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The bond order in the species O2, O(2)^(...

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)`

Text Solution

AI Generated Solution

The correct Answer is:
To determine the bond order of the species \( O_2 \), \( O_2^+ \), and \( O_2^- \), we will follow these steps: ### Step 1: Determine the number of electrons in each species - **For \( O_2 \)**: Each oxygen atom has 8 electrons, so for two oxygen atoms, the total number of electrons is \( 8 + 8 = 16 \). - **For \( O_2^+ \)**: This species has one less electron than \( O_2 \), so the total number of electrons is \( 16 - 1 = 15 \). - **For \( O_2^- \)**: This species has one extra electron compared to \( O_2 \), so the total number of electrons is \( 16 + 1 = 17 \). ### Step 2: Calculate the bond order for each species The bond order can be estimated based on the total number of electrons: - **For \( O_2 \)** (16 electrons): The bond order is 2. - **For \( O_2^+ \)** (15 electrons): The bond order is 2.5. - **For \( O_2^- \)** (17 electrons): The bond order is 1.5. ### Step 3: Arrange the bond orders in decreasing order Now, we can arrange the bond orders: 1. \( O_2^+ \) (bond order = 2.5) 2. \( O_2 \) (bond order = 2) 3. \( O_2^- \) (bond order = 1.5) ### Final Answer The order of bond order in the species \( O_2 \), \( O_2^+ \), and \( O_2^- \) follows: \[ O_2^+ > O_2 > O_2^- \]
To determine the bond order of the species \( O_2 \), \( O_2^+ \), and \( O_2^- \), we will follow these steps: ### Step 1: Determine the number of electrons in each species - **For \( O_2 \)**: Each oxygen atom has 8 electrons, so for two oxygen atoms, the total number of electrons is \( 8 + 8 = 16 \). - **For \( O_2^+ \)**: This species has one less electron than \( O_2 \), so the total number of electrons is \( 16 - 1 = 15 \). - **For \( O_2^- \)**: This species has one extra electron compared to \( O_2 \), so the total number of electrons is \( 16 + 1 = 17 \). ### Step 2: Calculate the bond order for each species ...
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Knowledge Check

  • The oxidation states of sulphur in the anions SO_(3)^(2-), S_(2)O_(4)^(2-) , and S_(2)O_(6)^(2-) follow the order

    A
    `S_(2)O_(6)^(2-)ltS_(2)O_(4)^(2-)ltSO_(3)^(2-)`
    B
    `S_(2)O_(4)^(2-)ltSO_(3)^(2-)ltS_(2)O_(6)^(2-)`
    C
    `SO_(3)^(2-)ltS_(2)O_(4)^(2-)ltS_(2)O_(6)^(2-)`
    D
    `S_(2)O_(4)^(-)+ltS_(2)O_(6)^(2-)ltSO_(3)^(2-)`

  • The oxidation states of sulphur in the anions SO_(3)^(2-), S_(2)O_(4)^(2-) , and S_(2)O_(6)^(2-) follow the order

    A
    `S_(2)O_(4)^(2-)gtS_(2)O_(6)^(2-)gtSO_(4)^(2-)gtSO_(3)^(2-)`
    B
    `S_(2)O_(6)^(2-)gtSO_(3)^(2-)gtS_(2)O_(4)^(2-)gtSO_(4)^(2-)`
    C
    `SO_(4)^(2-) gt S_(2)O_(6)^(2-)gtSO_(3)^(2-)gtS_(2)O_(4)^(2-)`
    D
    `SO_(3)^(2-) gtSO_(4)^(2-)gtS_(2)O_(4)^(2-)gtS_(2)O_(6)^(2-)`

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