Secondary 4 Pure Chemistry Periodic Table Quiz

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Secondary 4 Pure Chemistry Quiz - Periodic Table

Name: __________________________
Class: __________________________
Date: __________________________
Score: ________ / 40

Duration: 45 minutes
Total Marks: 40

Instructions:

1. Answer all questions in the spaces provided.
2. The number of marks is given in brackets [ ] at the end of each question or part question.
3. You may use a periodic table (provided in your exam booklet or reference sheet).
4. Write clearly and use correct chemical terminology.

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Section A: Multiple Choice & Short Recall (Questions 1-5)

1. Which property increases down Group 1 (the alkali metals)?
A. Melting point
B. Density
C. Electronegativity
D. First ionization energy
[1]

2. Element X is in Group 17 and Period 3 of the Periodic Table. Which statement about X is correct?
A. It is a solid at room temperature.
B. It forms an ion with a 1+ charge.
C. It is more reactive than the element above it in the group.
D. It has 7 electrons in its outer shell.
[1]

3. Why are noble gases (Group 18) generally unreactive?
A. They have high atomic masses.
B. They have a full outer shell of electrons.
C. They are all gases at room temperature.
D. They have low boiling points.
[1]

4. Which of the following elements is a transition metal?
A. Calcium
B. Iron
C. Silicon
D. Bromine
[1]

5. State the trend in the melting points of the elements in Group 17 (Halogens) as you go down the group.

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[1]

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Section B: Atomic Structure & Definitions (Questions 6-10)

6. Define the term isotope.

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[2]

7. An atom of an element has 13 protons and 14 neutrons.
(a) What is the nucleon number (mass number) of this atom? _______________ [1]
(b) In which Group of the Periodic Table is this element found? _______________ [1]

8. The table below shows some properties of three elements in Group 1: Lithium, Sodium, and Potassium.

Element	Melting Point (°C)	Reaction with Water
Lithium	180	Reacts steadily, fizzing
Sodium	98	Reacts vigorously, melts into a ball
Potassium	63	Reacts very vigorously, lilac flame

(a) Predict the melting point of Rubidium (the next element down the group).
Circle the most likely value: 100°C / 40°C / 200°C
[1]

9. Chlorine, Bromine, and Iodine are halogens (Group 17).

(a) Describe the colour and physical state of Bromine at room temperature and pressure.
Colour: __________________________
State: __________________________
[2]

10. Transition elements have different properties compared to Group 1 metals.

(a) State two physical properties typical of transition elements.

1. ---

2. ---

[2]

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Section C: Reactivity & Trends (Questions 11-15)

11. Explain, in terms of atomic structure, why Potassium is more reactive than Sodium.

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[3]

12. Write a balanced chemical equation, including state symbols, for the reaction between Sodium and water.

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[2]

13. A student adds aqueous chlorine to a solution of potassium iodide.
(i) State the observation.
___________________________________________________________________
[1]
(ii) Write the ionic equation for this reaction.
___________________________________________________________________
[2]

14. Explain why the reaction in Question 13 occurs, referring to the reactivity of the halogens.

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[2]

15. Element Z has the electron configuration 2, 8, 18, 7.

(a) In which Group and Period is Element Z located?
Group: _______________
Period: _______________
[2]

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Section D: Data Analysis & Application (Questions 16-20)

16. Would Element Z (from Q15) be more or less reactive than Chlorine? Explain your answer.

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[3]

17. The table below shows the atomic radii and first ionization energies for the Period 3 elements Sodium to Argon.

Element	Na	Mg	Al	Si	P	S	Cl	Ar
Atomic Radius (nm)	0.186	0.160	0.143	0.117	0.110	0.104	0.099	0.097
1st Ionization Energy (kJ/mol)	496	738	578	789	1012	1000	1251	1521

(a) Describe the trend in atomic radius across Period 3.

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[1]

18. Explain the trend in atomic radius across Period 3 in terms of protons and electron shells.

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[3]

19. There is a general increase in first ionization energy across Period 3, but Aluminium (Al) has a lower ionization energy than Magnesium (Mg). Suggest a reason for this drop.

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[2]

20. An unknown element, E, reacts with oxygen to form an oxide with the formula $EO_2$. This oxide is a solid with a very high melting point and does not conduct electricity.

(a) In which Group of the Periodic Table is element E likely to be found? _______________ [1]
(b) Is element E a metal or a non-metal? Explain your choice. _________________________ [1]
(c) Suggest one identity for element E. _______________ [1]

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Secondary 4 Pure Chemistry Quiz - Periodic Table (Answer Key)

1. B
Explanation: Density generally increases down Group 1. Melting point, electronegativity, and ionization energy all decrease.

2. D
Explanation: Group 17 elements have 7 valence electrons. A is incorrect (Chlorine is gas). B is incorrect (forms 1-). C is incorrect (reactivity decreases down Group 17).

3. B
Explanation: Noble gases have a stable octet (full outer shell), making them energetically stable and unreactive.

4. B
Explanation: Iron is a d-block element. Calcium is Group 2, Silicon is Group 14, Bromine is Group 17.

5. Melting points increase down Group 17.
Explanation: As the molecules get larger, the van der Waals forces between molecules become stronger, requiring more energy to overcome.

6. Isotopes are atoms of the same element (1 mark) with the same proton number but different nucleon numbers (or different numbers of neutrons) (1 mark).

7.
(a) 27 (13 protons + 14 neutrons) [1]
(b) Group 13 (or III) [1]
Explanation: 13 electrons means configuration 2,8,3. 3 valence electrons = Group 13.

8.
(a) 40°C [1]
Explanation: Trend is decreasing (180 -> 98 -> 63). 40 is the only value lower than 63.

9.
(a) Colour: Red-brown / Orange-brown [1]
State: Liquid [1]

10.
(a) Any two: High melting/boiling points, High density, Hard, Strong, Good conductors of heat/electricity, Magnetic. [2]

11. Potassium has more electron shells than Sodium (1). The outer electron is further from the nucleus and experiences more shielding (1). Therefore, the attraction between the nucleus and the outer electron is weaker, making it easier to lose (1).

12. $2Na(s) + 2H_2O(l) \rightarrow 2NaOH(aq) + H_2(g)$ [2]
1 mark for correct formulae, 1 mark for balancing and state symbols.

13.
(i) The solution turns brown / dark red / black precipitate forms (due to Iodine). [1]
(ii) $Cl_2 + 2I^- \rightarrow 2Cl^- + I_2$ [2]
1 mark for correct species, 1 mark for balancing.

14. Chlorine is more reactive than Iodine (1). Chlorine can displace Iodine from its halide solution because it is higher in Group 17 / has higher oxidizing power (1).

15.
(a) Group 17 [1], Period 4 [1]
Explanation: 7 valence electrons = Group 17. 4 shells = Period 4.

16. Less reactive [1].
Explanation: Element Z is further down the group than Chlorine (Period 4 vs Period 3) [1]. The outer electrons are further from the nucleus and more shielded, making it harder to gain an electron / lower effective nuclear attraction for incoming electrons [1].

17.
(a) Atomic radius decreases across the period. [1]

18. The number of protons (nuclear charge) increases [1]. The electrons are added to the same principal quantum shell (same shielding) [1]. Therefore, the attraction between the nucleus and the outer electrons increases, pulling the shell closer [1].

19. The electron removed from Aluminium is from a 3p orbital, which is higher in energy / further from the nucleus than the 3s orbital electrons removed from Magnesium [1]. Or: The 3p electron in Al is shielded by the 3s electrons [1].

20.
(a) Group 14 (or IV) [1]
Explanation: $EO_2$ implies valency of 4.
(b) Non-metal [1].
Explanation: Giant covalent structure (high MP, non-conductor) implies a non-metal like Silicon.
(c) Silicon [1]