Question

using the highlight tool, assign the hybridization of each carbon as follows: sp: red sp²: green sp³: blue

Explanation:

Step1: Recall hybridization rules

Carbon with 2 electron - group is $sp$ hybridized, 3 electron - group is $sp^{2}$ hybridized, and 4 electron - group is $sp^{3}$ hybridized.

Step2: Analyze double - bonded carbons

Double - bonded carbons have 3 electron - groups around them (one $\sigma$ bond, one $\pi$ bond and other bonds), so they are $sp^{2}$ hybridized.

Step3: Analyze single - bonded carbons

Single - bonded carbons have 4 electron - groups around them (4 $\sigma$ bonds), so they are $sp^{3}$ hybridized.

Answer:

For the double - bonded carbons in the structure, use the green highlighter ( $sp^{2}$ hybridization). For the single - bonded carbons in the structure, use the blue highlighter ( $sp^{3}$ hybridization). There are no $sp$ hybridized carbons in the given structure shown.