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# The bond order of a molecule is given by:A. the difference between the number of electrons in bonding and antibonding orbitalsB. total number of electrons in bonding and antibonding orbitalsC. twice the difference between the number of electrons in bonding and antibonding orbitalsD. half the difference number of electrons in bonding and antibonding orbitals

Last updated date: 20th 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.

-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 (Nb) 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 approximate 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.