Ions and Ionic Bonds Quiz
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5 questions, one answer each
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1. Which statement correctly describes how a positive ion (cation) is formed?
- A. An atom loses electrons to achieve a stable electron configuration
- B. An atom gains electrons to achieve a stable electron configuration
- C. An atom loses protons from its nucleus
- D. An atom gains neutrons to increase its mass
2. Why do ionic compounds have high melting points?
- A. Because the ions are held together by weak covalent bonds
- B. Because the electrostatic forces between oppositely charged ions in the giant lattice structure are very strong
- C. Because the molecules vibrate rapidly at room temperature
- D. Because ionic compounds contain delocalised electrons throughout their structure
3. A solid ionic compound is placed in water and dissolves. The resulting aqueous solution conducts electricity well. Why is this different from the solid compound's electrical conductivity?
- A. Solid ionic compounds conduct electricity because the ions are fixed in position and cannot move
- B. In solution, the ions are free to move and carry electrical charge, whereas in the solid lattice the ions are fixed in place
- C. Water molecules become charged when ionic compounds dissolve, allowing electrical conduction
- D. Aqueous solutions conduct electricity because the water molecules form covalent bonds with the ions
4. Sodium (Group I) reacts with chlorine (Group VII) to form sodium chloride. Which description correctly explains the bonding in this compound?
- A. Sodium and chlorine share electrons to form a covalent bond
- B. Sodium transfers one electron to chlorine, forming Na⁺ and Cl⁻ ions held together by electrostatic attraction
- C. Chlorine transfers electrons to sodium, forming Cl⁺ and Na⁻ ions
- D. Sodium and chlorine form a metallic bond because sodium is a metal
5. A mystery ionic compound has the following properties: solid at room temperature, melts at 2072 °C, does not conduct electricity when solid but conducts well when molten, and dissolves in water to give a conducting solution. Considering the structure and bonding of ionic compounds, which of the following best explains why the electrical conductivity only occurs in the molten and aqueous states?
- A. The compound only contains ions when melted or dissolved; in the solid state it contains molecules instead
- B. In the solid state, ions are fixed in rigid lattice positions and cannot move freely to carry charge; melting and dissolving breaks down the lattice, allowing ion mobility
- C. The compound becomes chemically different when heated or dissolved, producing new ions that can conduct electricity
- D. Solid ionic compounds are insulators because they lack a continuous lattice structure