Curriculum

VCE Chemistry Units 1 and 2 - 8 Practice Pack

Getting Started - VCE CHEM U12 - 8 Practice Packs

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Year 11 Guide - VCE CHEM U12 - 8 Practice Packs

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Unit 1 Content: How Can the Diversity of Materials Be Explained?

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Unit 2 Content: What Makes Water Such a Unique Chemical?

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Exam Technique - VCE Chemistry Units 1 and 2 - 8 Practice Pack

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Advanced Depth - VCE Chemistry Units 1 and 2 - 8 Practice Pack

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Examiner Intelligence - VCE Chemistry Units 1 and 2 - 8 Practice Pack

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Practice Exam 1 of 8 - VCE CHEM U12

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Practice Exam 2 of 8 - VCE CHEM U12

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Practice Exam 3 of 8 - VCE CHEM U12

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Practice Exam 4 of 8 - VCE CHEM U12

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Practice Exam 5 of 8 - VCE CHEM U12

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Practice Exam 6 of 8 - VCE CHEM U12

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Practice Exam 7 of 8 - VCE CHEM U12

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Practice Exam 8 of 8 - VCE CHEM U12

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After the Exam - VCE CHEM U12 - 8 Practice Packs

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Text lesson

VCE-CHEM-U12 4.1 📋 Practice Exam 1: Question Paper

Practice Exam 1

VCE Chemistry | Atomic Structure, Periodic Table, Chemical Bonding Naming

✎ Complete ALL questions on paper before opening the Model Answers lesson. No notes. Aim for 1 minute per mark.

SHORT ANSWER

Question 1 (4 marks)

Write the full electron configuration of iron (Fe, Z=26) and identify which subshell is incompletely filled.

✎ Write your answer on paper

Question 2 (4 marks)

Draw the Lewis structure of SO₂ and explain its shape using VSEPR theory.

✎ Write your answer on paper

Question 3 (4 marks)

Explain why the boiling point of HF (19.5°C) is much higher than HCl (-85°C) despite HCl having higher molar mass.

✎ Write your answer on paper

Question 4 (4 marks)

Name the following compounds: (i) FeCl₃ (ii) N₂O₅ (iii) Ca(OH)₂ (iv) HNO₃

✎ Write your answer on paper

Question 5 (4 marks)

The first ionisation energies (kJ/mol) of elements across Period 3 are: Na 496, Mg 738, Al 577, Si 786, P 1012, S 1000, Cl 1251, Ar 1521.
Explain the general trend and account for the anomaly at Al and S.

✎ Write your answer on paper

Question 6 (4 marks)

Calculate the number of protons, neutrons, and electrons in ⁸⁰Br⁻.

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Question 7 (4 marks)

Classify each bond as ionic, polar covalent, or non-polar covalent and explain: (i) Cl–Cl (ii) Na–Cl (iii) O–H (iv) C–H

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Question 8 (4 marks)

Write structural formulas and IUPAC names for the three structural isomers with molecular formula C₃H₈O that are alcohols.

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EXTENDED RESPONSE

Extended Response 1: Periodic Trends Electron Configuration

Question 9 (3 marks)

Extended Response 1: Periodic Trends Electron Configuration (a)
Explain the trend in atomic radius across Period 3 (Na to Ar) and down Group 1 (Li to Cs).

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Extended Response 1: Periodic Trends Electron Configuration

Question 10 (3 marks)

Extended Response 1: Periodic Trends Electron Configuration (b)
Explain why the second ionisation energy of Na is much greater than its first, but the increase from 1st to 2nd IE for Mg is less dramatic.

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Extended Response 1: Periodic Trends Electron Configuration

Question 11 (3 marks)

Extended Response 1: Periodic Trends Electron Configuration (c)
Arrange the following in order of increasing ionic radius and justify: Na⁺, Mg²⁺, Al³⁺, O²⁻, F⁻.

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Extended Response 2: Bonding Properties

Question 12 (4 marks)

Extended Response 2: Bonding Properties (a)
Compare the melting points of NaCl (801°C), SiO₂ (1710°C), Cl₂ (-101°C) and Na (98°C). Explain each in terms of bonding and structure.

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Extended Response 2: Bonding Properties

Question 13 (3 marks)

Extended Response 2: Bonding Properties (b)
Explain why CO₂ is a gas at room temperature but SiO₂ is a solid, despite both being oxides of Group 14 elements.

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✓ Finished? Open the next lesson – Model Answers – to mark your work.