Which of the following represents the correct Lewis structure for the neutral compound NOF?

• A. N with a single bond to O and a double bond to F, with one lone pair on N
• B. N with a triple bond to O and a single bond to F, with no lone pairs on N
• C. N with a double bond to O and a single bond to F, with one lone pair on N
• D. N with a single bond to O and a single bond to F, with one lone pair on N

Answer: (C)

Verified step by step guidance

1. Step 1: Determine the total number of valence electrons for the compound NOF. Nitrogen (N) has 5 valence electrons, oxygen (O) has 6, and fluorine (F) has 7. Add these together to get the total number of valence electrons.
2. Step 2: Identify the central atom. In this case, nitrogen (N) is the central atom because it is less electronegative than oxygen and fluorine.
3. Step 3: Arrange the atoms around the central atom and draw single bonds initially. Connect N to O and N to F with single bonds. This uses up 4 valence electrons (2 for each bond).
4. Step 4: Distribute the remaining valence electrons to satisfy the octet rule, starting with the most electronegative atoms. Place lone pairs on O and F to complete their octets, then place any remaining electrons on N.
5. Step 5: Adjust the bonding to ensure all atoms have a complete octet. If necessary, convert lone pairs on adjacent atoms into double or triple bonds with the central atom. In this case, form a double bond between N and O to satisfy the octet rule for all atoms, leaving one lone pair on N.