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Hexamminecobalt(III) chloride

Hexaamminecobalt(III) chloride
chloride
Hexamminecobalt(III)Chloride.jpg
Names
IUPAC name
Hexaamminecobalt(III) chloride
Other names
Cobalt hexammine chloride, hexaamminecobalt(III) chloride
Identifiers
ECHA InfoCard 100.030.991
UNII
Properties
H18N6Cl3Co
Molar mass 267.48 g/mol
Appearance yellow or orange crystals
Density 1.71 g/cm3,
Melting point decomposes
0.26 M (20 °C)
tribromide: 0.04 M (18 °C)
Solubility soluble in NH3
Structure
octahedral
0 D
Hazards
Main hazards poison
R-phrases (outdated) 36/37/38
S-phrases (outdated) none
Related compounds
Other anions
[Co(NH3)6]Br3
[Co(NH3)6](OAc)3
Other cations
[Cr(NH3)6]Cl3
[Ni(NH3)6]Cl2
Related compounds
[Co(H2NCH2CH2NH2)3]Cl3

[Co(NH3)5(H2O)]Cl3
[Co(NH3)5Cl]Cl2

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N  (what is YesYN ?)
Infobox references

[Co(NH3)5(H2O)]Cl3
[Co(NH3)5Cl]Cl2

Hexaamminecobalt(III) chloride is the chemical compound with the formula [Co(NH3)6]Cl3. This coordination compound is considered an archetypal "Werner complex", named after the pioneer of coordination chemistry, Alfred Werner. This salt consists of [Co(NH3)6]3+cations, each accompanied by three Cl anions. The cation itself is a metal ammine complex with six ammonia molecules as ligands on the cobalt atom.

Originally this compound was described as the luteo (Latin: yellow) complex of cobalt, but this name has been discarded as modern chemistry considers color less important than molecular structure. Other similar complexes also had color names, such as purpureo (Latin: purple) for a pentammine complex, and praseo (Greek: green) and violeo (Latin: violet) for two isomeric tetrammine complexes.

[Co(NH3)6]3+ is diamagnetic, with a low-spin 3d6octahedral Co(III) center. The cation obeys the 18-electron rule and is considered to be a classic example of an exchange inert metal complex. As a manifestation of its inertness, [Co(NH3)6]Cl3 can be recrystallized unchanged from concentrated hydrochloric acid: the NH3 is so tightly bound to the Co(III) centers that it does not dissociate to allow its protonation. In contrast, labile metal ammine complexes, such as [Ni(NH3)6]Cl2, react rapidly with acids reflecting the lability of the Ni(II)–NH3 bonds. Upon heating, hexamminecobalt(III) begins to lose some of its ammine ligands, eventually producing a stronger oxidant.

The chloride ions in [Co(NH3)6]Cl3 can be exchanged with a variety of other anions such as nitrate, bromide, and iodide to afford the corresponding [Co(NH3)6]X3 derivative. Such salts are bright yellow and display varying degrees of water solubility.


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