introduction electrolysis

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Ionic compounds 
Can conduct electricity when molten or dissolved in water
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Solid ionic compounds cannot conduct electricity because the ions are locked in place and not free to move
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Molten or dissolved ionic compounds 
Ions are free to move, so they can conduct electricity
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Electrolytes 
Liquids or solutions that can conduct electricity
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Electrolysis of molten ionic compound (e.g. lead bromide)
1. Positive lead ions attracted to negative electrode (cathode)
2. Lead ions gain 2 electrons to form lead atoms (reduction)
3. Negative bromide ions attracted to positive electrode (anode)
4. Bromide ions lose 1 electron to form bromine atoms (oxidation)
5. Bromine atoms pair to form bromine molecules
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introduction electrolysis

Cards (5)

4.3 Electrolysis

3.3 Electrolysis

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4.3 Electrolysis

4.3.1 The process of electrolysis

9.7 Electrolysis and Faraday's Laws

4.3.2 Electrolysis of molten ionic compounds

14.3.1 Electrolysis of Aqueous Solutions

4.3.1 The process of electrolysis

4.3.3 Using electrolysis to extract metals

4.3.4 Electrolysis of aqueous solutions

14.3.2 Faraday's Laws of Electrolysis

7.1 Introduction to Equilibrium

C7.1.3 PAG3: Electrolysis

2.4.1 Introduction to Mental Health

5.5 Introduction to Reaction Mechanisms

4.3.2 Electrolysis of molten ionic compounds

1. Introduction

4.10 Introduction to the Binomial Distribution

2.1 Introduction to the Spanish Renaissance