Step 1: Understanding the Concept:
Bonding electrons are those shared between atoms to form chemical bonds. Non-bonding electrons (lone pairs) are valence electrons that do not participate in bonding. We need to calculate the total count for each molecule.
Step 2: Key Formula or Approach:
1. Draw the Lewis structure for each molecule.
2. Count shared electrons (bonding) and lone pair electrons (non-bonding).
3. Check the ratio (Bonding : Non-bonding).
Step 3: Detailed Explanation:
For N₂: Nitrogen has 5 valence electrons. It forms a triple bond ($:N \equiv N:$).
Bonding electrons = 6 (3 pairs)
Non-bonding electrons = 4 (2 lone pairs)
Ratio = $6:4 = 3:2$.
For O₂ ($:O = O:$): Bonding = 4, Non-bonding = 8 (Ratio 1:2).
For F₂ ($:F - F:$): Bonding = 2, Non-bonding = 12 (Ratio 1:6).
For HCl ($H - Cl:$): Bonding = 2, Non-bonding = 6 (Ratio 1:3).
Step 4: Final Answer:
The ratio 3:2 is found in N₂.