The bond order in ${\mathrm{O}}_2^{2-}$ species is

The bond order of O₂^2- species can be determined using the molecular orbital theory. Let us analyze this step-by-step:

Electronic Configuration of O₂^2-

The total number of electrons in O₂^2- is 18. The molecular orbital configuration for O₂^2- is as follows:

    σ(1s)² σ*(1s)² σ(2s)² σ*(2s)² σ(2pz)² (π(2px)² = π(2py)²) 
    (π*(2px)² = π*(2py)²)

Here, the σ orbitals represent bonding molecular orbitals, while σ* and π* orbitals represent anti-bonding molecular orbitals.

Calculation of Bond Order

Bond order is calculated using the formula:

    Bond Order = (Nb - Na) / 2

• N_b: Number of bonding electrons
• N_a: Number of anti-bonding electrons

For O₂^2-:

• Number of bonding electrons (N_b) = 10
• Number of anti-bonding electrons (N_a) = 8

Substituting these values into the formula:

    Bond Order = (10 - 8) / 2 = 1

Interpretation of Bond Order

The bond order of O₂^2- is 1. This indicates that the species has a single bond between the two oxygen atoms. The species is also diamagnetic because all electrons are paired in its molecular orbitals.

Importance of Bond Order in O₂^2-

The bond order of O₂^2- helps in understanding the stability and bonding characteristics of this species. A bond order of 1 signifies that O₂^2- is less stable compared to O₂ or O₂⁺, which have higher bond orders.

The concept of bond order of O₂^2- is crucial in molecular orbital theory as it provides insights into the electronic arrangement and magnetic properties of the molecule.