Lesson 1.3.2

1.3.2 Electronic configurations and s, p, d blocks Quiz: Pearson Edexcel Chemistry, Unit 1

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 1.3.2, Electronic configurations and s, p, d blocks: 20 multiple choice questions for the Pearson Edexcel Chemistry (9CH0), Unit 1: Atomic Structure and the Periodic Table, written with Revision Ninja.

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The 20 questions

  1. What is the electronic configuration of a neutral sodium atom?

    • 1s2 2s2 2p6 3s1
    • 1s2 2s2 2p6 3s2
    • 1s2 2s2 2p5 3s2
    • 1s2 2s2 2p6 3p1

  2. The electronic configuration of an element is [Ar] 3d10 4s2 4p3. Which block does it belong to?

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

  3. Which ion has the same electron configuration as argon?

    • Al
    • Mg2+
    • Na+
    • Cl-

  4. Which electronic configuration is correct for a chromium atom (Z = 24)?

    • 1s2 2s2 2p6 3s2 3p6 3d4 4s2
    • 1s2 2s2 2p6 3s2 3p6 3d6
    • 1s2 2s2 2p6 3s2 3p6 4s2 4p4
    • 1s2 2s2 2p6 3s2 3p6 3d5 4s1

  5. What is the electronic configuration of the Fe3+ ion? (Fe has Z = 26.)

    • [Ar] 4s1 3d4
    • [Ar] 3d6
    • [Ar] 3d3
    • [Ar] 3d5

  6. Which block of the periodic table contains elements whose highest-energy electron is in an s sub-shell?

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

  7. How many unpaired electrons does an oxygen atom have? (Configuration 1s2 2s2 2p4.)

    • 2
    • 4
    • 0
    • 6

  8. Which diagram shows the correct electrons-in-boxes notation for nitrogen's 2p3 sub-shell?

    • Three boxes, two of which contain paired arrows
    • Three boxes, each containing one arrow
    • Two boxes each containing two arrows and one empty box
    • One box containing three arrows

  9. Which element has the electronic configuration [Ne] 3s2 3p3?

    • Nitrogen, which has a 2p3 configuration with three unpaired electrons in its outer shell of the atom
    • Aluminium, which has a 3s2 3p1 configuration with one unpaired electron in its outer shell of the atom
    • Phosphorus
    • Sulfur, which has a 3s2 3p4 configuration with two unpaired electrons in its outer shell of the atom

  10. What is the block of an element with configuration [Ar] 3d2 4s2?

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

  11. How many electrons are in the 3d sub-shell of a Mn2+ ion? (Mn has Z = 25.)

    • 3
    • 7
    • 2
    • 5

  12. A neutral atom has electronic configuration 1s2 2s2 2p6 3s2 3p3. What is its atomic number and identity?

    • 13, aluminium, which is a metal with three electrons in its outer shell and a 3p1 configuration
    • 14, silicon, which is a giant covalent element with four electrons in its outer shell of the atom
    • 16, sulfur, which is a simple molecular element with six electrons in its outer shell of the atom
    • 15, phosphorus

  13. Explain why Zn2+ is not regarded as a transition metal ion.

    • Zn2+ is [Ar] 4s2, so it has no d electrons at all and cannot be classed as a transition metal ion
    • Zn2+ is [Ar] 3d10 4s2, which contains a full 4s sub-shell and an incomplete d sub-shell in the same ion
    • Zn2+ is [Ar] 3d10, so it has a full d sub-shell rather than an incomplete one
    • Zn2+ is [Ar] 3d8, so it has an incomplete d sub-shell and therefore counts as a transition metal ion

  14. Explain why vanadium(II) ion has configuration [Ar] 3d3.

    • Vanadium loses one 4s and one 3d electron to form V2+, leaving the remaining electrons in a 3d3 4s1 pattern
    • Vanadium is [Ar] 3d3 4s2, and both 4s electrons are lost first to form V2+
    • Vanadium gains two electrons into the 3d sub-shell, which partly fills it and leaves the 4s2 pair unchanged
    • Vanadium loses 3d electrons first, so the 4s2 electrons remain in the ion and it gains extra stability

  15. Why does a Cu+ ion have configuration [Ar] 3d10?

    • Copper's 3d sub-shell is always full in every ion, so the Cu+ ion has exactly the same configuration as copper
    • Copper's configuration is [Ar] 3d10 4s1, so losing the single 4s electron leaves a full 3d sub-shell
    • Copper gains an electron into its 3d sub-shell when it forms the Cu+ ion, which completes the sub-shell
    • Copper's configuration is [Ar] 3d9 4s2, so losing one 3d electron leaves a full 3d sub-shell in the ion

  16. A student gives the configuration of Fe2+ as [Ar] 3d4 4s2. Which statement identifies the error?

    • Fe2+ should have lost 3d electrons only, so the configuration [Ar] 3d4 4s2 shown by the student is correct as written
    • Fe2+ is [Ar] 3d6, because the two 4s electrons are lost and the 3d count stays at six
    • Fe2+ is [Ar] 4s2 3d5, because 3d electrons are always lost before the 4s electrons in any ion of iron
    • Fe2+ should be [Ar] 3d8, since ions gain electrons from the solvent and so add them to the 3d sub-shell

  17. Which statement correctly explains how the s, p and d blocks are defined?

    • A block is set by the sub-shell that the last electron enters
    • A block is set by the number of protons in the nucleus, which determines which sub-shell type the atom fills
    • A block is set by the shell number of the outermost electron, regardless of which sub-shell it occupies
    • A block is set by the number of valence electrons alone, without any reference to the sub-shell being filled

  18. Which electronic configuration corresponds to the Ca2+ ion? (Ca has Z = 20.)

    • 1s2 2s2 2p6 3s2 3p4
    • 1s2 2s2 2p6 3s2 3p6 3d2
    • 1s2 2s2 2p6 3s2 3p6 4s2
    • 1s2 2s2 2p6 3s2 3p6

  19. Which atom has the electronic configuration 1s2 2s2 2p6 3s2 3p4?

    • Phosphorus
    • Sulfur
    • Selenium
    • Oxygen

  20. How many unpaired electrons does a ground-state chromium atom have?

    • 0
    • 4
    • 6
    • 2

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