The Bond Order of C2 is 2, H2 is 1, and N2 is 3. It is calculated by subtracting the number of anti-bonding
anti-bonding
In theoretical chemistry, an antibonding orbital is a type of molecular orbital that weakens the chemical bond between two atoms and helps to raise the energy of the molecule relative to the separated atoms. Such an orbital has one or more nodes in the bonding region between the nuclei.
https://en.wikipedia.org › wiki › Antibonding_molecular_orbital
Higher is the bond order, more stronger is the bond. Hence, higher is the bond energy and lower is the bond length. The bond orders of ethylene C2H4 and acetylene C2H2 are 2 and 3 respectively.
Bond order is the number of bonding pairs of electrons between two atoms. In a covalent bond between two atoms, a single bond has a bond order of one, a double bond has a bond order of two, a triple bond has a bond order of three, and so on.
In molecular orbital theory, bond order is defined as half of the difference between the number of bonding and antibonding electrons. Bond order = [(Number of electrons in bonding molecules) - (Number of electrons in antibonding molecules)]/2. Know that the higher the bond order, the more stable the molecule.
Flexi Says: A C2H2 molecule, also known as acetylene, has 3 covalent bonds. Each carbon atom forms a single covalent bond with a hydrogen atom and a triple covalent bond with the other carbon atom. So, there are a total of 3 covalent bonds in a C2H2 molecule.
So in N2 6 electrons are present in bonding molecular orbitals and no electrons are present in antibonding molecular orbitals so it is 6–0/2 =3 so bond order is…. 3… mean that N2 has triple bond….
where a bonding electron is an electron present in a bonding orbital, and an anti-bonding electron is an electron present in an anti-bonding orbital. Therefore, the bond order of N2 is 1, the bond order of O2 is 2, the bond order of O2+ is 2.5, and the bond order of O2- is 1.5.
The bond order shows the number of chemical bonds present between a pair of atoms. For instance, the bond order of diatomic nitrogen N≡N is 3 and bond order between the carbon atoms in H-H≡C-H is also three. The bond order describes the stability of the bond.
(I) Bond order of CO and N2 are 3 and 3. (II) Bond order of CO and N2 are same. (III) During the formation of N+2 from N2 bond length increases. (IV) During the formation of CO+ from CO, the bond length decreases.
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