The increasing order of the bond order of O2, O2-. O2+ and O22-?

By Ritesh|Updated : November 4th, 2022

The increasing order of the bond order of O2, O2-. O2+ and O22- is O22- < O2- < O2 < O2+. The total number of covalently bound electron pairs between two atoms in a molecule determines the bond order of a covalent bond. It can be determined by sketching the molecule's Lewis structure and adding up all the electron pairs that exist between the relevant atoms.

  • The bond order for single bonds is 1.
  • The bond order for double bonds is two.
  • The bond order for triple bonds is 3.

Bond Order

  • Every molecule has a hierarchy of bonds.
  • Each molecule has a unique bond configuration.
  • Half of the difference between the number of electrons in bond-free (nonbonding) and bond-filled (bonded) molecular orbitals is used to compute the bond order.

The formula to calculate the bond order:

BO = NB - NA/2

The quantity of electrons present in the bonding and antibonding molecular orbitals, is NA, NB

Step 1: Bond order calculation for a particular species:

BO for O2 = ½ (10 - 6) = 2

BO for O2- = ½ (10 - 7) = 1.5

BO for O2+ = ½ (10 - 5) = 2.5

BO for O22- = ½ (10 - 8) = 1

Step 2: Let us arrange according to increasing bond length

O22- < O2- < O2 < O2+

Summary:

The increasing order of the bond order of O2, O2-. O2+ and O22-?

O22- < O2- < O2 < O2+ is the increasing order of the bond order of O2, O2-. O2+ and O22- . The bond order is found by the total covalently bound electron pair numbers present in two atoms of a molecule.

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