Secondary 3 Chemistry Atomic Structure Bonding Quiz

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Secondary 3 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.
• For dot-and-cross diagrams, show only valence electrons.
• Use a ruler for any diagrams where appropriate.

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Section A: Atomic Structure & Fundamentals (Questions 1-7)

1. What is meant by the term monatomic? [1] \

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2. Draw the electronic structure of neon (Ne). [1]
   
   
   
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3. An element X has a nucleon number of 27 and 14 neutrons. (a) State the proton number of element X. [1] \

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   (b) Identify element X. [1] \

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4. Define the term isotopes. [2] \

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5. An element has two isotopes with relative masses of 35 and 37. The relative atomic mass of the element is 35.5. Which isotope is the most abundant? [1] \

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6. State the relative charge and relative mass of a proton. [2] Charge: ____________________
   Mass: _____________________

7. Explain why noble gases are chemically unreactive in terms of their electronic structure. [2] \

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Section B: Chemical Bonding (Questions 8-14)

8. Draw the 'dot and cross' diagram to show the bonding in magnesium oxide (MgO). Show only valence electrons. [2]
   
   
   
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9. Draw the 'dot and cross' diagram to show the bonding in phosphorus trichloride ($\text{PCl}_3$). Show only valence electrons. [2]
   
   
   
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10. Describe the formation of a covalent bond between two hydrogen atoms. [2] \

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11. Describe metallic bonding in terms of the arrangement of ions and electrons. [2] \

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12. Draw the 'dot and cross' diagram to show the bonding in carbon tetrachloride ($\text{CCl}_4$). Show only valence electrons. [2]
    
    
    
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13. Explain why ionic compounds generally have higher melting points than simple molecular covalent compounds. [3] \

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14. State whether the following compounds are ionic or covalent: [2] (a) Potassium Iodide: ____________________ (b) Sulfur Dioxide: ____________________

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Section C: Structure and Properties (Questions 15-20)

15. Compare the structures of diamond and graphite. Explain why graphite can conduct electricity while diamond cannot. [3] \

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16. Which macromolecule is able to conduct electricity? [1] \

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17. Sodium chloride ($\text{NaCl}$) has a melting point of 801 °C, while sulfur hexafluoride ($\text{SF}_6$) has a melting point of -51 °C. Explain this difference in terms of structure and bonding. [3] \

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18. By referring to the charges of the ions present, explain why magnesium oxide ($\text{MgO}$) has a higher lattice energy than sodium chloride ($\text{NaCl}$). [3] \

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19. State the atom in chlorofluorocarbons (CFCs) that is responsible for the depletion of the ozone layer. [1] \

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20. Describe the properties of a giant covalent structure in terms of its hardness and melting point. [2] \

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Answer Key - Secondary 3 Chemistry Quiz: Atomic Structure Bonding

1. Consisting of a single atom per particle/molecule. (1)
2. Diagram showing nucleus with 2 electrons in 1st shell, 8 in 2nd, 8 in 3rd. (1)
3. (a) $27 - 14 = 13$ (1) (b) Aluminium (1)
4. Atoms of the same element (same proton number) with different nucleon numbers (different number of neutrons). (2)
5. Isotope with relative mass 35. (1)
6. Charge: +1 (1); Mass: 1 (1)
7. They have a stable electronic configuration / full outer shell of electrons (2).
8. $\text{Mg}^{2+}$ (no valence electrons shown or empty shell) and $\text{O}^{2-}$ (8 valence electrons), both in square brackets with charges. (2)
9. P in center with 3 shared pairs of electrons with 3 Cl atoms. Each Cl has 6 non-bonding electrons. (2)
10. Two hydrogen atoms each contribute one electron to form a shared pair of electrons (2).
11. A lattice of positive metal ions surrounded by a "sea" of delocalised electrons (2).
12. C in center with 4 shared pairs of electrons with 4 Cl atoms. Each Cl has 6 non-bonding electrons. (2)
13. Ionic compounds have a giant ionic lattice with strong electrostatic forces of attraction between oppositely charged ions (1). These require significant energy to break (1). Simple molecular compounds have weak intermolecular forces (1).
14. (a) Ionic (1) (b) Covalent (1)
15. Diamond has a 3D tetrahedral network of C atoms; Graphite has layers of C atoms (1). Graphite has delocalised electrons that can move through the structure (1), whereas all valence electrons in diamond are fixed in covalent bonds (1).
16. Graphite (1).
17. $\text{NaCl}$ is a giant ionic lattice with strong electrostatic forces between $\text{Na}^+$ and $\text{Cl}^-$ ions (1). $\text{SF}_6$ consists of simple molecules with weak van der Waals forces/intermolecular forces (1). More energy is required to break the ionic bonds than the intermolecular forces (1).
18. $\text{Mg}^{2+}$ and $\text{O}^{2-}$ have higher charges than $\text{Na}^+$ and $\text{Cl}^-$ (1). Stronger electrostatic attraction exists between ions with higher charges (1), resulting in higher lattice energy (1).
19. Chlorine (Cl) (1).
20. Very hard (due to strong covalent bonds throughout the structure) (1) and very high melting point (requires high energy to break many strong covalent bonds) (1).