IBChemistrySLExam QuestionsModels of the Particulate Nature of MatterElectronic Configurations

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First teaching 2023

First exams 2025

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Electronic Configurations (SL IB Chemistry)

Exam Questions

1 hour20 questions

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Electronic Configurations

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Electronic Configurations

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11 mark

Using the Aufbau Principle and Hund’s rule, deduce which element below has the greatest number of unpaired electrons in its ground state.

  • Z = 13

  • Z = 14

  • Z = 15

  • Z = 16

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2
Sme Calculator1 mark

Which spectrum belongs to hydrogen?

eARGWkkX_hydrogen-spectrum

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    11 mark

    There are six unpaired electrons in atoms of element Z. What could element Z be?

    • sulfur

    • iron

    • carbon

    • chromium

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    21 mark

    The diagram shows three orbitals labelled 1, 2 and 3. 

    2-1-m-q5-mcqs-ib-chemistry

    What is the correct label for each orbital?

    • px, py and pz

    • s, pz and py

    • s, px and pz

    • s, px and py

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    31 mark

    What is the electronic configuration of an ion with a single negative charge and atomic number 17?

    • 1s2 2s2 2p6 3s1 3p6

    • 1s2 2s2 2p6 3s2 3p6

    • 1s2 2s2 2p6 3s1 3p5

    • 1s2 2s2 2p6 3s2 3p5

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    41 mark

    What is the correct sequence for the orbitals shown in an atom of vanadium in order of decreasing energy?

    • 3s 3p 4s 3d

    • 4s 3d 3s 3p

    • 4s 3d 3p 3s

    • 3d 4s 3p 3s

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    51 mark

    An element in the d block of the periodic table forms a +4 ion and has the electron configuration of [Ar] 3d1.

    What is the identity of the element?

    • Chromium

    • Copper

    • Vanadium

    • Silicon

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    61 mark

    Deduce the correct information about the element tin, Sn (Z = 50)

      Number of occupied
    main energy levels    		 Number of electrons in the
    highest main energy level

    A

    4

    4

    B

    4

    14

    C

    5

    4

    D

    5

    14

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      11 mark

      Which species produces a half-filled set of p orbitals on losing an electron?

      • Li+

      • F

      • N

      • N-

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      21 mark

      Which statement explains why electrons pair up in orbitals before occupying an orbital of a higher energy level?

      • the energy from repulsion is greater than the jump to a higher orbital

      • electrons occupy higher energy orbitals before lower energy orbitals

      • electrons in lower orbitals have higher energies

      • the energy from repulsion is less than the jump to a higher orbital

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      31 mark

      A line emission spectrum occurs when

      • electrons release energy as they move from high to low energy levels

      • electrons release energy as they move from low to high energy levels

      • electrons absorb energy as they move from high to low energy levels

      • electrons absorb energy as they move from low to high energy levels

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      4
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      Which statement is true about the spectra shown? hydrogen-spectrum-hl

      • All the lines in R have the same energy

      • Q and S could represent line emission spectra

      • Only S could represent a line emission spectrum for hydrogen

      • P indicates the element has 4 pairs of electrons at different energy levels 

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