How much is the oxidation state of Cl2O3
read rule number 1
http://www.chemistry.co.nz/redox_oxi_aa.htm
To determine the oxidation state of Cl2O3, we need to know the general rules for assignment of oxidation states:
1. The oxidation state of an element in its elemental form is always 0. This means that Cl2 (the diatomic form of chlorine) has an oxidation state of 0.
2. Oxygen usually has an oxidation state of -2, except in peroxides (where it is -1) and when bonded to fluorine (where it is positive).
3. The sum of oxidation states in a compound must equal the net charge of the compound, which in this case is 0 since Cl2O3 is a neutral compound.
We can use these rules to calculate the oxidation state of chlorine in Cl2O3:
Since oxygen usually has an oxidation state of -2, and there are three oxygen atoms in Cl2O3, the total oxidation number from oxygen is -6 (3 * -2).
According to the rule that the sum of oxidation states in a compound is equal to 0, the oxidation state of chlorine must be such that the sum of -6 and the oxidation state of chlorine is 0.
Let the oxidation state of chlorine be x. So, we have:
2x + (-6) = 0
Simplifying the equation, we get:
2x = 6
Dividing both sides by 2, we find that:
x = 3
Therefore, the oxidation state of chlorine in Cl2O3 is +3.