To determine the oxidation number of chlorine (Cl) in the compound [tex]\( \text{ClO}_2 \)[/tex], we can follow a systematic approach based on the rules for assigning oxidation numbers.
1. Identify the known oxidation numbers:
- The oxidation number of oxygen (O) is typically -2.
2. Calculate the total oxidation number contributed by oxygen:
- In [tex]\( \text{ClO}_2 \)[/tex], there are 2 oxygen atoms.
- Each oxygen atom has an oxidation number of -2.
- Therefore, the total oxidation number from all oxygen atoms is: [tex]\( 2 \times (-2) = -4 \)[/tex].
3. Set up an equation for the sum of oxidation numbers in the compound:
- The sum of the oxidation numbers in a neutral compound is 0.
- Let the oxidation number of chlorine be [tex]\( x \)[/tex].
- The equation is: [tex]\( x + (-4) = 0 \)[/tex].
4. Solve for [tex]\( x \)[/tex]:
- [tex]\( x - 4 = 0 \)[/tex].
- Adding 4 to both sides results in: [tex]\( x = 4 \)[/tex].
Therefore, the oxidation number of Cl in [tex]\( \text{ClO}_2 \)[/tex] is 4.
