Draw the Lewis Structure for CH3COOH and Determine the Geometry, Orbital Hybridization, and Bond Angles Around the Second Carbon

To begin with, the Lewis structure for acetic acid (CH₃

• Carbon (C) has 4 valence electrons, and there are two carbons in the molecule.
• Hydrogen (H) has 1 valence electron, and there are four hydrogens in the molecule.
• Oxygen (O) has 6 valence electrons, and there are two oxygens in the molecule.

Calculating the total valence electrons: 2(4) + 4(1) + 2(6) = 14 valence electrons.

The structure can be arranged as follows:

       H   H
        |   |
      H-C - C = O
          |   |
          O - H
   

In this structure, the first carbon (C1) is bonded to three hydrogens and the second carbon (C2). The second carbon (C2) has a double bond with one oxygen and a single bond with another oxygen along with a hydrogen atom.

Now, to determine the geometry around the second carbon (C2):

• The central carbon atom (C2) is surrounded by one hydrogen and two oxygen atoms, one of which forms a double bond with C2.
• This gives C2 a total of three regions of electron density (one double bond and two single bonds).

According to VSEPR theory, with three regions of electron density, the geometry around C2 will be trigonal planar. This is because the electron pairs will arrange themselves to minimize repulsion.

Now, for the hybridization around C2:

• The sp² hybridization occurs here, as C2 has three bonding regions (two single bonds and one double bond).

Finally, the bond angles:

• In a trigonal planar geometry, the ideal bond angles are approximately 120 degrees.

In conclusion, for the second carbon (C2) in CH_{32, the geometry is trigonal planar, and the bond angles are around 120 degrees.}