Nitrogen (N2) Molecule Lewis Structure
Nitrogen is a diatomic molecule and contains only two nitrogen atoms. Lewis structure of N2 molecule contains a triple bond and each nitrogen atom has one lone pair. There are many things to learn when we draw N2 lewis structure.
N2 lewis structure
There is a triple bond between nitrogen atoms and one lone pair exist on each nitrogen atom. There are several interesting steps in drawing nitrogen's lewis structure.
Steps of drawing lewis structure of N2 molecule
When we draw a lewis structure, guidelines are given. Number of steps in the guidelines can be changed according the complexity of the molecule or ion. Because N2 is a simple molecule, it is extremely easy to draw the lewis structure of it. However those all steps are mentioned and explained in detail in this tutorial for your knowledge.
- Find total number of electrons of the valance shells of nitrogen atoms
- Determine total electrons pairs existing as lone pairs and bonds
- Find center atom selection
- Mark lone pairs on atoms
- Mark charges on atoms if there are charges.
- Check the stability and minimize charges on atoms by converting lone pairs to bonds to obtain best lewis structure.
Total number of electrons of the valance shells of N2 molecule
There is only one element in the nitrogen molecule. Nitrogen is a group VA element in the periodic table and contains five electrons in its last shell. Now, we know how many electrons are there in valence shells of nitrogen atoms.
- valence electrons given by nitrogen atoms = 5 * 2 = 10
- Total valence electrons = 10
Total valence electrons pairs
Total valance electrons pairs = σ bonds + π bonds + lone pairs at valence shells
Total electron pairs are determined by dividing the number total valence electrons by two. For, N2 molecule, Total pairs of electrons are five in their valence shells.
Center atom of N2 molecule
Because, there are only two atoms and both atoms belongs to same element, do not need to worry about center atom selection.
Lone pairs on atoms
After determining the center atom and sketch of N2 molecule, we can start to mark lone pairs on atoms. Remember that, there are total of five electron pairs.
- There is already one bond in the drawn sketch. So, there are four remaining lone pairs to mark on nitrogen atoms.
- Because, there is no center atom, we can mark remaining lone pairs on both nitrogen atoms. One nitrogen atom will take three lone pairs and remaining one takes one lone pair.
- Now, all valence electrons pairs are marked in both nitrogen atoms.
Mark charges on atoms
There are charges on both nitrogen atoms. One nitrogen atom has +2 charge and other nitrogen atom has -2 charge.
Check the stability and minimize charges on atoms by converting lone pairs to bonds
Because, there are charges on both nitrogen atoms and those charges are large, above structure is not stable. Therefore, we need to reduce charges as below by converting lone pairs to bonds.
In the last structure, you see there are no charges on nitrogen atoms and valence shell has eight electrons to fulfill the octal in both nitrogen atoms.
Questions
how many lone pairs does nitrogen have?
In the lewis structure of nitrogen molecule, each nitrogen atom in N2 molecule has one lone pair in their valence shell (outer shell).
Are there a double bond in lewis structure of N2?
There is a triple bond in lewis structure of N2 molecule.
