Oxidation Number
Oxidation number, also called oxidation state, is the total number of electrons that benefits or loses to make an atom a chemical bond with another atom.
What are the Oxidation Numbers?
Chemists use an oxidation number (or oxidation state) to track the number of electrons of atoms in atoms. Oxidation numbers do not always match the actual charges on the molecules, and we can calculate the oxidation number for atoms involved in the covalent (as well as ionic) bond.
Let’s understand the oxidation numbers with some examples!
Let’s understand the oxidation numbers with some examples!
Guidelines for determining oxidation number
Oxidation numbers are usually written first with sign (++ or -), then the magnitude, which is in contrast to the charges on ions. Chemists use the following guidelines to determine the oxidation number:
Step 1. In their original state the atoms have an oxidation number of 0.
Step 2. In the monatomic (i.e. single atomic) ions, the atoms have an oxidation number equal to their charge.
Step 3. In compounds: Fluorine oxidation number is assigned -1; Oxygen is usually assigned a -2 oxidation number (except peroxide compounds where it is -1, and in binary compounds with fluorine where it is positive); And hydrogen is usually assigned a +1 oxidation number, except that when the hydride ion is present in the form of H−, then in which case rule 2 wins.
Step 4. In compounds, the oxidation number is assigned to all other atoms so that the sum of oxidation numbers on all atoms in species is equal to the charge on the species. Read More
Step 1. In their original state the atoms have an oxidation number of 0.
Step 2. In the monatomic (i.e. single atomic) ions, the atoms have an oxidation number equal to their charge.
Step 3. In compounds: Fluorine oxidation number is assigned -1; Oxygen is usually assigned a -2 oxidation number (except peroxide compounds where it is -1, and in binary compounds with fluorine where it is positive); And hydrogen is usually assigned a +1 oxidation number, except that when the hydride ion is present in the form of H−, then in which case rule 2 wins.
Step 4. In compounds, the oxidation number is assigned to all other atoms so that the sum of oxidation numbers on all atoms in species is equal to the charge on the species. Read More
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