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Sagot :
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:
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