Draw the Lewis structure of acetone, (CH3)2CO (C in the middle, with two Cs and an O bonded to it)

Draw the Lewis structure of acetone, (CH3)2CO (C in the middle, with two Cs and an O bonded to it). What is the hybridization on each carbon atom in the molecule? b. On the Lewis structure, identify every bond as a sigma or pi bond. (σ or π) c. For the Carbon-Hydrogen bond, what are the orbitals that overlap to make that bond?

The Correct Answer and Explanation is:

Here is the diagram of the Lewis structure of acetone ((CH₃)₂CO):

mathematicaCopyEdit       H   H
        \  /
    H — C — C == O
        / \
       H   C — H
            |
            H

Or more neatly, in a structural way:

mathematicaCopyEdit     H   H
      \  /
H — C — C == O
      / \
     H   C — H
          |
          H

Explanation:

Acetone is a ketone with the formula (CH₃)₂CO. The structure consists of a central carbonyl carbon that bonds to two methyl groups and an oxygen atom. Each methyl group has three hydrogen atoms attached to its carbon. The carbonyl carbon forms a double bond with oxygen, which consists of one sigma bond and one pi bond.

In this molecule, the hybridization of each atom determines how the atoms are arranged. The carbonyl carbon uses sp² hybridization because it forms three sigma bonds: one with each methyl carbon and one with oxygen. The remaining unhybridized p orbital on this carbon overlaps with a p orbital on oxygen to form the pi bond. This hybridization leads to a trigonal planar geometry around the carbonyl carbon, with bond angles close to 120 degrees.

The methyl carbons are sp³ hybridized because they form four sigma bonds: three with hydrogen atoms and one with the central carbon. This hybridization results in a tetrahedral geometry around each methyl carbon, with bond angles close to 109.5 degrees.

Each C-H bond results from the overlap of an sp³ orbital from the carbon with an s orbital from the hydrogen, forming a stable sigma bond. The C-C single bonds are sigma bonds formed by the overlap of sp³ and sp² orbitals. The C=O double bond includes a sigma bond formed by the overlap of sp² orbitals and a pi bond from the side-by-side overlap of unhybridized p orbitals.

This combination of hybridizations gives acetone its overall shape and bonding characteristics.