Compare the relative stabilities and magnetic behaviour of the following species
(a) `O_(2)^(Θ)` and `N_(2)^(o+)` (b) `O_(2)^(2-)` and `N_(2)^(Θ)` (c ) `O_(2)^(2-)` and `N_(2)^(2-)` .

Explanation

To compare the relative stabilities and magnetic behavior of the given species, we will follow these steps:

### Step 1: Determine the number of electrons in each species.
- **O₂²⁻**: Oxygen has 8 electrons, so O₂ has 16 electrons. With 2 additional electrons for the 2- charge, O₂²⁻ has 18 electrons.
- **N₂⁺**: Nitrogen has 7 electrons, so N₂ has 14 electrons. With 1 electron removed for the +1 charge, N₂⁺ has 13 electrons.
- **O₂**: 16 electrons (as calculated above).
- **N₂⁻**: 14 electrons + 1 for the -1 charge = 15 electrons.
- **O₂²⁻**: 18 electrons (as calculated above).
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