QQuestionChemistry
QuestionChemistry
"Question: Draw a valid Lewis structure for the molecule CH^3NO in which there are no nonzero formal charges on any of the atoms. This structure should not include any bonds between N and O.
What do you do with the oxygen?"
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Answer
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Step 1:I'll solve this Lewis structure problem step by step:
Step 2:: Determine the total number of valence electrons
Total = 4 + (3 \times 1) + 5 + 6 = 16 valence electrons
- Carbon (C): 4 valence electrons - Hydrogen (H) × 3: 1 electron each (3 total) - Nitrogen (N): 5 valence electrons - Oxygen (O): 6 valence electrons
Step 3:: Arrange atoms to avoid N-O bond
- Place carbon centrally - Attach hydrogens to carbon - Position nitrogen next to carbon - Place oxygen away from nitrogen
Step 4:: Connect atoms with single bonds
- Connect 3 hydrogens to carbon - Connect nitrogen to carbon - Distribute remaining electrons as lone pairs
Step 5:: Complete the Lewis structure
H-C-N=O
- Ensure each atom follows octet rule - Distribute remaining electrons as lone pairs - Verify no nonzero formal charges Final Lewis Structure: - Carbon has 4 single bonds - Nitrogen has one double bond to oxygen - Oxygen has two lone pairs - Hydrogens complete carbon's octet
Final Answer
The Lewis structure places the oxygen in a double-bonded position with nitrogen, away from a direct N-O single bond, while satisfying the octet rule for all atoms.
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