Simple method of determining oxidation number.
The oxidation number, also known as the oxidation state, of an atom is a measure of the number of electrons that an atom has gained or lost in a chemical reaction. It is a useful way to keep track of the distribution of electrons in a compound or ion, and can provide information about the reactivity and properties of a substance. Here is a simple method for determining the oxidation number:
For atoms in their elemental form, the oxidation number is always zero. For example, the oxidation number of oxygen in O2 is zero.
For monatomic ions, the oxidation number is equal to the charge on the ion. For example, the oxidation number of sodium in Na+ is +1.
In most compounds, the oxidation number of hydrogen is +1 and the oxidation number of oxygen is -2. There are some exceptions to this rule, such as in peroxides (where the oxidation number of oxygen is -1) and in compounds with highly electronegative elements like fluorine (where the oxidation number of hydrogen can be -1).
The sum of the oxidation numbers of all the atoms in a compound or ion must equal the overall charge of the compound or ion. For example, the oxidation number of sulfur in SO4^2- is +6, and the sum of the oxidation numbers of all the atoms is (-2) x 4 + (+6) = -8 + 6 = -2, which is the charge on the ion.
By following these rules, you can determine the oxidation number of each atom in a compound or ion.
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