1. Count Valence Electrons:

* Nitrogen (N) has 5 valence electrons each (2 N atoms = 10 electrons)

* Hydrogen (H) has 1 valence electron each (2 H atoms = 2 electrons)

* Chlorine (Cl) has 7 valence electrons each (2 Cl atoms = 14 electrons)

* Total valence electrons = 10 + 2 + 14 = 26 electrons

2. Central Atom:

* Nitrogen is the least electronegative element, so it will be the central atom.

3. Single Bonds:

* Connect the atoms with single bonds.

* This uses 6 electrons (3 bonds x 2 electrons/bond).

4. Remaining Electrons:

* You have 20 electrons left (26 - 6).

5. Fill Octet for Outer Atoms:

* Complete the octets (8 electrons) for the hydrogen and chlorine atoms by adding lone pairs.

* This uses 12 electrons (2 H atoms x 2 electrons + 2 Cl atoms x 3 electrons).

6. Fill Octet for Central Atoms:

* The nitrogen atoms now have 6 electrons each. Give each nitrogen atom one lone pair. This uses the remaining 8 electrons.

7. Check for Formal Charge:

* Calculate the formal charge on each atom to ensure the structure is the most stable. The formal charge should be as close to zero as possible.

* Formal Charge = (Valence Electrons) - (Non-bonding Electrons) - (1/2 Bonding Electrons)

Lewis Structure:

```

H Cl

\ /

N-N

/ \

Cl H

```

Important Notes:

* This molecule has resonance structures, meaning the double bond can shift between the two nitrogen atoms.

* The molecule has a planar geometry.

* The N-Cl bonds are polar, and the molecule as a whole is also polar.