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Decreasing order of stability of O(2), O...

Decreasing order of stability of `O_(2), O_(2)^(-), O_(2)^(+)` and `O_(2)^(2-)` is

A

`O_(2)^(+) gt O_(2) gt O_(2)^(-) gt O_(2)^(2-)`

B

`O_(2)^(2-) gt O_(2)^(-) gt O_(2) gt O_(2)^(-)`

C

`O_(2) gt O_(2)^(+) gt O_(2)^(2-) gt O_(2)^(-)`

D

`O_(2)^(-) gt O_(2)^(2-) gt O_(2)^(+) gt O_(2)`

Text Solution

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The correct Answer is:
To determine the decreasing order of stability of the species \( O_2, O_2^-, O_2^+, \) and \( O_2^{2-} \), we will use the concept of Molecular Orbital Theory (MOT) to calculate the bond order for each species. The bond order is directly related to the stability of the molecule: a higher bond order indicates greater stability. ### Step-by-Step Solution: 1. **Count the Total Electrons**: - The molecular oxygen \( O_2 \) has 16 electrons (8 from each oxygen atom). - For \( O_2^- \) (one extra electron), the total is 17 electrons. - For \( O_2^+ \) (one less electron), the total is 15 electrons. - For \( O_2^{2-} \) (two extra electrons), the total is 18 electrons. 2. **Calculate Bond Order**: - The bond order can be calculated using the formula: \[ \text{Bond Order} = \frac{(\text{Number of bonding electrons} - \text{Number of antibonding electrons})}{2} \] - However, for simplicity, we can use the following trick based on the total number of electrons: - 16 electrons: Bond order = 2 - 17 electrons: Bond order = 1.5 - 15 electrons: Bond order = 2.5 - 18 electrons: Bond order = 1 3. **Assign Bond Orders**: - For \( O_2 \) (16 electrons): Bond order = 2 - For \( O_2^- \) (17 electrons): Bond order = 1.5 - For \( O_2^+ \) (15 electrons): Bond order = 2.5 - For \( O_2^{2-} \) (18 electrons): Bond order = 1 4. **Determine the Order of Stability**: - Now, we can arrange the species based on their bond orders: - \( O_2^+ \) (Bond order = 2.5) → Most stable - \( O_2 \) (Bond order = 2) - \( O_2^- \) (Bond order = 1.5) - \( O_2^{2-} \) (Bond order = 1) → Least stable 5. **Final Answer**: - The decreasing order of stability is: \[ O_2^+ > O_2 > O_2^- > O_2^{2-} \]
To determine the decreasing order of stability of the species \( O_2, O_2^-, O_2^+, \) and \( O_2^{2-} \), we will use the concept of Molecular Orbital Theory (MOT) to calculate the bond order for each species. The bond order is directly related to the stability of the molecule: a higher bond order indicates greater stability. ### Step-by-Step Solution: 1. **Count the Total Electrons**: - The molecular oxygen \( O_2 \) has 16 electrons (8 from each oxygen atom). - For \( O_2^- \) (one extra electron), the total is 17 electrons. - For \( O_2^+ \) (one less electron), the total is 15 electrons. ...
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