What is the oxidation number of Fe in Fe2O3? Send a photo with step-by-step solution.
The Correct Answer and Explanation is:
Here is the step-by-step solution image for finding the oxidation number of Fe in Fe₂O₃:
Explanation
In the compound Fe₂O₃, we are asked to find the oxidation number of iron (Fe). To do this, we start by understanding that oxidation numbers are used to keep track of electron transfers in chemical compounds. Each element in a compound is assigned a number that represents how many electrons it has gained or lost relative to its elemental form.
Fe₂O₃ is composed of two iron (Fe) atoms and three oxygen (O) atoms. Oxygen is more electronegative than iron, and in nearly all compounds, oxygen has an oxidation number of -2. Therefore, the three oxygen atoms contribute a total oxidation number of 3 × -2 = -6.
Let the oxidation number of each iron atom be x. Since there are two iron atoms, the total contribution from iron is 2x. The compound Fe₂O₃ is neutral overall, meaning the sum of all oxidation numbers must equal zero.
So, we set up the equation:
2x + 3(-2) = 0
2x – 6 = 0
2x = 6
x = +3
This means each iron atom has an oxidation number of +3 in Fe₂O₃.
This positive oxidation number indicates that each iron atom has lost three electrons compared to its neutral state, making Fe³⁺ the ionic form in this compound. Understanding oxidation numbers is important in redox reactions, where electron transfer is involved. It helps in identifying which elements are oxidized and which are reduced.
Hence, the oxidation number of iron in Fe₂O₃ is +3.
