Iron II Oxide Formula:
Iron (II) Oxide is a non-organic compound consisting of one iron atom and one oxygen atom. Iron is a metallic element from group 8 on the periodic table, and it's a fundamental component of the Earth's composition. Iron is denoted by the symbol Fe with an atomic number of 26, while oxygen, symbolized by O with an atomic number of 8, is a highly reactive non-metal belonging to group 16 on the periodic table and ranks as the third most abundant element on Earth.
Iron II Oxide Formula
Regarding the formula of Iron (II) Oxide, it's part of a family of related non-stoichiometric compounds and is composed of iron and oxygen. There are several types of iron oxide, with Iron (II) oxide being one of them. Iron (II) oxide, also known as ferrous oxide or iron monoxide, is an ionic compound with the chemical formula FeO, which signifies one iron atom and one oxygen atom.
Approximately 9% of the Earth's crust is composed of Iron (II) Oxide. It typically appears as a black crystalline solid and finds wide applications in creating pigments and dyes used in pottery glazes. When exposed to water, it forms a light blue/green crystal. Iron (II) oxide is prone to oxidation in the presence of air, dissolves in acids but is not soluble in water and alkali. It readily absorbs carbon dioxide, forming iron(II) carbonate (
FeCO
3
), which is a strong base.
Iron II Oxide Formula Structure
Iron (II) oxide is found in a mineral called Wustite, which has a crystal lattice structure similar to rock salt. It has a cubic, rock salt structure, with iron atoms arranged in an octahedral pattern coordinated by oxygen atoms, and oxygen atoms arranged in an octahedral pattern coordinated by iron atoms.
Preparation of Iron II Oxide Formula
Iron (II) Oxide can be found in nature due to the incomplete oxidation of iron:
2Fe + O
2
→ 2FeO
Synthetic preparation involves the thermal decomposition of iron (II) oxalate, yielding iron (II) oxide, carbon dioxide, and carbon monoxide. This process must be carried out in an inert atmosphere to prevent the formation of iron
(III) oxide (Fe
2
O
3
)
:
FeC
2
O
4
→ FeO + CO
2
+ CO
Iron II Oxide Formula Balanced Equation
Balancing the equation for the formation of Iron (II) Oxide, we can observe that the number of atoms is currently unbalanced.
On the left side:
Fe = 1, O = 2
On the right side:
Fe = 2, O = 3
To balance the equation, we adjust the number of oxygen
(O
2
)
molecules:
Fe + 3O
2
→ 2Fe
2
O
3
Now, let's check the atom count:
Left side:
O = 3 x 2 = 6, Fe = 1
Right side:
O = 3, Fe = 2
To balance the oxygen atoms, we multiply the Fe on the left side by 2:
2Fe + 3O
2
→ 2Fe
2
O
3
Now, the atom count is balanced:
Left side:
O = 3 x 2 = 6, Fe = 2
Right side:
O = 6, Fe = 4
Both oxygen
(O)
and iron
(Fe)
are now balanced:
4Fe + 3O
2
→ 2Fe
2
O
3
Left side:
O = 6, Fe = 4
Right side:
O = 6, Fe = 4
Iron II Oxide Formula Positive and Negative Ion
Iron (II) Oxide
(FeO)
can form both positive and negative ions depending on its chemical context.
Positive Ion (Cation): Iron (II) can form a positive ion (cation) when it loses two electrons. In this case, it becomes
Fe²⁺
.
Negative Ion (Anion): In the context of oxygen ions
(O²⁻)
, iron
(II)
can form a negative ion (anion) when it gains two electrons. This results in the formation of a compound, iron(II) oxide
(FeO).
So, Iron (II) Oxide itself is an ionic compound with both a positive iron ion
(Fe²⁺)
and a negative oxygen ion
(O²⁻)
.
Physical Properties of Iron II Oxide
-
Chemical formula: FeO
-
Molar Mass: 71.844 g/mol
-
Density: 5.745 g/cm3
-
Appearance: Solid at room temperature (black crystals)
-
Solubility: Insoluble in water and alkali, but soluble in acids
-
Boiling point: 3,414 °C
-
Melting point: 1,377 °C
-
Magnetic Susceptibility: +7200·10−6 cm3/mol
-
Refractive Index: 2.23
Also Check -
Iron (II) Sulfate Formula
Chemical Properties of Iron II Oxide
Below
575 °C
, FeO tends to disproportionate into metals and
Fe
3
O
4
:
4FeO → Fe + Fe
3
O
4
It easily oxidizes when exposed to air, forming iron(III) oxide:
4FeO + O
2
→ 2Fe
2
O
3
Iron II Oxide (FeO) dissolves in sulfuric acid
(H
2
SO
4
)
, producing Iron (III) sulfate or ferric sulfate:
2FeO + 4H
2
SO
4
→ Fe
2
(SO
4
)
3
+ 4H
2
O + SO
2
Iron II Oxide (FeO) dissolves in nitric acid (HNO3), forming Ferric nitrate or Iron (III) nitrate:
3FeO + 10HNO
3
→ 5H
2
O + NO + 3Fe(NO
3
)
3
Reacting Iron II Oxide (FeO) with hydrogen chloride (HCl) produces Iron(II) chloride and water:
FeO + 2HCl → FeCl
2
+ H
2
O
When Iron II Oxide
(FeO)
reacts with silver nitrate
(AgNO
3
)
, it yields Silver oxide and Ferrous Nitrate:
2AgNO
3
+ FeO → Ag
2
O + Fe(NO
3
)
2
Iron II Oxide Hazards
Health Risks: Prolonged and high-level exposure to iron (II) oxide may lead to illness with flu-like symptoms and siderosis.
Respiratory Irritation: Inhaling fumes or dust containing iron (II) oxide can be hazardous, potentially causing throat and nasal irritation.
Uses of Iron II Oxide
Pigments and Dyes: Iron (II) oxide used as a coloring agent in pigments and dyes for pottery glazes.
Cosmetics and Tattoo Inks: It has received approval from the FDA for use in cosmetics and is found in some tattoo inks.
Steel Production: Iron (II) oxide serves as a raw material in the manufacturing of steel, which is used in building construction and car production.
Heat-Absorbing Glass: In its green crystalline form, it is used in heat-absorbing glass found in both automobiles and buildings.
Catalyst: It acts as a catalyst in various industrial processes.
Phosphate Remover: Iron (II) oxide can be used to remove phosphate in home aquariums.
