Iron(II) sulfide, also popular as iron sulfide or ferrous sulfide, is an inorganic, water-insoluble compound represented by the chemical formula FeS [1, 2]. In IUPAC nomenclature, it is called sulfanylideneiron . It naturally occurs as the minerals troilite and pyrrhotite . FeS has the nickel arsenide structure, with trigonal prismatic sulfides and octahedral iron centers .
Iron(II) Sulfide Identification
|CAS Number||1317-37-9 |
|PubChem CID||14828 |
|ChemSpider ID||8466211 |
|EC Number||215-268-6 |
|MDL Number||MFCD00011013 |
|InChI Key||MBMLMWLHJBBADN-UHFFFAOYSA-N |
Iron(II) Sulfide Composition and Synthesis
Fe + S → FeS
Reaction with Hydrochloric Acid
Iron sulfide reacts with hydrochloric acid to yield ferrous chloride and hydrogen sulfide, as indicated by the following reaction:
FeS + 2 HCl → FeCl2 + H2S
Properties and Characteristics of Iron(II) Sulfide
|Molar Mass/Molecular Weight||87.905 g/mol |
|Color and Appearance||Gray to brownish-black rods, lumps, or granular powder, colorless when pure |
|Melting Point||1194 °C, 2181 °F |
|Boiling Point||Decomposes |
|Density||4.75 g cm-3 |
|State of matter at room temperature||Solid |
|Solubility||Reacts in acids with the production of hydrogen sulfide, insoluble in nitric acid |
|Solubility in Water||0.00062 g/100 cc at 18 °C |
|Magnetic Susceptibility (χ)||1074 X 10-6 cm3/mol|
- As a pigment in ceramics, hair dyes, and glass containers [1, 7].
- Treating exhaust gases and lessening heavy metal pollution .
- To synthesize hydrogen sulfide in the laboratory .
Is It Safe
Iron sulfide can cause irritation to your skin, eyes, lungs, and gastrointestinal tract when inhaled . It is known to cause slight toxicity upon ingestion .
- Ferrous Sulfide – Pubchem.ncbi.nlm.nih.gov
- Iron(II) Sulfide – Chemspider.com
- Ferrous Sulfide – Chemicalbook.com
- Iron(II) Sulfide – Americanelements.com
- Structures Related to NaCl and NiAs – Chem.libretexts.org
- Iron and Sulfur Reaction – Rsc.org
- Iron(II) Sulfide – Hazmap.nlm.nih.gov
- Iron(II) Sulfide – Mccsd.net