Select the incorrect order(s) among the following :

C l O^{-} < B r O^{-} < I O^{-}

- disproportionation

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C l O_{4}^{-} < B r O_{4}^{-} < l O_{4}^{-}

- oxidising power

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H C l O < H C l O_{2} < H C l O_{3} < H C l O_{4}

- acid strength

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H O C l > H O I > H O B r

- acid strength

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Solution

The correct options are
B $C l O_{4}^{-} < B r O_{4}^{-} < l O_{4}^{-}$ - oxidising power
D $H O C l > H O I > H O B r$ - acid strength
1) The reduction potential values are as follows:
$C l O_{4}^{-} : 1.19 V$ ,
$B r O_{4}^{-} : 1.65 V$ ,
$B r O_{4}^{-} : 1.74 V$ .
So, the order of oxidising power is: $C l O_{4}^{-} < I O_{4}^{-} < B r O_{4}^{-}$ .
2) The correct order of acidic strength is: $H O C l < H O B r < H O I$ . As the electronegativity of halogens increases, the acidic character also increases.

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Arrange the following compounds according to the increasing order of oxidation state of chlorine.

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