Arrange the following species in the decreasing order of their bond dissociation energy :
`N_(2), N_(2)^(+), N_(2)^(-), N_(2)^(2-)`

Explanation

To arrange the species \( N_2, N_2^+, N_2^-, N_2^{2-} \) in decreasing order of their bond dissociation energy, we will analyze their electronic configurations and calculate their bond orders. The bond dissociation energy is directly related to the bond order; higher bond order means stronger bonds and thus higher bond dissociation energy.

### Step 1: Determine the number of electrons in each species
- **For \( N_2 \)**:
- Total electrons = 14 (7 from each nitrogen atom)

- **For \( N_2^+ \)**:
- Total electrons = 13 (one electron removed)
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