📚 Part 1: Understanding Ionic Bonding

1. What happens to electrons when sodium (Na) bonds with chlorine (Cl)?

Electrons are shared equally

Sodium loses an electron to chlorine

Chlorine loses an electron to sodium

No electrons are transferred

2. Which of the following are properties of ionic compounds? (Tick all that apply)

High melting points

Conduct electricity when solid

Conduct electricity when molten

Often soluble in water

3. The structure of ionic compounds is best described as:

Individual molecules

Giant ionic lattice

Simple molecular structure

Metallic structure

4. Complete the sentence: Ionic bonds form between _________ and _________ through _________ transfer.

✏️ Part 2: Writing Ionic Formulae

5. Write the correct ionic formula for each compound by balancing the charges:

a) Magnesium oxide (Mg²⁺ and O²⁻): __________

b) Aluminium chloride (Al³⁺ and Cl⁻): __________

c) Calcium fluoride (Ca²⁺ and F⁻): __________

d) Sodium sulfide (Na⁺ and S²⁻): __________

6. Explain why ionic compounds have high melting points:

7. Why do ionic compounds conduct electricity when molten or dissolved in water, but not when solid?

🔬 Part 3: Real-World Applications

8. Table salt (sodium chloride) dissolves easily in water. Using your knowledge of ionic bonding, explain why this happens:

9. Extension Challenge: Magnesium oxide (MgO) has a much higher melting point than sodium chloride (NaCl). Suggest why this might be, considering the charges on the ions:

10. Draw a simple diagram showing the arrangement of ions in an ionic lattice. Label the positive and negative ions and show the electrostatic attractions: