How to Write the Formula for Iron (II) nitrate
How to Write the Formula for Iron (II) nitrate

molecular formula FeN2O6 B083410 Iron(II) nitrate CAS No. 14013-86-6

Iron(II) nitrate

Cat. No.






M. Wt:

179.86 g/mol

InChI Key:




Attention: For research use only. Not for human or veterinary use.

Description Iron(II) nitrate is a chemical compound with the molecular formula Fe(NO3)2. It is a green crystalline solid that is soluble in water and ethanol. Iron(II) nitrate is commonly used in laboratory experiments and scientific research due to its unique properties and applications.
Synthesis Method Iron(II) nitrate can be synthesized by dissolving iron in nitric acid. The reaction can be represented as follows:

Fe + 2HNO3 → Fe(NO3)2 + H2

The resulting green crystalline solid can be purified by recrystallization. Alternatively, Iron(II) nitrate can also be obtained by reacting Iron(III) nitrate with Iron metal.

Scientific Research Application Iron(II) nitrate is widely used in scientific research due to its unique properties and applications. It is commonly used in the synthesis of Iron-containing compounds, such as Iron(II) oxide and Iron(II) sulfate. Iron(II) nitrate is also used as a catalyst in chemical reactions, such as the reduction of nitro compounds. Additionally, Iron(II) nitrate is used as a reagent in analytical chemistry to detect the presence of certain compounds.
Mechanism of Action Iron(II) nitrate acts as a Lewis acid, meaning it can accept an electron pair from a Lewis base. This property makes it useful in catalytic reactions. Additionally, Iron(II) nitrate can undergo oxidation-reduction reactions, where it can either donate or accept electrons. This property makes it useful in redox reactions.
Biochemical and Physiological Effects Iron(II) nitrate has been shown to have both positive and negative effects on biological systems. It is an essential nutrient for the human body, as it is required for the production of hemoglobin, a protein in red blood cells that carries oxygen. However, excessive intake of Iron(II) nitrate can lead to toxicity and can cause damage to the liver and other organs.
Advantages and Limitations for Lab Experiments Iron(II) nitrate has several advantages for lab experiments. It is readily available and relatively inexpensive. It is also stable under normal laboratory conditions. However, Iron(II) nitrate has some limitations. It is hygroscopic, meaning it can absorb moisture from the air, which can affect its properties. Additionally, Iron(II) nitrate can be hazardous if not handled properly.
Future Directions There are several future directions for research on Iron(II) nitrate. One area of research is the development of new catalysts for chemical reactions. Iron(II) nitrate has been shown to be an effective catalyst, but there is still room for improvement. Another area of research is the investigation of the effects of Iron(II) nitrate on biological systems. This research can help to better understand the role of Iron(II) nitrate in the human body and the potential risks associated with its use. Additionally, research can be conducted on the use of Iron(II) nitrate in environmental applications, such as the removal of pollutants from water.
CAS RN 14013-86-6
Product Name Iron(II) nitrate
Molecular Formula FeN2O6
Molecular Weight 179.86 g/mol
IUPAC Name iron(2+);dinitrate
InChI InChI=1S/Fe.2NO3/c;2*2-1(3)4/q+2;2*-1
SMILES [N+](=O)([O-])[O-].[N+](=O)([O-])[O-].[Fe+2]
Canonical SMILES [N+](=O)([O-])[O-].[N+](=O)([O-])[O-].[Fe+2]
Origin of Product United States


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