Draw a Lewis structure for CH3NO that has no formal charge. Draw an orbital picture for CH3NO and label all parts (including all the hybrid orbitals, non-hybrid orbitals, sigma bonds, and pi bond). Please include all the electrons.
The Correct Answer and Explanation is:
To draw the Lewis structure of CH3NO (methyl nitroxide), we need to satisfy the following conditions:
Step-by-step Process:
- Count the Valence Electrons:
- Carbon (C) has 4 valence electrons.
- Hydrogen (H) has 1 valence electron, and there are 3 hydrogens in CH3, contributing 3 electrons.
- Nitrogen (N) has 5 valence electrons.
- Oxygen (O) has 6 valence electrons.
- Total = 4 (C) + 3 (H) + 5 (N) + 6 (O) = 18 valence electrons.
- Place the Atoms:
- Carbon (C) is the central atom, attached to three hydrogens (H) and nitrogen (N).
- Nitrogen (N) will bond to oxygen (O).
- Form Bonds:
- Carbon (C) forms single bonds with three hydrogen atoms and one single bond with nitrogen.
- Nitrogen (N) forms a single bond with oxygen.
- To minimize formal charges, nitrogen will have a lone pair of electrons, and oxygen will have a lone pair as well.
- Distribute the Electrons:
- Carbon has 3 bonds with hydrogen (6 electrons) and 1 bond with nitrogen (2 electrons), leaving it with no lone pairs.
- Nitrogen has 1 bond with carbon (2 electrons) and 1 bond with oxygen (2 electrons). It also holds one lone pair.
- Oxygen has 1 bond with nitrogen (2 electrons) and 2 lone pairs.
Formal Charges:
- Carbon: 4 (valence) – 4 (bonds) = 0 formal charge.
- Hydrogen: 1 (valence) – 1 (bond) = 0 formal charge (for each H).
- Nitrogen: 5 (valence) – 3 (bonds + lone pair) = 0 formal charge.
- Oxygen: 6 (valence) – 2 (bonds + lone pair) = 0 formal charge.
So, this arrangement has no formal charges, and the molecule is neutral.
Orbital Diagram:
- Carbon:
- Hybrid Orbitals: sp³ (for bonding with 3 hydrogens and 1 nitrogen).
- Sigma Bonds: All the bonds with hydrogens and nitrogen (C-H and C-N).
- Nitrogen:
- Hybrid Orbitals: sp² (for bonding with C and O).
- Sigma Bonds: C-N and N-O bonds.
- Lone Pair: 1 lone pair on nitrogen (in an sp² hybrid orbital).
- Oxygen:
- Hybrid Orbitals: sp² (for bonding with nitrogen).
- Sigma Bonds: N-O bond.
- Lone Pairs: 2 lone pairs on oxygen (in sp² orbitals).
- Pi Bond: There is no pi bond in this molecule because there are no double or triple bonds, only single bonds.
This structure satisfies the octet rule and minimizes formal charges, making CH3NO a stable, neutral molecule.
