Secrets of Oxidation Number Calculation and quick revision of the topic.

1. Rule number 1: The oxidation state of any element in the free state is zero. Here free state means when an element is not bonded to any other element and also an atom of the element do not contain any charge. This is also true for diatomic, triatomic and polyatomic atoms.
2. Rule number 2: The oxidation state of a monoatomic ion is same as that of the charge present on the ion.
3. Rule number 3: The sum of the oxidation state of all the atoms present in a neutral compound is zero.
   1. The sum of the oxidation state of all the atoms present in a polyatomic ion is equal to the charge present on that ion.
4. Rule number 4: The oxidation state of metals of group I i.e. Li, Na, K, Rb, Cs, Fr in their compound is +1 and that of group II metals i.e. Be, Mg, Ca, Sc, Ba is +2 in their compounds.
5. Rule number 5: The oxidation number of oxygen in a compound is usually –2. If, however, the oxygen is in a class of compounds called peroxides(for example, hydrogen peroxide), then the oxygen has an oxidation number of –1. If the oxygen is bonded to fluorine, the number is +1.
6. The oxidation state of hydrogen in a compound is usually +1. If the hydrogen is part of a binary metal hydride like NaH etc. (compound of hydrogen and some metal), then the oxidation state of hydrogen is –1.
7. The oxidation number of fluorine is always –1. Chlorine, bromine, and iodine usually have an oxidation number of –1, unless they’re in combination with an oxygen or fluorine.

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