This common misconceptions covers Common Misconceptions within Electrolysis of Molten Compounds for GCSE Chemistry. Revise Electrolysis of Molten Compounds in Electrolysis for GCSE Chemistry with 21 exam-style questions and 14 flashcards. This topic appears regularly enough that it should still be part of a steady revision cycle. It is section 7 of 11 in this topic. Use this common misconceptions to connect the idea to the wider topic before moving on to questions and flashcards.
⚠️ Common Misconceptions
Misconception 1: "Electrons flow through the electrolyte"
Electrons do NOT travel through the electrolyte. Inside the electrolyte, it is the movement of IONS that carries the current — cations move towards the cathode and anions move towards the anode. Electrons only travel through the external circuit (the wires and power supply). This is why ionic solutions/melts can carry current even though electrons cannot pass through them directly.
Misconception 2: "The products of electrolysis are always the same as the compound's formula"
The products are the individual elements from the compound, but they may combine differently. For example, electrolysiing PbBr₂ gives Pb atoms at the cathode and Br₂ molecules at the anode (not individual Br atoms) because bromine exists as a diatomic molecule under normal conditions. Always think about what form each element takes at room temperature.
Misconception 3: "Reduction happens at the anode"
Reduction (gain of electrons) happens at the CATHODE (negative electrode). The anode is where oxidation (loss of electrons) occurs. Remember OIL RIG: Oxidation Is Loss, Reduction Is Gain. And CATions go to the CAThode — they GAIN electrons there.
Practice questions for Electrolysis of Molten Compounds
Which condition is required for electrolysis to occur with an ionic compound?
State the products formed at each electrode when molten lead bromide (PbBr₂) is electrolysed.