Question

answer the questions in the table about each labeled atom in the molecule below. note for advanced students: if the molecule has resonance, answer the questions for the specific resonance contributor shown, not the hybrid structure. atom atom a atom b atom c what is the electron - group geometry around each labeled atom? what is the hybridization of each labeled atom?

Explanation:

Step1: Analyze atom a

Atom a is a carbonyl - carbon. It has 3 electron - groups (two single bonds and one double bond). The electron - group geometry around a carbonyl - carbon is trigonal planar. Using the concept of hybridization, with 3 electron - groups, the hybridization is $sp^{2}$.

Step2: Analyze atom b

Atom b is a benzene - ring carbon. Each carbon in a benzene ring has 3 electron - groups (two single bonds and one double bond in the resonance - contributing structure). The electron - group geometry is trigonal planar. And the hybridization is $sp^{2}$ due to 3 electron - groups.

Step3: Analyze atom c

Atom c is a nitrogen in a $C = N$ double - bond. It has 3 electron - groups (a single bond, a double bond, and a lone pair). The electron - group geometry is trigonal planar. The hybridization is $sp^{2}$ as it has 3 electron - groups.

Answer:

Atom	Electron Group Geometry	Hybridization
Atom b	Trigonal planar	$sp^{2}$
Atom c	Trigonal planar	$sp^{2}$