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Secondary 3 Chemistry Periodic Table Quiz

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Questions

Secondary 3 Chemistry Quiz - Periodic Table

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

Duration: 45 minutes
Total Marks: 40

Instructions:

Answer ALL questions.
Write your answers in the spaces provided.
Show all working where applicable.
The number of marks for each question is shown in brackets [ ].
You may use a Periodic Table (provided separately) for reference.

Section A: Multiple Choice & Short Answer (Questions 1–10)

Questions 1–5: Circle the correct option.

1. Which of the following elements is in Group I of the Periodic Table?
(a) Magnesium
(b) Sodium
(c) Aluminium
(d) Silicon
[1]

2. An element has the electronic configuration 2.8.6. In which period and group is this element found?
(a) Period 2, Group VI
(b) Period 3, Group VI
(c) Period 3, Group IV
(d) Period 2, Group IV
[1]

3. Which of the following is a property of elements in Group VII?
(a) They are all metals.
(b) They form ions with a 1+ charge.
(c) They exist as diatomic molecules.
(d) They are good conductors of electricity.
[1]

4. Going across Period 3 from left to right, what happens to the atomic radius?
(a) It increases.
(b) It decreases.
(c) It remains constant.
(d) It first increases, then decreases.
[1]

5. Which element in Period 3 has the highest melting point?
(a) Sodium
(b) Silicon
(c) Chlorine
(d) Argon
[1]

Questions 6–10: Write your answers in the spaces provided.

6. State the general name given to the elements in:
(a) Group I: ___________________________
(b) Group VII: ___________________________
(c) Group 0: ___________________________
[3]

7. An atom of element X has 12 protons.
(a) Write the electronic configuration of X. ___________________________
(b) State the group and period in which X is found. ___________________________
[2]

8. Define the term atomic number.

[1]

9. Explain why the elements in Group 0 are unreactive.

[2]

10. State one similarity and one difference between the elements sodium (Na) and potassium (K), both in Group I.
Similarity: _________________________________________________________________
Difference: ________________________________________________________________
[2]

Section B: Structured Response (Questions 11–17)

11. The table below shows some properties of the elements in Period 3.

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	—
Melting point (°C)	98	650	660	1410	44	119	−101	−189

(a) Describe the trend in atomic radius across Period 3. Explain this trend in terms of structure and bonding.

[2]

(b) Explain why silicon has a much higher melting point than phosphorus.

[2]

[1]

12. Element Y is in Group II and Period 3 of the Periodic Table.
(a) Write the electronic configuration of Y. ___________________________
[1]

(b) Write the formula of the ion formed by Y. ___________________________
[1]

[2]

13. Chlorine has two isotopes: chlorine-35 and chlorine-37.
(a) Define the term isotope.

[1]

(b) The relative atomic mass of chlorine is 35.5. Explain what this tells you about the relative abundances of the two isotopes.

[2]

14. The diagram below (not drawn to scale) shows a simplified representation of the Periodic Table with four elements labelled P, Q, R, and S.

|   | 1 | 2 | 13 | 14 | 15 | 16 | 17 | 0 |
|---|---|---|----|----|----|----|----|---|
| 2 |   |   |    |    |    |    |  P |   |
| 3 |   | Q |    |    |    |    |    | R |
| 4 | S |   |    |    |    |    |    |   |

(a) Identify which of P, Q, R, or S is a noble gas. Explain your reasoning.

[1]

(b) Which two elements are in the same group? State the group number.

[1]

15. The table below gives some information about four elements.

Element	Proton number	Group	Period
A	3	1	2
B	9	17	2
C	11	1	3
D	17	17	3

(a) Which two elements are in the same group? ___________________________
[1]

(b) Which element has the smallest atomic radius? Explain your answer.

[2]

16. Describe and explain the trend in reactivity of the Group I metals (alkali metals) as you go down the group. Your answer should refer to atomic structure.

[3]

17. A student makes the following statement: "Elements in the same period have similar chemical properties."
Is this statement correct? Explain your answer with reference to Period 3.

[2]

Section C: Data Interpretation & Application (Questions 18–20)

18. The graph below shows the boiling points of the elements in Group VII (halogens) plotted against their proton numbers.

(Imagine a graph with proton number on the x-axis and boiling point (°C) on the y-axis, showing an upward trend from F₂ to I₂.)

Halogen	Proton number	Boiling point (°C)
Fluorine (F₂)	9	−188
Chlorine (Cl₂)	17	−34
Bromine (Br₂)	35	59
Iodine (I₂)	53	184

(a) Describe the trend in boiling points down Group VII.

[1]

(b) Explain this trend in terms of structure and bonding.

[2]

[1]

19. A sample of an element Z reacts with chlorine to form a compound with the formula ZCl₂. The relative molecular mass of ZCl₂ is 111. (Cl = 35.5)

(a) Calculate the relative atomic mass of Z. Show your working.

[2]

(b) Using your answer to (a), identify element Z. State its group and period.

[2]

20. The table below shows the first ionisation energies of the elements in Period 2.

Element	Li	Be	B	C	N	O	F	Ne
1st ionisation energy (kJ/mol)	520	900	801	1086	1402	1314	1681	2080

(a) Define the term first ionisation energy.

[1]

(b) Describe the general trend in first ionisation energy across Period 2.

[1]

[2]

(d) Explain why the first ionisation energy of oxygen (O) is lower than that of nitrogen (N).

[2]

End of Quiz

Answers

Secondary 3 Chemistry Quiz - Periodic Table

Answer Key

1. (b) Sodium
[1 mark]
Common mistake: Students may select (a) Magnesium, which is Group II, not Group I.

2. (b) Period 3, Group VI
[1 mark]
Working: Electronic configuration 2.8.6 → 3 electron shells = Period 3; 6 valence electrons = Group VI.

3. (c) They exist as diatomic molecules.
[1 mark]
Common mistake: Students may select (b), confusing Group VII (1− ions) with Group I (1+ ions).

4. (b) It decreases.
[1 mark]
Explanation: Across a period, the nuclear charge increases while the number of electron shells remains the same, pulling electrons closer to the nucleus.

5. (b) Silicon
[1 mark]
Explanation: Silicon has a giant covalent (macromolecular) structure with strong covalent bonds throughout, giving it the highest melting point in Period 3.

6.
(a) Alkali metals [1]
(b) Halogens [1]
(c) Noble gases (or inert gases) [1]
Common mistake: Students may write "noble gases" for Group I or confuse Group 0 with Group VIII.

7.
(a) 2.8.2 [1]
(b) Group II, Period 3 [1]
Working: 12 protons = 12 electrons. Filling shells: 2 in first, 8 in second, 2 in third → 2.8.2. Three shells = Period 3; 2 valence electrons = Group II.

8. The atomic number is the number of protons in the nucleus of an atom. [1]
Common mistake: Students may say "number of electrons" — this is only true for a neutral atom. The definition must refer to protons.

9. Elements in Group 0 have a full outer shell of electrons (stable electronic configuration / noble gas configuration). [1] This means they have no tendency to gain, lose, or share electrons. [1] Therefore, they do not readily undergo chemical reactions. [1]
Marking: Award 1 mark for "full outer shell" or equivalent; 1 mark for explaining no tendency to gain/lose/share electrons; 1 mark for linking to lack of reactivity.

10. Similarity: Both have 1 valence electron / both form 1+ ions / both are in Group I / both are soft metals / both react with water. [1]
Difference: Potassium is more reactive than sodium / potassium has more electron shells / sodium has a smaller atomic radius / potassium has a lower melting point. [1]
Accept any valid similarity and difference. The similarity must relate to a shared Group I property; the difference must relate to the trend down the group.

11.
(a) The atomic radius decreases across Period 3 from Na to Cl. [1] This is because the number of protons (nuclear charge) increases across the period, pulling the electrons in the same shell closer to the nucleus, while the number of electron shells remains constant. [1]
Marking: 1 mark for describing the trend; 1 mark for explanation in terms of increasing nuclear charge and same number of shells.

(b) Silicon has a giant covalent (macromolecular) structure with strong covalent bonds throughout the lattice, requiring a large amount of energy to break. [1] Phosphorus (P₄) has a simple molecular structure with weak intermolecular forces (van der Waals' forces) between molecules, requiring less energy to overcome. [1]
Marking: 1 mark for identifying the structure type of silicon; 1 mark for identifying the structure type of phosphorus and the weak forces between molecules.

(c) Argon is a noble gas and exists as individual atoms (monatomic), not as covalent molecules. Its atomic radius is measured as a van der Waals radius rather than a covalent radius, so it is not directly comparable. [1]
Accept any valid explanation that argon is monatomic / does not form covalent bonds / has a different type of radius.

12.
(a) 2.8.2 [1]
Working: Group II, Period 3 → 12 electrons → 2.8.2 (magnesium).

(b) Mg²⁺ [1]
Working: Group II elements lose 2 electrons to form 2+ ions.

(c) Reactivity increases down Group II. [1] This is because the atomic radius increases / the number of electron shells increases, so the outermost electrons are further from the nucleus and more shielded by inner shell electrons. [1] This means the outer electrons are more easily lost. [1]
Marking: 1 mark for stating the trend; 1 mark for explaining increasing atomic radius/shielding; 1 mark for linking to ease of electron loss.

13.
(a) Isotopes are atoms of the same element (same number of protons) that have different numbers of neutrons (different mass numbers). [1]
Marking: Must mention same element/same proton number AND different neutrons/different mass number.

(b) A relative atomic mass of 35.5 (midway between 35 and 37) indicates that chlorine-35 is more abundant than chlorine-37. [1] If the two isotopes were present in equal amounts, the relative atomic mass would be 36. The value of 35.5 is closer to 35, so there is more chlorine-35. [1]
Marking: 1 mark for stating chlorine-35 is more abundant; 1 mark for explaining the reasoning (weighted average closer to 35).

14.
(a) R is a noble gas. [1] It is in Group 0 (far right of the Periodic Table) and has a full outer shell of electrons. [1]
Note: Only 1 mark available — award for identifying R with a brief reason.

(b) P and S are in the same group — Group I. [1]
Working: P is in Period 2, Group 17 (Group VII); S is in Period 4, Group 1 (Group I). Q is in Period 3, Group 2 (Group II). R is in Period 3, Group 0. Checking: P (Group 17), Q (Group 2), R (Group 0), S (Group 1). None share a group. Re-examining: S is in Period 4, Group 1 = Group I. No other element is in Group I. P is in Group 17. Q is in Group 2. R is in Group 0. Therefore, no two elements are in the same group. However, if the diagram is interpreted differently: P (Period 2, Group 17), Q (Period 3, Group 2), R (Period 3, Group 0), S (Period 4, Group 1). No two share a group. Award mark for any valid pair with correct reasoning, or accept "none" with valid explanation.
Correction: Based on the diagram layout, P (Group 17) and no other element is in Group 17. The answer is: None of the elements are in the same group. However, if the question expects a pair, the most likely intended answer is that no two elements share a group. Award 1 mark for "None — all four elements are in different groups" with valid reasoning.

(c) Q is a metal. [1] It is in Group II (left side of the Periodic Table), and elements on the left side of the Periodic Table are metals. [1]
Note: Only 1 mark available — award for identifying Q with a valid reason.

15.
(a) B and D (both in Group 17) [1]
Working: B is in Group 17, D is in Group 17.

(b) Element B (fluorine) has the smallest atomic radius. [1] Across a period, atomic radius decreases due to increasing nuclear charge pulling electrons closer. B and D are both in Group 17, but B is in Period 2 (fewer electron shells) while D is in Period 3, so B is smaller. Comparing all four, B has the fewest electron shells and is furthest to the right. [1]
Marking: 1 mark for identifying B; 1 mark for explanation involving fewer shells and/or position in the period.

(c) C (sodium, Group I) and D (chlorine, Group VII) would form an ionic compound. [1] The formula is NaCl. [1]
Working: Sodium loses 1 electron to form Na⁺; chlorine gains 1 electron to form Cl⁻. The formula is NaCl.

16. Reactivity of Group I metals increases down the group. [1] As you go down the group, the number of electron shells increases, so the outermost electron is further from the nucleus. [1] The inner shell electrons provide more shielding, reducing the attraction between the nucleus and the outer electron. [1] This means the outer electron is more easily lost, making the metal more reactive. [1]
Marking: 1 mark for stating the trend; 1 mark for increasing number of shells/distance from nucleus; 1 mark for shielding effect; 1 mark for linking to ease of electron loss. Award max 3 marks.

17. The statement is incorrect. [1] Elements in the same period do not have similar chemical properties; elements in the same group do. For example, in Period 3, sodium is a highly reactive metal, silicon is a metalloid, and chlorine is a reactive non-metal — they have very different chemical properties. Chemical properties depend on the number of valence electrons, which is the same within a group, not a period. [1]
Marking: 1 mark for stating the statement is incorrect; 1 mark for explanation with reference to Period 3 or valence electrons.

18.
(a) The boiling points increase down Group VII. [1]
Marking: Accept "boiling point increases as proton number increases" or equivalent.

(b) Going down Group VII, the number of electrons in the halogen molecules increases, so the molecules become larger. [1] This results in stronger van der Waals' forces (intermolecular forces) between the molecules. [1] More energy is required to overcome these stronger forces, so the boiling point increases. [1]
Marking: 1 mark for larger molecules/more electrons; 1 mark for stronger van der Waals' forces; 1 mark for more energy needed.

(c) The boiling point of astatine would be higher than 184 °C (e.g., approximately 250–350 °C). [1] This is because the trend shows boiling points increasing down the group, and astatine is below iodine with more electrons and stronger intermolecular forces. [1]
Marking: 1 mark for predicting a value higher than 184 °C; 1 mark for explaining based on the trend. Accept any reasonable value above 184 °C.

19.
(a) ZCl₂ = 111
Z + 2(35.5) = 111
Z + 71 = 111
Z = 111 − 71 = 40 [2]
Marking: 1 mark for correct equation; 1 mark for correct answer (40).

(b) Relative atomic mass of 40 corresponds to calcium (Ca). [1] Calcium is in Group II and Period 4. [1]
Marking: 1 mark for identifying calcium; 1 mark for Group II, Period 4.

20.
(a) First ionisation energy is the energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous 1+ ions. [1]
Marking: Must include "one mole of electrons," "gaseous atoms," and "gaseous 1+ ions" for the mark. Accept abbreviated but correct definitions.

(b) The first ionisation energy generally increases across Period 2. [1]
Marking: Accept "increases from Li to Ne" or equivalent. Do not require mention of anomalies for this mark.

(c) In beryllium, the outer electron is in the 2s subshell, which is lower in energy and closer to the nucleus. [1] In boron, the outer electron is in the 2p subshell, which is slightly higher in energy and further from the nucleus, and is also partially shielded by the 2s electrons. [1] Therefore, the 2p electron in boron is easier to remove, giving a lower first ionisation energy.
Marking: 1 mark for identifying the subshell difference (2s vs 2p); 1 mark for explaining that 2p is higher in energy/further from nucleus/better shielded.

(d) In nitrogen, the 2p subshell has three electrons, each occupying a separate orbital (half-filled, which is relatively stable). [1] In oxygen, one of the 2p orbitals contains two electrons, and the electron-electron repulsion within that orbital makes one of the paired electrons easier to remove. [1] Therefore, oxygen has a lower first ionisation energy than nitrogen.
Marking: 1 mark for describing the electron arrangement in nitrogen (half-filled/stable); 1 mark for explaining electron-electron repulsion in oxygen's paired orbital.

End of Answer Key