Question

answer the questions below about the highlighted atom in this lewis structure: h — o — c == o h — c — h h in how many sigma bonds does the highlighted atom participate? in how many pi bonds does the highlighted atom participate? what is the orbital hybridization of the highlighted atom?

Explanation:

Step1: Identify sigma - bonds

A single bond is a sigma bond. The highlighted carbon atom has 4 single bonds (to three H - atoms and one C - atom). So, the number of sigma bonds is 4.

Step2: Identify pi - bonds

A double bond has 1 pi - bond and a single bond has 0 pi - bonds. The highlighted carbon atom is involved in only single bonds, so the number of pi - bonds is 0.

Step3: Determine orbital hybridization

The carbon atom has 4 electron - groups (4 single bonds). According to the VSEPR theory, when an atom has 4 electron - groups, its orbital hybridization is $sp^{3}$.

Answer:

In how many sigma bonds does the highlighted atom participate? 4
In how many pi bonds does the highlighted atom participate? 0
What is the orbital hybridization of the highlighted atom? $sp^{3}$