Structure, Molecular Geometry, and Hybridization of N2 Lewis

By demonstrating the bonding effect between atoms and molecules, chemistry plays a vital role in the scientific world.

The atom is the most essential component of a chemical element, from which protons, electrons, and neutrons are derived. They all contribute significantly to the creation of chemical bonding.

Numerous scientists have made remarkable contributions to various subfields of chemistry. In 1916, Gilbert N. Lewis, an American chemist, invented the concept of electron dot structure.

Atom and molecule are terms that describe the location of valence shell electrons in a chemical connection. The concept is also frequently known as Lewis structures or Lewis dot structures.

Lewis Dot Architecture

Using the chemical symbol, the Lewis structure identifies the atom and its position in the model of the molecule. In addition, it describes the chemical bonds between atoms inside the molecule.

The structure mostly reflects the arrangement of an element’s valence shell electrons. A valence electron is an electron that is located in the outermost shell of an atom.

To find the number of valence electrons, just record the element’s Group number from the Periodic Table.

Lewis depicted a covalent link between two electrons using lines, while each electron is represented by a dot in the diagram.

Drawing Rules for Lewis Structure

First, consult the Periodic Table for the atomic number of each atom.

Determine the total amount of valence electrons present in a molecule’s atoms.

Observe the octet rule, which states that ions and atoms must have eight electrons in their outer valence shell. (There is an exception to the duplet rule for hydrogen, which requires only two electrons for stability.)

While representing the bonds, it is important to be aware of lone and bound pairs.

Select the core atom by choosing the atom with the lowest electronegative charge.

Place the remaining electrons on the atoms’ terminals.

The most significant aspect of the Lewis dot structure is that only valence electrons participate in chemical bonding.

Instructions for Drawing the Lewis structure of N2

Below is the electron dot structure of a molecule of Nitrogen:

In the Periodic Table, Nitrogen is located in Group 5 throughout Period 2 in Periodic Period 2. According to the element’s electrical configuration, it has five electrons in its outermost valence shell.

According to the molecule N2, there are two atoms of Nitrogen. 5 * 2 = 10e is the total number of electrons present in the valence shell.

In order to display the chemical bonding between two atoms of the Nitrogen molecule, ten valence electrons must be positioned in the structure.

Now, place valence electrons around the N2 atoms.

Since there are two atoms of Nitrogen, allocate the valence electrons to each atom using dots, such as five dots surrounding each atom. The atom is represented by the symbol N.

There will be no central atom in the structure because both atoms have the same electronegativity.

Consider bonding and non-bonding electron pairs that directly affect the Lewis structure’s shape.

Create the covalent link by placing the two Nitrogen atoms close to one another and drawing a line to indicate the bond. Every bond contains two valence electrons. This bond is referred to as a solitary bond.

Display the remaining three electrons on the outside face of each atom.

To adhere to the octet rule (eight electrons per atom), each Nitrogen atom need three additional electrons, or six electrons, to form the proper structure.

After a single link is formed between the atoms, each atom has six electrons. According to the octet rule, each atom still requires two additional electrons to complete its outermost shell.

Currently, each atom contains seven electrons.

A triple covalent bond is characterised by the sharing of three pairs of electrons, which results in the distribution of six electrons.

Combination of Nitrogen (N2)

In chemistry, sigma () and pi () bonds are the most common forms of covalent bonds. Both bonds assist determine the type of hybridization by producing head-to-head overlap or by overlapping 2p orbitals.

Sigma bond is the initial link formed between atoms.

Due to the presence of a second or third bond, a pi bond is formed.

The valence-shell electron configuration of the nitrogen atom is 2s2 2px1 2py1 2pz1, indicating that 1s and 1p orbitals are hybridising to form a new set of two sp-orbitals.

The arrangement leads to N2 producing sp hybridization.

To create a bond, sp hybridization involves the overlap of sp-orbitals on both nitrogen atoms.

On the opposite side, the two p-orbitals carrying one electron each on both atoms create a connection. The next head-to-head overlap of p-orbitals containing one electron each produces an additional bond.

A single bond, double bond, and triple bond correspond to a bond, a bond plus a bond, and a bond plus two bonds, respectively, as deduced from the preceding discussion of overlapping.

The Molecular Structure of Nitrogen (N2)

To comprehend the molecular geometry of any molecule, it is crucial to grasp its Lewis structure and hybridization. N2 forms a triple covalent bond and sp hybridization, as mentioned previously.

As stated previously, the Lewis structure simply indicates which atoms contain lone pairs, whereas valence-shell, electron-pair repulsion (VESPER) predicts the form of a large number of molecules.

The VSEPR model is primarily concerned with the electron pairs surrounding the core atoms. It also accounts for the steric number, which is the number of electron-dense areas surrounding the atom.

Since each atom has steric number 2 by counting one triple bond and one lone pair, the geometry of diatomic N2 is linear and the bond angle is 180 degrees.

As a linear diatomic molecule, both atoms exert an equal amount of effect on the shared bound electrons, making this molecule nonpolar.

For additional information, please consult the polarity of N2.

N2 Molecular Orbital Diagram

There are molecular orbitals in molecules, where each molecule has its own electron configuration in terms of sigma and pi bonds.

According to molecular orbital theory, it describes a molecule’s magnetic properties, stability order, and number of bonds.

When two orbitals are joined, the result is a stable bonding molecular orbital, however when orbitals are subtracted, the result is an unstable anti-molecular bonding orbital (*), which has greater energy.

N2’s configuration, according to the energy level diagram, is 1S2, *1S2, 2S2, *2S, 2Px2, 2Py2, 2Pz1.

N2 MO diagram


In the Lewis structure of the N2 molecule, three lines reflect the development of a triple covalent bond between two atoms of Nitrogen. The two remaining 2p orbitals form two bonds, whereas electrons forming a pair between nitrogen atoms form a sigma bond.

The VSEPR model proposes that molecule geometry decreases valence electron repulsion. In this structure, the energy levels increase from lowest to highest order. Bond order= (Nb-Na)/2 is the formula for calculating.

Read more: Polar or nonpolar, BrF5?

Misha Khatri
Misha Khatri is an emeritus professor in the University of Notre Dame's Department of Chemistry and Biochemistry. He graduated from Northern Illinois University with a BSc in Chemistry and Mathematics and a PhD in Physical Analytical Chemistry from the University of Utah.


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