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DP IB Chemistry: SL

Topic Questions

Home / IB / Chemistry: SL / DP / Topic Questions / 2. Atomic Structure / 2.1 Atomic & Electronic Structure / Structured Questions: Paper 2


2.1 Atomic & Electronic Structure

Question 1a

Marks: 2
a)
Give the full electron configuration of the following atoms and ions.

ii)        Zinc (II) ion, Zn2+

[1]

iii)       Copper (II) ion, Cu2+

[1]

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    Question 1b

    Marks: 3
    b)
    Chlorine has two naturally occurring isotopes, 35Cl with a mass of 34.969 and 37Cl with a mass of 36.966. The relative atomic mass of Cl is 35.5. Calculate the percentage abundance of each isotope.
    [3]
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      Question 1c

      Marks: 2
      c)
      Predict whether the atomic radius of 35Cl or 37Cl would be the greater and give a reason for your answer. 
      [2]
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        Key Concepts
        Isotopes: Basics

        Question 1d

        Marks: 4
        d)
        A sample of cerium, Ce, was analysed in a  mass spectrometer. The relative abundances of three of the four main isotopes that were identified are shown in the table below.
        A sample of cerium, Ce, has four isotopes that have a known relative abundance. This sample has an Ar of 140.12.

        Isotope

        136Ce

        138Ce

        140Ce

        mCe

        Abundance (%)

        0.19

        0.25

        88.45

        To be calculated 


        Use the data from the table to calculate m, the mass number and the percentage abundance of isotope mCe.

        [4]

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          Question 2a

          Marks: 3
          a)
          A sample of element Z was extracted from a meteorite. The table shows the relative abundance of each isotope in a mass spectrum of this sample of Z. Calculate the relative atomic mass of Z and suggest an identity of Z. Give your answer to 1 d.p. 

          m/z value

          64

          66

          67

          68

          Relative abundance (%)

          38.9

          27.8

          14.7

          18.6

          [3]

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            Question 2b

            Marks: 3
            b)
            A naturally occurring sample of the element boron, B, has two isotopes of mass 10 and 11, and a relative atomic mass of 10.8.

                     Calculate the relative abundances of both isotopes in the sample of boron, B.

            [3]

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              Question 2c

              Marks: 1

              c)   Give the full electron configuration of the Cu+ ion. 

              [1]

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                Question 2d

                Marks: 3
                d)
                Calculate the percentage abundance of 63Cu with a mass of 62.9296 and 65Cu with a mass of 64.9278, when the average mass of the Cu isotope is 63.546. Give your answer to an appropriate number of significant figures.

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                  Question 3a

                  Marks: 1
                  a)
                  The diagram below shows electron transitions in a hydrogen atom in two regions of the electromagnetic spectrum.
                  hydrogen-emission-spectrum
                  Using section 3 of the Data booklet, predict which electron transition is most likely to correspond to the emission of red light.
                  [1]
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                    Question 3b

                    Marks: 1
                    b)
                    Using sections 1 and 3 of the data booklet, predict which electron transition will correspond to the greatest frequency of light emitted.
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                      Question 3c

                      Marks: 1
                      c)
                      The wavelengths of the first four lines for the Balmer series are shown below.
                      Balmer spectral line Wavelength in nm Colour
                      Hα 656 red
                      Hβ 486 cyan(blue)
                      Hγ 434 blue
                      Hδ 410 violet

                      Using section 1 of the Data booklet, determine the ratio of the frequencies Hα to Hγ to 2 decimal places.

                      [1]

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                        Question 3d

                        Marks: 1
                        d)
                        2-chloro-2-methylbutane contains some molecules with a molar mass of approximately 106 g mol-1  and some with a molar mass of approximately 108 g mol-1.

                                  Outline why there are molecules with different molar masses.

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                          Key Concepts
                          Isotopes: Basics

                          Question 4a

                          Marks: 2
                          a)
                          Outline why the chlorine atom has a smaller atomic radius than the sulfur atom.
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                            Question 4b

                            Marks: 1
                            b)

                            The mass spectrum of chlorine gas is shown.

                            chlorine-mass-spectrum

                             Outline the reason for the two peaks at m/z=35 and 37.

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                              Key Concepts
                              Isotopes: Basics

                              Question 4c

                              Marks: 2
                              c)

                              Explain the presence and relative abundance of the peak at m/z=74.

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