• Key data; description
  • History
  • hydrogen around us
  • Uses
  • Geology
  • Biology
  • hydrogen compounds
  • Reactions of hydrogen
  • Compounds
  • Bond enthalpies
  • Radii in compounds
  • Lattice energies
  • Reduction potentials
  • nuclear properties
  • NMR
  • Naturally occurring isotopes
  • Radioisotopes
  • electronic properties
  • Electronic configuration
  • Ionization energies
  • Electron affinities
  • Electronegativities
  • Effective nuclear charges
  • Electron binding energies
  • Atom radii
  • Valence shell radii
  • physical properties
  • Bulk properties (density, resistivity, etc.)
  • Thermal properties (melting point, etc.)
  • Thermodynamic properties
  • crystallography
  • Crystal structure
  • Elements

    55.845 (2)

    Name: ironGroup number: 8
    Symbol: FeGroup name: (none)
    Atomic number: 26Period number: 4
    Atomic weight: 55.845 (2)Block: d-block
    CAS Registry ID: 7439-89-6Voice:
    Standard state: solid at 298 KColour: lustrous, metallic, greyish tinge
    Classification: MetallicAvailability:

    iron sheet
    This sample is from The Elements Collection, an attractive and safely packaged collection of the 92 naturally occurring elements that is available for sale.

    Iron is a relatively abundant element in the universe. It is found in the sun and many types of stars in considerable quantity. Iron nuclei are very stable. Iron is a vital constituent of plant and animal life, and is the key component of haemoglobin.

    The pure metal is not often encountered in commerce, but is usually alloyed with carbon or other metals. The pure metal is very reactive chemically, and rapidly corrodes, especially in moist air or at elevated temperatures. Any car owner knows this. Iron metal is a silvery, lustrous metal which has important magnetic properties.

    iron filings salts cause sparks in flames.

    Iron filings salts cause sparks in flames. The picture above shows the result from adding iron filings to a burning mixture of potassium chlorate and sucrose. Do not attempt this reaction unless are a professionally qualified chemist and you have carried out a legally satisfactory hazard assessment.


    Here is a brief summary of the isolation of iron.

    It is not normally necessary to make iron in the laboratory as it is available commercially. Small amounts of pure iron can be made through the purification of crude iron with carbon monoxide. The intermediate in this process is iron pentacarbonyl, Fe(CO)5. The carbonyl decomposes on heatingto about 250°C to form pure iron powder.

    Fe + CO Fe(CO)5 (250°C) Fe + 5CO

    The Fe(CO)5 is a volatile oily complex which is easily flushed from the reaction vessel leaving the impurities behind. Other routes to small samples of pure iron include the reduction of iron oxide, Fe2O3, with hyrogen, H2.

    Nearly all iron produced commercially is used in the steel industry and made using a blast furnace. Most chemistry text books cover the blast furnace process. In essence, iron oxide, Fe2O3, is reduced with with carbon (as coke) although in the furnace the actual reducing agent is probably carbon monoxide, CO.

    2Fe2O3 + 3C 4Fe + 3CO2

    This process is one of the most significant industrial processes in history and the origins of the modern process are traceable back to a small town called Coalbrookdale in Shropshire (England) around the year 1773.

  • FeF2
  • FeF2.4H2O
  • FeF3
  • FeF3.3H2O
  • Chlorides
  • FeCl2
  • FeCl2.2H2O
  • FeCl2.4H2O
  • FeCl3
  • FeCl3.6H2O
  • Bromides
  • FeBr2
  • FeBr3
  • Iodides
  • FeI2
  • FeI3
  • Hydrides
    none listed
  • FeO
  • Fe2O3
  • Fe3O4
  • Sulfides
  • FeS
  • Selenides
  • FeSe
  • Tellurides
  • FeTe
  • Nitrides
  • Fe2N

  • Our data and resources are taken from Web Elements