Answer :

Answer:

The question seems to have a typo with multiple options listed under the same letter. However, let’s focus on determining the oxidation state of sulfur (S) in \(\text{S}_2\text{O}_8^{2-}\).

The compound \(\text{S}_2\text{O}_8^{2-}\) is known as peroxydisulfate. In this compound:

- Oxygen generally has an oxidation state of -2.

- Let the oxidation state of sulfur be \(x\).

The molecular formula can be analyzed as follows:

\[ 2x + 8(-2) = -2 \]

This simplifies to:

\[ 2x - 16 = -2 \]

\[ 2x = 14 \]

\[ x = +7 \]

So, the oxidation state of each sulfur atom in \(\text{S}_2\text{O}_8^{2-}\) is +7.

**Correct answer:** **b) +7**

Explanation: