Which of the following statements correctly describes the Lewis dot structure of neutral HNO?

• A. HNO has a single bond between H and O, and a double bond between O and N, with one lone pair on N.
• B. HNO has a triple bond between N and O, with H bonded to O, and no lone pairs.
• C. HNO has a single bond between H and N, and a double bond between N and O, with one lone pair on O.
• D. HNO has a single bond between H and N, and a single bond between N and O, with two lone pairs on N.

Answer: (C)

Verified step by step guidance

1. Step 1: Determine the total number of valence electrons for HNO. Hydrogen (H) has 1 valence electron, Nitrogen (N) has 5, and Oxygen (O) has 6. Add these together to get the total valence electrons available for bonding.
2. Step 2: Decide the skeletal structure of the molecule. Since hydrogen can only form one bond, it will be bonded to either nitrogen or oxygen. Consider typical bonding patterns: nitrogen often forms multiple bonds, and oxygen usually forms two bonds with lone pairs.
3. Step 3: Draw possible Lewis structures by connecting atoms with single, double, or triple bonds, ensuring the total number of electrons used matches the total valence electrons calculated. Remember to place lone pairs to complete the octet for nitrogen and oxygen where applicable.
4. Step 4: Check the formal charges on each atom in your Lewis structures. The best Lewis structure minimizes formal charges and places negative charges on the more electronegative atoms (oxygen in this case).
5. Step 5: Compare the given options with your Lewis structures and select the one that matches the correct bonding pattern (single bond between H and N, double bond between N and O, and one lone pair on O) and has the lowest formal charges.