3. Solids cannot conduct electricity because the ions cannot move freely 4. Electrolytic cell
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1 Chapter 6 Electrochemistry (Credits to Thennarasu Pannirselvam) Page 1 of Electrolysis : Process where molten or aqueous state compounds are broken down into their constitute elements by passing electricity through them 2. Electrolytic cell : A cell that used electrical energy to produce chemical energy Electrolyte Substance that conducts electricity in a molten (melted) or aqueous state. Non-electrolyte Substance that cannot conduct electricity in a molten or aqueous state Ionic Compounds : HCL, NaOH Covalent Compounds : Alcohol, naphthalene 3. Solids cannot conduct electricity because the ions cannot move freely 4. Electrolytic cell i) Anode : Positive Electrode, Attracts Anions (Negatively Charged Ions) ii) Cathode : Negative Electrode, Attracts Cations (Positively Charged Ions) iii) Decompose & Discharge Method
2 Chapter 6 Electrochemistry (Credits to Thennarasu Pannirselvam) Page 2 of Electrochemical Series (ECS) K + F - Na + SO 4 Ca 2+ - NO 3 Mg 2+ Cl - Al 3+ Br - Zn 2+ I - Fe 2+ Easier to discharge Sn 2+ Pb 2+ Ag + 6. Electrolysis Products (Common Observations) Anode Cathode Product Observation Product Observation Chlorine Gas,Cl 2 Greenish-yellow gas Almost all Metals Grey solid deposited bubbles released Bromine Gas, Br 2 Brown vapour released Copper metal Brown solid deposited Iodine Gas, I 2 Purple vapour released Hydrogen Gas, H 2 Colourless gas bubbles released Oxygen Gas, O 2 Colourless gas bubbles released
3 7. Chapter 6 Electrochemistry (Credits to Thennarasu Pannirselvam) Page 3 of 10 Electrolyte Ions Present Anode Cathode Molten Lead (II) Bromide, PbBr 2 Pb 2+ Br - Br - Br - 2Br - Br 2 + 2e - Brown gas released Pb 2+ Pb 2+ Pb e - Pb Grey solid deposited Copper (II) Sulphate Solution, CuSO 4 SO 4 SO 4, OH Hydroxide is lower than Sulphate in the ECS 4OH 2H 20 + O 2 + 4e - Colourless gas bubbles that light up glowing wooden splinter are released, is lower than in the ECS + 2e - Cu Brown solid deposited Observation of electrolyte (CuSO 4) : Blue colour of CuSO 4 turns colourless Concentration of decreases
4 Chapter 6 Electrochemistry (Credits to Thennarasu Pannirselvam) Page 4 of 10 Electrolyte Ions Present Anode Cathode Potassium Bromide Solution, KBr K + Br Br, Hydroxide is lower than Bromide in the ECS 4 2H 2O + O 2 + 4e - Colourless gas bubbles that light up glowing wooden splinter are released K +, Hydrogen is lower than Potassium in the ECS 2 + 2e - H 2 Colourless gas bubbles are released Apply concentration factor if : Concentration 1 mol dm -3 with Cl -, Br - and I - present 1 mol dm -3 of Sodium Chloride, NaCl Cl, Na +, Na + Cl Cl - Concentration of Cl is higher 2Cl - + 2e - Cl 2 Greenish-yellow has bubbles are released Hydrogen is lower than Sodium in the ECS 2 + 2e - H 2 Colourless gas bubbles are released
5 Chapter 6 Electrochemistry (Credits to Thennarasu Pannirselvam) Page 5 of 10 Apply type of electrode factor when Carbon electrodes are not used Copper (II) Sulphate Solution, CuSO 4 SO 4 SO 4, Cu + 2e - The copper electrode becomes thinner, is lower than in the ECS + 2e - Cu Brown solid deposited Silver Nitrate Solution, AgNO 3 Ag + - NO 3 NO 3-, Ag Ag + + e - The silver electrode becomes thinner Ag +, Ag + Ag + is lower than in the ECS Ag + + e - Ag Grey solid deposited
6 8. Uses of electrolysis Chapter 6 Electrochemistry (Credits to Thennarasu Pannirselvam) Page 6 of Extraction of metals 2. Purification of metals 3. Electroplating of metals List of ions : Al 3+, O List of ions :,,, SO 4 List of ions : Al 3+, O,, Anode : O Cathode : Al 3+ Anode : SO 4, Cathode :, Anode : O, Cathode : Al 3+, ½ equation : ½ equation : ½ equation : 2O O 2 + 4e - Al e - Al Cu + 2e - + 2e - Cu Al Al e - Al e - Al Note : 1. Cryolite lowers melting point of Al 2O 3 2. The C electrodes will corrode and has to be replaced from time to time because O 2 gas will react with C electrode to form CO 2 3. Aluminium metal will sink at the bottom and will be collected Impure copper becomes thinner Pure Copper becomes thicker Observation for electrolyte (CuSO 4) : Blue colour of CuSO 4 remains the same Concentration of remains the same Aluminium electrode become thinner Grey solid deposited on the iron spoon Purpose - to make object more attractive and resistant Condition for good quality of electroplating : i) Small electric current ii) Plated object must be turned slowly
7 4. Voltaic Cell Chapter 6 Electrochemistry (Credits to Thennarasu Pannirselvam) Page 7 of 10 K + Na + Ca 2+ Mg 2+ Al 3+ Zn 2+ Fe 2+ - More Electropositive - Easy to Release Electron - Act as a Negative Terminal Sn 2+ Pb 2+ Ag + Simple Voltaic Cell Plate Magnesium, Mg Copper, Cu Half-Equation Mg Mg e - + 2e - Cu Electro positivity Magnesium is more electropositive Overall Ionic Equation Mg + Mg 2+ + Cu Magnesium plate will become thinner Cu plate will become thicker Voltmeter Observation Voltmeter needle deflects because of the freely moving electrons producing current and voltage Electrolyte (CuSO 4) Solution changes from blue to colourless Terminal Negative Positive Energy Change Chemical Energy Electrical Energy
8 Danielle Cell Chapter 6 Electrochemistry (Credits to Thennarasu Pannirselvam) Page 8 of 10 Plate Zinc, Zn Copper, Cu Half-Equation Zn Zn e - + 2e - Cu Electro positivity Overall Ionic Equation Observation Zinc becomes thinner Zn is more electropositive Zn + Zn 2+ + Cu Electrodes Voltmeter Copper becomes thicker Voltmeter needle deflects because of the freely moving electrons producing current and voltage Electrolyte (CuSO 4) Solution changes from blue to colourless Terminal Negative Positive Energy Change Function of Salt Bridge/ Porous Pot i) To separate the electrolytes Examples of Salt Bridge i) NaCl ii) ii) To facilitate (allow) the movement of ions KCl Chemical Energy Electrical Energy
9 5. Voltmeter reading between two metals in a voltaic cell Chapter 6 Electrochemistry (Credits to Thennarasu Pannirselvam) Page 9 of 10 a. A potential difference (voltmeter reading) will be produced when two different metals are used in a voltaic cell b. The further the metal from another metal in the ECS, the higher the reading/ potential difference. Potential Differences between voltaic cells Pairs of metals Positive terminal Negative Terminal Voltage (v) Mg/Cu Cu Mg 2.7 Zn/Cu Cu Zn 1.1 Fe/Cu Cu Fe 0.8 Al/Cu Cu Al 2.0 Pb/Cu Cu Pb 0.5
10 Chapter 6 Electrochemistry (Credits to Thennarasu Pannirselvam) Page 10 of 10 A more electropositive metal can displace a less electropositive metal from its salt solution i) Zn metal dissolves ii) Brown Solid formed iii) Blue colour of Cu(NO 3) 2 turns colourless Explanation : Zinc, Zn is more electropositive and placed higher than Copper, Cu in the ECS. So, Zinc can displace Copper from Copper (II) Nitrate, i) The lead metal remains as a solid ii) No displacement of metal occurred Lead, Pb is less electropositive and placed lower than Magnesium, Mg in the ECS. So, Lead cannot displace Magnesium from Magnesium Cu(NO 3) 2 Sulphate, MgSO 4 Chemical Equation : Zn + Cu(NO 3) 2 Zn(NO 3) 2 + Cu No reaction Characteristics Electrolytic Cell Voltaic Cell Energy Change Electrical Energy Chemical Energy Chemical Energy Electrical Energy Electrodes Same Different Terminals Anode +, Cathode - Cathode more electropositive, anode less electropositive Electron Flow Anode Cathode Cathode Anode
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