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

Explanation

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`.