A LevelChemistryOCRExam Questions3. Periodic Table & EnergyPeriodicity

Periodicity (OCR A Level Chemistry A): Exam Questions

Exam code: H432

3 hours42 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 sodium atom has a larger atomic radius than a sulfur atom

  • A sodium atom has a larger first ionisation energy than a sulfur atom

  • A sodium atom has more protons than a sulfur atom

  • A sodium atom has more valence electrons than a sulfur atom

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 

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6
1 mark

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

  • s block

  • d block

  • f block

  • p block

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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

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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

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7
1 mark

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

  • B

  • C

  • N

  • O

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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

        6
        1 mark

        Strontium reacts more vigorously with water than calcium does.

        Which statement explains this trend in reactivity?

        • Strontium loses its two outer electrons more easily than calcium due to increased atomic radius and shielding.

        • Strontium has a smaller atomic radius than calcium.

        • The nuclear attraction for the outer electrons is stronger in strontium than in calcium.

        • Strontium reacts more vigorously because it has a higher nuclear charge than calcium.

        Choose your answer