Science (086) — AI-generated practice question

In the solid state, ions in an ionic compound are held in a fixed, rigid lattice structure. Although ions are present, they cannot move freely, so no electrical conduction occurs.

When the compound is melted (molten state), the lattice structure breaks down. The ions (cations and anions) become free to move. These freely moving ions act as charge carriers, allowing electricity to be conducted.

Thus, electrical conduction requires mobile charged particles — solid ionic compounds have ions but they are immobile, while molten ionic compounds have freely moving ions that carry current.

Source: Chapter 3 (ionic compounds), referenced in Chapter 4, Section 4.1

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• The key concept examiners look for: ions must be free to move to conduct electricity.
• In solid state → ions are in fixed positions (lattice) → no conduction.
• In molten state → lattice breaks → ions are mobile → conduction occurs.
• This question links Chapter 3 (ionic compounds) content; the passage in Chapter 4 confirms ionic compounds "conduct electricity in solution or in the molten state."
• Avoid confusing this with covalent compounds, which don't conduct even in molten state because they form no ions.