Common Misconceptions

⚠️ 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.