Electrolysis 4.0 / 5 based on 3 ratings ? ChemistryThe process of electrolysis, Using electrolysis to extract metals, Electrolysis of aqueous solutions and Representations of reactions at electrodes as half equationsGCSEAQA Created by: holly.preston12345Created on: 20-12-18 13:11 The process of electrolysis The process of electrolysis 1 of 25 What is electrolysis? Splitting up using electricity 2 of 25 What happens when an ionic compound is melted or dissolved in water? The ions are free to move- these are then able to conduct electricity and are called electrolytes 3 of 25 What does passing an electric current though electrolytes cause? Ions to move to the electrodes 4 of 25 What are the two types of electrodes? Anode, Cathode 5 of 25 What is an anode? Postive electrode 6 of 25 What is a cathode? Negative electrode 7 of 25 Where do the positively charged ions go? To the negative electrode 8 of 25 Where do the negatively charged ions go? To the positive electrode (anode) 9 of 25 Electrolysis of molten ionic compounds Electrolysis of molten ionic compounds 10 of 25 What happens when when a simple ionic compound (lead bromide) is electrolyzed in the molten state using inert electrodes? The metal (lead) is produced at the cathode and the non- metal (bromine) is produced at the anode 11 of 25 Extracting metals using electrolysis Extracting metals using electrolysis 12 of 25 How can metals be extracted from molten compounds? Using electrolysis 13 of 25 When is electrolysis used? used when the metal is too reactive to be extracted by reduction with carbon 14 of 25 Why is the process (electrolysis) expensive? Due to large amounts of energy needed to produce the electrical current 15 of 25 Give an example of electrolysis? Aluminium 16 of 25 Electrolysis of aqueous solutions Electrolysis of aqueous solutions 17 of 25 What will be produced at the negative electrode? Metal will be produced on the electrode if it is less reactive than hydrogen or Hydrogen will be produced if the metal is more reactive than hydrogen 18 of 25 What is formed at the positive electrode? Oxygen is produced at positive electrode unless the solution contains halide ions 19 of 25 When do the ions discharge ? When an aqueous solution is electrolyzed using inert electrodes 20 of 25 Representations or reactions at electrodes as half equations Representations or reactions at electrodes as half equations 21 of 25 What doing using inert electrodes depends on? Using inert electrodes depend on the relative reactivity of the elements involved 22 of 25 What happens at the cathode (negative electrode)? Positively charged ions gain electrons and so the reaction are REDUCTIONS 23 of 25 What happens at the anode (positive electrode)? Negatively charged ions lose electron so the reaction are OXIDATIONS 24 of 25 How can reactions at electrodes be represented by? Half equations 25 of 25
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