IB Chemistry SL 2.1.3 Ionic Compounds Questions

Use exam questions to connect three-dimensional ionic lattices and ion mobility with melting, conductivity and solubility.

Exam points

Represent an ionic compound as a giant three-dimensional lattice of alternating cations and anions held by electrostatic attraction.
Explain melting, brittleness, volatility and electrical conductivity from lattice structure and whether ions are fixed or mobile in the stated state.
Use ionic-lattice structure and ion mobility to interpret solubility or compare an ionic compound with a molecular/covalent substance.

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Study 2.1.3—Ionic compounds conceptsOpen the corresponding Concept lesson for explanations, examples and exam connections.

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Periodic trends enable chemists to predict the behaviour of related compounds.

$\quad \mathrm{Na}_{2} \mathrm{O}$ and $\mathrm{SO}_{3}$ are two oxides of period 3 elements.

$\quad \mathrm{Na}_{2} \mathrm{O}$ does not conduct electricity in the solid state but it does when molten. Pure $\mathrm{SO}_{3}$ does not conduct electricity in either the solid or liquid states. Explain these facts.

$\quad \mathrm{Na}_{2} \mathrm{O}$ ionic and $\mathrm{SO}_{3}$ covalent;
$\mathrm{Na}_{2} \mathrm{O}$ has ions which are free to move in the liquid state;
$\mathrm{SO}_{3}$ has no free charged particles;

Marking guidance:

Accept "no free moving ions"/ "no delocalized electrons".

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IB Chemistry SL 2.1.3 Ionic Compounds Questions question 1