Cobalt: the essentials
Cobalt atoms have 27 electrons and the shell structure is 184.108.40.206. The ground state electronic configuration of neutral cobalt is [Ar].3d7.4s2 and the term symbol of cobalt is 4F9/2.
Cobalt is a brittle, hard, silver-grey transition metal with magnetic properties similar to those of iron (ferromagnetic). Cobalt is present in meteorites. Ore deposits are found in Zaire, Morocco and Canada. The isotope cobalt-60 (60Co) is an artificially produced isotope used as a source of γ rays (its high energy radiation is useful for sterilisation in medicine and of foods). Cobalt salts colour glass a beautiful deep blue colour. Cobalt compounds are important catalysts in a number of industrial processes. Cobalt is required in small amounts for life and is the only metal found in vitamins (cobalt is the critical component of vitamin B12.
Marmite, which we eat here in England and love it or hate it is a source of vitamin B12, actually a cobalt complex. The equivalent, but blander, in Australia is Vegemite. Marmite is available in the USA. Try mixing it with peanut butter.
Cobalt: physical properties
Cobalt: heat properties
- Melting point: 1768 [1495 °C (2723 °F)] K
- Boiling point: 3200 [2927 °C (5301 °F)] K
- Enthalpy of fusion: 20.5 kJ mol-1
Cobalt: atom sizes
- Atomic radius (empirical): 135 pm
- Molecular single bond covalent radius: 111 (coordination number 4) ppm
- van der Waals radius: 240 ppm
- Pauling electronegativity: 1.88 (Pauling units)
- Allred Rochow electronegativity: 1.70 (Pauling units)
- Mulliken-Jaffe electronegativity: (no data)
Cobalt: orbital properties
- First ionisation energy: 760.40 kJ mol‑1
- Second ionisation energy: 1648.39 kJ mol‑1
- Third ionisation energy: 3232.3 kJ mol‑1
Cobalt: crystal structure
Cobalt: biological data
- Human abundance by weight: 20 ppb by weight
Cobalt salts in small amounts are essential to many life forms, including humans. It is at the core of a vitamin called vitamin-B12. Grazing animals do not to do well in areas where there is little cobalt in the soil.
Reactions of cobalt as the element with air, water, halogens, acids, and bases where known.
Cobalt: binary compounds
Binary compounds with halogens (known as halides), oxygen (known as oxides), hydrogen (known as hydrides), and other compounds of cobalt where known.
Cobalt: compound properties
Bond strengths; lattice energies of cobalt halides, hydrides, oxides (where known); and reduction potentials where known.
Cobalt: historyCobalt was discovered by Georg Brandt in 1735 at Sweden. Origin of name: from the German word "kobald" meaning "goblin" or evil spirit.
Naturally occurring cobalt consists of a single stable isotope: 59Co. Cobalt-59 has spin 7/2. The usual NMR reference is K3[Co(CN)6] in D2O. Cobalt-60 is an artifical isotope, and is an important γ-ray source.
Isolation: it is not normally necessary to make cobalt in the laboratory as it is available readily commercially. Many ores contain cobalt but not many are of economic importance. These include the sulphides and arsenides linnaeite, Co3S4, cobaltite, CoAsS, and smaltite, CoAs2. Industrially, however, it is normally produced as a byproduct from the produstion of copper, nickel, and lead.
Normally the ore is "roasted" to form a mixture of metals and metal oxides. Treatment with sulphuric acid leaves metallic copper as a residue and disolves out iron, cobalt, and nickel as the sulphates. Iron is obtained by precipitation with lime (CaO) while cobalt is produced as the hydroxide by precipitation with sodium hypochlorite (NaOCl)
2Co2+(aq) + NaOCl(aq) + 4OH-(aq) + H2O → 2Co(OH)3(s) + NaCl(aq)
The trihydroxide Co(OH)3 is heated to form the oxide and then reduced with carbon (as charcoal) to form cobalt metal.
2Co(OH)3 (heat) → Co2O3 + 3H2O
2Co2O3 + 3C → Co + 3CO2