Question

Explain the average oxidation state of iron in $F{{e}_{3}}{{O}_{4}}$.

Answer 1

Hint: The oxidation number also known as oxidation state which describes the degree of oxidation i.e. loss of electrons of an atom in a chemical compound. Conceptually the oxidation state may be positive, negative or zero.

Complete answer:
Oxidation states are typically represented by integers which may be positive, zero, or negative. In some cases, the average oxidation state of an element is a dfraction.
The substance which donates electrons during the oxidation process is known as oxidized substance. To determine in which compound nitrogen have greatest oxidation state we have to calculate the oxidation state of nitrogen in the given atom which can be calculated as follows:
$F{{e}_{3}}{{O}_{4}}$is known by the name iron oxide where iron is a chemical element having atomic number 26. Now we know oxidation state of oxygen is always two and there is negative charge present on the compound which corresponds that oxygen will contain -2 oxidation state now we have three iron atom and four oxygen atoms present in the given compound so the oxidation state of oxygen can be calculated by using the following method:
Let us suppose the oxidation state of iron is x
$F{{e}_{3}}{{O}_{4}}=3x-2\times 4=3x-8$
Now the value of x can be calculated by:
$3x-8=0;x=\dfrac{8}{3}$ which corresponds that oxidation state of iron in $F{{e}_{3}}{{O}_{4}}$ is $\dfrac{8}{3}$ which states that it can be +2 or +3 both.

Note:
The increase in oxidation state of an atom, through a chemical reaction, is known as an oxidation; a decrease in oxidation state is known as a reduction. Such reactions involve the formal transfer of electrons: a net gain in electrons being a reduction, and a net loss of electrons being an oxidation. For pure elements, the oxidation state is zero.