Question

7 choose the best answer using the periodic table. what is the correct lewis structure for nf₃?

Explanation:

Step1: Calculate total valence electrons

N has 5 valence electrons, each F has 7. Total: $5 + (3 \times 7) = 26$

Step2: Assign bonding electrons

N is central, forms 3 single bonds to F (6 electrons used, 20 left).

Step3: Assign lone pairs

Each F gets 3 lone pairs (6 electrons each, $3 \times 6 = 18$ electrons used), N gets 1 lone pair (2 electrons used). Total electrons: $6 + 18 + 2 = 26$, matching the total.

Step4: Verify octet rule

Each F has 8 electrons (2 bonding + 6 lone), N has 8 electrons (6 bonding + 2 lone). No double bonds needed.

Answer:

The second option (structure: :F: single-bonded to N, which is single-bonded to another :F: and :F:, with one lone pair on N and three lone pairs on each F)