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Using molelcular orbital theory, compare...

Using molelcular orbital theory, compare the bond energy and magnetic character of `O_(2)^(+)` and `O_(2)^(-)` species.

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AI Generated Solution

To compare the bond energy and magnetic character of the \( O_2^+ \) and \( O_2^- \) species using molecular orbital theory (MOT), we will follow these steps: ### Step 1: Determine the Number of Electrons - The molecular oxygen \( O_2 \) has 16 electrons (8 from each oxygen atom). - For \( O_2^+ \), we remove one electron, resulting in 15 electrons. - For \( O_2^- \), we add one electron, resulting in 17 electrons. ### Step 2: Write the Molecular Orbital Configuration ...
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Knowledge Check

  • The bond order in the species O_2, O_(2)^(+) and O_(2)^(-) follows the order

    A
    `O_(2) gt O_(2)^(+) gt O_(2)^(-)`
    B
    `O_(2)^(+) gt O_(2) gt O_(2)^(-)`
    C
    `O_(2) ^(-) gt O_(2) gt O_(2)^(+)`
    D
    `O_(2)^(+) gt O_(2) ^(-) gt O_(2)`

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