Iron - 26Fe: the essentials
- Name: iron
- Symbol: Fe
- Atomic number: 26
- Relative atomic mass (Ar): 55.845 (2)
- Standard state: solid at 298 K
- Appearance: lustrous, metallic, greyish tinge
- Classification: Metallic
- Group in periodic table: 8
- Group name: (none)
- Period in periodic table: 4
- Block in periodic table: d
- Shell structure: 2.8.14.2
- CAS Registry: 7439-89-6
Iron atoms have 26 electrons and the shell structure is 2.8.14.2. The ground state electronic configuration of neutral iron is [Ar].3d6.4s2 and the term symbol of iron is 5D4.
Iron: description
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. 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.
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: physical properties
Density of solid: 7874 kg m-3
Molar volume: 7.09 cm3
Thermal conductivity: 80 W m‑1 K‑1
Iron: heat properties
Melting point: 1811 [1538 °C (2800 °F)] K
Boiling point: 3134 [2861 °C (5182 °F)] K
Enthalpy of fusion: 20.5 kJ mol-1
Iron: atom sizes
Atomic radius (empirical): 140 pm
Molecular single bond covalent radius: 116 (coordination number 4) ppm
van der Waals radius: 244 ppm
Iron: electronegativities
Pauling electronegativity: 1.83 (Pauling units)
Allred Rochow electronegativity: 1.64 (Pauling units)
Mulliken-Jaffe electronegativity: (no data)
Iron: orbital properties
First ionisation energy: 762.47 kJ mol‑1
Second ionisation energy: 1562.98 kJ mol‑1
Third ionisation energy: 2957.4 kJ mol‑1
Iron: abundances
Universe: 1100000 ppb by weight
Crustal rocks: 63000000 ppb by weight
Human: 60000 ppb by weight
Iron: crystal structure
Iron: biological data
- Human abundance by weight: 60000 ppb by weight
Iron compounds are essential to all life. For example, it is an iron atom in haemoglobin that is responsible for carrying oxygen around the blood stream.
Iron: uses
Iron: reactions
Reactions of iron as the element with air, water, halogens, acids, and bases where known.
Iron: binary compounds
Binary compounds with halogens (known as halides), oxygen (known as oxides), hydrogen (known as hydrides), and other compounds of iron where known.
Iron: compound properties
Bond strengths; lattice energies of iron halides, hydrides, oxides (where known); and reduction potentials where known.
Iron: history
Iron was discovered by known since ancient times in unknown at not known. Origin of name: from the Anglo-Saxon word "iron" or "iren" (the origin of the symbol Fe comes from the Latin word "ferrum" meaning "iron"). Possibly the word iron is derived from earlier words meaning "holy metal" because it was used to make the swords used in the Crusades..Iron: isotopes
Iron isotopes are mainly used in nutritional studies, with Fe-57 and Fe-58 being the two most commonly used Fe isotopes. Studies have included iron-loss by human adolescents, conditions for effective iron absorption, interventions for anemia and genetic iron control. The Fe-54 isotope is used for the production of radioactive Fe-55 which in turn is used as an electron capture detector and in X-ray fluorescence. Fe-56 can be used for the production of radioactive Co-55 which is used as a tumor seeking agent in bleomycin.
Iron: isolation
Isolation: 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.