Draw the Lewis Structure for N₂ and Determine Its Electron and Molecular Geometries

To draw the Lewis structure for N₂ (nitrogen gas), follow these steps:

1. Count the total number of valence electrons: Nitrogen is in Group 15 of the periodic table, so each nitrogen atom has 5 valence electrons. Since there are two nitrogen atoms, the total number of valence electrons is 10.
2. Draw the skeletal structure: Place the two nitrogen atoms next to each other, as they are bonded together.
3. Distribute the electrons: Start by placing a single bond between the two nitrogen atoms. This uses 2 electrons. Now, distribute the remaining 8 electrons as lone pairs around each nitrogen atom. Each nitrogen atom will have 3 lone pairs.
4. Check the octet rule: Each nitrogen atom should have 8 electrons around it (2 from the bond and 6 from the lone pairs). This satisfies the octet rule.

The Lewis structure for N₂ looks like this:

  :N≡N:

Electron Geometry: The electron geometry around each nitrogen atom is linear because there are no lone pairs on the central atom (each nitrogen is considered a central atom in this diatomic molecule).

Molecular Geometry: The molecular geometry of N₂ is also linear. Since there are no lone pairs on the nitrogen atoms, the electron geometry and molecular geometry are the same.

In summary, the Lewis structure for N₂ shows a triple bond between the two nitrogen atoms, with each nitrogen atom having 3 lone pairs. Both the electron and molecular geometries are linear.