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Oxidation number of Xe in XeF(5)^(-) is ...

Oxidation number of Xe in `XeF_(5)^(-)` is :

A

`+1`

B

`+2`

C

`+3`

D

`+4`

Text Solution

AI Generated Solution

The correct Answer is:
To find the oxidation number of xenon (Xe) in the ion \( \text{XeF}_5^{-} \), we can follow these steps: ### Step-by-Step Solution: 1. **Identify the oxidation states of the elements involved**: - Fluorine (F) typically has an oxidation state of -1. 2. **Set up the equation based on the overall charge of the ion**: - The ion \( \text{XeF}_5^{-} \) has a total charge of -1. - Let the oxidation state of xenon (Xe) be \( x \). 3. **Write the equation for the total charge**: - The contribution to the charge from the five fluorine atoms is \( 5 \times (-1) = -5 \). - Therefore, the equation can be set up as: \[ x + 5(-1) = -1 \] 4. **Simplify the equation**: - This simplifies to: \[ x - 5 = -1 \] 5. **Solve for \( x \)**: - Adding 5 to both sides gives: \[ x = -1 + 5 \] - Thus, \[ x = 4 \] 6. **Conclusion**: - The oxidation number of xenon in \( \text{XeF}_5^{-} \) is +4. ### Final Answer: The oxidation number of Xe in \( \text{XeF}_5^{-} \) is +4. ---
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Knowledge Check

  • The oxidation state of Xe in XeF_(6) is

    A
    0
    B
    `+ 2`
    C
    `+ 6`
    D
    `- 6`.
  • A compound of Xe and F is found to have 53.5% Xe. What is the oxidation number of Xe in this comound?

    A
    `-4`
    B
    0
    C
    `+4`
    D
    `+6`
  • A compound of Xe and F is found to have 53.3% Xe (atomic weight=133). Oxidation number of Xe in this compound is

    A
    `+2`
    B
    0
    C
    `+4`
    D
    `+6`
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