Which is an acceptable Lewis structure for a diatomic nitrogen molecule?

Question

A.
Two N atoms connected with triple bonds in between them have two electrons above and two electrons below them
B.
Triple bonds connect two N atoms in a molecule. The N atom on the left side has an electron on its left and the N atom on the right has an electron on its right.
C.
Triple bonds connect two N atoms in a molecule. The N atom on the left side has an electron on its left and the N atom on the right has an electron on its right.
D.
Molecule structure of two N atoms connected with triple bonds in between them.
E.
Two N atoms are connected with triple bonds. The N atom on the left has two electrons on the left side, one above and one below, while the N atom on the right side has two electrons on the right side and one above and one below

Answer 1

The correct answer for an acceptable Lewis structure for a diatomic nitrogen molecule (N₂) is:

A. Two N atoms connected with triple bonds in between them have two electrons above and two electrons below them.

Here's the rationale:

1. A nitrogen molecule (N₂) consists of two nitrogen atoms.
2. Each nitrogen atom has five valence electrons, and to achieve a full octet (eight electrons), they form a triple bond, sharing three pairs of electrons.
3. In a Lewis structure, representing the shared electrons (in the triple bond) as lines (three lines for a triple bond) is common, and it’s also correct to indicate the lone pairs on each nitrogen atom.

Option A accurately describes the bonding and electron configuration in terms of lines for the triple bond and additional electrons in lone pairs.