Question

select the correct answer from each drop - down menu. describe the characteristics of a molecule of ammonia (nh₃). the lewis structure and table of electronegativities are given. h - n - h | h the bond polarities are, the molecular shape is, and the molecule is. bent linear tetrahedral trigonal planar trigonal pyramidal

Explanation:

Step1: Determine bond polarities

The electronegativity of N is 3.04 and of H is 2.20. The electronegativity difference $\Delta\chi=3.04 - 2.20=0.84$. Since $0<\Delta\chi < 1.7$, the N - H bonds are polar.

Step2: Determine molecular shape

N in $NH_3$ has 3 bonding pairs and 1 lone - pair. According to VSEPR theory, the electron - pair geometry is tetrahedral and the molecular shape is trigonal - pyramidal.

Step3: Determine molecular polarity

The bond dipoles in $NH_3$ do not cancel out due to the trigonal - pyramidal shape and the presence of the lone - pair on N. So, the molecule is polar.

Answer:

The bond polarities are polar, the molecular shape is trigonal - pyramidal, and the molecule is polar.