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IBChemistry: HLDPExam Questions3. Periodicity3.1 The Periodic Table & Periodic Trends

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First teaching 2014

Last exams 2024

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The Periodic Table & Periodic Trends (DP IB Chemistry: HL)

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3.1 The Periodic Table & Periodic Trends

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3.1 The Periodic Table & Periodic Trends

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11 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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21 mark
A periodic table is needed for this question
 
Sodium sulfide, Na2S, is a reactive yellow solid, produced when sodium and sulfur react together.
 
How do the ionic radius and atomic radius of sodium compare with those of sulfur?

  ionic radius atomic radius
A sodium < sulfur  sodium < sulfur 
B sodium < sulfur  sodium > sulfur
C sodium > sulfur  sodium > sulfur 
D sodium > sulfur  sodium < sulfur

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    31 mark

    Which property below decreases generally across the second period?

    • Atomic number

    • Atomic radius

    • Electronegativity

    • Ionisation energy

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    41 mark

    The trends in three physical properties of the elements of period 3 are shown in the graphs

     q4_3-1_periodic-table--periodic-trends-ib_sl_easy

    Which physical property is not illustrated?

    • Electrical conductivity 

    • Atomic radius

    • Melting point 

    • First ionisation energy

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    51 mark

    Silicon reacts with chlorine gas to produce silicon chloride. 

    How many moles of chlorine gas are needed to react with 1 mole of silicon?

    • 2

    • 3

    • 4

    • 5

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    61 mark

    This question refers to isolated gaseous species.

    The species O2-, Ne and Mg2+ are isoelectronic.

    In which order do their radii increase?

      Smallest rightwards arrow with blank on top Largest
    A Mg2+

    O2-

    		 Ne
    B Ne

    O2-

    Mg2+
    C Mg2+

    Ne

    O2-
    D O2- Ne Mg2+

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      71 mark

      Use of the periodic table is relevant to this question. 

      Which graph correctly shows the electronegativity of the elements Na, Mg, Al and Si, from period 3, plotted against their first ionisation energies?

      N_bcASI0_q7_3-1_periodic-table--periodic-trends_ib_sl_easy

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        81 mark

        Which period 3 element from sodium to silicon, has the largest atomic radius?

        • Magnesium

        • Sodium

        • Silicon

        • Aluminium

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        91 mark

        What is the correct classification for the element zirconium, Zr?

        • s block

        • d block

        • f block

        • p block

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        101 mark

        Why is the second ionisation energy of magnesium higher than the first ionisation energy?

        • Less shielding

        • Ionic radius increases

        • Nuclear charge is increasing

        • Greater attraction between positive nucleus and outer electron

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        11 mark

        Electron configurations for atoms of different elements are shown below. 

        Which electron configuration represents the element with the largest first ionisation energy?

        • 1s22s22p63s2

        • 1s22s22p63s23p4

        • 1s22s22p63s23p6

        • 1s22s22p63s23p64s2

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        21 mark

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

        Which equation correctly represents this statement?

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

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

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

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

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        31 mark

        A periodic table is need for this question 

        X, Y and Z  are consecutive elements in the third Period of the Periodic Table. Element Y has the highest first ionisation energy and also the lowest melting point of these three elements. 

        What could be the identities of X, Y and Z?

        • silicon, phosphorus, sulfur 

        • sodium, magnesium, aluminium

        • aluminium, silicon, phosphorus

        • magnesium, aluminium, silicon

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        41 mark

        An element in the d block of the periodic table forms a +4 ion and has the electron configuration of [Ar] 3d1.

        What is the identity of the element?

        • Chromium

        • Copper

        • Vanadium

        • Silicon

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        51 mark

        A periodic table is needed to answer this question 

        Which graph correctly shows the relative melting points of period 3 elements plotted against their relative electronegativities?

        q5_3-1_periodic-table--periodic-trends_ib_sl_medium

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          61 mark

          For the following pairs, which has the greatest difference in size?

          • Li and Cl

          • Na and Br

          • Li+ and Br-

          • Na+ and Cl-

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          71 mark

          A periodic table is needed for this question. 

          Elements X and Y are Period 3 elements that react together to form compound Z. Element X has the second smallest atomic radius in Period 3. Apart from argon, there is only one element in Period 3 which has a lower melting point than element Y.

           Which compound could be Z?

          • Na2S

          • MgS

          • MgCl 2

          • PCl 3

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          81 mark

          Which of these elements would form the largest ion with a noble gas electron configuration?

          • Gallium

          • Bromine

          • Arsenic

          • Rubidium

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          91 mark

          Use a periodic table to deduce the correct information about the element tin, Sn (Z = 50)

            Number of occupied
          main energy levels          		 Number of electrons in the
          highest main energy level

          A

          4

          4

          B

          4

          14

          C

          5

          4

          D

          5

          14

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            101 mark

            The order of the elements in the periodic table is

            • according to relative atomic mass

            • by nuclear charge

            • by reactivity

            • in order of electronegativity

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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

            		 K+ Cl–

            Ar

            B

            		 Cl–

            Ar

            K+

            C

            K+

            		 Ar Cl–
            D Ar K+ Cl–

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              21 mark

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

              1
              electrons shells are added across Period 3 which increases the nuclear force of attraction
              2
              the nuclear charge increases across Period 3 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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              31 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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              41 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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              51 mark

              Use of the periodic table is relevant to this question. 

              Sir Humphrey Davy discovered the elements magnesium, boron, sodium and calcium. 

              Which of the elements Sir Davy discovered has the third lowest first ionisation energy in its Period and the third smallest atomic radius in its Group?

              • magnesium

              • boron

              • sodium

              • calcium

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              61 mark

              Which of the following pairs does the second element have a higher 1st ionisation energy than the first element?

               

              First element

              Second element

              A

              Mg

              Al

              B

              N

              O

              C

              Ne

              Na

              D

              K

              Na

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                71 mark

                Shown on the graph are the relative values of the first ionisation energies of four elements that have consecutive atomic numbers. One of the elements reacts with hydrogen to form a covalent compound with formula HX. 

                Which element could be X?

                q7_3-1_periodic-table--periodic-trends_ib_-sl_hard

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                  81 mark

                  A periodic table is need for this question 

                  Below are four statements about energy levels and electrons. Which is the correct statement?

                  • 18 is the maximum number of electrons in the 4th energy level

                  • 10 is the maximum number of electrons in one d orbital

                  • Yttrium is the first element with an electron in an f subshell

                  • In a main energy level, the subshell with the highest energy is f

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                  91 mark

                  Element J has a lower first ionisation energy and higher melting point than the element preceding it in the periodic table. 

                  Its ion is isoelectronic with argon. 

                  What is the identity of element J?

                  • Na

                  • S

                  • P

                  • Al

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                  101 mark

                  Which statement about electron affinity and electronegativity is correct?

                  • Electron affinity increases down a group, but electronegativity decreases

                  • Electron affinity decreases down a group, but electronegativity increases

                  • Electron affinity and electronegativity both decrease down a group

                  • There is no clear trend in electron affinity down a group but electronegativity decreases

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