Question:
The bond order of peroxide ion is x. The bond order of superoxide ion is:
The bond order of peroxide ion is x. The bond order of superoxide ion is:
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In oxygen species: \(O_2^+ > O_2 > O_2^- > O_2^{2-}\) in bond order trend.
Updated On: Jun 19, 2026
- \(\frac{2}{3}x\)
- \(\frac{3}{2}x\)
- \(2x\)
- \(\frac{5}{2}x\)
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The Correct Option is B
Solution and Explanation
Step 1: Understanding peroxide ion bond order.
Peroxide ion is \(O_2^{2-}\). Its molecular orbital configuration gives a bond order of 1. This is because two extra electrons occupy antibonding orbitals, reducing bond order compared to oxygen molecule. So we take \(x = 1\).
Step 2: Understanding superoxide ion bond order.
Superoxide ion is \(O_2^{-}\). It has one extra electron compared to oxygen molecule. This reduces bond order slightly, giving bond order \(1.5\).
Step 3: Relating peroxide and superoxide bond orders.
We are given peroxide bond order as \(x = 1\). Superoxide bond order is \(1.5\), which is higher than peroxide.
Step 4: Expressing in terms of x.
Since peroxide bond order \(x = 1\), superoxide bond order becomes: \[ \frac{3}{2}x \]
Step 5: Final reasoning.
Thus, the bond order of superoxide ion is 1.5 times that of peroxide ion. This matches molecular orbital theory trends for oxygen species.
Final Answer: \[ \boxed{\frac{3}{2}x} \]
Peroxide ion is \(O_2^{2-}\). Its molecular orbital configuration gives a bond order of 1. This is because two extra electrons occupy antibonding orbitals, reducing bond order compared to oxygen molecule. So we take \(x = 1\).
Step 2: Understanding superoxide ion bond order.
Superoxide ion is \(O_2^{-}\). It has one extra electron compared to oxygen molecule. This reduces bond order slightly, giving bond order \(1.5\).
Step 3: Relating peroxide and superoxide bond orders.
We are given peroxide bond order as \(x = 1\). Superoxide bond order is \(1.5\), which is higher than peroxide.
Step 4: Expressing in terms of x.
Since peroxide bond order \(x = 1\), superoxide bond order becomes: \[ \frac{3}{2}x \]
Step 5: Final reasoning.
Thus, the bond order of superoxide ion is 1.5 times that of peroxide ion. This matches molecular orbital theory trends for oxygen species.
Final Answer: \[ \boxed{\frac{3}{2}x} \]
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