We have removed two electrons so the molecule becomes the ion f2 2 with a charge of 2. Fluorine molecule is formed by the combination of atomic orbitals of two fluorine atoms each having nine electrons thus making 18 electrons.
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Bond order of f2 2 ion. 0 5 is contributed by each electron to the bond order. Graphical presentation of bond order. R emove electrons from the antibonding homos.
F2 f2 so f2 f2. We must remove electrons from the antibonding homos. Which molecule should be the most stable.
To learn how to determine a bond order at a glance keep reading. The energy level diagram then looks like this. The higher the bond order the more stable the molecule.
Each electron contributes 0 5 to the bond order so we remove one electron each from the π 2px and π 2py orbitals. The graphical representation presented in fig. Of bonding electrons no.
Keeping this in consideration what is the bond order for the f2 molecule. These 18 electrons are filled in various molecular orbitals in the increasing order of their energies aufbau principle and on the basis of hund s rule and pauli s exclusion principle as. So the molecule becomes the ion f 2 2 with a charge of 2.
This can be calculated by subtracting the number of anti bonding electrons in the molecular orbitals from the. Determine the bond order in a molecule or ion with a. Determine the bond order for f 2 f 2 and f 2.
Of antibonding so in order of stability you have. The bond order is 1 2 no. The bond order for fluorine gas is 1.
Divide the result by 2 to get the result. To calculate bond order in chemistry subtract the number of the electrons in the antibonding molecules from the number of electrons in the bonding molecules. Molecular orbital diagram and bond order of fluorine molecule.
Therefore we remove one electron each from the π 2px and π 2py orbitals. 1 shows that bond order gradually increases to 1 in the range 0 2 electrons then falls to zero in the range 2 4 electrons then it further rises to 1 for 4 6 electrons and once again falls to zero for 6 8 electrons then again rises to 3 in the range 8 14 electrons and then finally falls to zero for.