what is the hybridization at O with the lewis structure of 2-propanone?
To determine the hybridization at an atom in a molecule, you can follow these steps:
1. Draw the Lewis structure of the molecule: The Lewis structure of 2-propanone (also known as acetone) can be represented as CH₃COCH₃, where the carbon chain is in the middle and the oxygen is bonded to one of the carbons.
2. Count the number of electron groups around the atom of interest: In this case, we are interested in the oxygen atom (O). The oxygen atom in 2-propanone is double-bonded to one carbon atom and has two lone pairs of electrons.
3. Determine the hybridization: Hybridization is the concept of mixing of atomic orbitals to form new hybrid orbitals that allow for the bonding in a molecule. It is usually based on the number of electron groups around an atom. The hybridization of an atom is determined by the formula:
Hybridization = Number of sigma bonds + Number of lone pairs
In the case of oxygen in 2-propanone, it has one sigma bond (with carbon) and two lone pairs. Therefore, the hybridization is: 1 sigma bond + 2 lone pairs = sp².
So, the hybridization of the oxygen atom in 2-propanone is sp².