Cobalt is a chemical element, lustrous silvery-gray ferromagnetic transition metal of Group 9 (VIIIB) of the periodic table with atomic number 27 and symbol Co. It is used in making different types of alloys, and large quantities of its compounds are used in the glass and ceramic industries. The hardness and tensile strength of cobalt are higher than steel. Finely divided metallic cobalt is pyrophoric like iron but compact metal is not attacked by air or water molecule at ordinary temperature. The metal is less readily dissolve in minerals acids like nitric acid and sulfuric acid. It does not attack by aqueous alkali but readily dissolved in fused KOH at 550 °C.
History and discovery
The history of the discovery of cobalt may be started with its naming. The name of the metal given from the German word cobold means evil spirit or goblin. In 1735, the Swedish chemist G. Brandt analyzed some specimens of the cobold and wrote about a new semi-metal which he named cobold. Brandit describes six semi-metals like mercury, bismuth, zinc, antimony, cobalt, and arsenic. Before 1776, many scientists believed that the element was a compound of iron and arsenic. The identity of cobalt as a new metal was established around 1780 by T Bergmann and other scientists.
Where is cobalt found?
Cobalt is less common among the first transition metals except for scandium. It is the thirtieth most abundant element of all known elements that found mainly with nickel and arsenic. The principal minerals of cobalt are arsenides and sulfides like smaltite, CoAs2, erythrite, Co3(AsO4)2. Besides arsenic, sulfur and iron contain 4 to 10 percent of cobalt, and a varying amount of silver, copper, and lead. South Africa and Canada are the main producers of cobalt and a small reserve of metal found in Australia and Russian countries.
Properties of cobalt
The hexagonal crystal lattice cobalt has valence shell electronic configuration [Ar] 3d7 4s2. The +2 and +3 oxidation number or state is important to derive different types of chemical bonding and compounds of metal. Co(II) is more stable than Co(III) in acid solutions. Finely divided metallic cobalt is pyrophoric like iron but the compact metal is not attacked by air or water at ordinary temperature. Some important properties are given below the table,
|Properties of Cobalt|
|Electronic configuration||[Ar] 3d7 4s2|
|Crystal structure||hexagonal closed packed crystal lattice|
|Heat capacity||24.81 J mol-1 K-1|
|Melting point||1495 °C|
|Boiling point||2927 °C|
|Oxidation states||+2, +3|
|Electrical resistivity||62.4 nΩ m|
|Electronegativity||1.88 (Pauling scale)|
|Ionization energy||1st: 760.4 kJ/mol
2nd: 1668 kJ/mol
3rd: 3232 kJ/mol
Cobalt on Periodic Table
Cobalt is placed on period-4 and group-9 on the periodic table with group members rhodium and iridium. It is a member of d-block elements or transition metals.
Facts about cobalt
- Cobalt is a lustrous silvery metal with a bluish tinge.
- The hardness and tensile strength of the metal are greater than the steel.
- It is a ferromagnetic metal with a high curie point (1121°C).
- The metal cobalt reacts with most of the halogens like fluorine, chlorine, bromine, and other non-metals like boron, carbon, phosphorus, sulfur on heating.
The oxidation state free energy diagram shows that the most common and important chemical compounds of cobalt are formed in +2 and +3 oxidation states. In acid solution, Co(II) is more stable than Co(III). Some important chemical compounds of metal are described below,
Cobalt(II) oxide (CoO) is formed when steam is passed over red hot metal or Co(II) carbonate, nitrate, etc. The oxide is an olive green solid stable up to 1000 °C. When heated CoO in the air it formed Co3O4. Co(II) oxide dissolved in concentrated alkali to form a deep blue solution of [Co(OH)4]-2. It has a rock salt structure. Normally the structure contains excess oxygen which behaves like a p-type semiconductor.
The brown hydrated cobalt(III) oxide is formed when Co(OH)2 is oxidized in alkaline medium. It may be dried at 150 °C to the composition Co2O3, H2O. Further heating, it forms Co2O3. Oxidation of aqueous Co(II) in alkaline medium by chlorine, oxygen, and ozone forms a black hydrous oxide CoO2, but this is not well characterized.
Several mixed oxide species of cobalt are formed in +4 oxidation state. For example, M2CoO3 (M = K, Rb, Cs), Li8CoO8 and Ba2CoO4. The last compounds have the same structure as K2SO4. It is prepared by heating Co(OH)2 with Ba(OH)2 or BaCO3 in oxygen at 1050 °C. Similarly, the fusion of CoO4 with NaO2 produces Na4CoO4. It contains the tetrahedral CoO4 anion with Na+ cation coordinated to oxygen atoms. A compound like Cs2CoF6 is prepared by fluorination of Cs2CoCl4 which is isomorphous with Cs2SiF6.
Cobalt halide compounds
The halide like CoF2 is made by heating the double salt (CoF2, 2NH4F) or by the action of HF on CoCl2. The other halides of Co(II) are obtained by direct reaction of cobalt metal and halogens like chlorine, bromine, and iodine.
Cobalt (III) fluoride
Cobalt (III) fluoride is a light brown powder having the chemical formula CoF3. It is obtained by heating CoF2 or CoCl2 in fluorine. CoF3 violently reacts with water by evolving oxygen. It is a strong fluorinating agent which fluorinating hydrocarbons to form fluorocarbons.
In the +3 state, cobalt has a d6 configuration which gains the advantage of large crystal field stabilization energy (CFSE) with strong field ligands. Werner shows that Co(II) forms a series of amine complexes and the orange hexamine, [Co(NH3)6]+3 is readily formed by aerial oxidation of aqueous Co(II) in presence of ammonia and ammonium salts. The low oxidation state of cobalt ( 1, O, and -1) are found with strongly pi-bonding ligands like carbonyl (CO), nitrosyl (NO), and cyanogen (CN–) ligands.
How to detect metal?
Cobalt metal may be detected conveniently by the deep blue color produced in borax beads which remains unchanged in reducing flame. The solution containing Co(II) produces a yellow precipitate with potassium nitrate solution in excess acetic acid medium.
Uses of Cobalt
Before the 19th century, large quantities of cobalt compounds are used in glass and ceramic industries. Today it is used in different fields like alloys or battery making and chemical catalyst.
- The blue pigments of cobalt compounds are used in glass and ceramic industries due to their artistic color. Nearly 30 percent of the total production of metal (about 10,000 tonnes per annum in the world) is used for making paints or coloring.
- The almost same quantity of cobalt is used in making high quality alloys. These alloys are used for making aircraft parts, gas turbine blades, and high-speed steel.
- Many cobalt compounds are also used as chemical catalysts in a number of organic chemistry, petroleum, and chemical industries.
- Cobalt salts are also used to speed up the oxidation of oil-based paints and hence it is used as a drying agent in paints.
- Radioactive Cobalt-60 is a beta emitter and used for the treatment of cancer.