Iron III Oxide Formula

Meaning of Iron III Oxide Formula

Iron III oxide formula is the common primary formula that students come across while studying chemistry in many classes. In general, the use of the formula and the reactions that are associated with its progress, ranging from basic to more complex as the students advance from a lower class to higher classes. Iron (III) oxide, which is also known as ferric oxide, is an inorganic chemical compound. It is the primary iron oxide that is important and contains a mineral known as hematite, making it an important source of Iron. Sometimes, this compound is also known as either rust or hydrated ferric oxide.


Iron (III) Oxide Chemical Formula

Fe\[_{2}\]O\[_{3}\] is the chemical formula of Iron (III) oxide or the chemical name of Fe\[_{2}\]O\[_{3}\] is Iron III oxide. This is derived by taking the compound valency. In general, Oxygen (O) holds a valency of 2, and Iron (Fe) holds a valency of 3. When we write the chemical formula, it is a common process where the compounds usually exchange valencies to attain a balanced and neutral state. Thus, the valency of Oxygen goes to Iron and vice versa.


Formula

Fe\[_{2}\]O\[_{3}\]

Density

5.242 g/cm\[^{3}\]

Molar Mass

159.69 g/mol

Boiling Point

Usually decomposes

Melting Point

1566 °C (Theoretical)

Fe\[_{2}\]O\[_{3}\] Chemical Name

Iron III oxide


Iron (III) Oxide Structural Formula

Fe\[_{2}\]O\[_{3}\] may be obtained in multiple polymorphs. As the main one, α, Iron adopts an octahedral coordination geometry. It means each Fe center is bound to the six oxygen ligands. And, in the γ polymorph, a few of the Fe sits on tetrahedral sites, holding four oxygen ligands.

The structural formula of iron (III) oxide is represented as follows:

[Image will be Uploaded Soon]


Preparation

Iron (III) oxide is the product of iron oxidation. It may be prepared in the laboratory by electrolyzing a sodium bicarbonate solution, an inert electrolyte, with an iron anode, which is represented chemically as:

4 Fe + 3 O\[_{2}\] + 2 H\[_{2}\]O → 4 FeO(OH)

The resulting hydrated iron (III) oxide, which is written here as FeO (OH), dehydrates around 200°C.

2FeO (OH) → Fe\[_{2}\]O\[_{3}\] + H\[_{2}\]O

FAQs (Frequently Asked Questions)

1. Give the Polishing Uses of Iron Oxide?

Answer: A fine powder of ferric oxide is called "red rouge," "jeweller’s rouge," or simply rouge. It can be used to put the final polish on lenses and metallic jewellery, and as a cosmetic, historically. Rouge cuts slower than a few modern polishes, such as cerium (IV) oxide, but still, it is used in optics fabrication and by jewellers for the superior finish that it can produce.


When polishing gold, the rouge leaves a tiny stain, which contributes to the finished piece's appearance. Rouge is sold as a paste, powder, which can be laced either on the polishing cloths or solid bar (with a grease or wax binder).

2. How to Calculate the Molar Mass of Iron?

Answer: Basically, the molar mass is the molecular, atomic, or formula mass of a substance expressed in grams instead of AMU (Atomic Mass Unit).


As the atomic mass of Iron is nearly 56 AMU (actually 55.85 AMU), the molar mass of Iron remains similar to atomic mass; 56g or 55.85g.

3. Give the Use of Red Iron Oxide?

Answer: Red iron oxides are used as pigments catalyst, iron ores, and thermite, and colour in hemoglobin. They are inexpensive and durable pigments in coating and coloured concrete, paints, colours commonly available in the earth end of the yellow, red, orange, black and brown range.

4. Explain the Liquid Phase of Iron Oxide?

Answer: Molten Fe2O3 can be expected to have a coordination number of near to 5 oxygen atoms up to each iron atom, based on the measurements of slightly Oxygen deficient, which are supercooled liquid iron oxide droplets, where the supercooling circumvents the requirement for the high oxygen pressures required more than the melting point to maintain stoichiometry.