Question

answer the questions below about the highlighted atom in this lewis structure: 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: Recall bond - type rules

A single bond is a sigma bond. A double bond consists of one sigma and one pi bond.

Step2: Analyze the highlighted atom

Assume the middle - carbon (the one in the double bond) is highlighted. It has two single bonds (sigma bonds) and one double bond (one sigma and one pi bond). So, the number of sigma bonds is 3.

Step3: Determine pi - bond count

Since the highlighted atom is in a double bond, the number of pi bonds it participates in is 1.

Step4: Find orbital hybridization

An atom with 3 sigma - bond regions and no lone pairs has $sp^{2}$ hybridization.

Answer:

In how many sigma bonds does the highlighted atom participate? 3
In how many pi bonds does the highlighted atom participate? 1
What is the orbital hybridization of the highlighted atom? $sp^{2}$