Question

What is the hybridization in $C{O}_2$ ?

Answer 1

Answer
The carbon atom has sp hybridization; the O atoms have $s{p}^2$hybridization.
Explanation:
You must first draw the Lewis structure for $C{O}_2$
According to VSEPR theory, we can use the steric number (SN) to determine the hybridization of an atom.
SN = number of lone pairs + number of atoms directly attached to the atom.
SN = 2 corresponds to sp hybridization.SN=3 corresponds to $s{p}^2$hybridization.We see that the C atom has SN = 2. It has no lone pairs, but it is attached to two other atoms.
It has sphybridization.
Each O atom has SN = 3. It has 2 lone pairs and is attached to 1 C atom.
Just as the carbon atom hybridized to form the best bonds, so do the oxygen atoms.
The valence electron configuration of O is $\left[He\right]2s^{2}2p^4$To accommodate the two lone pairs and the bonding pair, it will also form three equivalent $s{p}^2$ hybrid orbitals.
Two of the $s{p}^2$ orbitals contain lone pairs, while the remaining $s{p}^2$orbital and the unhybridized p orbital have one electron each.
We can see this arrangement in the C=O bond of formaldehyde, which is equivalent to the right-hand side of the O=C=O molecule.
There is a similar arrangement on the left side of the O=C=O molecule, but the $\pi$ bond is horizontal rather than vertical.