Question

The oxidation state of Fe in $F{{e}_{3}}{{O}_{4}}$ is:
a.) +3
b.) +(8/3)
c.) +6
d.) +2

Answer 1

For finding the oxidation state of Fe we will draw the structure of given compound$F{{e}_{3}}{{O}_{4}}$ it will be easy for us to find the oxidation state. Then we will see the oxidation states of oxygen and then according to the oxidation state of oxygen we will find the oxidation state of Fe.

Complete step by step answer:
We know that iron (II, III) oxide is the chemical compound with formula $F{{e}_{3}}{{O}_{4}}$. It occurs in nature as the mineral magnetite. It is one of a number of iron oxides, the others being iron(II) oxide (FeO), which is rare, and iron(III) oxide $F{{e}_{2}}{{O}_{3}}$ also known as hematite.
$F{{e}_{3}}{{O}_{4}}$ is known as ferrosoferric oxide is an iron oxide, Iron (II,III) oxide ($F{{e}_{3}}{{O}_{4}}$).
In this compound three types of bonding of Fe are there. In which one Fe is bonded with two oxygens and other each of two Fe are bonded with three oxygen.
For$F{{e}_{3}}{{O}_{4}}$, two Fe atoms have an oxidation state of +3 and one of +2. Structure of$F{{e}_{3}}{{O}_{4}}$:

Here we take the average of oxidation state:
Let the oxidation state of Fe is ‘n’
So, 3n -8 = 0
‘n’ = +8/3
So, the correct answer is “Option B”.

Note: Instead of averaging the oxidation states, we must keep them separated. This is called fragmenting, which occurs if there is an ionic compound, and the ions can be separated.