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ASChemistryCIEExam Questions1. Physical Chemistry1.1 Atomic Structure

Atomic Structure (CIE AS Chemistry)

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1.1 Atomic Structure

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1.1 Atomic Structure

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11 mark

In 1808 John Dalton published his atomic theory. This was the first complete attempt to describe matter in terms of atoms and contained four theories. 

Which of his theories is still considered to be correct today?

  • All matter is made of indivisible atoms.

  • All atoms are very small in size.

  • All the atoms of one element are different in mass from all the atoms of other elements.

  • All atoms of the same element will have the same mass.

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21 mark

The reaction shown occurs in gas clouds throughout the Universe.

H2 (g) + H2+ (g) → H (g) + H3+ (g)

What is the 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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    31 mark

    Which row is correct?

     

    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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      41 mark

      The phosphide ion, begin mathsize 16px style P presubscript 15 presuperscript 32 superscript 3 minus sign end superscript end style, is used in medicine as a radioactive 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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        51 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 14px style 1 over 1840 end style

        1 over 1840

        1

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          61 mark

          The trajectories of subatomic particles shot through an electric field produced in a vacuum are shown in the diagrams.

          1-1-q6-subatomic-particles-in-electric-field

          Which diagrams are correct?

          • 2 and 3

          • 1 and 2

          • 1, 2 and 3

          • 2 only

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          71 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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            81 mark

            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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            91 mark

            Which of the following statements describes a free radical?

            • A species with a lone pair of electrons

            • A species with a half-filled d-orbital

            • A species with one or more unpaired electrons

            • A species with a partially filled outer shell

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            101 mark

            Which of the following statements describes first ionisation energy?

            • The energy required to remove one mole of electrons from one mole of gaseous atoms.

            • The energy required to remove the outermost electron from each atom in one mole of gaseous atoms.

            • The energy required to remove the outermost electron from each atom in one mole of atoms.

            • The energy required to produce one mole of ions from one mole of gaseous atoms.

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            11 mark

            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 statement correctly describes the trend in metallic radius in group I elements Na to Rb? 

            1

            Increases moving down the group

            2

            Increases moving down due to the addition of electron shells 

            3

            Decreases moving down due to increasing nuclear forces

            • 1, 2 and 3

            • 2 and 3

            • 1 and 2

            • 1 only

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            41 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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            51 mark

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

            • Sulfur

            • Iron

            • Carbon

            • Chromium

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            61 mark

            The second ionisation energy of magnesium is 1451 kJ mol-1. 

            Which equation correctly represents this statement?

            • Mg+ (g) → Mg2+ + e-          ΔHӨ = -1451 kJ mol-1

            • Mg+ (g) → Mg2+ + e-          ΔHӨ = +1451 kJ mol-1

            • Mg (g) → Mg2+ + 2e-         ΔHӨ  = +1451 kJ mol-1

            • Mg (g) → Mg+ + e-            ΔHӨ = -1451 kJ mol-1

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            71 mark

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

            1-1-q17-s-and-p-orbitals

            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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            81 mark

            What is the electronic configuration of the ion with a single negative charge and the 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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            91 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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            101 mark

            The isotope Co presubscript 27 presuperscript 60 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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            11 mark

            The species Cl-, K+ and Ar are isoelectronic. This means that they have the same number of electrons. 

            In which order do their radii decrease?

             

            Largest   →   Smallest

            A

            B

            C

            D

            K+

            Cl-

            K+

            Ar

            Cl-

            Ar

            Ar

            K+

            Ar

            K+

            Cl-

            Cl-

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              21 mark

              The trajectories of subatomic particles shot through an electric field produced in a vacuum are shown in the diagram. The velocity is the same for all three particles.

              1-1-q22-subatomic-particles-in-electric-field-2

              Which statements are correct?

               

              1

              The proton and electron are deflected because they are charged particles.

               

              2

              The neutrons are undeflected as they have no charge.

               

              3

              The electron is deflected more than the proton because it has less mass.

              • 1, 2 and 3

              • 1 only

              • 2 and 3

              • 1 and 3

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              31 mark

              The atomic radius of the elements decreases moving across period 3. Which of the following statements explain this phenomenon?

              1

              Electrons shells are added moving across which increases the nuclear force of attraction.

              2

              The nuclear charge increases moving across due to increasing atomic number.

              3

              There is a greater force of attraction between the nucleus and the electrons.

              • 1 and 2

              • 1, 2 and 3

              • 2 and 3

              • 1 only

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              41 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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              51 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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              61 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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              71 mark

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

              • Li+

              • F

              • N+

              • N-

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              81 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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              91 mark

              The first ionisation energy of beryllium is higher than the first ionisation energy of boron. 

              Which statement explains why?

              • Boron has a full outer shell

              • Boron has a larger atomic radius than beryllium

              • Beryllium has a more stable electronic configuration

              • The atomic number of beryllium is higher than boron

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              101 mark

              The electronic configurations of four different atoms are shown. 

              Which atom has the highest first ionisation energy?

              • 1s2 2s2 2p6 3s2

              • 1s2 2s2 2p4

              • 1s2 2s2 2p6 

              • 1s2 2s2 

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