Periodicity (OCR A Level Chemistry)

Exam Questions

3 hours40 questions
11 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

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21 mark

Which element has the highest melting point?

  • Silicon

  • Phosphorus

  • Sulfur

  • Chlorine

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31 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

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41 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

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    51 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 

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    61 mark

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

    • s block

    • d block

    • f block

    • p block

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    71 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)

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    81 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

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    91 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

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    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

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    21 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

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    31 mark

    Which element has the highest melting point?

    • Silicon

    • Phosphorus

    • Sulfur

    • Chlorine

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    41 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

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    51 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

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    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

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    71 mark

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

    • B

    • C

    • N

    • O

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    81 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

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    91 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

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    101 mark

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

    • Na

    • Mg

    • K

    • Al

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    111 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.

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    11 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

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      21 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. 

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      31 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 

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      41 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

       

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        51 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

         

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