Paper 2 Bonding MCQ Practice
10 multiple-choice questions on chemical bonding for IGCSE Chemistry Paper 2. Covers ionic, covalent, and metallic bonding, dot-and-cross diagrams, and structure-property links.
Published by IGCSEChemistry.com.my
Chemistry teaching team: K. S. Tan (15+ years teaching IGCSE Chemistry) and Ms Yash (10+ years teaching IGCSE Chemistry) and Ms Kartini (15+ years teaching IGCSE Chemistry).
Mapped to Cambridge IGCSE Chemistry 0620 (2026–2028). Last updated 2026-08-19.
Ten multiple-choice questions in the style of IGCSE Chemistry Paper 2. Choose the best answer for each, then check the mark scheme.
Question 1
Which type of bonding involves the transfer of electrons from one atom to another?
A. Covalent bonding B. Metallic bonding C. Ionic bonding D. Hydrogen bonding
Answer
C
Ionic bonding involves the transfer of electrons from a metal atom to a non-metal atom. The metal loses electrons to form a positive ion (cation) and the non-metal gains electrons to form a negative ion (anion). The electrostatic attraction between opposite charges holds the compound together.
Question 2
Sodium chloride has a high melting point because it has:
A. strong covalent bonds between atoms. B. strong electrostatic forces between oppositely charged ions in a lattice. C. weak intermolecular forces between molecules. D. delocalised electrons holding atoms together.
Answer
B
Sodium chloride is an ionic compound with a giant ionic lattice. The strong electrostatic attractions between Na+ and Cl- ions extend throughout the structure in all directions. A large amount of energy is needed to overcome these forces, resulting in a high melting point.
Question 3
Which substance consists of simple molecules?
A. Sodium chloride B. Diamond C. Water D. Copper
Answer
C
Water (H₂O) consists of simple molecules. Each molecule contains two hydrogen atoms covalently bonded to one oxygen atom. The intermolecular forces between water molecules are weak, giving water a relatively low boiling point. NaCl is a giant ionic structure, diamond is a giant covalent structure, and copper is a metallic structure.
Question 4
Why does diamond have a very high melting point?
A. It contains ionic bonds. B. Each carbon atom forms four strong covalent bonds in a giant structure. C. It contains metallic bonds. D. It has strong intermolecular forces.
Answer
B
Diamond has a giant covalent structure in which each carbon atom is bonded to four other carbon atoms by strong covalent bonds. These bonds extend throughout the entire structure. Breaking these many strong bonds requires a very large amount of energy, so the melting point is extremely high (over 3500 degC).
Question 5
Which property is typical of a substance with a simple molecular structure?
A. High melting point B. Conducts electricity when solid C. Low boiling point D. Soluble in water but not in organic solvents
Answer
C
Simple molecular substances have low melting and boiling points because the intermolecular forces between molecules are weak and easily overcome. The strong covalent bonds within the molecules are not broken during melting or boiling. They generally do not conduct electricity because they have no free ions or electrons.
Question 6
In metallic bonding, what holds the metal atoms together?
A. Shared pairs of electrons between atoms B. Transfer of electrons from one atom to another C. Electrostatic attraction between positive metal ions and delocalised electrons D. Weak intermolecular forces
Answer
C
In metallic bonding, metal atoms lose their outer electrons, forming a lattice of positive ions. The lost electrons become delocalised (free to move throughout the structure). The electrostatic attraction between the positive metal ions and the sea of delocalised electrons holds the structure together.
Question 7
Why do ionic compounds conduct electricity when molten but not when solid?
A. The ions decompose when melted. B. The ions are free to move when molten but are held in fixed positions in the solid. C. New ions are created during melting. D. The electrons are released when the solid melts.
Answer
B
In solid ionic compounds, the ions are held in fixed positions in a lattice and cannot move to carry charge. When the compound melts, the ions become free to move and can carry electrical charge through the liquid. Similarly, when dissolved in water, the ions dissociate and are free to move.
Question 8
What type of bonding is present in a molecule of hydrogen chloride, HCl?
A. Ionic B. Covalent C. Metallic D. Ionic and covalent
Answer
B
HCl is formed between two non-metal atoms (hydrogen and chlorine), so the bonding is covalent. Each atom shares one electron to form a single shared pair of electrons (a single covalent bond). Both atoms achieve stable electron configurations through sharing.
Question 9
Graphite conducts electricity but diamond does not. This is because graphite:
A. has ionic bonds between layers. B. has delocalised electrons that are free to move between the layers. C. is softer than diamond. D. has weaker covalent bonds than diamond.
Answer
B
In graphite, each carbon atom forms only three covalent bonds, leaving one electron per atom delocalised. These delocalised electrons are free to move along the layers, allowing graphite to conduct electricity. In diamond, all four outer electrons of each carbon are used in covalent bonds, so there are no delocalised electrons and no electrical conductivity.
Question 10
Which of the following correctly describes a covalent bond?
A. The transfer of electrons from a metal to a non-metal B. A shared pair of electrons between two non-metal atoms C. The electrostatic attraction between positive and negative ions D. A sea of delocalised electrons surrounding metal ions
Answer
B
A covalent bond is a shared pair of electrons between two atoms, typically both non-metals. Each atom contributes one electron to the shared pair (in a standard covalent bond). Option A describes ionic bonding, C describes the ionic lattice force, and D describes metallic bonding.
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