1. 1 Oxidation-Reduction AKA Redox OB: Pages 158-172

2. Aim: How do oxidation numbers tell us what is happening in a reaction? Objectives 1.Students should be able to determine the oxidation states of elements alone or in a compound. 2.Students should be able to identify reactions that are Redox. 3.Students should be able to determine the species being oxidized and the species being reduced in a Redox reaction. 4.Students should be able to identify oxidizing agents and reducing agents in a reaction. 2

3. 3 Oxidation Number Rules Uncombined elements : Total charge = Compounds: Total charge = Polyatomic ions: Total charge = Elements within compounds and polyatomic ions =

4. 4 Oxidation Number Practice What are the oxidation numbers of each of the elements in the following substances? a) Na b) NaClc) Cl 2 d) H 2 SO 4 e) HNO 3 f) O 2 g) Cr 2 O 7 -2 h) PCl 5 i) NO 2 j) LiH k) H 2 Ol) SCN - HW: OB Pg. 160-161, Q 1-10; pg. 169 Q 1,9,13-15

5. 5 Regents Questions

6. 6 Recognizing Redox Reactions Not all reactions are Redox!! If any element’s oxidation state on the reactant side is different from the oxidation state on the product side, it is a redox rxn. Are these redox reactions? MnO 2 + 4HCl  MnCl 2 + Cl 2 + 2H 2 O HCl + KOH  H 2 O + KCl Zn + 2HCl  ZnCl 2 + H 2 2HCl + FeS  FeCl 2 + H 2 S HW: OB Pg. 162, Q 11-14; Pg. 169-170, Q 6,16-17

7. 7 During Redox reactions, are electrons lost or gained? Loss of e - = Oxidation (LEO) = charge _____ Gain of e - = Reduction (GER) = charge _____ Na + Cl 2  NaCl Which one is being oxidized? ______ Which one is being reduced? ______ Redox = whenever an atom loses an electron, another atom has to gain it. So oxidation does not happen without reduction. The total charge of the products = the total charge of the reactants. LEO says GER!

8. 8 Agents In a reaction the element that is oxidized is the reducing agent. oxidized = reducing agent The element that is reduced is the oxidizing agent. reduced = oxidizing agent

9. 9 oxidized = reducing agent reduced = oxidizing agent HW: OB Pg. 162, Q 16-31

10. Exit Write a redox reaction that we learned about in the acid/base unit. What are the oxidation states of all of the species in your reaction? Which species was reduced? Which species was oxidized? Which species loses electrons? Which species gains electrons? Which species is the reducing agent and which species is the oxidizing agent? 10

11. Aim: How is Redox demonstrated in a voltaic cell? Objectives: 1.Students should know that there are two types of electrochemical cells and which one is spontaneous and which one requires energy, in which one is chemical energy converted to electrical energy and in which one electrical energy is converted to chemical energy. 2.Students should be able to draw and label all the parts of a voltaic cell set-up. 3.Students should know where oxidation occurs and where reduction occurs in a voltaic cell. 4.Students should be able to determine the direction and location of electron flow in a voltaic cell. 5.Students should know the purpose of the salt bridge. 6.Students should be able to identify which anode gains mass and which one loses mass and why. 11

12. 12 Electrochemical Cells: Application of Redox Reactions Electrochemical cells involve a chemical reaction and a flow of electrons. During a redox reaction there is an exchange (flow) of electrons. An electrochemical cell is used to channel and control this flow of electrons for use as electricity. There are two types of electrochemical cells: voltaic (galvanic) cells (spontaneous) in which chemical energy is converted to electrical energy and electrolytic cells (require energy) in which electrical energy is converted to chemical energy. There are two metal bars or surfaces in an electrochemical cell that can conduct electricity called electrodes. Oxidation and reduction occur at the electrodes.

13. 13 Components of Voltaic Cells Electrodes: 2 metals, one in each beaker of solution containing that metal ion. Ex. Zn metal in a beaker containing Zn 2+ ions and Cu metal in a beaker containing Cu 2+ ions. Wires connecting the two pieces of metal and attached to a voltmeter. Electrons flow through the wire and the voltmeter measures the flow. Salt bridge connecting the two beakers containing different types of ions. The purpose of the salt bridge is to provide a path for ions to flow.

14. 14 Diagram of a Voltaic (Galvanic) Cell http://www.mhhe.com/physsci/chemistry/essentialchemistry/flash/galvan5.swf

15. Quick Check What am I? 1.I am like a battery…I convert chemical energy into electrical energy. 2.In a voltaic cell, I am a metal bar where oxidation or reduction takes place. 3.In a voltaic cell, electrons flow through me from one metal bar to the other. 4.Ions flow through me from one beaker to another. 5.I measure the flow of electrons. 15

16. 16 Voltaic Cells AnodeCathode Oxidation AN OX Reduction RED CAT ( - )( + ) Higher on Table J Lower on Table J Electron Flow: Anode Cathode In a voltaic cell, a spontaneous chemical reaction (a reaction that does not require an input of energy) produces a flow of electrons. Chemical energy is converted to electrical energy. A battery is an example. Voltaic = spontaneous redox rxn

17. 17 Table J When given two metals, oxidation occurs at the metal that is ___________on Table J. In a spontaneous redox reaction, metals will replace metal ions below them on Table J. For example: Li + KCl  LiCl + K spontaneous K + LiCl  no reaction Are the following reactions spontaneous? Zn + HCl Co + FeSO 4 Rb + KCl Cu + PbSO 4

18. Quick Check 1.In a voltaic cell, a _______ _______ reaction occurs where _________energy is converted to _________energy. 2.An example of a voltaic cell is a _______. 3.In a voltaic cell, the electrode where oxidation takes place is called the _________. Reduction takes place at the _________. 4.In a voltaic cell, the charge of the anode is _____. The charge of a cathode is _____. 5.The metal that will be the anode is _______ active than the metal that will be the cathode. That means the anode will appear ______ on Table J. 6.Electrons flow from the ___________ to the ________. 7.The anode will _____ mass and the cathode will _____ mass. 18

19. 19 Voltaic Cell Diagram HW: pg. 168, Q 37-41, pg. 170-172, Q 24, 26-30

20. 20 Answers

21. Aim: How is redox demonstrated in an electrolytic cell? Objectives: 1.Students should be able to write redox half-reactions when provided with complete reactions. 2.Students should be able to identify parts of an electrolytic cell, including the energy source. 3.Students should know where oxidation occurs and where reduction occurs in an electrolytic cell. 4.Students should be able to determine the direction of electron flow in an electrolytic cell. 5.Students should be able to identify which anode gains mass and which one loses mass and why. 6.Students should understand how electrolytic cells are used for electroplating. 7.Students should be able to distinguish differences between voltaic cells and electrolytic cells. 21

22. 22 Half-Reactions Shows either the oxidation part or the reduction part. Example: Cu + Ag +1  Cu +2 + Ag Oxidation #s: ___ ___ ___ ___ Oxidation Half: Reduction Half: Balance the equation:

23. 23 Half-Reactions Practice Ni + Sn +4  Ni +2 + Sn +2 Ox. Half: Red. Half: Zn + H +  Zn +2 + H 2 Ox. Half: Red. Half: S -2 + O 2  S +4 + O -2 Ox. Half: Red. Half: HW: OB Pg. 164-165 Q 32-36, Pg. 169-170 Q 11,21,22,31,32

24. 24 Sketch a galvanic cell based on the half-reactions shown below. Al 3+ (aq) + 3e- → Al(s) Ni 2+ (aq) + 2e- ​ → Ni(s) a. Label the anode and the cathode. b. Indicate where oxidation and reduction are occurring. c. Show the direction of flow of the electrons. d. Show the direction of the movement of the ions. e. Write a balanced ionic equation for the reaction Quick Check: Half-Reactions and Voltaic Cells

25. 25 Electrolytic Cell An electrolytic cell requires an electric current to force a nonspontaneous chemical reaction to occur. Electrolytic = requires energy Used for electrolysis: alternator in a car, separate water and salts into their elements, electroplating AnodeCathode Oxidation AN OX Reduction RED CAT (+)(-) Electron Flow: Anode Cathode

26. 26 Diagram of an Electrolytic Cell

27. 27 Electroplating HW: OB Pg. 137, Q 23,25,40WB Pg. 9:33, Q 22,23,30,31

28. 28 CharacteristicVoltaicElectrolytic Use Redox Rxns? Charge of the anode Charge of the cathode Oxidation occurs at the… Reduction occurs at the… Direction of e - flow Spontaneous? Has a battery? HW: Pg. 172, Q 33-47