Question

the complete lewis electron - dot diagram for hconh₂ is shown above. identify the hybridization of the valence orbitals for the carbon atom and the approximate hydrogen - carbon - nitrogen bond angle according to vsepr theory.
a sp hybridized and 180°
b sp² hybridized and 120°
c sp² hybridized and 180°
d sp³ hybridized and 120°

Explanation:

Step1: Analyze carbon - bonding situation

The carbon atom in $HCONH_2$ has 3 bonding regions (a double - bond to oxygen and single - bonds to hydrogen and nitrogen).

Step2: Determine hybridization

According to the rule that the number of hybrid orbitals equals the number of bonding regions around the atom, with 3 bonding regions, the carbon is $sp^{2}$ hybridized.

Step3: Determine bond angle

For $sp^{2}$ hybridized atoms with 3 bonding regions and no lone pairs on the central atom, the molecular geometry is trigonal planar and the bond angle is approximately $120^{\circ}$ according to VSEPR theory.

Answer:

B. $sp^{2}$ hybridized and $120^{\circ}$