To determine the oxidation state of chlorine (Cl) in [tex]$HClO_3$[/tex], we need to apply the rules for assigning oxidation states and consider the known oxidation states of hydrogen (H) and oxygen (O).
1. Assign Oxidation States:
- Hydrogen (H) generally has an oxidation state of +1.
- Oxygen (O) generally has an oxidation state of -2.
2. Set Up the Equation:
The sum of the oxidation states of all atoms in a neutral compound must equal zero. In this case, the chemical formula is [tex]$HClO_3$[/tex]. We'll assign:
- The oxidation state of H as +1.
- The oxidation state of each O as -2.
- The oxidation state of Cl as x (which we need to find).
So, the equation based on the oxidation states will be:
[tex]\[ (+1) + (x) + 3(-2) = 0 \][/tex]
3. Simplify the Equation:
Substitute the known values and solve for x:
[tex]\[ 1 + x + 3(-2) = 0 \][/tex]
[tex]\[ 1 + x - 6 = 0 \][/tex]
[tex]\[ x - 5 = 0 \][/tex]
[tex]\[ x = 5 \][/tex]
Therefore, the oxidation state of Cl in [tex]$HClO_3$[/tex] is [tex]\( \boxed{+5} \)[/tex].
