Ionic Bonding and Ionic Compounds Quiz

1. Which of the following best describes ionic bonding?

• A. The electrostatic attraction between oppositely charged ions formed by the transfer of electrons from a metal to a non-metal
• B. The sharing of electrons between two non-metal atoms
• C. The attraction between a metal atom and a non-metal atom without any electron transfer
• D. The strong forces between atoms within a molecule

2. When a sodium atom forms an ionic compound, what happens to its electrons?

• A. It gains one electron to form Na⁻
• B. It loses one electron to form Na⁺
• C. It loses two electrons to form Na²⁺
• D. It shares electrons with another atom

3. Why do ionic compounds have high melting points?

• A. The ions are small in size
• B. The electrostatic forces between oppositely charged ions in the giant ionic lattice are very strong and require large amounts of energy to overcome
• C. The compound contains a metal element
• D. The ions are arranged in a regular repeating pattern

4. A solid ionic compound does not conduct electricity, but when it is melted, it conducts electricity. Which explanation is correct?

• A. Melting creates new ions in the compound
• B. Melting breaks the ionic lattice structure, allowing the ions to move freely and carry electrical charge
• C. Melting reduces the charge on the ions
• D. Melting converts the ionic compound into a covalent compound

5. Using your knowledge of electron transfer, explain why an aluminium atom and three chlorine atoms form the compound AlCl₃ rather than AlCl₂ or AlCl₄.

• A. Aluminium has 3 outer electrons and transfers one to each of three chlorine atoms, forming Al³⁺ and three Cl⁻ ions
• B. Chlorine atoms always form compounds with three other atoms
• C. AlCl₃ is the most stable because it has the lowest density
• D. Aluminium transfers all its electrons to chlorine atoms randomly