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Unit 5

Unit 5. Electrochemistry. Unit 5 Part 1.

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Unit 5

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  1. Unit 5 Electrochemistry

  2. Unit 5 Part 1 • By the end of Part 1, students will be able to describe the essential components of reacting systems that involve electron transfer, determine the stoichiometry of redox reactions by balancing redox reactions, and apply their findings to perform redox titrations. Vocabulary • half-reaction, oxidation, oxidation number, oxidizing agent, redox reaction, redox titration, reducing agent, reduction

  3. ElectroChem Intro Video • http://www.youtube.com/watch?v=kfgtU9DDvdY

  4. 5.1 Introduction What we need to learn… • define and identify • oxidation • reduction • oxidizing agent • reducing agent • half-reaction • redox reaction

  5. What IS ELECTROCHEMISYTY??????

  6. Battery Reactions

  7. Corrosion

  8. Preventing Corrosion

  9. Electroplating

  10. Refining Metals

  11. Electrochemistry • The branch of chemistry which is concerned with the conversion of chemical energy to electrical energy, and vice versa • OXIDATION REACTION: A half-cell reaction in which electrons are lost from a species (the species gives off electrons).REDUCTION REACTION: A half-cell reaction in which a species gains electrons (the species accepts electrons). LEO the lion says GER” LEO → Lose Electrons, Oxidation GER → Gain Electrons, Reduction

  12. For every reduction reaction there must be an accompanying oxidation reaction because… • We couldn’t have a substance accept electrons if there wasn’t a substance which would give off electrons in the first place! • A reaction involving the loss and gain of electrons is called a reduction-oxidation reaction, or REDOX reaction.

  13. In the reaction: 2 Ag+(aq) + Cu(s) → 2 Ag(s) + Cu2+(aq) • Ag+ is the “agent” which causes Cu (s) to become oxidized. Ag+ is called the OXIDIZING AGENT. • Cu(s) is the “agent” which causes Ag+ to become reduced. Cu(s) is called the REDUCING AGENT. NOTE: The OXIDIZING AGENT is itself REDUCED. The REDUCING AGENT is itself OXIDIZED.

  14. For Example: In the reaction: Zn(s) + I2(s) → Zn2+(aq) + 2 I-(aq) • The half-cell reactions are: Zn(s) → Zn2+(aq) + 2 e- I2(s) + 2 e- → 2 I-(aq) • The Zn(s)loses electrons and is being OXIDIZED. • The I2(s)gains electrons and is being REDUCED. • Since Zn(s) is oxidized, then Zn(s) is the REDUCING AGENT. • Since I2(s) is reduced, then I2(s) is the OXIDIZING AGENT.

  15. Homework…. • Read SWB pages 189 -192 • Do exercises #1-2 page 192

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