The correct order of bond orders of `C_2^(2-), N_2^(2-)` and `O_2^(2-)` is, respectively

Options

A. `C_2^(2-) lt N_2^(2-) lt O_2^(2-)`
B. `O_2^(2-) lt N_2^(2-) lt C_2^(2-)`
C. `C_2^(2-) lt O _2^(2-) lt N_2^(2-)`
D. `N_2^(2-) lt C_2^(2-) lt O_2^(2-)`

Explanation

To determine the correct order of bond orders for the species \( C_2^{2-} \), \( N_2^{2-} \), and \( O_2^{2-} \), we will first calculate the bond order for each molecule using the molecular orbital theory.

### Step 1: Determine the number of electrons in each species

1. **For \( C_2^{2-} \)**:
- Carbon (C) has 6 electrons. Therefore, \( C_2 \) has \( 2 \times 6 = 12 \) electrons.
- The \( 2- \) charge means there are 2 additional electrons, giving us \( 12 + 2 = 14 \) electrons.

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