Lesson 3.2.1.2

3.2.1.2 Physical properties of Period 3 elements Quiz: AQA Chemistry, Unit 2

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 3.2.1.2, Physical properties of Period 3 elements: 20 multiple choice questions for the AQA Chemistry (7405), Unit 2: Inorganic chemistry, written with Revision Ninja.

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The 20 questions

  1. What is the trend in atomic radius across Period 3 from sodium to chlorine?

    • Remains constant
    • Decreases
    • Increases then decreases
    • Increases

  2. Which factor causes atomic radius to decrease across Period 3?

    • Increasing electron shielding
    • Increasing shell number
    • Decreasing nuclear charge
    • Increasing nuclear charge

  3. Which Period 3 element has the largest atomic radius?

    • Sodium
    • Aluminium
    • Chlorine
    • Magnesium

  4. What is the general trend in first ionisation energy across Period 3?

    • Continuous decrease
    • General increase
    • Remains constant
    • General decrease

  5. Why is the first ionisation energy of magnesium higher than that of sodium?

    • Higher energy subshell
    • Greater electron shielding
    • Higher nuclear charge
    • Lower nuclear charge

  6. Why is the first ionisation energy of aluminium lower than that of magnesium?

    • Electron in 3s
    • Lower nuclear charge
    • Higher nuclear charge
    • Electron in 3p

  7. Why is the first ionisation energy of sulfur lower than that of phosphorus?

    • Electron pair repulsion
    • Outer electron in 3s
    • Greater electron shielding
    • Higher nuclear charge

  8. Which Period 3 element has the highest melting point?

    • Aluminium
    • Sodium
    • Silicon
    • Sulfur

  9. Why does magnesium have a higher melting point than sodium?

    • Larger ionic radius
    • Weaker metallic bonds
    • Fewer delocalised electrons
    • More delocalised electrons

  10. Which force must be overcome to melt simple molecular Period 3 elements?

    • Ionic bonds
    • Covalent bonds
    • London forces
    • Metallic bonds

  11. Which Period 3 element has the lowest melting point?

    • Argon
    • Chlorine
    • Sodium
    • Sulfur

  12. Why is the first ionisation energy of argon higher than chlorine?

    • Outer electron in 4s
    • Lower nuclear charge
    • Higher nuclear charge
    • Greater electron shielding

  13. Why is the first ionisation energy of silicon higher than aluminium?

    • Increased electron shielding
    • Greater nuclear charge
    • Lower nuclear charge
    • Outer electron in 3s

  14. Which factor remains constant across Period 3 atoms?

    • First ionisation energy
    • Atomic radius
    • Number of shells
    • Nuclear charge

  15. Why is the atomic radius of sodium larger than chlorine?

    • Greater electron shielding
    • More electron shells
    • Lower nuclear charge
    • Higher nuclear charge

  16. Which Period 3 element from sodium to silicon has the highest melting point?

    • Aluminium
    • Silicon
    • Sodium
    • Magnesium

  17. What main factor causes sodium to have a lower first ionisation energy than magnesium?

    • Greater shielding
    • Smaller atomic radius
    • Lower nuclear charge
    • Higher nuclear charge

  18. Which main bonding forces must be overcome when melting phosphorus, sulfur, and chlorine?

    • Van der Waals forces
    • Ionic bonds
    • Covalent bonds
    • Metallic bonds

  19. The first ionisation energy of Na is 496 kJ/mol and of Mg is 738 kJ/mol. What is the difference between them?

    • 738 kJ/mol
    • 1234 kJ/mol
    • 496 kJ/mol
    • 242 kJ/mol

  20. What is the first ionisation energy of sodium, in kJ/mol?

    • 578 kJ/mol
    • 496 kJ/mol
    • 1251 kJ/mol
    • 738 kJ/mol

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