Question

provide the hybridization and molecular geometry for the indicated atoms in the following molecules. part 1 of 3 the highlighted c atom. hybridization: molecular geometry: select part 2 of 3 the n atom in the highlighted group. hybridization:

Explanation:

Step1: Determine the number of electron - groups around the C atom in part 1

The carbon atom in the $H_2C = O$ has 3 electron - groups (two single bonds to H and one double bond to O).

Step2: Find the hybridization for part 1

Based on the number of electron - groups, the hybridization is $sp^2$.

Step3: Determine the molecular geometry for part 1

With 3 electron - groups and no lone pairs on the central C atom, the molecular geometry is trigonal planar.

Step4: Determine the number of electron - groups around the N atom in part 2

The nitrogen atom in $CH_3CH_2NH_2$ has 4 electron - groups (three single bonds to H and one single bond to C, plus one lone pair).

Step5: Find the hybridization for part 2

Based on 4 electron - groups, the hybridization is $sp^3$.

Step6: Determine the molecular geometry for part 2

With 4 electron - groups and one lone pair on the central N atom, the molecular geometry is trigonal pyramidal.

Answer:

Part 1:
Hybridization: $sp^2$
Molecular geometry: trigonal planar
Part 2:
Hybridization: $sp^3$
Molecular geometry: trigonal pyramidal