Write the molecular orbital configuration of the following species :
` (a) O_2 " " (b)O_(2)^(-) " " (c ) O_(2)^(+) " "(d) O_(2)^(2+)`
(i) Calculate their bond order.
(ii) Predict their magnetic behaviour.
(iii) Which of these does show highest paramagnetism?

Explanation

To solve the problem, we will determine the molecular orbital configurations for each of the species \( O_2 \), \( O_2^- \), \( O_2^+ \), and \( O_2^{2+} \). We will then calculate their bond orders, predict their magnetic behavior, and identify which species exhibits the highest paramagnetism.

### Step-by-Step Solution:

**(a) For \( O_2 \):**
1. **Determine the total number of electrons:**
- Oxygen has 8 electrons, so \( O_2 \) has \( 8 + 8 = 16 \) electrons.

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