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Secondary 4 Combined Science Chemistry Periodic Table Quiz
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Questions
Secondary 4 Combined Science Chemistry Quiz - Periodic Table
Name: ___________________________
Class: ___________________________
Date: ___________________________
Score: ________ / 40
Duration: 45 minutes
Total Marks: 40
Instructions
- Answer all questions in the spaces provided.
- Show all working where applicable. Answers without working may not receive full marks.
- The number of marks for each question is shown in brackets, e.g. [2].
- You may use a calculator where necessary.
- A copy of the Periodic Table is provided on the last page of this quiz.
Section A: Multiple Choice Questions (Questions 1–5) [10 marks]
For each question, choose the one best answer and write the letter in the space provided.
1. Which of the following statements best describes the modern Periodic Table?
A. Elements are arranged in order of increasing relative atomic mass.
B. Elements are arranged in order of increasing proton number.
C. Elements are arranged in order of increasing number of neutrons.
D. Elements are arranged in order of increasing number of electron shells.
Answer: ________ [1]
2. An element X has the electronic configuration 2.8.6. Which group and period does element X belong to?
A. Group II, Period 3
B. Group V, Period 3
C. Group VI, Period 3
D. Group VIII, Period 3
Answer: ________ [1]
3. Which of the following is a property of elements in Group I?
A. They form ions with a charge of 2+.
B. They are good conductors of electricity.
C. They exist as diatomic molecules.
D. They form acidic oxides.
Answer: ________ [1]
4. Going across Period 3 from sodium to argon, which property generally increases?
A. Atomic radius
B. Metallic character
C. Electronegativity
D. Tendency to lose electrons
Answer: ________ [1]
5. Which of the following elements is a noble gas?
A. Nitrogen
B. Chlorine
C. Krypton
D. Bromine
Answer: ________ [1]
Section B: Short Answer Questions (Questions 6–14) [18 marks]
6. Define the term period as used in the Periodic Table. [2]
7. An element Y is in Group VII and Period 3 of the Periodic Table.
(a) Write the electronic configuration of element Y. [1]
(b) State the formula of the ion formed by element Y. [1]
(c) Is element Y a metal or a non-metal? Give a reason for your answer. [2]
8. The table below shows information about four elements, P, Q, R, and S.
| Element | Proton Number | Group |
|---|---|---|
| P | 3 | I |
| Q | 11 | I |
| R | 19 | I |
| S | 12 | II |
(a) Which element has the largest atomic radius? Explain your answer. [2]
(b) Which two elements are in the same period? Explain how you know. [2]
9. Explain why the elements in Group 0 (noble gases) are generally unreactive. [2]
10. State two physical properties and two chemical properties of transition metals. [4]
Physical properties: (i) ________________________________________________________________________ (ii) _______________________________________________________________________
Chemical properties: (i) ________________________________________________________________________ (ii) _______________________________________________________________________
11. Describe the trend in reactivity of Group I metals as you go down the group. Explain this trend in terms of atomic structure. [3]
12. Element Z is in Period 2 and Group V.
(a) Write the electronic configuration of element Z. [1]
(b) State whether element Z is a metal or non-metal. [1]
13. Explain why atomic radius decreases across a period from left to right. [2]
14. Chlorine and bromine are both in Group VII.
(a) Which element is more reactive? [1]
(b) Explain your answer in terms of atomic structure. [2]
Section C: Structured / Data Response Questions (Questions 15–20) [12 marks]
15. The table below gives some information about the first five elements in Period 3.
| Element | Symbol | Proton Number | Melting Point (°C) | Electrical Conductivity |
|---|---|---|---|---|
| Sodium | Na | 11 | 98 | Good |
| Magnesium | Mg | 12 | 650 | Good |
| Aluminium | Al | 13 | 660 | Good |
| Silicon | Si | 14 | 1410 | Poor (semiconductor) |
| Phosphorus | P | 15 | 44 | Poor |
(a) Describe the trend in melting point across these five elements. [2]
(b) Explain why sodium, magnesium, and aluminium are good conductors of electricity. [2]
(c) Silicon is described as a semiconductor. What does this mean? [1]
(d) Suggest a value for the melting point of sulfur (the next element after phosphorus in Period 3). Explain your reasoning. [2]
16. The diagram below shows the first ionisation energies of the first 20 elements.
(Sketch description for student: A graph of first ionisation energy (y-axis) against proton number (x-axis) for elements with proton numbers 1 to 20. The graph shows a general upward trend with notable drops at proton numbers 3, 11, and 19, and peaks at proton numbers 2, 10, and 18.)
(a) State the general trend in first ionisation energy across a period. [1]
(b) Explain why there is a drop in first ionisation energy from element 2 (helium) to element 3 (lithium). [2]
(c) Explain why noble gases (elements 2, 10, 18) have the highest first ionisation energies in their respective periods. [2]
17. Element T has a proton number of 17.
(a) Write the electronic configuration of element T. [1]
(b) To which group and period does element T belong? [1]
(c) Element T reacts with sodium to form a compound. Write the formula of this compound. [1]
(d) Explain, in terms of electron transfer, how the compound in (c) is formed. [2]
18. The table below shows the boiling points of the Group VII elements.
| Element | Boiling Point (°C) |
|---|---|
| Fluorine | –188 |
| Chlorine | –35 |
| Bromine | 59 |
| Iodine | 184 |
(a) Describe the trend in boiling point down Group VII. [1]
(b) Explain this trend in terms of the forces between molecules. [3]
(c) Predict the boiling point of astatine (At), the element below iodine in Group VII. [1]
19. A student makes the following statement: "All metals are found on the left side of the Periodic Table and all non-metals are found on the right side."
Evaluate this statement. Is it fully correct? Explain your reasoning with reference to the position of specific elements. [3]
20. The table below shows properties of three unknown elements, X, Y, and Z.
| Property | Element X | Element Y | Element Z |
|---|---|---|---|
| Melting point (°C) | 1535 | –101 | 660 |
| Conducts electricity? | Yes | No | Yes |
| Forms basic oxide? | Yes | No | Yes |
| Forms ionic chloride? | Yes | No | Yes |
(a) Classify each element as a metal or non-metal. [2]
Element X: __________________________________________________________________
Element Y: __________________________________________________________________
Element Z: __________________________________________________________________
(b) Element Z is in Period 3. Suggest the identity of element Z. Give a reason for your answer. [2]
(c) Element Y forms a diatomic molecule. Suggest the formula of this molecule. [1]
END OF QUIZ
Answers
Secondary 4 Combined Science Chemistry Quiz - Periodic Table
Answer Key
Section A: Multiple Choice Questions
1. B [1]
Explanation: The modern Periodic Table arranges elements in order of increasing proton number (atomic number), not relative atomic mass. This was a key development from Mendeleev's original table.
2. C [1]
Explanation: Electronic configuration 2.8.6 means the element has 3 electron shells (Period 3) and 6 valence electrons (Group VI).
3. B [1]
Explanation: Group I elements (alkali metals) are metals and therefore good conductors of electricity. They form 1+ ions (not 2+), do not exist as diatomic molecules, and form basic oxides (not acidic oxides).
4. C [1]
Explanation: Electronegativity increases across a period from left to right because the nuclear charge increases while the number of electron shells remains the same, resulting in a stronger attraction for bonding electrons. Atomic radius decreases, metallic character decreases, and the tendency to lose electrons decreases.
5. C [1]
Explanation: Krypton is a Group 0 (Group VIII) noble gas. Nitrogen is Group V, chlorine is Group VII, and bromine is Group VII.
Section B: Short Answer Questions
6. [2]
A period is a horizontal row of elements in the Periodic Table. [1] Elements in the same period have the same number of electron shells. [1]
Marking note: Award 1 mark for "horizontal row" and 1 mark for linking to the same number of electron shells (or same principal quantum number).
7.
(a) 2.8.7 [1]
Explanation: Group VII, Period 3 means 3 electron shells and 7 valence electrons.
(b) Cl⁻ (or Y⁻) [1]
Explanation: Group VII elements gain one electron to form a 1− ion.
(c) Non-metal [1] because it is in Group VII / it gains electrons to form a negative ion / it has 7 valence electrons and needs to gain one electron to achieve a stable noble gas configuration. [1]
Marking note: Award 1 mark for correct classification and 1 mark for a valid reason.
8.
(a) Element R (proton number 19) has the largest atomic radius. [1] This is because R is furthest down Group I, meaning it has the most electron shells, so the outermost electron is furthest from the nucleus. [1]
Marking note: Students must identify R and give a reason in terms of number of electron shells.
(b) P (proton number 3) and S (proton number 12) are in the same period. [1] This is because both have 2 electron shells (P: 2.1 and S: 2.8.2), placing them in Period 2. [1]
Alternative acceptable answer: Q (proton number 11) and S (proton number 12) are in the same period because both have 3 electron shells (Period 3).
Marking note: Award 1 mark for identifying a correct pair and 1 mark for a valid explanation based on electronic configuration or number of electron shells.
9. [2]
Noble gases have a full outer shell of electrons (stable electronic configuration). [1] Therefore, they do not need to gain, lose, or share electrons, making them generally unreactive. [1]
Marking note: Award 1 mark for "full outer shell" / "stable configuration" and 1 mark for linking this to lack of tendency to react.
10. [4]
Physical properties (any two):
(i) High melting and boiling points [½]
(ii) Good conductors of electricity [½]
(iii) Good conductors of heat [½]
(iv) High density [½]
(v) Hard and strong [½]
Chemical properties (any two):
(i) Form coloured compounds [½]
(ii) Act as catalysts [½]
(iii) Show variable oxidation states / form ions with different charges [½]
(iv) Form complex ions [½]
Marking note: Award ½ mark per correct property, up to 2 marks for physical and 2 marks for chemical.
11. [3]
The reactivity of Group I metals increases going down the group. [1] This is because the atomic radius increases / the number of electron shells increases, so the outermost electron is further from the nucleus. [1] The attraction between the nucleus and the outermost electron is weaker, so the electron is more easily lost. [1]
Marking note: Award 1 mark for stating the trend, 1 mark for explaining in terms of atomic structure, and 1 mark for linking to ease of electron loss.
12.
(a) 2.5 [1]
Explanation: Period 2 means 2 electron shells; Group V means 5 valence electrons.
(b) Non-metal [1]
Explanation: Group V elements in Period 2 (nitrogen, phosphorus) are non-metals.
13. [2]
Going across a period, the proton number increases [1] but the number of electron shells stays the same, so the increased nuclear charge pulls the electron shells closer to the nucleus, resulting in a smaller atomic radius. [1]
Marking note: Award 1 mark for mentioning increasing proton number/nuclear charge and 1 mark for explaining the effect on electron shells/radius.
14.
(a) Chlorine [1]
Explanation: Chlorine is higher up in Group VII than bromine.
(b) Chlorine has fewer electron shells / a smaller atomic radius than bromine, [1] so the outermost electron shell is closer to the nucleus and the attraction between the nucleus and incoming electrons is stronger, making it easier for chlorine to gain an electron. [1]
Marking note: Award 1 mark for comparing number of shells/atomic size and 1 mark for linking to electron gain/electronegativity.
Section C: Structured / Data Response Questions
15.
(a) The melting point increases from sodium to silicon, reaching a peak at silicon, [1] then drops sharply for phosphorus. [1]
Marking note: Award 1 mark for describing the general increase and 1 mark for noting the drop after silicon.
(b) Sodium, magnesium, and aluminium have delocalised (mobile) electrons that are free to move throughout the metallic lattice. [1] When a voltage is applied, these electrons move and carry charge, conducting electricity. [1]
Marking note: Award 1 mark for mentioning delocalised/mobile electrons and 1 mark for explaining how they conduct.
(c) A semiconductor is a material that conducts electricity poorly under normal conditions but can conduct better under certain conditions (e.g., when heated or when impurities are added). [1]
Marking note: Accept any reasonable definition indicating intermediate conductivity.
(d) A value below 44 °C (e.g., around 0–40 °C). [1] This is because the trend shows that after the peak at silicon, the melting points of the remaining non-metallic elements (phosphorus, sulfur, chlorine, argon) are much lower, as they exist as simple molecules with weak intermolecular forces. [1]
Marking note: Award 1 mark for a reasonable value below 44 °C and 1 mark for a valid explanation referencing the trend or weak intermolecular forces.
16.
(a) First ionisation energy generally increases across a period. [1]
(b) Lithium has one electron in its outermost shell (2.1), which is in the second electron shell, further from the nucleus than helium's electrons (which are in the first shell). [1] The outermost electron in lithium is also shielded by the inner shell of electrons, so it is easier to remove, resulting in a lower first ionisation energy. [1]
Marking note: Award 1 mark for mentioning the outer shell being further from the nucleus and 1 mark for mentioning electron shielding.
(c) Noble gases have a full outer shell (stable electronic configuration). [1] This means a large amount of energy is required to remove an electron from a stable, complete shell, giving them the highest first ionisation energies in their periods. [1]
Marking note: Award 1 mark for "full outer shell" / "stable configuration" and 1 mark for linking to high energy required to remove an electron.
17.
(a) 2.8.7 [1]
Explanation: Proton number 17 means 17 electrons: 2 in the first shell, 8 in the second, 7 in the third.
(b) Group VII, Period 3 [1]
Explanation: 3 electron shells = Period 3; 7 valence electrons = Group VII.
(c) NaCl [1]
Explanation: Sodium (Na) is Group I and forms Na⁺; chlorine (Cl) is Group VII and forms Cl⁻. The formula is NaCl.
(d) Sodium atom loses one electron to form Na⁺, and chlorine atom gains that electron to form Cl⁻. [1] The oppositely charged ions are held together by strong electrostatic forces of attraction (ionic bond). [1]
Marking note: Award 1 mark for describing electron transfer and 1 mark for mentioning ionic bond / electrostatic attraction.
18.
(a) The boiling point increases going down Group VII. [1]
(b) Going down Group VII, the molecules become larger / the number of electrons increases, [1] so the van der Waals' forces (intermolecular forces) between molecules become stronger. [1] More energy is needed to overcome these stronger forces, so the boiling point increases. [1]
Marking note: Award 1 mark for mentioning increasing molecular size/number of electrons, 1 mark for identifying van der Waals'/intermolecular forces, and 1 mark for linking to energy required.
(c) A value above 184 °C (e.g., 200–300 °C). [1]
Explanation: Since boiling point increases down the group, astatine (below iodine) should have a higher boiling point than iodine (184 °C).
Marking note: Accept any value above 184 °C.
19. [3]
The statement is partially correct but not fully accurate. [1] Most metals are indeed found on the left side and centre of the Periodic Table (Groups I, II, III, and transition metals), while non-metals are found on the right side (Groups V, VI, VII, and 0). [1] However, hydrogen is placed on the left side of the Periodic Table but is a non-metal, which is an exception to the statement. [1]
Alternative acceptable point: Some elements near the dividing line (e.g., silicon, germanium) are metalloids and have properties of both metals and non-metals.
Marking note: Award 1 mark for evaluating the statement as not fully correct, 1 mark for describing the general pattern, and 1 mark for giving a valid exception or qualification.
20.
(a) Element X: Metal [½] — high melting point, conducts electricity, forms basic oxide, forms ionic chloride.
Element Y: Non-metal [½] — low melting point, does not conduct, does not form basic oxide, does not form ionic chloride.
Element Z: Metal [½] — conducts electricity, forms basic oxide, forms ionic chloride.
Note: Only 2 marks total for this part — award ½ per correct classification.
Marking correction: Award 1 mark for each correct classification (X = metal, Y = non-metal, Z = metal). Total: 2 marks (accept ½ per element × 3 = 1.5, rounded — but to be precise: 1 mark for X correct, 1 mark for Y correct, Z is implied).
Clarified marking: 1 mark for X (metal), 1 mark for Y (non-metal). Z follows from the same reasoning.
(b) Element Z is magnesium (Mg). [1] This is because it is in Period 3, is a metal, forms a basic oxide and an ionic chloride, and has a melting point of 660 °C, which matches the known melting point of magnesium. [1]
Alternative acceptable answer: Aluminium (Al) — also Period 3 metal with melting point 660 °C. Accept either Mg or Al with valid reasoning.
Marking note: Award 1 mark for a reasonable suggestion and 1 mark for supporting evidence from the data.
(c) Y₂ (e.g., if Y is a Group VI element like sulfur, S₂; or if Group VII, Cl₂; or if Group V, N₂). [1]
Explanation: Non-metals in Groups V–VII typically exist as diatomic molecules. Accept any reasonable diatomic formula (e.g., O₂, N₂, Cl₂, F₂, Br₂, I₂).
Marking note: Accept any valid diatomic molecular formula for a non-metal.
END OF ANSWER KEY