IBChemistry: HLDPTopic Questions2. Atomic Structure2.1 Atomic & Electronic Structure

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First teaching 2014

Last exams 2024

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Atomic & Electronic Structure (DP IB Chemistry: HL)

Topic Questions

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2.1 Atomic & Electronic Structure

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2.1 Atomic & Electronic Structure

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11 mark

The reaction shown occurs in gas clouds throughout the Universe.

H2(g) + H2+(g) → H(g) + H3+(g)

Which is the correct atomic structure of the H3+ ion?

             

     protons        

     neutrons          

           electrons            

A

B

C

D

3

3

2

2

0

0

1

1

1

2

1

2

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    21 mark

    Which row is correct regarding atomic structure?

           

         The atomic number is the number of

        The proton number is the number of

         The mass number is the number of

    A

    B

    C
    D

    atoms

    electrons

    electrons

    protons

    protons

    neutrons

    neutrons

    protons

    protons

    nucleons

    protons

    nucleons

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      31 mark

      The phosphide ion,  straight P presubscript 15 space end presubscript presuperscript 32 space end presuperscript superscript 3 minus end superscript, is used in medicine as a radiotherapy treatment for some forms of cancer. 

      What is the composition of the phosphide ion?

                 

            protons     

          neutrons     

         electrons   

      A

      B

      C

      D

      15

      15

      17

      17

      17

      17

      15

      15

      32

      18

      15

      32

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        41 mark

        Which option correctly describes the relative charges and masses of the subatomic particles?

                  

              proton    

           neutron   

            electron    

            the relative mass of an electron    

        A


        B


        C


        D

        +1


        0


        +1


        0

        0


        +1


        0


        +1

        -1


        +1


        -1


        -1

        1


        begin mathsize 16px style 1 over 1840 end style

        begin mathsize 16px style 1 over 1840 end style


        1

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          51 mark

          Which row correctly describes the characteristics of the nucleus and surrounding space?

                  

                           nucleus                           

                       surrounding space                 

          A

          B

          C

          D

          small, dense and neutral

          large, dense and positive

          large, dense and neutral

          small, dense and positive

          mainly empty space

          densely populated with electrons

          densely populated with electrons

          mainly empty space

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            61 mark

            A periodic table is need for this question

            X is a particle with 19 electrons and 20 neutrons. 

            Three species are shown below:

                     1         

                40Ca+

                     2

                39K+

                     3

                38Ar

            Which of the three species could particle X be?

            • 1 only

            • 1 and 2

            • 2 and 3

            • 1, 2 and 3

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            71 mark

            The elements of the periodic table have different isotopes.

            What is different about the nuclei of stable isotopes?

            • the same number of protons, but different number of neutrons

            • the same number of protons, and the same number of neutrons

            • a different number of protons, and a different number of neutrons

            • a different number of protons, and the same number of neutrons

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            81 mark

            Iron has many different naturally occurring isotopes.

                          Isotope            

                   % Abundance        

                  Isotopic mass      

               54Fe

            5.845

            53.9396

               56Fe

            91.754

            55.9349

               57Fe

            2.119

            56.9354

               58Fe

            0.282

            57.9333



            Using the information given, what is the average atomic mass of iron?

            • 56.1858 amu

            • 54.200 amu

            • 59.270 amu

            • 55.845 amu

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            91 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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            101 mark

            Which electron transition would emit radiation of the longest wavelength?

            2-1-e-q10-mcqs-ib-chemistry

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              11 mark

              A periodic table is needed for this question

              In which of the following species are the numbers of protons, neutrons and electrons all different?

              • 23Na+

              • 27Al

              • 19F-

              • 32S2-

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              21 mark

              The atomic number of an element gives the number of protons in the nucleus which is also equal to the number of electrons. Which statement explains why atoms are neutral?

              • one proton has a mass 1840 times greater than one electron

              • the charge on an electron is equal and opposite to the charge on a proton

              • the difference in charge between electrons and protons is balanced by the neutrons

              • electrons are spread out in shells around the nucleus while protons are concentrated inside the nucleus

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              31 mark

              Which statements correctly describe the distribution of mass and charge in the atom?

                   1    

                 the negative charge is concentrated in one area outside the nucleus         

                   2

                 the mass is concentrated inside the nucleus

                   3

                 the negative charge is spread around outside the nucleus

              • 1 and 3

              • 1 and 2

              • 2 and 3

              • 1, 2 and 3

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              41 mark

              A periodic table is needed for this question

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

              • sulfur

              • iron

              • carbon

              • chromium

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              51 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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              61 mark

              A periodic table is needed for this question

              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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              71 mark

              A periodic table is needed for this question

              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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              81 mark

              The isotope  space presubscript 27 presuperscript 60 C o is used in the treatment of cancer cells in the body. 

              Which statements about this isotope are correct?

                   1     

              the charge on the nucleus is +27                                                    

                   2

              there are 33 neutrons in the nucleus

                   3 

              it has the same number of neutrons as other isotopes of cobalt

              • 1 and 2

              • 1 and 3

              • 2 only

              • 1, 2 and 3

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              91 mark

              The mass spectrum of element X is shown below.

              2-1-m-q9-mcqs-ib-chemistry
              Which of the following statements is correct?

              • X has a relative atomic mass between 70 and 71

              • The three isotopes of X are separated after being converted to anions

              • The most abundant isotope of X contains 71 neutrons

              • The isotope of X with mass 72 will be deflected the most

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              101 mark

              A periodic table is needed for this question

              Which row correctly describes the subatomic particles found in 26Mg2+?

                           

                   protons        

                   neutrons      

                   electrons       

              A

              10

              14

              12

              B

              12

              14

              10

              C

              12

              26

              10

              D

              14

              12

              12

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                11 mark

                Element X is in period 2 and has the first seven ionisation energies in kJ mol-1 as shown.

                    1300    

                    3380    

                    5330    

                    7460    

                    11 010    

                    13 320    

                    71 200    

                What is the electronic configuration of element X?

                • 1s2 2s2 2p4

                • 1s2 2s2 2p2

                • 1s2 2s2 2p3

                • 1s2 2s2 2p6

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                21 mark

                For the successive ionisation energies of oxygen, where would the highest jump be expected to occur?

                • second ionisation energy

                • first ionisation energy

                • seventh ionisation energy

                • sixth ionisation energy

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                31 mark

                Which statement explains the similarity in chemical behaviour for isotopes of the same element?

                • they may have the same electronic configuration, depending on the reaction

                • they have the same electronic configuration

                • their mass numbers are different

                • they have different numbers of neutrons

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                41 mark

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

                • Li+

                • F

                • N

                • N-

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                51 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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                61 mark

                An element consists of two isotopes 69X and 71X, whose abundances are 60% and 40% respectively. What is the relative atomic mass of element X?

                • 69.2

                • 69.8

                • 70.0

                • 70.2

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                71 mark

                Which equation is correct for the third ionization energy for the element nitrogen?

                • N+(g) → N4+(g)  + 3e-

                • N2+(g) → N3+(g)  + e-

                • N(g) → N3+(g)  + 3e-

                • N3+(g) → N4+(g)  + e-

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                81 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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                91 mark

                A spectral line that would be found in the visible spectrum of the hydrogen emission spectrum would be

                • n1 → n2

                • n2 → n3

                • n3 → n2

                • n3 → n∞

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