What is the oxidation state of Cl in each ion? a. ClO- b. ClO2- c. ClO3- d. ClO4-
The Correct Answer and Explanation is:
Let’s go through the oxidation states of chlorine in each ion one by one:
a. ClO⁻ (Hypochlorite ion)
In the hypochlorite ion (ClO⁻), oxygen has an oxidation state of -2. Since the ion has an overall charge of -1, the sum of the oxidation states of chlorine and oxygen must equal -1.
- Let the oxidation state of chlorine be x.
- The total charge equation will be:
x + (-2) = -1
x – 2 = -1
x = +1
So, the oxidation state of chlorine in ClO⁻ is +1.
b. ClO₂⁻ (Chlorite ion)
In the chlorite ion (ClO₂⁻), oxygen has an oxidation state of -2. With a charge of -1, the sum of the oxidation states of chlorine and the two oxygens must equal -1.
- Let the oxidation state of chlorine be x.
- The total charge equation will be:
x + 2(-2) = -1
x – 4 = -1
x = +3
So, the oxidation state of chlorine in ClO₂⁻ is +3.
c. ClO₃⁻ (Chlorate ion)
In the chlorate ion (ClO₃⁻), oxygen has an oxidation state of -2. With a charge of -1, the sum of the oxidation states of chlorine and the three oxygens must equal -1.
- Let the oxidation state of chlorine be x.
- The total charge equation will be:
x + 3(-2) = -1
x – 6 = -1
x = +5
So, the oxidation state of chlorine in ClO₃⁻ is +5.
d. ClO₄⁻ (Perchlorate ion)
In the perchlorate ion (ClO₄⁻), oxygen again has an oxidation state of -2. With a charge of -1, the sum of the oxidation states of chlorine and the four oxygens must equal -1.
- Let the oxidation state of chlorine be x.
- The total charge equation will be:
x + 4(-2) = -1
x – 8 = -1
x = +7
So, the oxidation state of chlorine in ClO₄⁻ is +7.
Summary:
- a. ClO⁻: Oxidation state of Cl is +1.
- b. ClO₂⁻: Oxidation state of Cl is +3.
- c. ClO₃⁻: Oxidation state of Cl is +5.
- d. ClO₄⁻: Oxidation state of Cl is +7.
Each of these species has chlorine in different oxidation states based on the number of oxygen atoms it is bonded to, which influences the overall charge distribution.
