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Based on molecular orbital theory, as the bond order of a molecule decreases, its stability also reduces. The bond order is calculated using the formula: Bond order = 1/2 (Nb - Na). For the following species: O2+, O2, O2-, and O2^2-, the bond orders are as follows: O2+ = 1/2 (10 - 5) = 2.5, O2 = 1/2 (10 - 6) = 2, O2- = 1/2 (10 - 7) = 1.5, and O2^2- = 1/2 (10 - 8) = 1.0. Arrange these species in the correct order of stability.

1. O2+ > O2 > O2- > O2^2-
2. O2^2- > O2- > O2 > O2+
3. O2 > O2+ > O2- > O2^2-
4. O2- > O2^2- > O2+ > O2

Correct answer: O2+ > O2 > O2- > O2^2-

Solution

The bond order directly correlates with molecular stability. Higher bond order indicates greater stability. Based on the calculated bond orders, the stability order is O2+ > O2 > O2- > O2^2-.

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