Question

The oxidation state of sulphur in \( \text{Na}_2 \text{S}_4 \text{O}_6 \) is

• A. +6
• B. +5
• C. \( \frac{5}{2} \)
• D. -2

Hint:

To find the oxidation state of an element in a compound, use the rule that the sum of oxidation states in a neutral molecule must equal zero.

Answer 1

The Correct Option is B

Step 1: Assign oxidation states.
In \( \text{Na}_2 \text{S}_4 \text{O}_6 \), sodium (Na) has an oxidation state of +1, and oxygen (O) has an oxidation state of -2. Let the oxidation state of sulfur (S) be \( x \).
Step 2: Solve for the oxidation state of sulfur.
The total charge on the molecule is zero, so: \[ 2(+1) + 4x + 6(-2) = 0 \] Solving for \( x \), we get \( x = +5 \). Final Answer: \[ \boxed{+5} \]