Answer: The oxidation state of chlorine (Cl) in ClO– is +1.
Step-by-step explanation:
To determine the oxidation state of iodine (I) in IO3– and chlorine (Cl) in ClO–, we can use the oxidation state rules.
For IO3– (iodate ion):
The sum of the oxidation states for all atoms in a polyatomic ion equals the charge of the ion. In this case, the charge is -1.
Oxygen typically has an oxidation state of -2.
There are three oxygen atoms in the iodate ion.
Let x be the oxidation state of iodine (I). Then, we can write the equation:
x + 3(-2) = -1
x - 6 = -1
x = +5
The oxidation state of iodine (I) in IO3– is +5.
For ClO– (hypochlorite ion):
The sum of the oxidation states for all atoms in a polyatomic ion equals the charge of the ion. In this case, the charge is -1.
Oxygen typically has an oxidation state of -2.
Let y be the oxidation state of chlorine (Cl). Then, we can write the equation:
y + (-2) = -1
y - 2 = -1
y = +1
The oxidation state of chlorine (Cl) in ClO– is +1.