Metallic Bonding Quiz
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5 questions, one answer each
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1. What are the charged particles in a metallic lattice called?
- A. Anions
- B. Delocalised electrons only
- C. Positive metal ions
- D. Neutral atoms
2. Why do metals conduct electricity?
- A. Their ions are free to move
- B. Delocalised electrons are free to move and carry charge through the structure
- C. They contain free protons
- D. They have covalent bonds
3. What is metallic bonding?
- A. Sharing of electron pairs between two non-metal atoms
- B. Transfer of electrons from one atom to another
- C. Electrostatic attraction between positive ions and delocalised electrons
- D. Attraction between two neutral atoms only
4. Which property of metals is best explained by layers of ions sliding over each other while delocalised electrons continue to hold the structure together?
- A. High melting point
- B. Electrical conductivity
- C. Malleability
- D. Density
5. A student compares a metal and an ionic solid, both hit with a hammer. Why does the metal bend into shape but the ionic solid shatters?
- A. The metal has no ions, so nothing repels
- B. In the metal, delocalised electrons keep attracting the ions as layers slide, whereas in the ionic lattice, sliding brings like-charged ions together, causing repulsion and fracture
- C. The ionic solid is a gas at room temperature
- D. Metals are always softer than ionic solids regardless of structure