Common Misconceptions
Part of Ionic Compounds — GCSE Chemistry
This common misconceptions covers Common Misconceptions within Ionic Compounds for GCSE Chemistry. Revise Ionic Compounds in Bonding & Structure for GCSE Chemistry with 20 exam-style questions and 20 flashcards. This is a high-frequency topic, so it is worth revising until the explanation feels precise and repeatable. It is section 8 of 12 in this topic. Use this common misconceptions to connect the idea to the wider topic before moving on to questions and flashcards.
Topic position
Section 8 of 12
Practice
20 questions
Recall
20 flashcards
⚠️ Common Misconceptions
Misconception 1: "Ionic compounds conduct electricity because they have ions"
Having ions is necessary but not sufficient. The ions must be FREE TO MOVE. Solid ionic compounds have ions arranged in a fixed lattice — they cannot move, so no conduction occurs. It is only when the ionic compound is melted or dissolved that ions become mobile and conduction is possible. Always include "free to move" in your answer.
Misconception 2: "Ionic compounds are made of molecules"
Ionic compounds do NOT contain molecules. A molecule is a group of atoms held together by covalent bonds with a fixed composition. Ionic compounds form giant lattices with no set boundary or fixed unit — the structure extends indefinitely. The formula (e.g., NaCl) represents the simplest ratio of ions, not a discrete molecule.
Misconception 3: "Ionic bonds break when the compound conducts electricity"
The ionic bonds (electrostatic attractions) are not broken by the passage of electricity — the compound is simply providing a path for charges to move through. However, at the electrodes, chemical reactions DO occur (electrolysis), so the compound is changed chemically. The conduction itself does not break the ionic bonds throughout the bulk of the liquid.