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DP IB Chemistry: SL

Topic Questions

Home / IB / Chemistry: SL / DP / Topic Questions / 3. Periodicity / 3.1 The Periodic Table & Periodic Trends / Structured Questions: Paper 2


3.1 The Periodic Table & Periodic Trends

Question 1a

Marks: 3
a)
This question refers to the elements in the first three periods of the Periodic Table.
Select an element from the first three periods that fits each of the following descriptions.

i)
The element with the highest first ionisation energy

[1]

ii)
The element that forms a 1 ion with the same electron configuration as helium

[1]

iii)
An element which forms a compound with hydrogen in which the element has an oxidation number of −4

[1]

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    Question 1b

    Marks: 5
    b)
    This question is about the elements which have atomic numbers 33 to 37.

    The first ionisation energies of these elements are shown in the table below.

    Element

    As

    Se

    Br

    Kr

    Rb

    Ionisation energy value in kJ /mol-1

    947

    941

    1340

    1351

    403

    i)
    Suggest the formulae of the hydrides of arsenic and selenium

    [2]

    ii)
    Explain why the first ionisation energy of rubidium is lower than that of krypton

    [2]

    iii)
    State which of the elements, arsenic to rubidium, has atoms with the smallest atomic radius

    [1]

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      Question 1c

      Marks: 3
      c)
      The first 3 elements of Period 3 show a general increase in melting point.

      Explain this trend in melting point across these Period 3 elements.

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        Question 1d

        Marks: 3
        d)
        This question is about hydrogen, the element with the atomic number Z = 1.
        Hydrogen can be placed in several different positions in periodic tables. One is immediately above lithium in Group 1 as shown in section 6 of the data booklet. Another is in the centre of the first row.
        Evaluate the position of hydrogen when it is placed immediately above lithium and state one reason in favour and two against. 

        [3]

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          Question 2a

          Marks: 2
          a)
          This question is about Period 4 of the Periodic Table. 
          State and explain which of K+ and Ca2+ is the smaller ion.

          [2]

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            Key Concepts
            Atomic & Ionic Radius

            Question 2b

            Marks: 1
            b)
            Write the electron configuration for a Ca+ ion.

            [1]

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              Question 2c

              Marks: 4
              c)
              The first ionisation energies of the elements H to K are shown below.
              periodicity-diagram-1
              State and explain the trend in first ionisation energies shown by the elements with the atomic numbers 2, 10 and 18.

               [4]

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                Question 3a

                Marks: 3
                a)
                Electrons in atoms occupy orbitals.
                The figure below shows the first ionisation energies for six consecutive elements labelled AF
                periodicity-diagram-2
                Complete the graph of the first ionisation energies for the next five elements.

                [3]

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                  Question 3b

                  Marks: 2
                  b)
                  Explain why the value of the first ionisation energy for D is greater than for C.

                  [2]

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                    Question 3c

                    Marks: 4
                    c)
                    The sequence of the first three elements in the Periodic Table is hydrogen, helium and then lithium.
                    Explain why the first ionisation energy of hydrogen is less than that of helium but greater than that of lithium.

                    [4]

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                      Question 4a

                      Marks: 3
                      a)
                      First ionisation energies decrease down groups in the Periodic Table.
                      Explain this trend and the effect on the reactivity of groups containing metals.

                      [3]

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                        Question 4b

                        Marks: 3
                        b)
                        The ionisation energy values show a general increase across period 4 from gallium to krypton. 
                        State and explain how selenium deviates from this trend. 

                        [3]

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                          Question 4c

                          Marks: 1
                          c)
                          Give one other element from period 2 or 3 which also deviates from this general trend, similar to selenium.

                          [1]

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                            Question 4d

                            Marks: 6
                            d)
                            State and explain the trends in electronegativity down group 2 and across period 3.

                            [6]

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                              Key Concepts
                              Electron Affinity