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DP IB Chemistry: SL

Topic Questions

Home / IB / Chemistry: SL / DP / Topic Questions / 4. Chemical Bonding & Structure / 4.2 Resonance, Shapes & Giant Structures / Structured Questions: Paper 2


4.2 Resonance, Shapes & Giant Structures

Question 1a

Marks: 3
a)
Yellow phosphorus reacts with chlorine to form phosphorus trichloride, PCl3.
i)
Draw the Lewis (electron dot) structure of phosphorus trichloride.
[1]
ii)
Predict the Cl-P-Cl bond angle and molecular geometry of the phosphorus trichoride molecule.
[2]
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    Question 1b

    Marks: 4
    b)
    Phosphorus trichloride, PCl3, can form a co-ordinate bond with a hydrogen ion to form HPCl3+.
    i)
    Draw the Lewis (electron dot) structure of HPCl3+.
    [2]
    ii)
    Predict the bond angle and molecular geometry of HPCl3+.
    [2]
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      Question 1c

      Marks: 4
      c)
      BCl3 has three electron domains in a trigonal planar structure.
      BCl3 is not a polar molecule, but PCl3 is.
      Explain this difference using section 8 of the Data booklet.
      [4]
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        Key Concepts
        Molecular polarity

        Question 1d

        Marks: 2
        d)
        PCl4+ has the same electron domain geometry as HPCl3+.
        Explain why PCl4+ is not a polar molecule.
        [2]
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          Key Concepts
          Molecular polarity

          Question 2a

          Marks: 3
          a)
          This question is about the geometry of a number of common molecules.

          simple-molecules

          i)
          Which molecule(s) has/ have tetrahedral structures with respect to the electron domain geometry?
          [1]
          ii)
          What is the molecular geometry of CO2?
          [1]
          iii)
          Draw the 3D representation of ammonia, NH3.
          [1]

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            Question 2b

            Marks: 3
            b)
            Estimate the H-O-H bond angle in water, H2O, using VSEPR theory.
            Explain your answer.
            [3]
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              Question 2c

              Marks: 3
              c)
              Suggest a way in which the bond angle in ammonia / NH3 could become 109.5o and explain your answer.
              [3]
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                Question 2d

                Marks: 3
                d)
                Ozone, O3, is another simple molecule which has the following structure:

                4-2-ib-sl-sq-easy-q2d-ozone-display-formula-with-lone-pairs

                i)
                Estimate the O-O-O bond angle in ozone using VSEPR theory.
                [1]
                ii)
                Explain why the actual bond lengths present in ozone are equal.
                [2]

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                  Question 3a

                  Marks: 4
                  a)
                  Carbon has three naturally occurring allotropes; diamond, graphite and buckminsterfullerene, C60.
                  State how many atoms each carbon is directly bonded to in each of the allotropes, explaining any differences.

                  [4]

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                    Question 3b

                    Marks: 3
                    b)
                    Describe the differences in the structures of the three allotropes of carbon.

                    [3]

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                      Question 3c

                      Marks: 4
                      c)
                      Describe and explain the differences in electrical conductivity between the three allotropes of carbon.

                      [4]

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                        Question 3d

                        Marks: 2
                        d)
                        Graphene can be made from graphite.
                        Describe a similarity and difference between these two structures.
                        [2]
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                          Question 4a

                          Marks: 4
                          a)
                          Silicon and carbon are in the same group of the Periodic Table. They both form covalent bonds.

                          4-2-ib-sl-sq-easy-q4a-silicon-dioxide

                          O=C=O (carbon dioxide)

                          Both silicon and carbon form dioxides, but silicon dioxide has a melting point of 1710 oC whilst carbon dioxide has a melting point of -78 oC.
                          Explain this difference with reference to the structure and bonding present in each dioxide.
                          [4]

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                            Question 4b

                            Marks: 3
                            b)
                            How many oxygen atoms are bonded to each carbon and to each silicon?
                            Explain how this links to the formula of each compound.
                            [3]
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                              Question 4c

                              Marks: 2
                              c)
                              Predict the O-C-O and O-Si-O bond angles respectively in CO2 and in SiO2.

                              [2]

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                                Question 4d

                                Marks: 4
                                d)
                                Predict and explain the solubility of both SiO2 and CO2 in water.

                                [4]

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