Question

The correct dot formulation for nitrogen trichloride has:
A. \[2N - Cl\] bonds, \[1N = Cl\]bond, and 8 lone pairs of electrons.
B. \[3N - Cl\] bonds and 10 lone pairs of electrons.
C. \[1N - Cl\] bond, \[2N = Cl\]bonds, and 7 lone pairs of electrons.
D. \[3N = Cl\] bonds and 6 lone pairs of electrons.

Answer 1

Hint: The geometry structure of the nitrogen trichloride is tetrahedral. The shape of this compound is pyramidal.

Complete Step by Step Solution:
1. The electronic configuration of the nitrogen atom \[[He]2{s^2}2{p^3}\]and the chlorine atom is \[[Ne]3{s^2}3{p^5}\].
2. The valence electrons of the nitrogen atom and chlorine atom are five and seven.
3. The total number of valence electrons of the nitrogen trichloride is twenty-six including the three chlorine atoms.
4. The nitrogen forms three bonds with the three chlorine atoms in which three electrons of nitrogen and three electrons of each chlorine are used to form a structure.
5. A total of six electrons are used to form this compound and a total of twenty electrons are remaining as lone pairs on the nitrogen and chlorine atoms.
6. There is one lone pair on the nitrogen and three lone pairs on each chlorine atom.
7. The dot structure of nitrogen trichloride is presented below:

Image: nitrogen trichloride

Thus, the option (B) is correct.

Additional information:
1. The structure of nitrogen trichloride is tetrahedral that includes both lone pairs and bond pairs since the lone pair is considered to be the bond pair.
2. The structure of nitrogen trichloride is trigonal pyramidal when considering only the bond pairs but not the lone pair.

Note: The Hybridization of the nitrogen trichloride \[s{p^3}\]that involves one 2s and three 2p orbitals that mix to form a new orbital with the same energy.