A Level Chemistry H3 Periodic Table Quiz

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A-Level Chemistry H3 Quiz - Periodic Table

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Duration: 60 minutes
Total Marks: 40
Topic: Periodic Table (syllabus-first content; no past-year exam evidence available for H3 Chemistry 9813)

Instructions:

• Answer all 20 questions.
• Section A: short structured items (1–8). Section B: data and pattern analysis (9–14). Section C: extended reasoning (15–20).
• Show all working and reasoning where marks are awarded for method.
• Use the Data Booklet periodic table if needed.

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Section A: Core Periodic Trends (Questions 1–8)

1. State the trend in first ionisation energy down Group 2 from Be to Ba. [1]

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2. Write the electron configuration of a neutral phosphorus atom using the noble gas shorthand. [1]

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3. Explain why atomic radius decreases across Period 3 from Na to Cl. [2]

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4. Identify the element in Period 3 with the highest electronegativity and give its symbol. [1]

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5. Give the formula of the oxide formed when magnesium burns in air and state whether it is basic, amphoteric, or acidic. [2]

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6. State the block in the periodic table to which the element with proton number 24 belongs and justify your answer using its electron configuration. [2]

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7. The following shows successive ionisation energies (kJ mol⁻¹) for an element X: 738, 1451, 7733, 10540. To which group does X belong? [1]

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8. Define the term "transition element" as used in the periodic table. [1]

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Section B: Data and Pattern Analysis (Questions 9–14)

9. The table below gives atomic radii (pm) for Period 3 elements:

Element	Na	Mg	Al	Si	P	S	Cl
Atomic radius (pm)	186	160	143	117	110	104	99

Plot a graph of atomic radius against atomic number (Z = 11 to 17) and describe the trend shown. [3]

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10. Using the Data Booklet, compare the melting points of Na, Si, and Cl₂. Explain the differences in terms of bonding and structure. [3]

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11. The first ionisation energies (kJ mol⁻¹) of Period 3 are: Na 496, Mg 738, Al 578, Si 786, P 1012, S 1000, Cl 1251, Ar 1521. Account for the anomaly that Al has a lower first ionisation energy than Mg. [2]

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12. Chlorides of Period 3 elements show different behaviours in water. Complete the table:

Chloride	Equation with water	pH of solution
NaCl	no reaction	7
MgCl₂	$MgCl_2 + 6H_2O \rightleftharpoons [Mg(H_2O)_6]^{2+} + 2Cl^-$	?
AlCl₃	$AlCl_3 + 3H_2O \rightarrow Al(OH)_3 + 3HCl$	?

State the pH range for MgCl₂ and AlCl₃ solutions. [2]

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13. The relative abundances of isotopes of element Y are: $^{63}Y$ 69%, $^{65}Y$ 31%. Calculate the relative atomic mass of Y to 1 decimal place. [2]

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14. Explain why the d-block elements show a much smaller variation in atomic radius across a period compared to s- and p-block elements. [2]

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Section C: Extended Reasoning (Questions 15–20)

15. (a) Define shielding effect. (b) Explain how shielding and nuclear charge together determine the size of an atom down a group. [3]

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16. The electronegativity values (Pauling) are: Li 1.0, Be 1.5, B 2.0, C 2.5, N 3.0, O 3.5, F 4.0. (a) State the general trend across Period 2. (b) Explain the trend using atomic structure. [3]

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17. A student claims: "Across Period 3, the metallic character of oxides increases." Evaluate this statement with two examples and the underlying periodicity concept. [3]

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18. Given the following successive ionisation energies (kJ mol⁻¹): 580, 1800, 2700, 11600, 14800. (a) Deduce the group of the element. (b) Write the formula of its chloride and state its bonding type. [3]

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19. (a) What is meant by "effective nuclear charge" ($Z_{eff}$)? (b) How does $Z_{eff}$ change across a period and how does this relate to electron affinity? [3]

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20. The table shows boiling points (°C): HF −19.5, HCl −85, HBr −67, HI −35. (a) Explain why HF has an anomalously high boiling point. (b) Why does boiling point increase from HCl to HI? [3]

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A-Level Chemistry H3 Quiz - Periodic Table: Answer Key

Topic: Periodic Table (syllabus-first; no past-year H3 papers exist for 9813)

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1. [1 mark]
First ionisation energy decreases down Group 2.
Teaching note: Down the group, extra electron shells are added and shielding increases, so the outer electron is less tightly held despite higher nuclear charge.

2. [1 mark]
$[Ne]\,3s^2 3p^3$
Teaching note: P has Z = 15; Ne core is 10 electrons, remaining 5 go into 3s and 3p.

3. [2 marks]
Across Period 3, proton number increases so nuclear charge increases. Electrons are added to the same shell, so shielding increases only slightly. The stronger effective nuclear charge pulls electrons closer.
[1] increased nuclear charge; [1] same shell / poor shielding → smaller radius.

4. [1 mark]
Chlorine, Cl.
Teaching note: Highest electronegativity in Period 3 (excluding Ar, noble gas).

5. [2 marks]
$2Mg + O_2 \rightarrow 2MgO$; basic oxide.
[1] formula MgO; [1] basic.

6. [2 marks]
d-block. Config: $[Ar]\,3d^5 4s^1$ (Cr, Z=24). The differentiating electron enters the 3d subshell.
[1] d-block; [1] config justifies d-electron.

7. [1 mark]
Group 2.
Teaching note: Large jump after 2nd IE shows 2 valence electrons.

8. [1 mark]
A transition element is a d-block element that forms at least one ion with a partially filled d-subshell.

9. [3 marks]
Graph: x-axis Z=11–17, y-axis radius pm; points joined show steady decrease.
Trend: atomic radius decreases from Na (186 pm) to Cl (99 pm).
[1] correct plot; [1] decrease stated; [1] mention smooth decrease with Z.

10. [3 marks]
Na: low mp (~98 °C) metallic bonding, delocalised e⁻ weak. Si: very high mp (~1414 °C) giant covalent network. Cl₂: low mp (−101 °C) molecular, weak London forces.
[1] each correct comparison with bonding.

11. [2 marks]
Mg config $[Ne]3s^2$ (filled s stable). Al $[Ne]3s^2 3p^1$; p-electron is higher energy and easier to remove → lower IE than Mg.
[1] Mg filled 3s; [1] Al p-electron removed more easily.

12. [2 marks]
MgCl₂ solution slightly acidic (pH ~6–7 due to $[Mg(H_2O)_6]^{2+}$ hydrolysis). AlCl₃ strongly acidic (pH < 3 from HCl).
[1] MgCl₂ pH ~5–7; [1] AlCl₃ acidic.

13. [2 marks]
$A_r = (63 \times 0.69) + (65 \times 0.31) = 43.47 + 20.15 = 63.62 \approx 63.6$
[1] calculation; [1] answer 63.6.

14. [2 marks]
d-electrons shield poorly but added d-electrons do not increase nuclear charge as effectively; size change across d-block is small due to similar $Z_{eff}$.
[1] poor shielding; [1] small change explained.

15. [3 marks]
(a) Shielding = inner electrons repel outer electrons, reducing nuclear pull. [1]
(b) Down group, shells increase → shielding increases, nuclear charge increases too, but shielding dominates → radius increases. [2]

16. [3 marks]
(a) Electronegativity increases left to right. [1]
(b) Nuclear charge rises, atomic radius falls, electron density pulled stronger. [2]

17. [3 marks]
Statement false. Na₂O basic, Al₂O₃ amphoteric, SO₃ acidic. Oxides become less basic / more acidic across period. [1] eval; [2] examples.

18. [3 marks]
(a) Group 3 (large jump after 3rd IE). [1]
(b) MCl₃; ionic/covalent polar. [2]

19. [3 marks]
(a) $Z_{eff}$ = nuclear charge felt after shielding. [1]
(b) Increases across period → stronger e⁻ attraction → higher electron affinity. [2]

20. [3 marks]
(a) HF H-bonding raises bp. [1.5]
(b) HCl→HI: London forces increase with Mr. [1.5]