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Identify the oxidation state for each atom in the following reaction:


4Fe + 3O2 → 2Fe2O3

AElemental iron (Fe)
BElemental oxygen (O2)
COne iron atom in Fe2O3
DOne oxygen atom in Fe2O3

Verified Answer :

A0 because Fe is uncharged
b) 0 because O in O2 is uncharged as well
c) +3 because each Fe atom lost 3 electrons
d) -2 because each oxygen aim gained 2 elections

Answer:   a. Elemental iron (Fe) : 0

b. Elemental oxygen \((O_2)\) : 0

c. One iron atom in \(Fe_2O_3\): +3

d. One oxygen atom in \(Fe_2O_3\) : -2

Explanation:

Oxidation reaction is defined as the reaction in which a substance looses its electrons. The oxidation state of the substance increases.

Reduction reaction is defined as the reaction in which a substance gains electrons. The oxidation state of the substance gets reduced.

In neutral ionic compound , the oxidation states are exchanged to give the molecular formula. Thus in \(Fe_2O_3\) iron has oxidation state of +3 and oxygen has oxidation state of -2.

For the reaction :

\(4Fe+3O_2\rightarrow 2Fe_2O_3\)

On reactant side:

Oxidation state of iron in elemental state = 0

Oxidation state of oxygen = 0

On product side:

Oxidation state of iron = +3

Oxidation state of oxygen = -2

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