Metallic Bonding Quiz
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5 questions, one answer each
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1. What is metallic bonding?
- A. Sharing of electron pairs between two non-metal atoms
- B. Electrostatic attraction between oppositely charged ions
- C. Electrostatic attraction between positive metal ions and delocalised electrons
- D. Transfer of electrons from a metal to a non-metal atom
2. Why are metals good conductors of electricity?
- A. Their ions are negatively charged
- B. Delocalised electrons are free to move through the structure
- C. They have very high melting points
- D. Their atoms are very small
3. Which property of metals is best explained by layers of ions sliding over each other?
- A. High melting point
- B. Malleability and ductility
- C. Electrical conductivity
- D. Low density
4. Which statement correctly compares metals with diamond?
- A. Both conduct electricity because both have delocalised electrons
- B. Diamond conducts electricity but metals do not
- C. Metals conduct electricity due to delocalised electrons; diamond does not, as it has no free electrons or ions
- D. Neither metals nor diamond conduct electricity
5. A student says 'metals have high melting points because covalent bonds must be broken.' Explain why this is incorrect and give the correct reason.
- A. It is correct — metals contain strong covalent bonds
- B. Incorrect — metals have weak intermolecular forces, not covalent bonds
- C. Incorrect — the strong electrostatic attraction between positive ions and delocalised electrons throughout the lattice must be overcome, not covalent bonds
- D. Incorrect — metals have low melting points, not high ones