from Mg to Zn. • Electrons will not flow Zn to Mg. Electrons from Mg reduce the Zn cations. Mg dissolves as it becomes Mg+2 No reaction

  24. 10.5 Which Way Do Electrons Flow?—The EMF Series (Continued) Electromotive Force (EMF) Series

  25. 10.5 Which Way Do Electrons Flow?—The EMF Series (Continued) What will happen if a piece of Zn metal is placed in a solution of Al3+ ions?

  26. 10.5 Which Way Do Electrons Flow?—The EMF Series (Continued) What will happen if a piece of Zn metal is placed in a solution of Al3+ ions? Al is higher on the EMF series, so Zn will not spontaneously give up its electrons to Al3+.

  27. 10.6 Another Look at Oxidation: The Corrosion of Metals (Continued) • What is the Statue of Liberty made of? Fe frame inside for support with a copper metal sculpture outside

  28. 10.6 Another Look at Oxidation: The Corrosion of Metals (Continued) CuO is green • Oxidation on the Statue of Liberty • Copper slowly combines with oxygen in the air. • The formed Cu2+ could oxidize the Fe skeleton of the statue, endangering the structure.

  29. 10.6 Another Look at Oxidation: The Corrosion of Metals (Continued)

  30. 10.6 Another Look at Oxidation: The Corrosion of Metals (Continued) • Sacrificial metals • Metal piece designed to oxidize in place of another metal • Active metalschosen • Mg very common choice

More Related