Lesson 3.1.1

3.1.1 Periodicity Quiz: OCR Chemistry, Unit 2

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 3.1.1, Periodicity: 20 multiple choice questions for the OCR Chemistry (H432), Unit 2: Periodic table and energy, written with Revision Ninja.

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The 20 questions

  1. How are elements arranged in the modern periodic table?

    • Decreasing atomic number
    • Increasing atomic number
    • Increasing atomic mass
    • Increasing neutron number

  2. Where is the highest energy electron located in a p-block element?

    • s sub-shell
    • d sub-shell
    • f sub-shell
    • p sub-shell

  3. What state must species be in for first ionisation energy measurement?

    • Aqueous state
    • Gaseous state
    • Liquid state
    • Solid state

  4. Which factor causes first ionisation energy to decrease down Group 2?

    • Increased atomic radius
    • Decreased atomic radius
    • Increased nuclear charge
    • Decreased electron shielding

  5. Which sub-shell contains the outermost electron in aluminium?

    • 3d sub-shell
    • 3s sub-shell
    • 2p sub-shell
    • 3p sub-shell

  6. Why is oxygen easier to ionise than nitrogen across Period 2?

    • Greater electron shielding
    • Smaller atomic radius
    • Increased nuclear charge
    • Electron pair repulsion

  7. A large jump between second and third ionisation energies indicates how many valence electrons?

    • Two
    • Eight
    • Three
    • One

  8. What trend in melting point occurs from sodium to silicon across Period 3?

    • They increase
    • They remain constant
    • They fluctuate
    • They decrease

  9. What type of electrostatic attraction holds a giant metallic lattice together?

    • Cations and delocalised electrons
    • Shared electron pairs
    • Dipoles and hydrogen bonds
    • Oppositely charged ions

  10. Which moving particles allow metals to conduct electricity?

    • Mobile ions
    • Delocalised electrons
    • Covalent bonds
    • Positive cations

  11. What type of structure is found in diamond?

    • Simple molecular lattice
    • Giant covalent lattice
    • Giant ionic lattice
    • Giant metallic lattice

  12. How many covalent bonds does each carbon atom form in graphite?

    • One
    • Four
    • Two
    • Three

  13. What type of bonding must be broken to melt silicon?

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

  14. Which forces are overcome when solid chlorine melts?

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

  15. How many atomic layers of carbon make up graphene?

    • Hundreds
    • Two
    • One
    • Three

  16. Which element in period 3 has the highest first ionisation energy?

    • Magnesium
    • Sodium
    • Argon
    • Chlorine

  17. Which period 3 element has the lowest first ionisation energy?

    • Argon
    • Aluminium
    • Sodium
    • Magnesium

  18. Which block of the periodic table contains elements that typically form coloured ions?

    • s-block
    • d-block
    • f-block
    • p-block

  19. In which group and period is an element with electron configuration 1s2 2s2 2p6 3s2 3p1?

    • Group 13, period 1
    • Group 13, period 3
    • Group 3, period 1
    • Group 3, period 3

  20. What main factor causes the general increase in first ionisation energy across Period 3?

    • Increasing nuclear charge
    • Decreasing nuclear charge
    • Increasing shielding
    • Increasing atomic radius

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