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Ch. 9: Lesson 2 -Intro to Redox Reactions-

Ch. 9: Lesson 2 -Intro to Redox Reactions-. Brief Charge Reminder. Electrons have a charge Neutral atoms have an overall charge of Adding an e- makes charge go Removing an e- makes charge go. Oxidation and Reduction.

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Ch. 9: Lesson 2 -Intro to Redox Reactions-

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  1. Ch. 9: Lesson 2 -Intro to Redox Reactions-

  2. Brief Charge Reminder • Electrons have a charge • Neutral atoms have an overall charge of • Adding an e- makes charge go • Removing an e- makes charge go

  3. Oxidation and Reduction • Reduction is a gain of electrons (charge is reduced) • Oxidation is a loss of electrons (charge is increased) • Ag  Ag = = • Cl  Cl = = Equation with e-Process + -

  4. Reduction reduces charge • Oxidation is just the other one

  5. Identifying what’s oxidized and what’s reduced • First assign oxidation #’s, then see how they change from start to finish Ex: C + H2O  CO + H2

  6. Oxidation/Reduction Practice MnO2 + 4 HCl  MnCl2 + Cl2 + 2 H2O

  7. Redox Reactions • Redox reactions involve REDuction and OXidation • SAT Word Alert: PORTMANTEAU -THIS MEANS- • Both have to happen at the same time

  8. Remembering How Redox Works • LEO says GER: • Losing e- is • Gaining e- is • OIL RIG • Oxidation is e- • Reduction is e-

  9. Conclusion Questions • For Now: Review book page 162, # 11-15, on back of paper slips to hand in before you leave • For HW: same page, #16-25, in notebooks

  10. Ch. 9: Lesson 3 -Recognizing Redox Reactions & Their Parts-

  11. 3 Forms of Redox Reactions • A + B  AB • Ex: 2 H2 + O2 2 H2O • AB  A + B • Ex: 2 NaCl  2 Na + Cl2 • A + BC  AC + B • Ex: Zn + Cu(NO3)2 Zn(NO3)2 + Cu

  12. Recognizing Redox Reactions • 1. Single element(s) on either side of the equation 2 Li + Zn(NO3)2 2 Li(NO3) + Zn • 2. Elements change oxidation # from reactant to product • 2 K + Cl2 2 KCl • Increasing ox # means e- , was • Decreasing ox# means e- , was

  13. Agents • Reducing agents cause something else to be reduced, but get oxidized themselves • Oxidizing agents cause something else to be oxidized, but get reduced themselves 2 Sr + O2 2 SrO Reduced: Oxidized: Reducing agent: Oxidizing agent:

  14. Ox: Rd: OxAg: RdAg: Ox: Rd: OxAg: RdAg: Ox: Rd: OxAg: RdAg: 2 Cs + Br2 2 CsBr 3 Mg + N2 Mg3N2 4 Fe + 3 O2 2 Fe2O3

  15. Spectator Ions • Spectators are atoms or ions without a charge change, just along for the ride Cu + 2 AgNO3 Cu(NO3)2 + 2 Ag

  16. Labeling Things In Equations Cu + 2 AgNO3 Cu(NO3)2 + 2 Ag • Make sure equation is balanced, find ox# for each species • What is being oxidized? • What is being reduced? • What is the oxidizing agent? • What is the reducing agent? Any spectator ions?

  17. Labeling Things In Equations Zn + 2 HCl  ZnCl2 + H2 • Make sure equation is balanced, find ox# for each species • What is being oxidized? • What is being reduced? • What is the oxidizing agent? • What is the reducing agent? Any spectator ions?

  18. Labeling Things In Equations NaCl + AgNO3 AgCl + NaNO3 • Make sure equation is balanced, find ox# for each species • What is being oxidized? • What is being reduced? • What is the oxidizing agent? • What is the reducing agent? This is double replacement. Double replacement’s are not redox reactions.

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