A Level H2 Chemistry Atomic Structure Bonding Quiz

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A-Level Chemistry H2 Quiz - Atomic Structure Bonding

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Duration: 60 minutes
Total Marks: 40
Topic: Atomic Structure Bonding (atomic-structure-bonding)
Version: 1 of 5 (Practice Quiz)

Instructions:

• Answer all 20 questions.
• Section A: Short structured questions (1–10). Section B: Data and bonding interpretation (11–15). Section C: Extended written responses (16–20).
• Show all working where calculations are required.
• Use the Data Booklet where relevant.
• This quiz is syllabus-first generated content and is not derived from official past-year papers.

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Section A: Atomic Structure Fundamentals (Questions 1–10)

1. [2 marks]
State the relative charge and relative mass of a proton, a neutron, and an electron.

Proton: charge ______ , mass ______
Neutron: charge ______ , mass ______
Electron: charge ______ , mass ______

2. [1 mark]
An atom has proton number 17 and nucleon number 35. Deduce the number of neutrons in this atom.

Number of neutrons: ______

3. [2 marks]
Explain, in terms of charge distribution, why a beam of electrons is deflected more than a beam of protons when passed through the same electric field.

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4. [2 marks]
Isotopes of chlorine are $^{35}\text{Cl}$ and $^{37}\text{Cl}$. State two similarities and one difference between these isotopes.

Similarities: (i) ____________________ (ii) ____________________
Difference: ____________________

5. [2 marks]
Write the full electronic configuration of a neutral sulfur atom (proton number 16).

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6. [2 marks]
State the shape and relative energy order of the following orbitals: 1s, 2s, 2p, 3s, 3p, 4s. Use the notation "lowest energy first".

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7. [3 marks]
The first five successive ionisation energies (in kJ mol⁻¹) of element X are: 738, 1451, 7733, 10540, 13630. Deduce the group of X in the Periodic Table and explain your reasoning.

Group: ______
Reasoning: ________________________________________________________

8. [2 marks]
State the number of orbitals and the maximum number of electrons in a d subshell.

Number of orbitals: ______
Maximum electrons: ______

9. [1 mark]
An ion $\text{Y}^{3-}$ has 18 electrons. Deduce the proton number of element Y.

Proton number: ______

10. [2 marks]
Explain why the second ionisation energy of sodium is much larger than its first ionisation energy.

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Section B: Bonding and Structure (Questions 11–15)

11. [3 marks]
Draw a dot-and-cross diagram for the covalent molecule $\text{CO}_2$. Show only the outer shell electrons of C and O.

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12. [3 marks]
Using VSEPR theory, predict the shape and bond angle of $\text{NH}_3$. Explain the deviation from the tetrahedral angle.

Shape: ______
Bond angle: ______
Explanation: ________________________________________________________

13. [3 marks]
State the type of intermolecular force present in each of the following: (i) $\text{CH}_4$, (ii) $\text{HCl}$, (iii) $\text{H}_2\text{O}$. For $\text{H}_2\text{O}$, state why it is especially strong.

(i) ______ (ii) ______ (iii) ______
Reason for $\text{H}_2\text{O}$: ________________________________________________________

14. [4 marks]
The table below shows boiling points of hydrides in Group 16.

Compound	Boiling point / °C
$\text{H}_2\text{O}$	100
$\text{H}_2\text{S}$	-60
$\text{H}_2\text{Se}$	-41

Explain the trend and anomaly using intermolecular forces.

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15. [3 marks]
Describe the bonding in metallic sodium. Include the terms "delocalised electrons" and "electrostatic attraction" in your answer.

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Section C: Extended Responses (Questions 16–20)

16. [3 marks]
Deduce the polarity of the molecule $\text{BF}_3$ given that B–F bonds are polar but the molecule is symmetrical. Explain your answer with reference to bond polarity and molecular shape.

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17. [4 marks]
Compare the structure and bonding of ionic $\text{MgO}$ and giant molecular $\text{C}$ (diamond). In your answer, refer to lattice type, particles present, and melting point trend.

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18. [3 marks]
Explain how hydrogen bonding affects the density of ice compared to liquid water.

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19. [3 marks]
A molecule $\text{X}$ has the formula $\text{CH}_2\text{O}$ (methanal). Draw its Lewis structure, state the type of covalent bonds formed (σ/π), and predict its shape.

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20. [4 marks]
Successive ionisation energies (kJ mol⁻¹) for element Z are: 495, 4562, 6912, 9543, 13353, 16610. Deduce the electronic configuration of Z and identify its block in the Periodic Table. Show your reasoning from the data.

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A-Level Chemistry H2 Quiz - Atomic Structure Bonding (Answer Key)

Topic: Atomic Structure Bonding
Version: 1 of 5
Total Marks: 40
Note: Syllabus-first practice content; not official past-paper derived.

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Section A Answers

1. [2 marks]

• Proton: charge +1, mass 1
• Neutron: charge 0, mass 1
• Electron: charge –1, mass ~1/1836 (or 0.0005)
  (Award ½ mark per correct pair; teaching: relative mass uses proton/neutron ≈ 1, electron negligible.)

2. [1 mark]
Neutrons = 35 – 17 = 18
(Method: nucleon number – proton number.)

3. [2 marks]
Electrons have much smaller mass than protons (1/1836) so for the same electric force (F = qE), acceleration (a = F/m) is far greater; hence greater deflection. Also both negatively charged so deflect opposite to proton beam.
(Mark: 1 for mass difference, 1 for correct deflection reasoning.)

4. [2 marks]
Similarities: same proton number (17), same electron configuration / same chemical properties.
Difference: different nucleon number (35 vs 37) / different number of neutrons.
(1 mark for two similarities, 1 for difference.)

5. [2 marks]
1s² 2s² 2p⁶ 3s² 3p⁴
(Full config required; 1s²2s²2p⁶3s²3p⁴ acceptable. Deduct if superscripts omitted.)

6. [2 marks]
Order: 1s < 2s < 2p < 3s < 3p < 4s.
Shapes: s = spherical; p = dumbbell (3 orientations); d = cloverleaf (5 orbitals).
(1 for order, 1 for shapes.)

7. [3 marks]
Group: 2
Reasoning: Large jump after 2nd IE (1451 → 7733) shows removal of core electron after 2 valence electrons removed.
(1 mark group, 2 marks reasoning with reference to jump.)

8. [2 marks]
Number of orbitals: 5; Maximum electrons: 10.
(d subshell has 5 orbitals × 2 e⁻.)

9. [1 mark]
Y³⁻ has 18 e⁻ → neutral Y has 15 e⁻ → proton number 15.
(Oxygen family, P.)

10. [2 marks]
After first IE, Na⁺ has stable noble gas config (2,8). Second electron removed from inner shell (n=2) closer to nucleus with greater effective nuclear charge → much more energy needed.
(1 for stable config, 1 for inner shell.)

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Section B Answers

11. [3 marks]
O=C=O; each O has 2 lone pairs; C shares 4 e⁻ (double bonds).
Dot-and-cross: C (4 e⁻) with two O (6 e⁻ each) forming two double bonds.
(1 for linear, 1 for double bonds, 1 for lone pairs shown.)

12. [3 marks]
Shape: trigonal pyramidal; bond angle 107° (approx).
Explanation: 3 bonding pairs + 1 lone pair → tetrahedral electron arrangement; lone pair repels more, compressing angle from 109.5°.
(1+1+1.)

13. [3 marks]
(i) induced dipole (van der Waals)
(ii) permanent dipole–dipole
(iii) hydrogen bonding
Reason: O is highly electronegative and H bonded to O allows strong H-bond network.
(1 each; H₂O reason within iii mark.)

14. [4 marks]
Trend H₂S < H₂Se: increasing Mr → stronger van der Waals. Anomaly: H₂O much higher due to hydrogen bonding (strong IMF) absent in H₂S/Se.
(2 for trend, 2 for H-bond explanation.)

15. [3 marks]
Na atoms lose outer e⁻ to form Na⁺ ions in lattice; valence e⁻ delocalised across structure; electrostatic attraction between + ions and delocalised e⁻ holds metal together.
(1 delocalised, 1 electrostatic, 1 lattice.)

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Section C Answers

16. [3 marks]
B–F bonds polar (F more EN). Molecule trigonal planar symmetrical; bond dipoles cancel vectorially → overall non-polar.
(1 bond polar, 1 symmetry, 1 cancel → non-polar.)

17. [4 marks]
MgO: ionic lattice, Mg²⁺/O²⁻, strong electrostatic forces, very high mp. Diamond: giant covalent, C atoms, strong directional covalent bonds, very high mp. Both high mp but different particles/bonds.
(2 for MgO, 2 for diamond.)

18. [3 marks]
In ice, H-bonds form open hexagonal lattice → molecules further apart → lower density than liquid where H-bonds continually break/forming more compact.
(1 open lattice, 1 lower density, 1 comparison.)

19. [3 marks]
Lewis: H₂C=O; C forms 2 σ (to H, to O) + 1 π (to O). Shape: trigonal planar at C, ~120°.
(1 structure, 1 bond types, 1 shape.)

20. [4 marks]
Jump after 1st IE → 1 valence e⁻ → Group 1. Config: 1s² 2s² 2p⁶ 3s¹. Block: s-block.
(1 config, 1 group, 1 block, 1 reasoning from jump.)