Draw the complete Lewis structure for NH2Cl using lines for bonds and pairs of dots for nonbonding electrons

To draw the Lewis structure for NH₂Cl, we first need to identify the total number of valence electrons available in the molecule. Nitrogen (N) has 5 valence electrons, each hydrogen (H) has 1 (and there are 2 H atoms), and chlorine (Cl) has 7 valence electrons. So, the total is:

5 (for N) + 2 × 1 (for H) + 7 (for Cl) = 5 + 2 + 7 = 14 valence electrons.

We start by placing the nitrogen atom in the center because it is less electronegative than chlorine. We then connect the nitrogen to the two hydrogen atoms using single bonds. After that, we connect the nitrogen to the chlorine atom also with a single bond. This accounts for 6 of the 14 valence electrons (2 electrons for each bond, 3 bonds total).

Now we place the remaining 8 electrons. The chlorine atom requires 6 more electrons to complete its octet, which we illustrate as 3 lone pairs of dots around the chlorine. The nitrogen atom is surrounded by 3 bonds, which means it has 6 electrons involved in bonds, so it also satisfies the octet rule.

Here is the completed Lewis structure: