A Level H1 Chemistry Atomic Structure Bonding Quiz

A-Level Chemistry H1 Quiz - Atomic Structure Bonding

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

Duration: 60 minutes
Total Marks: 40
Topic: Atomic Structure Bonding (atomic-structure-bonding)

Instructions:

• Answer all 20 questions.
• Section A: Short structured questions (1–8).
• Section B: Data interpretation and bonding diagrams (9–14).
• Section C: Calculations and extended reasoning (15–20).
• Show all working for calculation questions. Use chemical notation where required.

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Section A: Short Structured Questions (1–8)

1. State what is meant by the term isotope. [1]

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2. Give the number of protons, neutrons and electrons in a neutral atom of $^{40}_{20}\text{Ca}$. [1]

Protons: ______ Neutrons: ______ Electrons: ______

3. Write the full electronic configuration of a chlorine atom, atomic number 17. [1]

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4. State the meaning of the term first ionisation energy. [1]

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5. State the type of bonding present in magnesium oxide, MgO. [1]

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6. Draw a dot-and-cross diagram to show the bonding in the molecule $\text{H}_2\text{O}$. Show only outer shell electrons. [2]

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7. Using VSEPR theory, predict the shape and bond angle of the molecule $\text{BF}_3$. [2]

Shape: __________________ Bond angle: _________

8. State the strongest type of intermolecular force present between $\text{NH}_3$ molecules. [1]

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Section B: Data Interpretation and Bonding Diagrams (9–14)

9. The first five successive ionisation energies of an element E are given below:

Ionisation	1st	2nd	3rd	4th	5th
IE / kJ mol⁻¹	496	4562	6912	9543	13353

Deduce the group of element E in the Periodic Table and explain your reasoning. [3]

Group: ______
Explanation: ___________________________________________________________

10. The diagram below shows the orbital overlap in a molecule of ethene, $\text{C}_2\text{H}_4$.

Generated diagram for Q10.

State the type of bond formed by the side-by-side overlap of p orbitals in this molecule. [1]

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11. Predict the shape and bond angle of the $\text{SF}_6$ molecule using VSEPR theory. Explain your answer. [3]

Shape: __________________ Bond angle: _________
Explanation: ___________________________________________________________

12. Explain why a $\text{H}_2\text{O}$ molecule is polar whereas a $\text{CO}_2$ molecule is non-polar, despite both containing polar bonds. [3]

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13. The table shows the melting points of four substances.

Substance	$\text{NaCl}$	$\text{I}_2$	$\text{SiO}_2$	$\text{Mg}$
Melting point / °C	801	114	1713	650

Identify the type of structure and bonding for each that accounts for the trend. [4]

$\text{NaCl}$: ________________________
$\text{I}_2$: ________________________
$\text{SiO}_2$: ________________________
$\text{Mg}$: ________________________

14. Deduce the electronic configuration of the $\text{Fe}^{2+}$ ion (atomic number of Fe = 26) using the s, p, d notation. [2]

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Section C: Calculations and Extended Reasoning (15–20)

15. Calculate the relative atomic mass of element X given the following isotopic abundances:
$^{63}\text{X}$: 69.2%, $^{65}\text{X}$: 30.8%. [2]

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16. The successive ionisation energies of element Y show a large jump after the 3rd ionisation. Deduce the number of electrons in the outer shell of Y and state its group. Hence write the formula of its oxide. [3]

Outer shell electrons: ______ Group: ______ Oxide formula: ______

17. A sample of neon contains the isotopes $^{20}\text{Ne}$ (90.5%) and $^{22}\text{Ne}$ (9.5%). Calculate the relative atomic mass of this neon sample to 1 decimal place. [2]

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18. Explain, in terms of electrostatic attractions, why the lattice energy of $\text{MgO}$ is more exothermic than that of $\text{NaF}$. [3]

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19. A molecule of $\text{PCl}_5$ has trigonal bipyramidal shape. State the bond angles in the equatorial and axial positions and explain using VSEPR theory how this minimises repulsion. [4]

Equatorial: _________ Axial: _________
Explanation: ___________________________________________________________

20. A student claims that "$\text{CO}_2$ has a higher boiling point than $\text{H}_2\text{O}$ because it has more electrons." Using your knowledge of intermolecular forces, evaluate this claim. [4]

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