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Chapter 11 Oxidation (氧化) and Reduction (还原)

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Presentation on theme: "Chapter 11 Oxidation (氧化) and Reduction (还原)"— Presentation transcript:

1 Chapter 11 Oxidation (氧化) and Reduction (还原)
Acid-base reaction: Transfer of proton Oxidation and reduction: transfer of electron

2 Fig 11.1 formation of sodium chloride
11.1 Oxidation is the loss of electrons and reduction is the gain of electrons Oxidation is the process whereby a reactant loses one or more electrons. Reduction is the opposite process whereby a reactant gains one or more electrons. Oxidation and reduction are complementary and simultaneous processes. 2Na + Cl NaCl 2Na Na+ + 2e- Oxidation Cl2 + 2e Cl Reduction In this reaction, sodium is acting as a reducing agent (还原剂), which is any reactant that causes another reactant to be reduced. Conversely, the chlorine causes oxidation of the sodium and so it is acting as an oxidizing agent (氧化剂). Fig 11.1 formation of sodium chloride

3 Different elements have different oxidation and reduction tendencies
Little tendency to lose or gain electrons Tendency to gain electrons Tendency to lose electrons

4 11.2 Photography works by selective oxidation and reduction

5 11.3 The energy of flowing electrons can be harnessed
Electrochemistry (电化学) is the study of the relationship between electrical energy and chemical change: Use oxidation-reduction reaction to produce an electric current or use an electric current to produce an oxidation-reduction reaction. Fig 11.7 the salt bridge completes the electric circuit

6 The electricity of a battery comes from oxidation-reduction reactions
A voltaic cell, which is an all-in-one, self-contained unit, is called a battery. Batteries are either disposable or rechargeable. Principle of batteries: Two materials that oxidize and reduce each other are connected by a medium through which ions travel to balance an external flow of electrons.

7 Disposable batteries ZnCl2 (ag) + 2NH3 (g) Zn(NH3)2Cl2 (s)
Reduction 2NH4++2e NH3+H2 Fig 11.8 a common dry-cell battery with a graphite rod immersed in a paste of ammonium chloride, manganese dioxide, and zinc chloride Oxidation Zn Zn2++2e- ZnCl2 (ag) + 2NH3 (g) Zn(NH3)2Cl2 (s) 2MnO2 (s) + H2 (g) Mn2O3 (s) + H2O (l) Electrode (电极) cathode (阳极): where chemicals are reduced. Anode (阴极): where chemicals are oxidized.

8 Alkaline battery Zn (s) + 2OH- (aq) ZnO (s) + H2O (l) +2 e- Oxidation
Fig11.19 Alkaline batteries last a lot longer than dry-cell batteries and give a steadier voltage, but they are expensive Zn (s) + 2OH- (aq) ZnO (s) + H2O (l) +2 e- Oxidation 2MnO2 (s) + 2e Mn2O3 (s) + 2OH- (aq) Reduction

9 Rechargeable battery engine
Fig (a) electrical energy from the battery forces the starter motor to start the engine. (b) the combustion of fuel keeps the engine running and provides energy to spin the alternator, which recharges the battery. Note that the battery has a reversed cathode-anode orientation during recharging Oxidation Pb + SO42-  PbSO4 + 2e Reduction of elemental Pb to pb2+ Reduction PbO2 + SO4- + 4H+ + 2e  PbSO4 + 2H2O Oxidation of elemental pb4+ to pb2+ engine alternator Oxidation PbSO4 + 2e  Pb + SO42- Reduction of elemental Pb2+ to pb Reduction PbSO pb H2O  PbO2 + SO4- + 4H+ + 2e Oxidation of elemental pb2+ to pb4+

10 Fuel cells (燃料电池) are highly efficient sources of electrical energy
Oxidation 2H2+4OH H2O+4e- Reduction 4e-+O2+2H2O OH- Fig11.11 the hydrogen-oxygen fuel cell Porous graphite electrodes

11 Fig 11.12 because this bus is powered by a fuel cell, its tail pipe emits mostly water vapor

12 Electrical energy can produce chemical change
Electrolysis (电解) is the use of electrical energy to produce chemical change. Fig the electrolysis of water produces hydrogen gas and oxygen gas in a 2:1ratio by volume, which is in accordance with the chemical formula for water:H2O. For this process to work, ions must be dissolved in the water so that the electricity can be conducted between the electrodes Electrical energy + 2H2O  2H2 (g) + O2

13 Oxidation 2AlOF32-+6F-+C 2AlF63-+CO2+4e-
Figure 11.15 The melting point of aluminum oxide(2030℃) is too high for it to be efficiently electrolyzed to aluminum metal. When the oxide is mixed with the mineral cryolite. The melting point of the oxide drops to a more reasonable 980℃. A strong electric current passed through the molten aluminum oxide-cryolite mixture generates aluminum metal at the cathode, where aluminum ions pich up electrons and so are reduced to elemental aluminum Oxidation 2AlOF32-+6F-+C AlF63-+CO2+4e- Molten Al2O3+Na3AlF6 mixture Power source cathode Reduction AlF63-+3e Al +6F-

14 11.4 Oxygen is responsible for corrosion and combustion
Iron to rust: 4Fe + 3O2 +3H2O    2Fe2O3 .3H2O A thin layer of protective layer was formed during the oxidation of aluminum. Since aluminum has higher tendency to be oxidized, a thin layer of aluminum on iron can protect iron from corresion. Figure 11.20 As electrons flow into the hubcap and give it a negative charge, positively charged chromiun ions move from the solution to the hubcap and are reduced to chromium metal, which deposits as a coating on the hubcap. The solution is kept supplied with ions as chromium atoms in the cathode are oxidized to Cr2+ ions Cathodic protection Electroplating

15 Combustion is also an oxidation-reduction reaction.
Many well “designed” oxidation-reduction reactions happen in our bodies.

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