What is the oxidation number of S in `S_(8)`.

Answer

To find the oxidation number of sulfur (S) in the molecular form \( S_8 \), we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Molecule**: We are looking at the molecule \( S_8 \), which is a cyclic molecule consisting of eight sulfur atoms.

2. **Understand the Nature of the Molecule**: \( S_8 \) is a neutral molecule, meaning it does not carry any overall charge.

3. **Assign Oxidation Numbers**: In a neutral molecule, the sum of the oxidation numbers of all atoms must equal zero.

4. **Determine the Oxidation Number of Sulfur**: Since all sulfur atoms in \( S_8 \) are identical and contribute equally to the overall charge, we can denote the oxidation number of sulfur as \( x \).

5. **Set Up the Equation**: For \( S_8 \), we have:
\[ 8x = 0 \]
This equation arises because there are eight sulfur atoms, and their total oxidation number must equal the overall charge of the molecule, which is zero.

6. **Solve for \( x \)**:
\[ x = \frac{0}{8} = 0 \]

7. **Conclusion**: Therefore, the oxidation number of sulfur in \( S_8 \) is 0.

### Final Answer:
The oxidation number of sulfur (S) in \( S_8 \) is 0.