How to draw the Lewis structure for N2+

The correct answer and explanation is :

Drawing the Lewis Structure for N₂⁺ (Nitrogen Dication)

To draw the Lewis structure for the nitrogen molecule ion, N₂⁺, follow these steps:

1. Determine the total number of valence electrons:

Nitrogen (N) has 5 valence electrons.
N₂ (molecular nitrogen) would have 10 valence electrons (5 from each nitrogen).
Since the molecule has a positive charge (N₂⁺), one electron is removed, leaving it with 9 valence electrons.

2. Choose a skeletal structure:

For N₂⁺, since it’s a diatomic molecule, place the two nitrogen atoms next to each other, sharing electrons.

3. Distribute the electrons:

Start by forming a bond between the two nitrogen atoms. Each single bond represents 2 electrons.
After forming the single bond, you’ll have used 2 electrons, leaving 7 electrons to distribute.
These remaining electrons will be placed as lone pairs on the nitrogen atoms.

4. Make sure all atoms follow the octet rule:

Each nitrogen atom needs 8 electrons to satisfy the octet rule. Since one electron is removed (due to the positive charge), the structure is slightly incomplete. To complete the octet:
A triple bond between the two nitrogen atoms will be formed, utilizing 6 electrons (3 pairs). This leaves one electron.
The remaining electron is placed as a lone pair on one of the nitrogen atoms.

5. Review the structure:

Both nitrogen atoms share 6 electrons (from the triple bond) and have a lone electron left, but the positive charge makes the molecule have one fewer electron overall.
Each nitrogen atom will have one lone electron, and there will be a formal positive charge on the molecule as a whole.

6. Final Lewis Structure:

The N₂⁺ structure can be represented as:

   :N≡N:⁺

Here, the triple bond between the two nitrogen atoms is represented by the triple equals sign (≡), and the lone electron (a single dot) is shown next to one of the nitrogen atoms. The positive charge is indicated above the molecule.

Explanation:

The N₂⁺ ion is a nitrogen molecule that has lost one electron, resulting in 9 valence electrons instead of the 10 found in the neutral N₂ molecule. The Lewis structure emphasizes the following points:

Bonding: The two nitrogen atoms are held together by a triple bond, formed by three shared pairs of electrons. This satisfies the need for each nitrogen atom to reach an octet of electrons, except for one electron that is left as a lone pair on one nitrogen.
Charge: The positive charge on N₂⁺ indicates that there is one fewer electron than in the neutral N₂ molecule. This causes the structure to be slightly electron-deficient, with a formal charge on the entire molecule.
Electron Distribution: The triple bond is the most stable arrangement for N₂⁺, as it maximizes the number of electrons shared between the nitrogen atoms. The single remaining electron is placed as a lone pair on one of the nitrogen atoms, resulting in a molecule that has a formal charge on the entire ion.

Thus, the Lewis structure for N₂⁺ is a diatomic molecule with a triple bond between the two nitrogen atoms, and a lone electron on one nitrogen, while the ion carries a formal positive charge.