There is S-S bond in

Options

A. `H_(2)S_(2)O_(3)`
B. `H_(2)S_(2)O_(6)`
C. `H_(2)S`
D. `S_(3)O_(9)`

Answer

To determine whether there is an S-S bond in the compounds H2S2O3, H2S2O6, H2S, and S3O9, we need to analyze the oxidation states of sulfur in each compound. Here’s a step-by-step solution:

### Step 1: Analyze H2S2O3
1. **Write the equation for oxidation state calculation:**
\[ 2(1) + 2(S) + 3(-2) = 0 \]
Simplifying this gives:
\[ 2 + 2S - 6 = 0 \implies 2S - 4 = 0 \implies S = +3 \]

2. **Determine the presence of S-S bond:**
- Since the oxidation state of sulfur (+3) is less than the maximum oxidation state of +6, there is an S-S bond in H2S2O3.

### Step 2: Analyze H2S2O6
1. **Write the equation for oxidation state calculation:**
\[ 2(1) + 2(S) + 6(-2) = 0 \]
Simplifying this gives:
\[ 2 + 2S - 12 = 0 \implies 2S - 10 = 0 \implies S = +5 \]

2. **Determine the presence of S-S bond:**
- Since the oxidation state of sulfur (+5) is also less than +6, there is an S-S bond in H2S2O6.

### Step 3: Analyze H2S
1. **Identify the structure:**
- H2S has only one sulfur atom, so there cannot be an S-S bond.

### Step 4: Analyze S3O9
1. **Write the equation for oxidation state calculation:**
\[ 3(S) + 9(-2) = 0 \]
Simplifying this gives:
\[ 3S - 18 = 0 \implies 3S = 18 \implies S = +6 \]

2. **Determine the presence of S-S bond:**
- Since the oxidation state of sulfur is +6, it indicates the presence of S=O bonds rather than S-S bonds.

### Conclusion
- The compounds with S-S bonds are **H2S2O3** and **H2S2O6**.
- **H2S** does not have an S-S bond, and **S3O9** also does not have an S-S bond.

### Final Answer
There is an S-S bond in **H2S2O3** and **H2S2O6**.

---