ASChemistryOCRExam Questions3. Periodic Table & EnergyPeriodicity

Periodicity (OCR AS Chemistry A): Exam Questions

Exam code: H032

3 hours41 questions

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Periodicity

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1
1 mark

What determines the order of elements in the Periodic Table?

  • First ionisation energy

  • Number of electrons in the outer shell

  • Number of protons in the nucleus

  • Relative atomic mass

Choose your answer

2
1 mark

Which element has the highest melting point?

  • Silicon

  • Phosphorus

  • Sulfur

  • Chlorine

Choose your answer

3
1 mark

Electron configurations for atoms of different elements are shown below.

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

  • 1s22s2

  • 1s22s22p4

  • 1s22s22p6

  • 1s22s22p63s2

Choose your answer

4
1 mark

Sodium sulfide, Na2S, is a reactive yellow solid, produced when sodium and sulfur react together.

Which of the following statements is correct?

A

The ions have the same ionic radii

B

The atoms have the same atomic radii

C

Sodium < sulfur

D

Sodium > sulfur

    Choose your answer

    5
    1 mark

    The trends in three physical properties of the elements of Period 3 are shown in the graphs below.

    periodicity-trends-period-3

     

    Which physical property is not illustrated?

    • First ionisation energy 

    • Atomic radius

    • Melting point

    • Electrical conductivity 

    Choose your answer

    6
    1 mark

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

    • s block

    • d block

    • f block

    • p block

    Choose your answer

    7
    1 mark

    What is the correct equation for the second ionisation energy of rubidium, Rb?

    • Rb+ (g) → Rb2+ (g) + e-

    • Rb (g) → Rb+ (g) + e-

    • Rb2+ (g) → Rb3+ (g) + e-

    • Rb2+ (g) + e- → Rb+ (g)

    Choose your answer

    8
    1 mark

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

    • Less shielding

    • Ionic radius increases

    • Nuclear charge increases

    • Greater attraction between positive nucleus and outer electron

    Choose your answer

    9
    1 mark

    Why does aluminium have a higher melting point than magnesium?

    • Aluminium has its valence electron in the p orbital

    • Lower charge on the cation and increasing number of delocalised electrons

    • Higher charge on the cation and increasing number of delocalised electrons

    • Higher charge on the cation and increasing number of localised electrons

    Choose your answer

    10
    1 mark

    The trend in melting points of some Period 3 elements can be represented as:

    S8  > P4 > Cl2

    What intermolecular force explains this trend in melting point?

    • Permanent dipole- dipole

    • Covalent bonding

    • Hydrogen bonding 

    • Induced dipole-dipole interactions

    Choose your answer

    1
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    1 mark

    In the Periodic Table, element X is in Group 3 and element Y is in Group 16 (6). What is the likely formula of an ionic compound of X and Y?

    • X3Y6

    • X3Y2

    • X2Y3

    • X6Y3

    Choose your answer

    2
    1 mark

    What determines the order of elements in the Periodic Table?

    • First ionisation energy

    • Number of electrons in the outer shell

    • Number of protons in the nucleus

    • Relative atomic mass

    Choose your answer

    3
    1 mark

    Which element has the highest melting point?

    • Silicon

    • Phosphorus

    • Sulfur

    • Chlorine

    Choose your answer

    4
    1 mark

    Which trend in the periodic table is correct?

    • Melting point decreases from lithium to carbon

    • Boiling point decreases from fluorine to iodine

    • First ionisation energy decreases from lithium to caesium

    • First ionisation energy increases from nitrogen to oxygen

    Choose your answer

    5
    1 mark

    Which statement best explains why phosphorus has a larger first ionisation energy than sulfur?

    • P atoms have less repulsion between p-orbital electrons than S atoms

    • P atoms have a smaller nuclear charge than S atoms

    • P atoms lose an electron from the 3s subshell, while S atoms lose an electron from the 3p subshell

    • P atoms have an odd number of electrons, while S atoms have an even number

    Choose your answer

    6
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    1 mark

    The first five successive ionisation energies of an element Z are shown below.

    1st

    2nd

    3rd

    4th

    5th

    495

    4563

    6914

    9543

    13351

    What is the formula of a hydroxide of Z?

    • ZOH

    • Z(OH)2

    • Z(OH)3

    • Z(OH)4

    Choose your answer

    7
    1 mark

    Which p-block element contains atoms with one unpaired electron?

    • B

    • C

    • N

    • O

    Choose your answer

    8
    1 mark

    Which statement below shows the correct information about diamond and graphite?

    • Diamond and graphite both conduct electricity due to delocalised electrons in their structure

    • The bond angles in the two structures are not the same

    • Diamond is macromolecular and graphite is simple molecular

    • All the valence electrons are covalently bonded in both graphite and diamond

    Choose your answer

    9
    1 mark

    Consecutive elements X, Y and Z, are in the third period of the periodic table. Element Y has the highest first ionisation energy and 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

    Choose your answer

    10
    1 mark

    Which of the following metals would have the highest melting point?

    • Na

    • Mg

    • K

    • Al

    Choose your answer

    11
    1 mark

    Which statement best explains why nitrogen has a larger first ionisation energy than oxygen?

    • N atoms have less repulsion between p-orbital electrons than O atoms.

    • N atoms have a smaller nuclear charge than O atoms.

    • N atoms lose an electron from the 2s subshell, while O atoms lose an electron from the 2p subshell.

    • N atoms have an odd number of electrons, while O atoms have an even number.

    Choose your answer

    1
    1 mark

    Successive ionisation energies of four elements in Period 3 are shown below.

    Which letter could represent magnesium?

     

    1st (kJ mol-1)

    2nd (kJ mol-1)

    3rd (kJ mol-1)

    4th (kJ mol-1)

    5th (kJ mol-1)

    A

    1251

    2298

    3822

    5159

    6542

    B

    738

    1451

    7733

    10543

    13630

    C

    496

    4563

    6913

    9544

    13352

    D

    578

    1817

    2745

    11577

    14842

      Choose your answer

      2
      1 mark

      Which statement about trends in first ionisation energies is correct?

      • The first ionisation energy generally increases across a period due to increased nuclear charge and shielding.

      • First ionisation energy drops between magnesium and aluminium because the outer electron is in the 3p subshell which is higher in energy than the 3s orbital. 

      • First ionisation energy drops between nitrogen and oxygen because the spin-pair repulsion of the 2p electron means that this electron is higher energy.

      • First ionisation energy down a group increases due to increased nuclear charge. 

      Choose your answer

      3
      1 mark

      The successive ionisation energies of elements X and Y are shown below.

      Element X

      IE

      1st

      2nd

      3rd

      4th

      5th

      6th

      7th

      8th

      IE (kJ mol-1)

      590

      1145

      4912

      6491

      8153

      10496

      12270

      14206

       

      Element Y

      IE

      1st

      2nd

      3rd

      4th

      5th

      6th

      7th

      8th

      IE (kJ mol-1)

      1012

      1907

      2914

      4964

      6274

      21267

      25431

      29872

       

      X and Y form ions with the same electron configuration as argon.

      What are the identities of elements X and Y respectively?

      • Calcium and phosphorus 

      • Sodium and oxygen

      • Magnesium and nitrogen

      • Phosphorus and potassium 

      Choose your answer

      4
      1 mark

      In which row is the first ionisation energy of atom Y greater than that of atom X?

       

      Element X

      Element Y

      A

      1s22s22p63s2

      1s22s22p63s23p1

      B

      1s22s22p63s23p3

      1s22s22p63s23p4

      C

      1s22s22p63s23p5

      1s22s22p63s23p6

      D

      1s22s22p63s23p6

      1s22s22p63s23p64s1

       

        Choose your answer

        5
        1 mark

        Which row is correct?

        Property

        Increasing order

        Atomic radius

        Nitrogen, oxygen, fluorine

        First ionisation energy

        Lithium, beryllium, boron

        Electronegativity

        Nitrogen, carbon, boron

        Melting Point

        Neon, fluorine, oxygen

         

          Choose your answer