Question

1
2
h₂n nh₂
1 = sp³; 2 = sp²
1 = sp³; 2 = sp³
1 = sp²; 2 = sp²
1 = sp²; 2 = sp³

Explanation:

Step1: Determine hybridization of atom 1

For the amino group (\( -NH_2 \)) (atom 1), the nitrogen has 4 electron - pair domains (3 bonding pairs with H and 1 lone pair). According to the VSEPR theory, the hybridization is \( sp^3 \). The formula for hybridization \( H=\frac{V + M - C+A}{2}\), where \( V\) is the number of valence electrons of the central atom (\( V = 5\) for N), \( M\) is the number of monovalent atoms (\( M = 2\) for two H atoms), \( C\) is the charge for cation, \( A\) is the charge for anion (here \( C = A=0\)). So \( H=\frac{5 + 2}{2}=\frac{7}{2}=3.5\approx4\) (rounding up for hybridization), which corresponds to \( sp^3\) hybridization.

Step2: Determine hybridization of atom 2

For the carbonyl - adjacent nitrogen (atom 2), due to resonance (the lone pair on nitrogen can delocalize into the adjacent carbonyl group). The nitrogen has 3 electron - pair domains (2 bonding pairs with H and 1 delocalized lone pair that is in a p - orbital for resonance). Using the formula \( H=\frac{V + M}{2}\) (since the lone pair is delocalized and we consider the idealized resonance - hybrid structure where the electron - pair geometry is trigonal planar). \( V = 5\) (valence electrons of N), \( M = 2\) (two H atoms). But because of resonance, the effective \( H = 3\) (trigonal planar electron - pair geometry), and the hybridization is \( sp^2\).

Answer:

\(1 = sp^3; 2 = sp^2\)