Secondary 4 Combined Science Chemistry Atomic Structure Bonding Quiz

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Secondary 4 Combined Science Chemistry Quiz - Atomic Structure Bonding

Name: ____________________
Class: ____________________
Date: ____________________
Score: ________ / 45

Duration: 60 Minutes
Total Marks: 45 Marks

Instructions:

• Answer all questions in the spaces provided.
• Show all working for calculation questions.
• Use a ruler for any diagrams.

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Section A: Atomic Structure and the Periodic Table (Questions 1-7)

1. State the number of protons, electrons, and neutrons in an atom of $^{23}_{11}\text{Na}$. [2] Protons: _________ Electrons: _________ Neutrons: _________

2. Define the term isotopes. [1]

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3. An element X has the electronic structure 2, 8, 7. (a) Identify the group and period of element X. [2] Group: _________ Period: _________ (b) Explain how the electronic structure determines its period. [1] ___________________________________________________________________________

4. Compare the atomic radius of Lithium (Li) and Potassium (K). Which is larger? Explain your answer. [2]

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5. Draw the electronic structure of a Magnesium ion ($\text{Mg}^{2+}$). Show only the outer electrons. [2] (Space for drawing)

6. Explain why Group 1 elements are more reactive as you move down the group. [2]

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7. Complete the table below for the following particles: [3]

Particle	Protons	Electrons	Neutrons
$\text{Cl}^-$
$\text{Ca}^{2+}$

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Section B: Ionic and Covalent Bonding (Questions 8-15)

8. Describe the formation of an ionic bond between Sodium (Na) and Chlorine (Cl). [2]

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9. Draw a dot-and-cross diagram to show the bonding in a molecule of Hydrogen Chloride ($\text{HCl}$). Show outer electrons only. [2] (Space for drawing)

10. Explain why Sodium Chloride ($\text{NaCl}$) has a high melting point. [2]

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11. A substance Y is a gas at room temperature and does not conduct electricity. State the type of bonding present in substance Y. [1]

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12. Draw the electronic structure of a Nitrogen molecule ($\text{N}_2$). Show only outer electrons. [2] (Space for drawing)

13. Compare the electrical conductivity of Graphite and Diamond. Explain the difference in terms of their structure. [3]

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14. Explain why covalent molecular substances, such as water, generally have lower boiling points than ionic compounds. [2]

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15. Describe the structure and bonding in a piece of Copper metal. [2]

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Section C: Properties and Applications (Questions 16-20)

16. Substance Z is a solid that conducts electricity in both the solid and molten state. Identify the type of bonding in Z. [1]

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17. Why is Aluminium widely recycled rather than being extracted from its ore (bauxite)? [1]

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18. Given the relative atomic masses: $\text{C}=12, \text{O}=16, \text{H}=1$. Calculate the relative molecular mass of Glucose ($\text{C}_6\text{H}_{12}\text{O}_6$). [2]

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19. A compound has the formula $\text{Al}_2\text{O}_3$. (a) State the type of bonding in this compound. [1] ___________________________________________________________________________ (b) Explain why this compound is soluble in water but does not conduct electricity as a solid. [2] ___________________________________________________________________________

20. Predict the formula of the compound formed between Magnesium (Group 2) and Nitrogen (Group 15). Show your working. [2]

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Answer Key - Atomic Structure Bonding Quiz

1. Protons: 11, Electrons: 11, Neutrons: 12 (23 - 11 = 12). [2 marks]
2. Atoms of the same element with the same number of protons but different numbers of neutrons. [1 mark]
3. (a) Group 17 (or VII), Period 3. [2 marks] (b) It has 3 occupied electron shells. [1 mark]
4. Potassium (K) is larger. It has more electron shells than Lithium, increasing the distance between the nucleus and the valence electrons. [2 marks]
5. Diagram should show $\text{Mg}^{2+}$ with 2 shells (2, 8) and a $2+$ charge indicated. [2 marks]
6. As you move down the group, atomic radius increases. The valence electron is further from the nucleus, resulting in weaker nuclear attraction and making it easier to lose the electron. [2 marks]
7. $\text{Cl}^-$: P=17, E=18, N=18; $\text{Ca}^{2+}$: P=20, E=18, N=20. [3 marks]
8. Sodium loses one valence electron to become $\text{Na}^+$; Chlorine gains one electron to become $\text{Cl}^-$. The strong electrostatic attraction between the oppositely charged ions forms the ionic bond. [2 marks]
9. Diagram showing H sharing one pair of electrons with Cl. Cl should have 7 other valence electrons. [2 marks]
10. It has a giant ionic lattice with strong electrostatic forces of attraction between $\text{Na}^+$ and $\text{Cl}^-$ ions, which require significant energy to overcome. [2 marks]
11. Covalent bonding (molecular). [1 mark]
12. Diagram showing two N atoms sharing three pairs of electrons (triple bond). [2 marks]
13. Graphite conducts; Diamond does not. Graphite has delocalised electrons that can move through the structure; Diamond has all valence electrons bonded in a rigid tetrahedral lattice. [3 marks]
14. Covalent molecules have weak intermolecular forces of attraction between molecules, which require little energy to overcome compared to the strong ionic bonds in a lattice. [2 marks]
15. Metallic bonding: A lattice of positive metal ions surrounded by a "sea" of delocalised electrons. [2 marks]
16. Metallic bonding. [1 mark]
17. Recycling requires significantly less energy than the extraction of aluminium from bauxite. [1 mark]
18. $(6 \times 12) + (12 \times 1) + (6 \times 16) = 72 + 12 + 96 = 180$. [2 marks]
19. (a) Ionic bonding. [1 mark] (b) In solid state, ions are in fixed positions and cannot move. When dissolved in water, the lattice breaks and ions are free to move and carry charge. [2 marks]
20. $\text{Mg}^{2+}$ and $\text{N}^{3-}$. To balance charges: $3 \times (+2) + 2 \times (-3) = 0$. Formula: $\text{Mg}_3\text{N}_2$. [2 marks]