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Year 9–10 · Year 9–10 Science

Year 9–10 Science — Chemistry

Year 9–10 chemistry covers atomic structure, chemical reactions and the properties of acids and bases. These topics are the direct precursor to VCE Chemistry Units 1 and 2, and students who understand balancing equations and electron configuration before Year 11 have a significant head start.

Key Concepts & Formulas

  • Atom: nucleus (protons + neutrons) surrounded by electrons in shells

  • Atomic number = protons; mass number = protons + neutrons; isotopes have the same atomic number, different mass numbers

  • Electron configuration (shells): 2 in first shell, 8 in second, 8 in third (for elements up to Ca)

  • Valence electrons: electrons in the outermost shell; determine an element's chemical behaviour

  • Ionic compounds: formed by transfer of electrons between metals and non-metals; named metal first, then non-metal with -ide suffix

  • Covalent molecules: formed by sharing electrons between non-metals

  • Chemical equation: reactants → products; must be balanced (same number of each atom on both sides)

  • Types of reactions: synthesis (A + B → AB), decomposition (AB → A + B), displacement (A + BC → AC + B), combustion (fuel + O₂ → CO₂ + H₂O)

  • Acids: donate H⁺ ions in solution; pH < 7; react with metals to produce hydrogen gas and a salt

  • Bases: accept H⁺ ions; pH > 7; react with acids in neutralisation: acid + base → salt + water

Practice Questions

4 questions

Attempt each question before reading the hint. These are styled to match school assessment format.

Q1.Balance the equation: ___ Fe + ___ O₂ → ___ Fe₂O₃.

2 marks

Q2.Write the electron configuration for Chlorine (atomic number 17) and explain why it typically forms an ion with a −1 charge.

3 marks

Q3.Classify each reaction type: (a) 2H₂ + O₂ → 2H₂O (b) CaCO₃ → CaO + CO₂ (c) Zn + 2HCl → ZnCl₂ + H₂.

3 marks

Q4.A solution has pH 3. Is it acidic, neutral or basic? Describe the colour change if universal indicator is added.

2 marks

Common Mistakes to Avoid

These are the errors that students most frequently make in Chemistry — and that examiners are specifically watching for.

  • Changing the subscripts when balancing equations — only change coefficients (numbers in front); never alter subscripts

  • Forgetting that ionic compound names end in -ide: NaCl = sodium chloride, not sodium chlor

  • Thinking acids are always dangerous liquids — many foods are acidic (vinegar, lemon juice) and safe to consume

  • Confusing pH: pH < 7 = acidic, pH 7 = neutral, pH > 7 = basic (alkaline)

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