Oxidation And Reduction Reactions

The correct option is ( is reducing while is oxidising): .

Let's calculate the oxidation states of the underlined elements in each compound: 1. K O :
- The oxidation state of oxygen in peroxides is always -1. - To balance the charges, the oxidation state of potassium (K) in K O is +1.
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Thus, the oxidation states of the elements are K = +1 and O = -1. The underlined element here is K, and its oxidation state is +1.
2. H O : - The oxidation state of hydrogen (H) is +1.
- The oxidation state of oxygen (O) in peroxides is -1.
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Thus, the oxidation states of the elements in H O are H = +1 and O = -1. The underlined element is oxygen, and its oxidation state is -2 (as per typical peroxide rule).
3. H SO :
- The oxidation state of hydrogen (H) is +1.
- The oxidation state of oxygen (O) is -2.
- In H SO , sulfur (S) has an oxidation state of +6, as the sum of oxidation states of hydrogen (2 × +1) and oxygen (4 × -2) must balance the compound.
Therefore, S = +6.

Thus, the correct oxidation states for the underlined elements in these compounds are: - K = +1, O = -1, and S = +6. The correct answer is (1) +2, -2, and +6.