《大学化学 Chemistry》课程PPT教学课件（英文）Chapter 11 Oxidation（氧化）and Reduction（还原）

Chapter11 Oxidation(氧化)and Reduction(还原) Acid-base reaction: Transfer of proton Oxidation and reduction transfer of electron

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

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+Cl2—+2NaC 2Na -+2Na++2e- Oxidation C|2+2e 2CI- Reduction In this reaction sodium is acting as a reducing agent(还原剂), which is any reactant that causes another reactant to be Fig 11.1 formation of sodium chloride reduced. Conversely, the chlorine causes oxidation of the sodium and so it is acting as an oxidizing agent(氧化剂)

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 + Cl2 2NaCl • 2Na 2Na+ + 2e- Oxidation • Cl2 + 2e- 2Cl- 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

Different elements have different oxidation and reduction tendencies Little endency to lose or endency gaIn electrons Na Mg to gain Cr Mn Fe co Ni cu zn/Ga electrons Tendency to ldse Ru Rh Pd Ag cd In Sn SbT electrons Re Os Pt Au Hg Ti pb Bi Po AtRn Hs M 11 123 5圆除的网四 Ce pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu ThPauNpPuam jMa No r

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

11.2 Photography works by selective oxidation and eduction O Tehimis exposed The Nm is developed Camera ler Ught tight Oxidation Br Br Oxidation 2C6H O2- 2C: H4O,+ 2e+2H* 是 eduction Ag+ Ag Reduction 2AgBr+ 2e lAg @ is hued and washed mdm如mh⑤ptm时gau The negative is dark wher Hypo solution Naro, folowed Black-and-white photography invoives a series of ouidaton-reducton reactions

11.2 Photography works by selective oxidation and reduction

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 /aso, lution usO,Mouton Use oxidation reduction reaction to produce an electric current or use an dn is aided to Cu a eath electric current to Nel reacion produce an oxidation-reduction reaction Fig 11.7 the salt bridge completes the electric circuit

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

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

• 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

Disposable batteries Reduction 2NH++2e 2NH +H 2 Fig 11.8 a common Carbon dry-cell battery with a Electrons(e-) (cathode) graphite rod Light bulb Electrolyte paste immersed in a paste of ammonium chloride, manganese mangan dioxide mixture|本 dioxide, and zinc chloride Zinc negative Electrons(e-) Electrons(e-) Oxidation Zn Zn2++2e Zncl2(ag)+ 2NH3(g)-+Zn(NH3)2Cl2 (s) 2Mno2(S)+H2(g)一→Mn2O3(s)+H2O() Electrode(电极) cathode(阳极): Where chemicals are reduced Anode(阴极 Where chemicals are oxidized

Disposable batteries 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. Fig 11.8 a common dry-cell battery with a graphite rod immersed in a paste of ammonium chloride, manganese dioxide, and zinc chloride Reduction 2NH4 ++2e- 2NH3+H2 Oxidation Zn Zn2++2e-

Alkaline battery 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(+2e-OⅪ dation 2Mno2(s)+ 2e--Mn2O3 (s)+ 20H-(ag) Reduction

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

Rechargeable battery engine Fig 11.10 (a)electrical energy from the battery forces the starter motor to start the engine.(b) the combustion of fuel Oxidation Pb +S0,2--PbSo,+ 2e keeps the engine Reduction of elemental Pb to pb+ running and provides energy to spin the Reduction Pbo,+ So4+ 4H++2e- PbSo,+ 2H,O alternator, which Oxidation of elemental pb4+ to pb2+ recharges the battery. Note that the battery has a reversed cathode- engine anode orientation during recharging alternator Oxidation PbSO4+ 2e>Pb+sO Reduction of elemental Pb2+ to pb Reduction Pbso pb4+4+ 2H20>PbO2+ SO4 4H+ 2e Oxidation of elemental pb2+ to pbt

Rechargeable battery engine Oxidation Pb + SO4 2- → 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 + SO4 2- Reduction of elemental Pb2+ to pb Reduction PbSO pb4+ 4 + 2H2O → PbO2 + SO4 - + 4H+ + 2e Oxidation of elemental pb2+ to pb4+ Fig 11.10 (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

Fuel cells(燃料电池) are high! efficient sources of electrIcal energy Oxd:→4Ho4 e:Fuel cell Reduction 4e +0+21一→4oH Electron Flow Load Hydrog xyge ●●0 Hydroxyl Wate lons Anode Cathode Fig 11.11 the Electrolyte drogen Porous graphite electrodes oxygen fuel cell

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