O Level Chemistry Atomic Structure Bonding Quiz

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O-Level Chemistry Quiz - Atomic Structure Bonding

Name: ___________________________
Class: ___________________________
Date: ___________________________
Score: _______ / 40

Duration: 50 minutes
Total Marks: 40

Instructions:

• Answer all 20 questions.
• Section A: Multiple-choice style short items (1 mark each).
• Section B: Structured short-answer questions (2 marks each).
• Section C: Extended response with diagrams, data, and reasoning (3–4 marks each).
• Write your answers in the spaces provided.
• Use proper chemical notation where required.

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Section A (Questions 1–5, 1 mark each)

1. An atom of sodium has proton number 11 and nucleon number 23. How many neutrons does it have?

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2. Which of the following is an isotope of carbon-12 ($^{12}_{6}\text{C}$)?

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3. What type of bonding is present in magnesium oxide?

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4. In a covalent bond, what is shared between two atoms?

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5. Which particle is responsible for electrical conduction in metallic bonding?

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Section B (Questions 6–10, 2 marks each)

6. State the number of protons, electrons, and neutrons in an atom of $^{40}_{20}\text{Ca}$.
Protons: _______
Electrons: _______
Neutrons: _______

7. Write the formula of the ion formed when a potassium atom loses one electron.

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8. Draw a dot-and-cross diagram to show the bonding in a hydrogen molecule ($\text{H}_2$).

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9. Explain why diamond has a very high melting point.

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10. A sample of chlorine contains two isotopes: $^{35}\text{Cl}$ and $^{37}\text{Cl}$. What is meant by the term "isotopes"?

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Section C (Questions 11–20, 3–4 marks each)

11. Chlorine has proton number 17. Write the electronic configuration of a chloride ion ($\text{Cl}^-$).
_________________________________ (3 marks)

12. Magnesium reacts with oxygen to form magnesium oxide.
(a) Write the equation for the formation of magnesium oxide from its ions. (2 marks)
(b) Draw the dot-and-cross diagram for $\text{MgO}$. (2 marks)

13. The table below shows the proton number and nucleon number of three atoms.

Atom	Proton number	Nucleon number
X	6	12
Y	6	14
Z	7	14

(a) Which two atoms are isotopes of the same element? (1 mark)
(b) State the number of neutrons in atom Y. (1 mark)
(c) Explain your answer to (a). (2 marks)

14. Describe the structure and bonding in graphite and explain why it is a good lubricant.
_________________________________ (4 marks)

15. A student draws the following diagram to represent a sodium atom.

Image pending generation: diagram for Q15.

State the electron arrangement of sodium and explain how it forms a sodium ion. (3 marks)

16. Ethanol ($\text{C}_2\text{H}_5\text{OH}$) is a simple molecular covalent substance. Explain why it has a low boiling point. (3 marks)

17. The diagram shows the arrangement of ions in a crystal of sodium chloride.

Image pending generation: diagram for Q17.

(a) What is the term for this type of structure? (1 mark)
(b) Explain why solid sodium chloride does not conduct electricity but molten sodium chloride does. (3 marks)

18. Silicon dioxide ($\text{SiO}_2$) and carbon dioxide ($\text{CO}_2$) are both oxides of Group 14 elements.
(a) State the type of structure for each. (2 marks)
(b) Explain why $\text{SiO}_2$ has a much higher melting point than $\text{CO}_2$. (2 marks)

19. A sample of copper is alloyed with zinc to form brass.
(a) What is an alloy? (1 mark)
(b) Explain why brass is harder than pure copper. (3 marks)

20. The relative atomic masses of two isotopes of boron are 10 and 11. In a sample, 20% is $^{10}\text{B}$ and 80% is $^{11}\text{B}$. Calculate the relative atomic mass of the boron sample. Show your working. (4 marks)

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O-Level Chemistry Quiz - Atomic Structure Bonding: Answer Key

Total Marks: 40
Topic: Atomic Structure Bonding

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Section A Answers (1 mark each)

1. 12
Teaching note: Neutrons = nucleon number − proton number = 23 − 11 = 12. The nucleon number is the total of protons + neutrons.

2. $^{13}_{6}\text{C}$ (or any carbon with proton number 6 and different nucleon number)
Teaching note: Isotopes have the same proton number but different nucleon number. Carbon always has 6 protons.

3. Ionic bonding
Teaching note: Magnesium oxide is formed by transfer of electrons from Mg to O, forming Mg²⁺ and O²⁻ held by electrostatic forces.

4. A pair of electrons (shared electron pair)
Teaching note: A covalent bond is a shared pair of electrons between two non-metal atoms.

5. Delocalised electrons (electrons in the "sea of electrons")
Teaching note: In metallic bonding, valence electrons are free to move throughout the metal lattice, carrying current.

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Section B Answers (2 marks each)

6. Protons: 20, Electrons: 20, Neutrons: 20
Working: Proton number = 20 → 20 protons. Neutral atom → 20 electrons. Neutrons = 40 − 20 = 20.
Marking: 1 mark for protons/electrons correct, 1 mark for neutrons.

7. $\text{K}^+$
Teaching note: Potassium (proton no. 19) loses 1 electron to achieve stable noble gas config, forming K⁺.

8. H• + •H → H••H (or H:H with crosses/dots shown)
Teaching note: Each H contributes 1 electron; they share a pair. Award 2 marks for correct shared pair diagram with both atoms showing 2 electrons.

9. Diamond has a giant covalent structure with many strong covalent bonds between carbon atoms in a tetrahedral network. A large amount of energy is needed to break these bonds, so melting point is very high.
Marking: 1 mark for giant covalent / strong covalent bonds, 1 mark for energy needed to break bonds.

10. Atoms of the same element with the same number of protons but different numbers of neutrons (therefore different nucleon numbers).
Marking: 1 mark same proton number, 1 mark different neutron/nucleon number.

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Section C Answers (3–4 marks each)

11. 2,8,8 (3 marks)
Teaching note: Cl has 17 protons → 17 e⁻ as atom: 2,8,7. Gains 1 e⁻ to form Cl⁻ → 18 e⁻: 2,8,8.
Marking: 1 mark for 2,8,7 atom reference, 1 mark for gain of electron, 1 mark for 2,8,8.

12. (a) $\text{Mg}^{2+} + \text{O}^{2-} \rightarrow \text{MgO}$ (2 marks)
(b) Dot-and-cross: Mg (2,8,2) loses 2 e⁻ to O (2,6) → Mg²⁺ (2,8) and O²⁻ (2,8,8); show transfer. (2 marks)
Teaching note: Mg transfers 2 electrons to O; ionic compound formed. Award for correct electron origin and final arrangements.

13. (a) X and Y (1 mark)
(b) 8 neutrons (1 mark: 14 − 6)
(c) X and Y both have proton number 6 (same element, carbon) but different nucleon numbers (12 vs 14), meaning different neutron numbers. This matches the definition of isotopes. (2 marks)
Marking: 1 for same proton no., 1 for different nucleon/neutron.

14. Graphite has a giant covalent structure of carbon atoms arranged in layers of hexagonal rings. Each carbon forms 3 covalent bonds, leaving 1 delocalised electron per atom (conducts electricity). Layers are held by weak van der Waals forces, so they slide over each other easily, making graphite a good lubricant. (4 marks)
Marking: 2 for structure (layers, covalent, delocalised e⁻), 2 for sliding/weak forces explanation.

15. Electron arrangement: 2,8,1. Sodium atom loses 1 electron from outer shell to form Na⁺ (2,8), achieving stable octet like neon. (3 marks)
Teaching note: From diagram, shell 3 has 1 e⁻; loss gives 2,8.
Marking: 1 for 2,8,1, 1 for loss of 1 e⁻, 1 for Na⁺ stable config.

16. Ethanol consists of simple molecules with weak intermolecular forces (van der Waals / hydrogen bonds between molecules). Little energy is needed to overcome these forces, so it boils at low temperature. (3 marks)
Marking: 1 simple molecular, 1 weak forces, 1 low energy to separate.

17. (a) Giant ionic lattice (1 mark)
(b) Solid NaCl: ions fixed in lattice, no mobile charge carriers → no conduction. Molten NaCl: ions free to move, carry current → conducts. (3 marks)
Marking: 1 fixed ions, 1 mobile when molten, 1 conduction due to moving ions.

18. (a) $\text{SiO}_2$: giant covalent; $\text{CO}_2$: simple molecular. (2 marks)
(b) $\text{SiO}_2$ has a network of strong covalent bonds throughout requiring lots of energy to break; $\text{CO}_2$ molecules held by weak intermolecular forces only. (2 marks)

19. (a) A mixture of a metal with another element. (1 mark)
(b) Zinc atoms disrupt the regular layers of copper atoms, making it harder for layers to slide, so brass is harder than pure copper. (3 marks)
Marking: 1 disruption of layers, 2 explanation of hardness.

20. $A_r = (0.20 \times 10) + (0.80 \times 11) = 2.0 + 8.8 = 10.8$ (4 marks)
Working:
Step 1: Convert % to fractions: 20% = 0.20, 80% = 0.80.
Step 2: Multiply each mass by abundance: 10×0.20=2.0; 11×0.80=8.8.
Step 3: Sum = 10.8.
Marking: 1 for %→decimal, 1 per product, 1 for sum.