Question

1. choose the best answer.

how many lone pairs of electrons are present in the lewis structure for h₂co?
0
2
6
3

Explanation:

Step1: Identify lone pairs on each atom

In the Lewis structure of \( \ce{H2CO} \) (formaldehyde), we analyze each atom:

• Hydrogen (\( \ce{H} \)): Each \( \ce{H} \) is bonded to \( \ce{C} \) with a single bond, so no lone pairs (since \( \ce{H} \) has 1 valence electron, used in bonding).
• Carbon (\( \ce{C} \)): Bonded to two \( \ce{H} \) and double - bonded to \( \ce{O} \), so no lone pairs (carbon has 4 valence electrons, all used in bonding).
• Oxygen (\( \ce{O} \)): In the Lewis structure, the oxygen has two lone pairs (the two pairs of dots shown around the oxygen atom).

Step2: Count total lone pairs

Since only the oxygen atom has lone pairs and it has 2 lone pairs, the total number of lone pairs in the Lewis structure of \( \ce{H2CO} \) is 2.

Answer:

2 (corresponding to the option "2")