Which of the following best represents the correct Lewis dot structure for the neutral compound NF_3?

• A. N is at the center with three single bonds to F atoms, and two lone pairs on N; each F atom has two lone pairs.
• B. N is at the center with three single bonds to F atoms, and no lone pairs on N; each F atom has three lone pairs.
• C. N is at the center with three single bonds to F atoms, and one lone pair on N; each F atom has three lone pairs.
• D. N is at the center with three double bonds to F atoms, and no lone pairs on N; each F atom has two lone pairs.

Answer: (C)

Verified step by step guidance

1. Step 1: Determine the total number of valence electrons for the NF_3 molecule. Nitrogen (N) has 5 valence electrons, and each fluorine (F) has 7 valence electrons. Since there are three fluorine atoms, calculate the total as \$5 + 3 \times 7$.
2. Step 2: Arrange the atoms with nitrogen as the central atom because it is less electronegative than fluorine. Connect each fluorine atom to nitrogen with a single bond. Each single bond represents 2 electrons.
3. Step 3: Distribute the remaining valence electrons to complete the octets of the fluorine atoms first. Each fluorine needs 8 electrons total (including bonding electrons), so add lone pairs to each fluorine until their octets are complete.
4. Step 4: Place any leftover electrons on the central nitrogen atom as lone pairs. Remember that nitrogen also aims to complete its octet (8 electrons total, counting bonding and lone pairs).
5. Step 5: Verify the structure by counting the total electrons used and ensuring all atoms have complete octets. Confirm that the nitrogen has one lone pair and each fluorine has three lone pairs, consistent with the correct Lewis structure for NF_3.