Which of the following best represents the correct Lewis dot structure for a neutral N_2 molecule?

• A. :N≡N:
• B. N–N
• C. :N=N:
• D. :N–N:

Answer: (A)

Verified step by step guidance

1. Step 1: Determine the total number of valence electrons for the N₂ molecule. Each nitrogen atom has 5 valence electrons, so for N₂, total valence electrons = 5 × 2 = 10.
2. Step 2: Connect the two nitrogen atoms with a single bond initially, which uses 2 electrons. Subtract these from the total valence electrons to find the remaining electrons to distribute.
3. Step 3: Distribute the remaining electrons to satisfy the octet rule for each nitrogen atom. Remember that nitrogen atoms tend to form multiple bonds to complete their octet.
4. Step 4: Adjust the bonding by increasing the number of bonds between the nitrogen atoms (single, double, or triple) and redistribute electrons as lone pairs to ensure each nitrogen has 8 electrons total.
5. Step 5: Identify the structure where both nitrogen atoms have a complete octet and the total number of electrons used equals 10. The correct Lewis structure for N₂ is the one with a triple bond between the two nitrogen atoms and one lone pair on each nitrogen, represented as :N≡N:.