answer the questions in the table about each labeled atom in the molecule below.\nnote for advanced…

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

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

Answer

Explanation:

Step1: Analyze atom a

Atom a is a carbon in a double - bonded ring. It has 3 electron groups (2 single bonds and 1 double bond). The electron - group geometry around an atom with 3 electron groups is trigonal planar. Using the concept of hybridization, 3 electron groups correspond to $sp^{2}$ hybridization.

Step2: Analyze atom b

Atom b is a carbon in a triple bond. It has 2 electron groups (1 single bond and 1 triple bond). The electron - group geometry around an atom with 2 electron groups is linear. For 2 electron groups, the hybridization is $sp$.

Step3: Analyze atom c

Atom c is a nitrogen in a triple bond. It has 2 electron groups (1 triple bond and 1 lone pair). The electron - group geometry around an atom with 2 electron groups is linear. The hybridization of an atom with 2 electron groups is $sp$.

Answer:

Atom Electron group geometry Hybridization
Atom a Trigonal planar $sp^{2}$
Atom b Linear $sp$
Atom c Linear $sp$