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Oxides of Period 3 – acidic, basic and amphoteric (virtual lab)

ChemistryInorganic ChemistryAges 15–16Virtual lab

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A virtual lab: burn sodium, magnesium, aluminium, silicon, phosphorus and sulfur in oxygen, add each oxide to water with universal indicator, then test it with hydrochloric acid and sodium hydroxide. A results table, balanced equations and a trend chart show basic Na₂O and MgO, amphoteric Al₂O₃ (and ZnO for comparison) and acidic SiO₂, P₄O₁₀ and SO₂, linked to the change from ionic to giant covalent to simple molecular structures.

Lesson: Period 3 elements and their oxides: reactions with oxygen and water, acid–base character and bonding

What it shows

Across Period 3 the oxides change from basic to acidic. Sodium and magnesium oxides are ionic lattices that react with water to give alkaline solutions and neutralise acids. Aluminium oxide is ionic with some covalent character and is amphoteric: insoluble in water, it reacts with both acids and alkalis, like zinc oxide. Silicon dioxide is a giant covalent solid, insoluble in water but acidic towards hot alkali. Phosphorus and sulfur oxides are simple molecular and form acidic solutions. The melting points follow the bonding: very high for the ionic and giant covalent oxides, low for the molecular ones.

How to use

Choose an Element, then press 1. Burn in oxygen. Next press 2. Add to water + indicator and read the pH on the universal indicator chart, then 3. Test with HCl and 4. Test with NaOH. Run all steps does the four steps in order. Each result enters the table. Repeat for the other elements, then open Period 3 trend. Reset clears the table.

Parameters you can change

  • Element Sodium (Na), Magnesium (Mg), Aluminium (Al), Silicon (Si), Phosphorus (P), Sulfur (S), Zinc (Zn), for comparison
  • Opening view Lab bench, Period 3 trend

Questions to explore

  1. Why does universal indicator stay green with aluminium oxide, although the oxide reacts with both acid and alkali?
  2. How does the pH of the oxide solutions change from sodium to sulfur, and why?
  3. Why does silicon dioxide have a much higher melting point than phosphorus(V) oxide?

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