Difluoroamine (NHF2) is a colorless, highly reactive, and explosive gas that primarily used to introduce the difluoroamino (-NF?) functional group into organic molecules. Here is its lewis structure and steps to draw it.

Step 1: Calculate total valence electrons

N: Group VA, 5 valence electrons

H: 1

F: 7 × 2 = 14

Total valence electrons: 5 + 1 + 14 = 20 e?

Step 2: Determine the central atom

N has lower electronegativity than F and H, so it serves as the central atom;

Connect the skeleton: N is bonded to one H and two F atoms; all bonds are single bonds.

Step 3: Construct the σ-bond skeleton

3 single bonds; bonding electrons: 3 × 2 = 6 e?

Remaining electrons: 20 ? 6 = 14 e?

Step 4: Fill in lone pairs on peripheral F atoms

Each F atom has only one single bond and requires 3 lone pairs (6 e?) to satisfy the octet rule;

Total electrons for F lone pairs: 2 × 6 = 12 e?

Remaining electrons after allocation: 14 ? 12 = 2 e?

Step 5: Place remaining electrons on the central N atom

2 e? = 1 lone pair on the N atom

Verify total electron count

Bonding electrons (6) + F lone pairs (12) + N lone pair (2) = 20 e?; matches the total valence electron count

Verify octet rule

N: 3 single bonds (6 bonding electrons) + 1 lone pair (2 e?) = 8 electrons; satisfies the octet rule;

H is stable with 2 electrons; all F atoms satisfy the octet rule.