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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

Quizzes




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Topic Content:

  • Theory Questions & Answers – Quantum Numbers Orbitals & Electrical Structure

Theory Questions – Quantum Numbers Orbitals & Electrical Structure

1. Name and explain four quantum numbers that define an atom.

2. (a) In which orbital will the fifth electron in Nitrogen atom most likely   to be found?

(b). Draw the orbital

3. (a) What is an atomic orbital?

(b) Give the number of orbitals that are contained in the following: s, p, d and f subshells. 

4. Without referring to the periodic table, name the elements, give their electronic structure, and name the groups to which the elements with the following atomic numbers belong: 3, 9, 12, 17, and 20.

 

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Evaluation Questions

1. Name and explain four quantum numbers that define an atom.

Answer:

Principal Quantum Number [n]: Each energy level can take 2n2 electrons. They are denoted by the letters K L M N. The principal quantum number (n) has integral values of 1, 2, 3, 4 etc.

Subsidiary [Or Azimuthal] Quantum Number [l]: Each energy level consists of one or more energy sub-levels. Subsidiary quantum numbers [l] have integral values ranging from 0, 1, 2, 3, n-1

Magnetic Quantum Number [m]: Magnetic quantum number shows the number of orbitals in each energy level and sub-level. It has values ranging from -1 through 0 to +1.

Spin Quantum Number [s]: The spinning of an electron about its own axis in an orbital is due to its magnetic property. The spin quantum number has values ½ and –½

 

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These show that there are two directions of spin: clockwise and anti-clockwise. Each energy level in a subshell can hold two electrons of opposite spin. This rule is called the Pauli Exclusion Principle.

 

2. (a) In which orbital will the fifth electron in the Nitrogen atom most likely be found?

Answer:p-orbital

 

(b) Draw the orbital

Answer:

 

3. (a) What is an atomic orbital?

Answer: An atomic orbital is a region or space in which an electron in a given energy level is most likely to be found

(b) Give the number of orbitals that are contained in the following:

s, p, d and f subshells. 

Answer:

s – One number of orbital

p – Three numbers of orbital

d – Five numbers of orbital

f – Seven numbers of orbital

 

4. Without referring to the periodic table, name the elements, give their electronic structure, and name the groups to which the elements with the following atomic numbers belong: 3, 9, 12, 17, and 20.

Answer:

Atomic Number Name of elements Electronic structure Groups
3 Lithium (Li) 1S2 2S1 Alkali metals (1)
9 Fluorine (F) 1S2 2S2 2P5 Halogens (7)
12 Magnesium (Mg) 1S2 2S2 2P6 3S2 Alkaline earth metals (2)
17 Chlorine (Cl) 1S2 2S2 2P6 3S2 3P5 Halogens (7)
20 Calcium (Ca) 1S2 2S2 2P6 3S2 3P6 4S2 Alkaline earth metals (2)

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