Cobalt(II) hydroxide

Cobalt(II) hydroxide

cobalt(II) hydroxide
Names
IUPAC name
Cobalt(II) hydroxide
Other names
Cobaltous hydroxide, cobalt hydroxide, β-cobalt(II) hydroxide
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.040.136 Edit this at Wikidata
EC Number
  • 244-166-4
UNII
UN number 3550
  • InChI=1S/Co.2H2O/h;2*1H2/q+2;;/p-2 checkY
    Key: ASKVAEGIVYSGNY-UHFFFAOYSA-L checkY
  • InChI=1/Co.2H2O/h;2*1H2/q+2;;/p-2
    Key: ASKVAEGIVYSGNY-NUQVWONBAS
  • [Co+2].[OH-].[OH-]
Properties
Co(OH)2
Molar mass 92.948 g/mol
Appearance rose-red powder or bluish-green powder
Density 3.597 g/cm3
Melting point 168 °C (334 °F; 441 K) (decomposes)[1]
3.20 mg/L
1.0×10−15
Solubility soluble in acids, ammonia; insoluble in dilute alkalis
Structure
rhombohedral
Thermochemistry
79.0 J·mol−1·K−1[1]
-539.7 kJ·mol−1
Hazards
GHS labelling:
GHS06: ToxicGHS07: Exclamation markGHS08: Health hazardGHS09: Environmental hazard
Warning
H302, H317, H319, H330, H334, H360, H372
P201, P202, P260, P261, P264, P270, P271, P272, P280, P281, P284, P285, P301+P312, P302+P352, P304+P340, P304+P341, P305+P351+P338, P308+P313, P310, P314, P320, P321, P330, P333+P313, P337+P313, P342+P311, P363, P403+P233, P405, P501
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 0: Will not burn. E.g. waterInstability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazards (white): no code
1
0
2
Safety data sheet (SDS) Oxford University
Related compounds
Other anions
 Cobalt(II) chloride
Cobalt(II) bromide
Cobalt(II) iodide
Other cations
 Iron(II) hydroxide
Nickel(II) hydroxide
Copper(II) hydroxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY verify (what is checkY☒N ?)

Cobalt(II) hydroxide or cobaltous hydroxide is the inorganic compound with the formula Co(OH)
2, consisting of divalent cobalt cations Co2+
 and hydroxide anions OH−
. The pure compound, often called the "beta form" (β-Co(OH)
2) is a pink solid insoluble in water.[2][3]

The name is also applied to a related compound, often called "alpha" or "blue" form (α-Co(OH)
2), which incorporates other anions in its molecular structure. This compound is blue and rather unstable.[2][3]

Cobalt(II) hydroxide is most used as a drying agent for paints, varnishes, and inks, in the preparation of other cobalt compounds, as a catalyst and in the manufacture of battery electrodes.

Preparation

Cobalt(II) hydroxide precipitates as a solid when an alkali metal hydroxide is added to an aqueous solution of Co2+ salt.[4] For example,

Co2+ + 2 NaOH → Co(OH)2 + 2 Na+

The compound can be prepared by reacting cobalt(II) nitrate in water with a solution of triethylamine N(C
2H
5)
3 as both the base and a complexing agent.[3] It can also be prepared by elecrolysis of a solution of cobalt nitrate with a platinum cathode.[5]

Reactions

Cobalt(II) hydroxide decomposes to cobalt(II) oxide at 168 °C under vacuum and is oxidized by air.[4] The thermal decomposition product in air above 300 °C is Co3O4.[6][7]

Like iron(II) hydroxide, cobalt(II) hydroxide is a basic hydroxide, and reacts with acids to form cobalt(II) salts. It also reacts with strong bases to form solutions with dark blue cobaltate(II) anions, [Co(OH)4]2− and [Co(OH)6]4−.[8]

Structure

The (β) form of cobalt(II) hydroxide has the brucite crystal structure, i.e. the arrangement of the atoms in the crystal are the same as the arrangement of the atoms in Mg(OH)2. The Co(II) centers are bonded to six hydroxide ligands. Each hydroxide ligand bridges to three Co(II) sites. The O-H bonds are perpendicular to the planes defined by the oxygen atoms, projecting above and below these layers.[9] Ignoring the H atoms, the packing of the anion and cations is also described as the cadmium iodide structure, in which the cobalt(II) cations have octahedral molecular geometry.[8]

The beta form can be obtained as platelets with partial hexagonal geometry, 100-300 nm wide and 5-10 nm thick.[5][3]

Alpha Cobalt (II) Hydroxide

Alpha form

The so-called "alpha form" (α-Co(OH)2) is not a polymorph of the pure (β) form, but rather a more complex compound in which hydroxide-cobalt-hydroxide layers have a residual positive charge and alternate with layers of other anions such as nitrate, carbonate, chloride, etc. (the hydrotalcite structure).[3] It is usually obtained as a blue precipitate when a base like sodium hydroxide is added to a solution of a cobalt(II) salt. The precipitate slowly converts to the beta form.[10]

Nanotubes

Cobalt hydroxide can be obtained in the form of nanotubes, which may be of interest in nanotechnology and materials science. [11]

Cobalt hydroxide nanotubes. Scale bars: (a,b) 500 nm, inset 200  nm; (c,e) 50 nm; (d) 100  nm.

References

Wikimedia Commons has media related to Cobalt(II) hydroxide.
  1. ^ a b Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, Florida: CRC Press. p. 513. ISBN 0-8493-0594-2.
  2. ^ a b Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, Florida: CRC Press. p. 454. ISBN 0-8493-0594-2.
  3. ^ a b c d e Xiaohe Liu, Ran Yi, Ning Zhang, Rongrong Shi, Xingguo Li, and Guanzhou Qiu (2008): "Cobalt hydroxide nanosheets and their thermal decomposition to cobalt oxide nanorings". Chemistry: An Asian Journal, volume 3, issue 4, pages 732-738. doi:10.1002/asia.200700264
  4. ^ a b 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. ^ a b P. Benson, G. W. D. Briggs, and W. F. K. Wynne-Jones (1964): "The cobalt hydroxide electrode—I. Structure and phase transitions of the hydroxides". Electrochimica Acta, volume 9, issue 3, pages 275-280. doi:10.1016/0013-4686(64)80016-5
  6. ^ Jayashree, R. S.; Kamath, P. Vishnu (1999). "Electrochemical synthesis of a-cobalt hydroxide". Journal of Materials Chemistry. 9 (4): 961–963. doi:10.1039/A807000H.
  7. ^ Xu, Z. P.; Zeng, H. C. (1998). "Thermal evolution of cobalt hydroxides: a comparative study of their various structural phases". Journal of Materials Chemistry. 8 (11): 2499–2506. doi:10.1039/A804767G.
  8. ^ a b Wiberg, Nils; Wiberg, Egon; Holleman, A. F. (2001). Inorganic Chemistry. Academic Press. pp. 1478–1479. ISBN 0-12-352651-5. Retrieved 2009-03-27.
  9. ^ Lutz, H.D.; Möller, H.; Schmidt, M. (1994). "Lattice vibration spectra. Part LXXXII. Brucite-type hydroxides M(OH)2 (M = Ca, Mn, Co, Fe, Cd) — IR and Raman spectra, neutron diffraction of Fe(OH)2". Journal of Molecular Structure. 328: 121–132. doi:10.1016/0022-2860(94)08355-x.
  10. ^ Liu, Zhaoping; Ma, Renzhi; Osada, Minoru; Takada, Kazunori; Sasaki, Takayoshi (2005). "Selective and Controlled Synthesis of α- and β-Cobalt Hydroxides in Highly Developed Hexagonal Platelets". Journal of the American Chemical Society. 127 (40): 13869–13874. doi:10.1021/ja0523338. PMID 16201808.
  11. ^ Ni, Bing; Liu, Huiling; Wang, Peng-Peng; He, Jie; Wang, Xun (2015). "General synthesis of inorganic single-walled nanotubes". Nature Communications. 6: 8756. Bibcode:2015NatCo...6.8756N. doi:10.1038/ncomms9756. PMC 4640082. PMID 26510862.