📚 Part 1: Understanding Covalent Bonds

1. What is a covalent bond?

Sharing of electrons between non-metal atoms

Transfer of electrons from metal to non-metal

Attraction between positive and negative ions

Sharing of electrons between metal atoms

2. Which of the following molecules contain covalent bonds? (Select all that apply)

H₂O (water)

NaCl (sodium chloride)

CO₂ (carbon dioxide)

CH₄ (methane)

MgO (magnesium oxide)

3. In a covalent bond, atoms share electrons to achieve:

A full outer electron shell (octet rule)

A positive charge

A negative charge

Equal numbers of protons and neutrons

4. Fill in the blanks: In the molecule H₂, two hydrogen atoms ________ one pair of electrons to form a ________ covalent bond.

In the molecule H₂, two hydrogen atoms _____________ one pair of electrons to form a _____________ covalent bond.

✏️ Part 2: Drawing Lewis Structures

5. Draw the Lewis dot structure for water (H₂O) in the box below. Show all electrons as dots or lines.

6. Draw the Lewis dot structure for ammonia (NH₃) in the box below.

7. Explain why oxygen forms two covalent bonds in water (H₂O).

8. Complete the comparison table below by writing characteristics in each column:

9. Explain why covalent compounds generally have lower melting points than ionic compounds.

10. Extension Challenge: Research and explain the difference between polar and non-polar covalent bonds. Give one example of each.