Cambridge AS & A Level Chemistry Quiz

Topics 3.2 to 4.2: Chemical Bonding & States of Matter

📝 Quiz Instructions

This quiz covers Chemical Bonding (3.2–3.7) and States of Matter (4.1–4.2) from the Cambridge A Level Chemistry syllabus.

Time Limit: 45 minutes for 30 multiple-choice questions
Format: All questions appear on this page – no navigation needed
Submission: Results are automatically sent to your teacher
Scoring: Each correct answer = 1 point (Total: 30 points)
Requirements: Enter your full name before submission

Quiz Questions (1-30)

1. Ionic bonding is best described as:

(a) Sharing of electrons between atoms (b) Electrostatic attraction between positive ions and delocalised electrons (c) Electrostatic attraction between oppositely charged ions (d) Overlap of atomic orbitals

2. Which of the following compounds has ionic bonding?

(a) H₂O (b) NaCl (c) CH₄ (d) CO₂

3. Metallic bonding is due to:

(a) Attraction between positive ions and delocalised electrons (b) Sharing of electron pairs between metal atoms (c) Transfer of electrons from metal to non-metal (d) Hydrogen bonding between metal atoms

4. Covalent bonding involves:

(a) Transfer of electrons (b) Electrostatic attraction between ions (c) Sharing of electron pairs between nuclei (d) Delocalised electrons in a lattice

5. Which molecule contains a coordinate (dative) bond?

(a) NH₃ (b) H₂O (c) NH₄⁺ (d) CH₄

6. A σ bond is formed by:

(a) Sideways overlap of p orbitals (b) End-to-end overlap of orbitals (c) Overlap of d orbitals only (d) Ionic interaction

7. Which molecule contains both σ and π bonds?

(a) H₂ (b) N₂ (c) CH₄ (d) NaCl

8. According to VSEPR theory, the shape of BF₃ is:

(a) Tetrahedral (b) Trigonal planar (c) Linear (d) Pyramidal

9. Which molecule has a bond angle of approximately 107°?

(a) H₂O (b) NH₃ (c) CH₄ (d) CO₂

10. Hydrogen bonding occurs when hydrogen is bonded to:

(a) Carbon (b) Any non-metal (c) Highly electronegative atoms like N, O, F (d) Metals

11. Which property is due to hydrogen bonding in water?

(a) Low boiling point (b) High surface tension (c) Low density of ice (d) Both (b) and (c)

12. Van der Waals forces include:

(a) Only London dispersion forces (b) Only dipole-dipole interactions (c) London dispersion, dipole-dipole, and hydrogen bonding (d) Only ionic bonds

13. Which type of bonding is generally strongest?

(a) Ionic bonding (b) Covalent bonding (c) Metallic bonding (d) Intermolecular forces

14. The ideal gas equation is:

(a) \( PV = nRT \) (b) \( P = \frac{nRT}{V} \) (c) \( V = \frac{nR}{PT} \) (d) \( T = \frac{PV}{nR} \)

15. An ideal gas assumes:

(a) No intermolecular forces and particles have zero volume (b) Strong intermolecular forces (c) Large particle size (d) Particles are stationary

16. Which of the following has a giant ionic lattice?

(a) Iodine (I₂) (b) Sodium chloride (NaCl) (c) Silicon dioxide (SiO₂) (d) Copper (Cu)

17. Graphite is an example of:

(a) Giant ionic structure (b) Simple molecular structure (c) Giant molecular (covalent) structure (d) Metallic structure

18. Which substance has high electrical conductivity in solid state?

(a) Diamond (b) Graphite (c) Sodium chloride (d) Ice

19. The lattice structure of magnesium oxide is:

(a) Simple molecular (b) Giant ionic (c) Giant metallic (d) Giant covalent

20. Which factor does NOT affect the melting point of a giant ionic lattice?

(a) Ionic charge (b) Ionic radius (c) Colour of the ions (d) Lattice energy

21. Silicon dioxide (SiO₂) has a high melting point because:

(a) It has weak intermolecular forces (b) It is a simple molecule (c) It has a giant covalent structure with strong bonds (d) It contains ions

22. In metallic bonding, electrical conductivity is due to:

(a) Fixed ions (b) Delocalised electrons (c) Covalent bonds (d) Hydrogen bonds

23. Which statement about diamond is true?

(a) It conducts electricity (b) It has a layered structure (c) Each carbon atom is bonded to four others in a tetrahedral arrangement (d) It is soft and slippery

24. Which substance is likely to be soluble in water due to ionic nature?

(a) CH₄ (b) CCl₄ (c) MgCl₂ (d) I₂

25. The shape of SF₆ is:

(a) Tetrahedral (b) Octahedral (c) Trigonal bipyramidal (d) Square planar

26. Bond energy is defined as:

(a) Energy released when a bond is formed (b) Energy required to break one mole of a covalent bond in the gaseous state (c) The distance between two bonded nuclei (d) The attraction between two ions

27. Which compound can expand its octet?

(a) CH₄ (b) NH₃ (c) PCl₅ (d) H₂O

28. Electronegativity is:

(a) The energy required to remove an electron (b) The ability of an atom to attract electrons in a covalent bond (c) The size of an atom (d) The charge on an ion

29. Which element has the highest electronegativity?

(a) Carbon (b) Oxygen (c) Fluorine (d) Nitrogen

30. In the gas equation \( PV = nRT \), the constant R is:

(a) 0.0821 L·atm/mol·K (b) 8.314 J/mol·K (c) Both (a) and (b) are correct values (d) 22.4 L/mol

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Quiz Results

Cambridge International AS & A Level Chemistry 9701 Syllabus • Topics 3.2–4.2