How metals and non-metals swap electrons to make charged ions, how those ions lock into a giant lattice, and how to build any ionic formula.
Theme · StructureStructure 2.1
This is the Standard Level lesson, covering S2.1.1–S2.1.3. Taking Chemistry at Higher Level? The HL version adds lattice enthalpy — how ionic charge and radius set the strength of ionic bonding.
👆 Toggle the electron transfer · build formulae · click each property
1. Making ions by electron transfer S2.1.1
When a metal reacts with a non-metal, electrons transfer from the metal to the non-metal. The metal becomes a positive cation, the non-metal a negative anion — both reaching a full, stable outer shell. Predict the charge from the group: Group 1 → 1+, Group 2 → 2+, Group 13 → 3+; Group 15 → 3−, Group 16 → 2−, Group 17 → 1−.
Before: neutral atomsSodium has 1 outer electron; chlorine has 7. Toggle to transfer that single electron.
2. Build an ionic formula S2.1.2
An ionic compound is neutral overall, so the positive and negative charges must cancel. Pick a cation and an anion — the builder balances the charges for you (and adds brackets around polyatomic ions when there's more than one).
Ionic formula builder
NaClNa⁺ + Cl⁻ → charges balance 1 : 1
The seven polyatomic ions you must know: ammonium NH₄⁺, hydroxide OH⁻, nitrate NO₃⁻, hydrogencarbonate HCO₃⁻, carbonate CO₃²⁻, sulfate SO₄²⁻, phosphate PO₄³⁻.
3. The giant ionic lattice & properties S2.1.3
Ionic compounds don't exist as molecules — they form a giant 3D lattice of alternating cations and anions, held by strong electrostatic attractions in all directions. We write them with the empirical formula (the simplest ratio). Click a property to see how the lattice explains it.
Going to HL? The HL lesson adds lattice enthalpy: a measure of ionic bond strength that increases with higher ionic charge and smaller ionic radius (so MgO ≫ NaCl). → Open the HL version
Common mistakes examiners see
What charge does a Group 16 (oxygen group) element form?✗ 6−.✓ 2− — it gains 2 electrons to fill its outer shell (e.g. O²⁻, S²⁻).
Why don't solid ionic compounds conduct electricity?✗ They have no charged particles.✓ They DO have ions, but the ions are fixed in the lattice and can't move. When molten or dissolved, the ions are free to move and carry charge.
What is the formula of calcium nitrate?✗ CaNO₃.✓ Ca(NO₃)₂ — Ca²⁺ needs two NO₃⁻ ions to balance, so the polyatomic ion is bracketed and subscripted.
Are ionic compounds made of molecules?✗ Yes, like NaCl molecules.✓ No — they are giant lattices. The formula (e.g. NaCl) is the empirical ratio, not a molecule.