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SS2: CHEMISTRY - 1ST TERM

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  1. Periodicity and Periodic Table I | Week 1
    5 Topics
    |
    1 Quiz
  2. Quantum Numbers Orbitals & Electrical Structure | Week 2
    6 Topics
    |
    1 Quiz
  3. Periodicity and Periodic Table II | Week 3
    12 Topics
    |
    1 Quiz
  4. Periodicity and Periodic Properties III | Week 4
    11 Topics
    |
    1 Quiz
  5. Periodicity and Periodic Properties IV | Week 5
    5 Topics
    |
    1 Quiz
  6. Mass-Volume Relationship in Reaction | Week 6
    8 Topics
    |
    1 Quiz
  7. Types of Reactions: Oxidation and Reduction | Week 7 & 8
    7 Topics
    |
    1 Quiz
  8. Oxidation – Reduction Reaction II | Week 9
    3 Topics
    |
    1 Quiz
  9. Electrode Potential and Electrochemical Cells I | Week 10
    6 Topics
    |
    1 Quiz
  10. Electrode Potential and Electrochemical Cells II | Week 11
    5 Topics
    |
    1 Quiz
  11. Electrolysis I | Week 12
    8 Topics
    |
    1 Quiz
  12. Electrolysis II | Week 13
    8 Topics
    |
    1 Quiz

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Topic Content:

  • Theory Questions & Answers – Periodicity and Periodic Table II

Theory Questions – Periodicity and Periodic Table II:

1. (a) The ionization energies of Lithium and Potassium are 5.4 and 4.3 respectively; predict the ionization energy of Sodium.

(b) 

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Evaluation Questions

    1. (a) The ionization energies of Lithium and Potassium are 5.4 and 4.3 respectively; predict the ionization energy of Sodium.

    Answer:  Ionisation energy decreases in a group from top to bottom as atomic size increases. The ionization energy will be between 5.4 and 4.3 and can be a value of 4.9.

     

    (b) Explain why the second ionization energy of Sodium is much bigger than the first, whereas the magnitude of the difference between the first and second ionization energy of magnesium is not much.

    Answer:

    Sodium only has one electron in its outermost shell (3rd shell) after removing that, the second shell contains  8 complete electrons (forming a stable octet) it will be hard to remove electrons from the second shell. Unlike Magnesium which has two electrons in its outermost shell, after removing the first electron it will be easy to remove the second as it’s a single electron and also factoring electron repulsion.

     

    2 (a) Define the following

    i. Ionization Energy

    Answer:  Ionization Energy is the energy required to remove the most loosely bound electron from a gaseous atom to form a positive ion

    ii. Atomic Radius

    Answer:  Atomic Radius is the distance between the centre of the nucleus and the outermost electron shell of an atom. It decreases across the period and increases down the group.

    iii. Electronegativity

    Answer:  Electronegativity is the power of an atom in a molecule to attract electrons. It increases across the period and decreases down the group.

     

    (b) Discuss their trend across the period and down the group in the periodic table.

    Answer:

    2b i. Ionization Energy increases across the period and decreases down the group

    ii. Atomic Radius decreases across the period and increases down the group

    iii. Electronegativity increases across the period and decreases down the group.

     

    3(a) List three periodic properties of elements that generally increase across the period of the periodic table.

    Answer:

    • Ionization Energy
    • Electron Affinity
    • Electronegativity

     

    (b) Arrange the following elements in order of decreasing electronegativity 16S, 9F, 17Cl.

    16S, 9F, 17Cl

    Answer:

    In order of decreasing electronegativity

    9F

    17Cl

    16S

    ∴ 9F > 17Cl > 16S

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