The oxidation unmber of two S stoms in `Na_(2)S_(2)O_(3)` are ………….and …………….

Answer

To determine the oxidation numbers of the two sulfur atoms in the compound \( \text{Na}_2\text{S}_2\text{O}_3 \), we can follow these steps:

### Step 1: Identify the oxidation states of other elements in the compound.
In \( \text{Na}_2\text{S}_2\text{O}_3 \):
- Sodium (Na) has an oxidation state of +1.
- Oxygen (O) typically has an oxidation state of -2.

### Step 2: Set up the equation based on the overall charge of the compound.
The overall charge of the compound is neutral (0). Therefore, we can set up the equation based on the oxidation states:

\[ \text{Total oxidation state} = 2(\text{oxidation state of Na}) + 2(\text{oxidation state of S}) + 3(\text{oxidation state of O}) = 0 \]

Substituting the known values:

\[ 2(+1) + 2x + 3(-2) = 0 \]

Where \( x \) is the oxidation state of sulfur.

### Step 3: Solve the equation.
Now, let's simplify the equation:

\[ 2 + 2x - 6 = 0 \]

This simplifies to:

\[ 2x - 4 = 0 \]

Adding 4 to both sides gives:

\[ 2x = 4 \]

Dividing by 2:

\[ x = 2 \]

### Step 4: Analyze the structure of the compound.
In \( \text{Na}_2\text{S}_2\text{O}_3 \), there are two sulfur atoms, and they can have different oxidation states due to their different bonding environments.

### Step 5: Determine the oxidation states of the individual sulfur atoms.
In \( \text{Na}_2\text{S}_2\text{O}_3 \):
- One sulfur atom is bonded to three oxygen atoms (thiosulfate structure), which typically has a higher oxidation state. This sulfur has an oxidation state of +6.
- The other sulfur atom is bonded to the first sulfur and has a lower oxidation state, which is -2.

### Conclusion:
Thus, the oxidation numbers of the two sulfur atoms in \( \text{Na}_2\text{S}_2\text{O}_3 \) are +6 and -2.

### Final Answer:
The oxidation numbers of the two sulfur atoms in \( \text{Na}_2\text{S}_2\text{O}_3 \) are +6 and -2.

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