- Acetone, C3H60(CH3COCH3) Lewis structure using dots to represent bonding electrons: Lewis structure using lines to represent pairs of bonding electrons: Label the carbon atoms A,B, &C. Carbon atom A: Total number of electron groups: Number of lone pairs: Number of bonding groups/pairs: Bond angles: Electron geometry: Molecular geometry: Hybridization: Number of hybrid orbitals: Carbon atom B: Total number of electron groups: Number of lone pairs: Number of bonding groups/pairs: Bond angles: Electron geometry: Molecular geometry: Hybridization: Number of hybrid orbitals: Carbon atom C Total number of electron groups: Number of lone pairs: Number of bonding groups/pairs: Bond angles: Electron geometry: Molecular geometry: Number of hybrid orbitals: Hybridization: Is this molecule polar? (Y/N) Can this molecule hydrogen bond with itself? Number of sigma bonds: Number of pi bonds: None 1. Acetone, C3H6O(CH3COCH3) Lewis structure using dots to represent bonding electrons: Lewis structure using lines to represent pairs of bonding electrons: Label the carbon atoms A,B, &C. | Carbon atom A: Total number of electron groups: Number of bonding groups/pairs: Electron geometry: Molecular geometry: Hybridization: Carbon atom B: Total number of electron groups: Number of bonding groups/pairs: Electron geometry: Molecular geometry: Number of hybrid orbitals: I Electron geometry: Molecular geometry: Hybridization: Carbon atom C Total number of electron groups: Number of bonding groups/pairs: Number of lone pairs: Bond angles: Number of hybrid orbitals: Number of lone pairs: Bond angles: Hybridization: Is this molecule polar? (Y/N) Can this molecule hydrogen bond with itself? Number of sigma bonds: Number of pi bonds: Number of lone pairs: Bond angles: Number of hybrid orbitals: MacBook Pro
The correct answer and explanation is:
Here’s a detailed explanation and the correct answers for each part of the question about acetone (C₃H₆O):
Lewis Structure
- Dot Representation:
- Central carbon (B) is double-bonded to oxygen and single-bonded to two methyl groups (A and C).
- Dots around oxygen represent its lone pairs.
- Line Representation:
- A double line between carbon (B) and oxygen.
- Single lines connecting carbon (B) to carbons (A) and (C).
- Carbon (A) and (C) are bonded to three hydrogens each.
Carbon Atom A (CH₃ group)
- Total electron groups: 4 (3 bonding pairs with hydrogens, 1 bond with carbon B).
- Number of lone pairs: 0.
- Number of bonding groups/pairs: 4.
- Bond angles: Approximately 109.5°.
- Electron geometry: Tetrahedral.
- Molecular geometry: Tetrahedral.
- Hybridization: sp³.
- Number of hybrid orbitals: 4.
Carbon Atom B (C=O group)
- Total electron groups: 3 (1 double bond with oxygen, 2 single bonds with carbons A and C).
- Number of lone pairs: 0.
- Number of bonding groups/pairs: 3.
- Bond angles: Approximately 120°.
- Electron geometry: Trigonal planar.
- Molecular geometry: Trigonal planar.
- Hybridization: sp².
- Number of hybrid orbitals: 3.
Carbon Atom C (CH₃ group)
- Total electron groups: 4 (3 bonding pairs with hydrogens, 1 bond with carbon B).
- Number of lone pairs: 0.
- Number of bonding groups/pairs: 4.
- Bond angles: Approximately 109.5°.
- Electron geometry: Tetrahedral.
- Molecular geometry: Tetrahedral.
- Hybridization: sp³.
- Number of hybrid orbitals: 4.
Other Characteristics
- Polarity: Yes, acetone is polar because the C=O bond creates a dipole moment.
- Hydrogen Bonding with Itself: No, acetone cannot hydrogen bond with itself, as it lacks a hydrogen atom directly bonded to an electronegative atom like oxygen or nitrogen.
- Number of Sigma Bonds: 9 (6 C-H bonds, 2 C-C bonds, and 1 C=O sigma bond).
- Number of Pi Bonds: 1 (from the C=O double bond).
Explanation (Summary)
Acetone’s structure is dictated by the hybridization and geometry of each carbon atom. Carbon A and C exhibit sp³ hybridization, leading to tetrahedral geometry with approximately 109.5° bond angles. Carbon B, as part of the C=O group, is sp² hybridized, resulting in trigonal planar geometry and 120° bond angles. The molecule’s polar nature arises from the electronegative oxygen, creating a net dipole moment. Acetone does not form hydrogen bonds with itself but has strong dipole-dipole interactions. Its sigma and pi bonds further contribute to its chemical reactivity.