Past Paper Practice
Topic 2.2.3: Electronic Configuration
Cambridge IGCSE Chemistry 0620 | Papers 2, 4 & 6 Style
⚠️ EXAMINATION INSTRUCTIONS
- • Answer ALL questions in the spaces provided
- • Show all working for calculation questions
- • For drawing questions, label all parts clearly
- • Use the "Reveal Answer" button to check your work after attempting each question
ASection A: Writing Electronic Configurations
Question 1
[1 mark]Write the electronic configuration of Potassium (K, proton number 19).
Question 2
[1 mark]Write the electronic configuration of the Aluminium ion (Al³⁺). The proton number of aluminium is 13.
Question 3
[1 mark]Write the electronic configuration of Chlorine (Cl, proton number 17).
Question 4
[1 mark]Write the electronic configuration of the Oxide ion (O²⁻). The proton number of oxygen is 8.
Question 5
[1 mark]An element has the electronic configuration 2,8,8,2. State the group number of this element in the Periodic Table.
BSection B: Drawing Electronic Structures
Drawing Requirements: You must show (1) the nucleus with correct number of protons, (2) all electron shells as circles, and (3) all electrons positioned on the shells.
Question 6
[2 marks]Draw the electronic structure of Oxygen (O, proton number 8). Show the nucleus and all electrons.
Draw your answer in the space above
Question 7
[2 marks]Draw the electronic structure of Sodium (Na, proton number 11). Show the nucleus and all electrons.
Draw your answer in the space above
Question 8
[2 marks]Draw the electronic structure of a Magnesium ion (Mg²⁺). The proton number of magnesium is 12.
Draw your answer in the space above
Question 9
[2 marks]Draw the electronic structure of Fluorine (F, proton number 9). Show the nucleus and all electrons.
Draw your answer in the space above
Question 10
[2 marks]Draw the electronic structure of Neon (Ne, proton number 10). Show the nucleus and all electrons.
Draw your answer in the space above
CSection C: Identification from Configuration
Question 11
[1 mark]Element X has the electronic configuration 2,8,5. Identify element X.
Question 12
[2 marks]Element Y has the electronic configuration 2,8,8. (a) Identify element Y. (b) State which group of the Periodic Table element Y belongs to.
Question 13
[2 marks]An element has the electronic configuration 2,8,7. (a) How many electrons are in the outer shell? (b) Suggest which group this element belongs to.
Question 14
[2 marks]Ion Z has the electronic configuration 2,8 and a charge of 2+. (a) How many protons does ion Z have? (b) Identify element Z.
Question 15
[3 marks]An element has 3 electron shells. The outer shell contains 4 electrons. (a) Write the electronic configuration. (b) Identify the element. (c) State the period number.
📋 Exam Summary & Key Points
🎯 Writing Configurations:
- • First shell: maximum 2 electrons
- • Second shell: maximum 8 electrons
- • Third shell: fills to 8 before fourth starts
- • Write as: 2,8,8,1 (comma-separated)
🎨 Drawing Structures:
- • Always label the nucleus with protons (e.g., 8+)
- • Draw shells as circles around nucleus
- • Place electrons evenly on each shell
- • Check: Total electrons = Proton number (for atoms)
🔍 Ions vs Atoms:
- • Positive ions: LOSE electrons (fewer electrons than protons)
- • Negative ions: GAIN electrons (more electrons than protons)
- • Nucleus never changes (proton number = atomic number)
- • Example: Mg²⁺ has 12p but only 10e⁻
📊 Periodic Table Links:
- • Number of shells = Period number
- • Outer shell electrons = Group number (I-VII)
- • Group 0: Full outer shell (8 electrons)
- • Example: 2,8,7 = Period 3, Group VII
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