Cobalt compounds explained

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

Inorganic compounds

Halides

Many halides of cobalt(II) are known.e cobalt(II) fluoride (CoF₂) which is a pink solid, cobalt(II) chloride (CoCl₂) which is a blue solid, cobalt(II) bromide (CoBr₂) which is a green solid, and cobalt(II) iodide (CoI₂) which is a blue-black solid. In addition to the anhydrous forms, these cobalt halides also have hydrates. Anhydrous cobalt(II) chloride is blue, while the hexahydrate is red-purple. Because the color change of cobalt(II) chloride in different hydrates, it can be used to manufacture color-changing silica gel.

Anhydrous cobalt halides react with nitric oxide at 70~120 °C to generate [Co(NO)₂X]₂ (X = Cl, Br or I). The complex of cobalt halides and triethylphosphine ((C₂H₅)₃P) can absorb nitric monoxide in benzene to form the diamagnetic material Co(NO)X₂(P(C₂H₅)₃)^[1]

In the reaction + e⁻ →, the potential is +1.92 V, which is higher than that of Cl₂ to Cl⁻ (+1.36 V). 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(III) fluoride (CoF₃) can exist stably. It is a fluorinated reagent and reacts violently with water.^[2]

Oxides and hydroxides

Cobalt can form various oxides, such as CoO, Co₂O₃ and Co₃O₄. Co₃O₄, at 950 °C, decomposes to CoO.^[3]

Soluble cobalt salts react with sodium hydroxide to obtain cobalt(II) hydroxide (Co(OH)₂):^[4]

Co(NO₃)₂ + 2 NaOH → Co(OH)₂↓ + 2 NaNO₃

Cobalt(II) hydroxide can be oxidized to the Co(III) compound CoO(OH) 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,^[5] CoAs₂ and other substances. The former three compounds are of interest as catalysts for water electrolysis.^{[6] [7]}

Cobalt(II) azide (Co(N₃)₂) is another binary compound of cobalt and nitrogen that can explode when heated. Cobalt(II) and azide can form complexes.^[8] Cobalt pentazolide Co(N₅)₂ was discovered in 2017, and it exists in the form of the hydrate [Co(H₂O)₄(N₅)₂]·4H₂O. It decomposes at 50~145 °C to form cobalt(II) azide, becoming anhydrous and releasing nitrogen, and exploding when heated further. This compound can be obtained by reacting (N₅)₆(H₃O)₃(NH₄)₄Cl^[9] or Na(H₂O)(N₅)]·2H₂O^[10] and [Co(H₂O)₆](NO₃)₂ at room temperature. Hydrogen bonding of water stabilizes this molecule.

Cobalt can easily react with nitric acid to form cobalt(II) nitrate Co(NO₃)₂. Cobalt(II) nitrate exists in the anhydrous form and the hydrate form, of which the hexahydrate is the most common. Cobalt nitrate hexahydrate (Co(NO₃)₂·6H₂O) is a red deliquescence crystal that is easily soluble in water,^[11] and its molecule contains cobalt(II) hydrated ions ([Co(H₂O)₆]²⁺) and free nitrate ions.^[12] 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(II) . 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(III), in hexol, in (the anion of Erdmann's salt),^[13] and in .^[13]
• carbonate, as in the green triscarbonatocobaltate(III) anion.^{[14] [13] [15]}
• nitrite as in .^[13]
• hydroxide, as in hexol.
• chloride, as in tetrachloridocobaltate(II) .
• bicarbonate, as in .^[13]
• oxalate, as in trisoxalatocobaltate(III) .^[13]

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 tris(triphenylphosphine)cobalt(I) chloride . The more electronegative (and harder) oxide and fluoride can stabilize Co⁴⁺ and Co⁵⁺ derivatives, e.g. caesium hexafluorocobaltate(IV) (Cs₂CoF₆) and potassium percobaltate (K₃CoO₄).^[16]

Alfred Werner, a Nobel-prize winning pioneer in coordination chemistry, worked with compounds of empirical formula . One of the isomers determined was cobalt(III) 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 tris(ethylenediamine)cobalt(III), 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.^{[17] [18]}

Organic compounds

See main article: article and Organocobalt chemistry. Vitamin B12 is a cobalt-centered organic biomolecule, soluble in water, and involved in the methylation and synthesis of nucleic acid and neurotransmitter.^[19] The main source is the offal or meat of herbivorous animals.^[20]

Dicobalt octacarbonyl (Co₂(CO)₈) is an orange-red crystal with two isomers in solution:^[21]

It reacts with hydrogen or sodium to form HCo(CO)₄ or NaCo(CO)₄. It is a catalyst in carbonylation and hydrosilylation reactions.^[22]

Cobaltocene (Co(C₅H₅)₂) 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.^[23] It is a structural analog to ferrocene, with cobalt in place of iron. Cobaltocene is much more sensitive to oxidation than ferrocene.^[24]

See also

• Iron compounds
• Nickel compounds
• Rhodium compounds

Notes and References

1. 申泮文 等. 无机化学丛书 第九卷 锰分族 铁系 铂系. 科学出版社, 2017. ISBN 9787030305459
2. Holleman, A. F.; Wiberg, E.; Wiberg, N. (2007). "Cobalt". Lehrbuch der Anorganischen Chemie (in German) (102nd ed.). de Gruyter. pp. 1146–1152. ISBN 978-3-11-017770-1.
3. https://worldwide.espacenet.com/textdoc?DB=EPODOC&IDX=US4389339 US 4389339
4. O. Glemser "Cobalt(II) Hydroxide" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 1521.
5. Journal of Materials Chemistry A. Royal Society of Chemistry. Recent advances in cobalt phosphide based materials for energy-related applications. Jianmei Wang. Zhen Liu. Yiwei Zheng. Liang Cui. Wenrong Yang. Jingquan Liu. 22 September 2017. 19 October 2017. 10.1039/c7ta08386f. 5. 44 . 22913–22932.
6. Angewandte Chemie International Edition. 53. 21. May 19, 2014. 5427–5430. Highly Active Electrocatalysis of the Hydrogen Evolution Reaction by Cobalt Phosphide Nanoparticles. Eric J.. Popczun. Carlos G.. Read. Christopher W.. Roske. Nathan S.. Lewis. Raymond E.. Schaak. 11 April 2014. 10.1002/anie.201402646. 24729482 .
7. Synthesis and X‑ray Characterization of Cobalt Phosphide (Co₂P) Nanorods for the Oxygen Reduction Reaction. ACS Nano. Vicky V. T.. Doan-Nguyen. Sen Zhang. Edward B.. Trigg. Rahul. Agarwal. Jing Li. Dong Su. Karen I.. Winey. Christopher B.. Murray. April 13, 2015. July 14, 2015. 9 . 8 . 8108–8115 . 10.1021/acsnano.5b02191. 26171574 . 1213384 .
8. 10.1021/ja01525a020 . On the Reaction between Cobalt(II) and Azide Ions in Aqueous and Aqueous-organic Solutions¹ . 1959 . Senise . Paschoal . Journal of the American Chemical Society . 81 . 16 . 4196–4199 .
9. 10.1002/anie.201701070 . A Symmetric Co(N₅)₂ (H₂ O)₄ ⋅4 H₂ O High-Nitrogen Compound Formed by Cobalt(II) Cation Trapping of a Cyclo-N₅ ⁻ Anion . 2017 . Zhang . Chong . Yang . Chen . Hu . Bingcheng . Yu . Chuanming . Zheng . Zhansheng . Sun . Chengguo . Angewandte Chemie International Edition . 56 . 16 . 4512–4514 . 28328154 .
10. 10.1038/nature23662 . A series of energetic metal pentazolate hydrates . 2017 . Xu . Yuangang . Wang . Qian . Shen . Cheng . Lin . Qiuhan . Wang . Pengcheng . Lu . Ming . Nature . 549 . 7670 . 78–81 . 28847006 . 2017Natur.549...78X . 4459874 .
11. Book: 10.1002/14356007.a07_281.pub2 . Cobalt and Cobalt Compounds . Ullmann's Encyclopedia of Industrial Chemistry . 2005 . Donaldson . John Dallas . Beyersmann . Detmar . 9783527303854 .
12. Prelesnik, P. V.; Gabela, F.; Ribar, B.; Krstanovic, I. (1973). "Hexaaquacobalt(II) nitrate". Cryst. Struct. Commun. 2 (4): 581–583.
13. 10.1021/ja01104a019 . Complex Acids of Cobalt and Chromium. The Green Carbonatocobalt(III) Anion^* . 1953 . McCutcheon . Thomas P. . Schuele . William J. . Journal of the American Chemical Society . 75 . 8 . 1845–1846 .
14. 10.1021/ja01504a004 . A General Synthesis of Cobalt(III) Complexes; A New Intermediate, Na₃[Co(CO₃)₃]·3H₂O . 1960 . Bauer . H. F. . Drinkard . W. C. . Journal of the American Chemical Society . 82 . 19 . 5031–5032 .
15. 10.1007/s10973-009-0606-2 . Determination of the structural formula of sodium tris-carbonatocobaltate(III), Na3[Co(CO3)3]·3H2O by thermogravimetry . 2010 . Tafesse . Fikru . Aphane . Elias . Mongadi . Elizabeth . Journal of Thermal Analysis and Calorimetry . 102 . 91–97 . 97142236 .
16. Book: Holleman, A. F.. Wiberg, E.. Wiberg, N.. Lehrbuch der Anorganischen Chemie. 102nd. de Gruyter. 2007. de. 978-3-11-017770-1. 1146–1152. Cobalt.
17. Werner, A. . Zur Kenntnis des asymmetrischen Kobaltatoms. V. Chemische Berichte. 1912. 45. 121–130. 10.1002/cber.19120450116.
18. Book: https://books.google.com/books?id=9d893122U6kC&pg=PR31. 31–33. Early Theories of Coordination Chemistry. Coordination chemistry. 978-3-527-31802-5. Gispert, Joan Ribas. 2008. Wiley . 2015-06-27. 2016-05-05. https://web.archive.org/web/20160505203708/https://books.google.com/books?id=9d893122U6kC&pg=PR31. dead.
19. 10.1016/j.jns.2005.03.009 . Vitamin B12, demyelination, remyelination and repair in multiple sclerosis . 2005 . Miller . Ariel . Korem . Maya . Almog . Ronit . Galboiz . Yanina . Journal of the Neurological Sciences . 233 . 1–2 . 93–97 . 15896807 . 6269094 .
20. 陈辉．现代营养学．北京：化学工业出版社，2005：76
21. 10.1021/ic50168a037 . Infrared spectra of matrix-isolated dicobalt octacarbonyl. Evidence for the third isomer . 1977 . Sweany . Ray L. . Brown . Theodore L. . Inorganic Chemistry . 16 . 2 . 415–421 .
22. Book: Charles M. Starks. Charles Leonard Liotta. Marc Halpern. Phase-transfer catalysis: fundamentals, applications, and industrial perspectives. 2011-05-16 . 1994. Springer. 978-0-412-04071-9. 600–.
23. 10.1021/cr940053x . Chemical Redox Agents for Organometallic Chemistry . 1996 . Connelly . Neil G. . Geiger . William E. . Chemical Reviews . 96 . 2 . 877–910 . 11848774 .
24. Book: James E. House. Inorganic chemistry. 2011-05-16 . 2008 . Academic Press . 978-0-12-356786-4 . 767–.