|Classification:||Cobalt is a transition metal|
|Melting point:||1495 oC, 1768 K|
|Boiling point:||2930 oC, 3203 K|
|Neutrons in most abundant isotope:||32|
|Electron configuration:||[Ar] 3d7 4s2|
|Density @ 20oC:||8.90 g/cm3|
|Atomic volume:||6.7 cm3/mol|
|Structure:||hcp: hexagonal close pkd|
|Specific heat capacity||0.42 J g-1 K-1|
|Heat of fusion||16.190 kJ mol-1|
|Heat of atomization||426 kJ mol-1|
|Heat of vaporization||373.3 kJ mol-1|
|1st ionization energy||758.4 kJ mol-1|
|2nd ionization energy||1646 kJ mol-1|
|3rd ionization energy||3232.2 kJ mol-1|
|Electron affinity||63.8 kJ mol-1|
|Minimum oxidation number||-1|
|Min. common oxidation no.||0|
|Maximum oxidation number||5|
|Max. common oxidation no.||3|
|Electronegativity (Pauling Scale)||1.88|
|Polarizability volume||7.5 Å3|
|Reaction with air||mild, w/ht ? Co3O4|
|Reaction with 15 M HNO3||vigorous, ? Co(NO3)2, NOx|
|Reaction with 6 M HCl||mild, ? H2, CoCl2|
|Reaction with 6 M NaOH||–|
|Atomic radius||135 pm|
|Ionic radius (1+ ion)||–|
|Ionic radius (2+ ion)||83.8 pm|
|Ionic radius (3+ ion)||71.8 pm|
|Ionic radius (1- ion)||–|
|Ionic radius (2- ion)||–|
|Ionic radius (3- ion)||–|
|Thermal conductivity||100 W m-1 K-1|
|Electrical conductivity||17.9 x 106 S m-1|
|Freezing/Melting point:||1495 oC, 1768 K|
Discovery of Cobalt
Since ancient times cobalt compounds have been used to produce blue glass and ceramics.
The element was first isolated by Swedish chemist George Brandt in 1735. He showed it was the presence of the element cobalt that caused the blue color in glass, not bismuth as previously thought.
In about 1741 he wrote, “As there are six kinds of metals, so I have also shown with reliable experiments… that there are also six kinds of half-metals: a new half-metal, namely cobalt regulus in addition to mercury, bismuth, zinc, and the reguluses of antimony and arsenic.”
The word cobalt is derived from the German ‘kobold’, meaning goblin or elf.
Appearance and Characteristics
Cobalt and its compounds are considered to be slightly toxic by skin contact and moderately toxic by ingestion.
Cobalt is a bluish-white, lustrous, hard, brittle metal. It is ferromagnetic.
Uses of Cobalt
Cobalt is used in alloys for aircraft engine parts and in alloys with corrosion/wear resistant uses.
Cobalt is widely used in batteries and in electroplating.
Cobalt salts are used to impart blue and green colors in glass and ceramics.
Radioactive 60Co is used in the treatment of cancer.
Cobalt is essential to many living creatures and is a component of vitamin B12.
Abundance and Isotopes
Abundance earth’s crust: 25 parts per million by weight, 8 parts per million by moles
Abundance solar system: 4 parts per million by weight, 0.7 parts per million by moles
Cost, pure: $21 per 100g
Cost, bulk: $4.40 per 100g
Source: Cobalt is not found as a free element in nature. It is found in mineral ores. The main ores of cobalt are cobaltite (CoAsS), erythrite (hydrated arsenate of cobalt), glaucodot (Co,Fe)AsS, and skutterudite (Co,Ni)As3. Cobalt is generally produced as a by-product of nickel and copper mining.
Cite this Page
For online linking, please copy and paste one of the following:
<a href="http://www.chemicool.com/elements/cobalt.html">Cobalt Element Facts</a>
To cite this page in an academic document, please use the following MLA compliant citation:
"Cobalt." Chemicool Periodic Table. Chemicool.com. 16 Oct. 2012. Web. <http://www.chemicool.com/elements/cobalt.html>.