Ionic vs Covalent Properties

Name:

Date:

📚 Part 1: Understanding the Basics

Key Definitions:

Ionic compounds: Formed when electrons are transferred from metal atoms to non-metal atoms, creating charged ions held together by electrostatic forces.

Covalent compounds: Formed when atoms share electrons to complete their outer electron shells.

Interesting Fact: Table salt (sodium chloride) is ionic and conducts electricity when dissolved, whilst sugar (sucrose) is covalent and doesn't conduct electricity at all!

1. Which type of bonding occurs between a metal and a non-metal?

Ionic bonding

Covalent bonding

Metallic bonding

Hydrogen bonding

2. Which properties are typical of ionic compounds? (Select all that apply)

High melting points

Conduct electricity when dissolved

Often gases at room temperature

Form crystalline structures

3. Covalent compounds typically have _______ melting points and _______ conduct electricity.

Fill in the blanks: _____________ and _____________

4. Which compound would you expect to have the highest melting point?

Water (H₂O)

Sodium chloride (NaCl)

Methane (CH₄)

Carbon dioxide (CO₂)

🔬 Part 2: Extended Analysis

5. Explain why ionic compounds conduct electricity when dissolved in water, but covalent compounds generally do not. Use your knowledge of bonding and ion formation in your answer.

6. A student finds a white crystalline solid that dissolves in water. When they test the solution with a conductivity meter, it lights up brightly. What type of bonding is most likely present in this compound? Justify your answer.

7. Think Deeper: Diamond is made entirely of carbon atoms covalently bonded together, yet it has an extremely high melting point (over 3500°C). How does this compare to typical covalent compounds like water or methane? What might explain this difference?

🎯 Part 3: Quick Recap & Application

8. Complete the comparison table by filling in the missing properties:

Ionic Compounds:

• Melting point: _____________

• Electrical conductivity: _____________ when dissolved

• Structure: _____________

Covalent Compounds:

• Melting point: _____________

• Electrical conductivity: _____________

• Structure: _____________ molecules

9. Debate Question: "All compounds with high melting points must be ionic." Do you agree or disagree with this statement? Give evidence to support your position.

Model Answers:

Q1: Ionic bonding | Q2: High melting points, Conduct electricity when dissolved, Form crystalline structures | Q3: low, do not | Q4: Sodium chloride (NaCl) | Q5: Ionic compounds form ions when dissolved which carry electric current; covalent compounds remain as neutral molecules | Q8: Ionic - High, Conducts, Crystalline; Covalent - Low, Does not conduct, Discrete