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# Find out the bond order in ${{N}_{2}}$ molecule and also draw the energy level diagram.

Last updated date: 16th Jun 2024
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Hint: Bond order is introduced by Linus Pauling, . The bond number itself is that the number of electron pairs (bonds) between a pair of atoms. Bond number gives a sign of the steadiness of a bond. Isoelectronic species have the same bond number.

Complete step by step Solution:
If there are greater than two atoms within the molecule, follow these steps to see the bond order: Draw the Lewis structure. Count the entire number of bonds. Count the amount of bond groups between individual atoms. Divide the amount of bonds between atoms by the overall number of bond groups within the molecule. Bond order is defined as half the difference between the amount of electrons in bonding molecular orbital (${{N}_{b}}$) and therefore the number of electrons within the antibonding molecular orbitals (${{N}_{a}}$). The bond order describes the steadiness of the bond. The molecular orbital provides a simple understanding of the concept of the bond order of an attraction. It gives us an estimated quantity of the degree of covalent bonds between the atoms. i.e., Bond order =$\dfrac{1}{2}({{N}_{b}}-{{N}_{a}})$
Here ${{N}_{b}}$ is the no of bonding electrons and ${{N}_{a}}$ is the no of antibonding electrons. Number of bonds during a molecule is additionally referred to as bond order.
Energy diagram of ${{N}_{2}}$ is:

Bond order of ${{N}_{2}}=\dfrac{1}{2}(10-4)=\dfrac{1}{2}\times 6=3$, so it has 3 bonds.

Note: If there are unpaired electrons present in the orbitals then it is paramagnetic otherwise diamagnetic. The length of the bond is decided by the quantity of bonded electrons (the bond order). the upper the bond order, the stronger the pull between the 2 atoms and also the shorter the bond length. Generally, the covalent radii of the two atoms gives us the approximate length between the bonds.