Why in the case of H2O2 the oxidation state of Oxygen is -1?
When we have to take the oxidation state for oxygen as -1?
Why in the case of H2O2 the oxidation state of Oxygen is -1?
When we have to take the oxidation state for oxygen as -1?
The oxidation number of H is +1. The oxidation number of O is -1
You assign oxidation numbers to the elements in a compound by using the Rules for Oxidation Numbers.
The important rules for this problem are:
-
The oxidation number of H is +1, but it is -1 in when combined with less electronegative elements.
-
The oxidation number of O in compounds is usually -2, but it is -1 in peroxides.
-
The sum of the oxidation numbers of all the atoms in a neutral compound is 0.
The oxidation number of H is +1 (Rule 1).
If you know that H2O2 is hydrogen peroxide, you can immediately assign oxygen the ON = -1.
If you don't know that H2O2 is hydrogen peroxide, you can use Rule 3.
The oxidation number of H is +1. For two H atoms, the sum is +2.
Since H2O2 has no charge, the total oxidation number of the two O atoms must be -2.
The oxidation number of one oxygen atom must be -1.
You assign oxidation numbers to the elements in a compound by using the Rules for Oxidation Numbers.
The important rules for this problem are:
-
The oxidation number of H is +1, but it is -1 in when combined with less electronegative elements.
-
The oxidation number of O in compounds is usually -2, but it is -1 in peroxides.
-
The sum of the oxidation numbers of all the atoms in a neutral compound is 0.
The oxidation number of H is +1 (Rule 1).
If you know that H2O2 is hydrogen peroxide, you can immediately assign oxygen the ON = -1.
If you don't know that H2O2 is hydrogen peroxide, you can use Rule 3.
The oxidation number of H is +1. For two H atoms, the sum is +2.
Since H2O2 has no charge, the total oxidation number of the two O atoms must be -2.
The oxidation number of one oxygen atom must be -1.
