The Lewis structure for nitrogen (N₂) can be drawn by following a few simple steps. First, we recognize that nitrogen is a diatomic molecule consisting of two nitrogen atoms bonded together.
1. **Determine the Total Number of Valence Electrons**: Each nitrogen atom has 5 valence electrons, so for N₂, we have a total of 10 valence electrons.
2. **Draw the Skeleton Structure**: Place the two nitrogen atoms next to each other. Connect them with a single bond.
3. **Distribute the Remaining Electrons**: Initially, we have used 2 electrons for the single bond. This leaves us with 8 electrons remaining. To satisfy the octet rule for both nitrogen atoms, we will have to increase the bonding between them. We can convert the single bond into a double bond by sharing more electrons.
4. **Form Double Bond**: To achieve a fulfilling octet, we add another bond between the two nitrogen atoms, which consumes 2 more electrons. Now we have used 4 electrons (2 for each of the two bonds) and have 6 electrons left.
5. **Complete the Octet**: We can then form a triple bond by adding one more bond, which will use 2 additional electrons. Now, all 10 electrons are accounted for, and both nitrogen atoms now have 8 electrons in their valence shell, which satisfies the octet rule.
In summary, the Lewis structure for N₂ is represented as:
N≡N
This shows that nitrogen molecules have a strong triple bond between the two nitrogen atoms, indicating a stable diatomic molecule.