To complete the Lewis structure for chloramine (NH₂Cl), follow these steps:
1. Count the total number of valence electrons:
- Nitrogen has 5 valence electrons.
- Each hydrogen atom has 1 valence electron, for a total of 2 electrons from hydrogen.
- Chlorine has 7 valence electrons.
- Total: 5 (N) + 2 (2H) + 7 (Cl) = 14 valence electrons.
2. Arrange the atoms with nitrogen in the center, bonded to the two hydrogen atoms and the chlorine atom.
3. Use pairs of electrons to form the chemical bonds between the atoms. Each single bond between N and H and between N and Cl uses 2 electrons.
- 1 bond between N and H: 2 electrons.
- 1 bond between N and the other H: 2 electrons.
- 1 bond between N and Cl: 2 electrons.
- Total used for bonds: 2 + 2 + 2 = 6 electrons.
4. Fill in the remaining electrons as lone pairs to satisfy the octet rule (or duet rule for hydrogen, which only needs 2 electrons).
- Nitrogen needs 8 electrons in total, including bonding and lone pairs. It already has 3 bonds, contributing 6 electrons, so it needs 2 more electrons (1 lone pair).
- Chlorine needs 8 electrons, it has 1 bond (2 electrons) and needs 6 more electrons (3 lone pairs) to complete its octet.
5. Distribute the remaining electrons:
- Nitrogen: 1 lone pair (2 electrons).
- Chlorine: 3 lone pairs (6 electrons).
The complete Lewis structure will be:
```
H
|
H-N-Cl
:
```
Therefore, the tiles that correctly represent this structure are:
1. After [tex]$N - H =$[/tex]
2. Place 0 under the first [tex]$\square$[/tex] (indicative of zero more electrons between N and H).
3. Place [tex]$:$[/tex] (a colon) under the second [tex]$\square$[/tex] to represent a lone pair of electrons on nitrogen.
4. Place 4 under the left-over [tex]$\square$[/tex], signifying that the nitrogen atom shares 4 electrons.
Note: While the exact placement of the tiles might vary depending on the layout, these are the correct representations for nitrogen’s bonding and lone pairs.
