VCE Chemistry
Unit 1

Area of Study 1: How do chemical structures explain properties and reactions?

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IN THIS AoS1

Helps students understand why different materials behave the way they do by examining the structure and bonding of atoms.

Students explore how elements are organised in the periodic table, how atoms form metals, ionic compounds and covalent substances, and how these structures determine properties such as conductivity, melting point and reactivity.

  • You will be able to:

    • Describe ionic, covalent and metallic bonding.

    • Draw Lewis structures and predict molecular shapes.

    • Link structure to properties like melting point & conductivity.

    • Compare metal reactivity and explain corrosion.

    • Identify ions using precipitation reactions.

    • Use chromatography to separate and analyse mixtures.

  • 1️⃣ Elements & the Periodic Table

    • Atoms form ions, isotopes and elements.

    • Periodic trends help explain reactivity and bonding.

    2️⃣ Covalent Substances & Molecular Shapes

    Students learn:

    • How atoms share electrons.

    • Shapes of molecules (linear, bent, pyramidal, tetrahedral).

    • Why molecules are polar or non-polar.

    • How intermolecular forces affect boiling points and solubility.

    3️⃣ Metals

    Students explore:

    • Metallic bonding.

    • Why metals conduct electricity and heat.

    • Malleability and ductility.

    • Reactivity with water, oxygen and acids.

    4️⃣ Ionic Compounds

    Students learn:

    • How ions form and arrange into lattices.

    • Why ionic compounds have high melting points.

    • Why they conduct electricity when molten or in solution.

    • How to predict precipitates using solubility rules.

    5️⃣ Chromatography

    Students explore:

    • Used to separate colours, dyes, inks and pollutants.

    • Chromatography helps detect pollutants in water.

    • Designing materials with lower toxicity supports green chemistry.

  • Conceptual Questions

    1. Explain why graphite conducts electricity but diamond does not.

    2. Why does electronegativity increase across a period?

    3. Describe why ionic compounds are brittle but metals are malleable.

    4. Predict the shape and polarity of NH₃.

    5. Explain how chromatography separates substances.

    Calculation Questions

    1. Calculate the Rf value of a dye that travelled 3.5 cm while the solvent travelled 7.0 cm.

    2. Determine the ionic formula for a compound made of magnesium ions and phosphate ions.

    3. Write full and ionic equations for the reaction between AgNO₃(aq) and NaCl(aq).

    • Confusing bonding types (ionic vs covalent vs metallic).

    • Forgetting that shape determines polarity.

    • Using solubility rules incorrectly.

    • Assuming all solids conduct electricity.

    • Practice drawing Lewis structures daily.

    • Memorise common polyatomic ions.

    • Review periodic table trends visually.

    • Understand WHY properties arise, not just what they are.

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