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Write which one out of O(2)^(+) and O(2...

Write which one out of `O_(2)^(+) and O_(2)^(2-) ` is more stable on the basis of bond order calculations .

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To determine which ion, \( O_2^+ \) or \( O_2^{2-} \), is more stable based on bond order calculations, we need to follow these steps: ### Step 1: Determine the number of electrons in each ion - For \( O_2^+ \): Oxygen (O) has 8 electrons, so \( O_2 \) has \( 8 + 8 = 16 \) electrons. Since \( O_2^+ \) has lost one electron, it has \( 16 - 1 = 15 \) electrons. - For \( O_2^{2-} \): \( O_2 \) has 16 electrons, and since it has gained two electrons, it has \( 16 + 2 = 18 \) electrons. ### Step 2: Write the electron configuration for each ion - For \( O_2^+ \) (15 electrons): ...
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Which our of O_(2)^(+)and O_(2)^(-) is more stable on the basis of bond order calculations ?

Which out of O_(2)^(+) and O_(2)^(-) is more stable?

Knowledge Check

  • Bond order of O_(2), O_(2)^(-) and O_(2)^(2-) is in order

    A
    `O_(2)^(-) lt O_(2)^(2-) lt O_(2) lt O_(2)^(+)`
    B
    `O_(2)^(2-) lt O_(2)^(-) lt O_2 lt O_(2)^(+)`
    C
    `O_(2)^(+) lt O_(2) lt O_(2)^(-) lt O_(2)^(2-)`
    D
    `O_(2) lt O_(2)^(+) lt O_(2)^(-) lt O_(2)^(2-)`

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