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What is the oxidation state of Cs in a...

What is the oxidation state of Cs in
a. `Cs_(2)O_(2)` , b. `Cs_(2)O` , c. `CsO_(2)`

Text Solution

Verified by Experts

a. Let the oxidation state of Cs in `Cs_(2)O_(2)` is x. Since `Cs_(2)O_(2)` contains a peroxide linkage `(O_(2)^(2-))`, the oxidation state of peroxide ion is `(-1xx2= -2)`, therefore `2x - 2 = 0`
`implies x= +1`
Thus the oxidation state of Cs in `Cs_(2)O_(2)` is +I.
b. Let the oxidation state of Cs in `Cs_(2)O` is 'x'. Since `Cs_(2)O` contains `O^(2-)` ion, the oxidation state of oxide ion is `-2`.
`:. 2x -2=0 implies x = +1`
Thus, the oxidation state of Cs in `Cs_(2)O` is `+1` .
c. Let the oxidation state of Cs in `CsO_(2)` is 'x' . Since `CsO_(2)` contains superoxide ion `(O_(2)^(Θ))` is `-1`. Therefore.
`x-1=0`
`x= +1`
Thus, oxidation state of Cs in `CsO_(2)` is `+1`.
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Knowledge Check

  • The hybrid state of C in CS_2 should be

    A
    `sp^2`
    B
    sp
    C
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    D
    no specific

  • Chlorination of CS_(2) gives

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    B
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    C
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    D
    `COCl_(2)`

  • Chlorination of CS_(2) gives,

    A
    carbon tetrachloride
    B
    chloroform
    C
    both of these
    D
    none of these

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