IB Chemistry SL 2.1.3 Ionic Compounds Question Bank

Practise IB Chemistry SL 2.1.3 by linking three-dimensional ionic lattices to melting behaviour, conductivity in solids or melts, solubility and brittleness.

Exam points

compare ionic attraction using ionic charge and radius within a lattice
explain conductivity by whether charged ions are fixed or mobile in the state given
deduce an ionic structure from a combination of melting, solubility and conductivity data

[Maximum number: 3]

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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2.1.3—Ionic compounds question 1