Cobalt compounds

Cobalt compounds are chemical compounds formed by cobalt with other elements.

Inorganic compounds

Halides

Many halides of cobalt are known: cobalt fluoride which is a pink solid, cobalt chloride which is a blue solid, cobalt bromide which is a green solid, and cobalt iodide which is a blue-black solid. In addition to the anhydrous forms, these cobalt halides also have hydrates. Anhydrous cobalt chloride is blue, while the hexahydrate is magenta in colour. Because cobalt chloride changes color upon hydration, it can be used to manufacture color-changing silica gel.
Anhydrous cobalt halides react with nitric oxide at 70~120 °C to generate ₂. The complex of cobalt halides and triethylphosphine can absorb nitric monoxide in benzene to form the diamagnetic material CoX₂
In the reaction + e⁻ →, the potential is +1.92 V, which is higher than that of Cl₂ to Cl⁻. Therefore, the interaction of Co³⁺ with Cl− produces Co²⁺ and releases chlorine gas. The potential from F₂ to F⁻ is as high as +2.87 V, and cobalt fluoride can exist stably. It is a fluorinated reagent and reacts violently with water.

Oxides and hydroxides

Cobalt can form various oxides, such as CoO, Co₂O₃ and Co₃O₄. Co₃O₄, at 950 °C, decomposes to CoO.
Soluble cobalt salts react with sodium hydroxide to obtain cobalt hydroxide :
Cobalt hydroxide can be oxidized to the Co compound CoO under alkaline conditions.

Pnictogenides

Cobalt powder reacts with ammonia to form two kinds of nitrides, Co₂N and Co₃N. Cobalt reacts with phosphorus or arsenic to form Co₂P, CoP, CoP₂, CoAs₂ and other substances. The former three compounds are of interest as catalysts for water electrolysis.
Cobalt azide is another binary compound of cobalt and nitrogen that can explode when heated. Cobalt and azide can form complexes. Cobalt pentazolide Co₂ was discovered in 2017, and it exists in the form of the hydrate ·4H₂O. It decomposes at 50~145 °C to form cobalt azide, becoming anhydrous and releasing nitrogen, and exploding when heated further. This compound can be obtained by reacting ₆₃₄Cl or Na]·2H₂O and cobalt nitrate|₂ at room temperature. Hydrogen bonding of water stabilizes this molecule.
Cobalt can easily react with nitric acid to form cobalt nitrate Co₂. Cobalt nitrate exists in the anhydrous form and the hydrate form, of which the hexahydrate is the most common. Cobalt nitrate hexahydrate is a red deliquescent crystal that is easily soluble in water, and its molecule contains cobalt hydrated ions and free nitrate ions. It can be obtained by precipitation from solution.

Coordination compounds

As for all metals, molecular compounds and polyatomic ions of cobalt are classified as coordination complexes, that is, molecules or ions that contain cobalt linked to one or more ligands. These can be combinations of a potentially infinite variety of molecules and ions, such as:

water, as in the cation hexaaquocobalt. This pink-colored complex is the predominant cation in solid cobalt sulfate ·_x, with x = 6 or 7, as well as in water solutions thereof.
ammonia, as in cis-diaquotetraamminecobalt, in hexol, in , and in.
carbonate, as in the green triscarbonatocobaltate anion.
nitrite as in.
hydroxide, as in hexol.
chloride, as in tetrachloridocobaltate.
bicarbonate, as in.
oxalate, as in trisoxalatocobaltate.

These attached groups affect the stability of oxidation states of the cobalt atoms, according to general principles of electronegativity and of the hardness–softness. For example, Co³⁺ complexes tend to have ammine ligands. Because phosphorus is softer than nitrogen, phosphine ligands tend to feature the softer Co²⁺ and Co⁺, an example being triscobalt chloride. The more electronegative oxide and fluoride can stabilize Co⁴⁺ and Co⁵⁺ derivatives, e.g. caesium hexafluorocobaltate and potassium percobaltate.
Alfred Werner, a Nobel-prize winning pioneer in coordination chemistry, worked with compounds of empirical formula. One of the isomers determined was cobalt hexammine chloride. This coordination complex, a typical Werner-type complex, consists of a central cobalt atom coordinated by six ammine orthogonal ligands and three chloride counteranions. Using chelating ethylenediamine ligands in place of ammonia gives triscobalt, which was one of the first coordination complexes to be resolved into optical isomers. The complex exists in the right- and left-handed forms of a "three-bladed propeller". This complex was first isolated by Werner as yellow-gold needle-like crystals.

Organic compounds

is a cobalt-centered organic biomolecule, soluble in water, and involved in the methylation and synthesis of nucleic acid and neurotransmitter. The main source is the offal or meat of herbivorous animals.
Dicobalt octacarbonyl is an orange-red crystal with two isomers in solution:
It reacts with hydrogen or sodium to form HCo₄ or NaCo₄. It is a catalyst in carbonylation and hydrosilylation reactions.
Cobaltocene is a cyclopentadiene complex of cobalt. It has 19 valence electrons and is easily oxidized to with a stable structure of 18 electrons by reaction. It is a structural analog to ferrocene, with cobalt in place of iron. Cobaltocene is much more sensitive to oxidation than ferrocene.