AQA · Chemistry · 8462
GCSE Chemistry: Electrolysis of molten ionic compounds
Chemical changes · AQA GCSE Chemistry (8462), specification point 4.4.3.2. Cards are generated from the exam board's own specification for "Electrolysis of molten ionic compounds", and every card links back to the page it came from. Specification © AQA — used with attribution.
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Which product forms at the cathode when molten lead bromide is electrolysed?
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Lead (the metal). Pb²⁺ ions gain electrons at the negative cathode.
Which product forms at the anode when molten lead bromide is electrolysed?
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Bromine (the non-metal). Br⁻ ions lose electrons at the positive anode.
In electrolysis of a molten ionic compound, where is the metal produced?
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At the cathode (negative electrode), because positive metal ions are attracted there and gain electrons.
In electrolysis of a molten ionic compound, where is the non-metal produced?
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At the anode (positive electrode), because negative non-metal ions are attracted there and lose electrons.
Molten ionic compounds are electrolysed using ? electrodes so the electrodes do not react with the products.
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inert
Why must an ionic compound be molten (or dissolved) for electrolysis to work?
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Only when molten or dissolved are the ions free to move and carry charge to the electrodes; in a solid they are fixed in the lattice.
What are the products of electrolysing molten zinc chloride?
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Zinc at the cathode and chlorine at the anode.
Which compound is a safer alternative to lead bromide for practical electrolysis of a molten salt?
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Anhydrous zinc chloride (avoids toxic lead and bromine).
Give the half equation for the cathode reaction in molten lead bromide electrolysis.
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Pb²⁺ + 2e⁻ → Pb
Give the half equation for the anode reaction in molten lead bromide electrolysis.
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2Br⁻ → Br₂ + 2e⁻
What is a binary ionic compound?
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An ionic compound made of only two elements — a metal and a non-metal (e.g. PbBr₂, ZnCl₂).
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