Summary
Cobalt(III) nitrate is an inorganic compound with the chemical formula Co(NO3)3.[1] It is a green, diamagnetic solid that sublimes at ambient temperature.[2]
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| IUPAC name
Cobalt(III) nitrate
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3D model (JSmol)
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| ECHA InfoCard | 100.290.572 |
PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| Co(NO3)3 | |
| Molar mass | 244.96 g/mol |
| Appearance | green crystals hygroscopic |
| Density | 2.49 g/cm3 |
| 5.07 g/100 mL | |
| Structure | |
| cubic | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references
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StructureEdit
The compound is a molecular coordination complex. The three bidentate nitrate ligands give a distorted octahedral arrangement.[3] The nitrate ligands are planar. With D3 symmetry, the molecule is chiral. The Co-O bond lengths are about 190 pm long. The O-Co-O angles for the two oxygens in the same nitrate is about 68 degrees.[4] The same geometry seems to persist in carbon tetrachloride solution.[3]
Preparation and reactionsEdit
Cobalt(III) nitrate can be prepared by the reaction of dinitrogen pentoxide N
2O
5 with cobalt(III) fluoride CoF
3.[3] It can be purified by vacuum sublimation at 40 °C.[4][2]
Cobalt(III) nitrate oxidizes water, the initial green solution rapidly turns pink, with formation of cobalt(II) ions and release of oxygen.[1] Cobalt(III) nitrate can be intercalated in graphite, in the ratio of 1 molecule for each 12 carbon atoms.[2]
See alsoEdit
ReferencesEdit
- ^ a b W. Levason and C. A. McAuliffe (1974): "Higher oxidation state chemistry of iron, cobalt, and nickel". Coordination Chemistry Reviews, volume 12, issue 2, pages 151-184. doi:10.1016/S0010-8545(00)82026-3
- ^ a b c E. Stumpp, G. Nietfeld, K. Steinwede, and K. D. Wageringel (1983) "Reaction of anhydrous metal nitrates with graphite". Synthetic Metals, Evolume 7, issues 1–2, pages 143-151. doi:10.1016/0379-6779(83)90097-8
- ^ a b c R. J. Fereday, N. Logan and D. Sutton (1969): "Anhydrous cobalt(III) nitrate: preparation, spectra, and reactions with some organic ligands". Journal of the Chemical Society A: Inorganic, Physical, Theoretical, volume 1969, issue 0, pages 2699-2703. doi:10.1039/J19690002699
- ^ a b J. Hilton and S. C. Wallwork (1968): "The crystal structure of cobalt(III) nitrate", Chemical Communications, volume 1968, issue 15, pages 871-871. doi:10.1039/C19680000871
| HNO3 | He | ||||||||||||||||
| LiNO3 | Be(NO3)2 | B(NO 3)− 4 |
RONO2 | NO− 3 NH4NO3 |
HOONO2 | FNO3 | Ne | ||||||||||
| NaNO3 | Mg(NO3)2 | Al(NO3)3 | Si | P | S | ClONO2 | Ar | ||||||||||
| KNO3 | Ca(NO3)2 | Sc(NO3)3 | Ti(NO3)4 | VO(NO3)3 | Cr(NO3)3 | Mn(NO3)2 | Fe(NO3)2 Fe(NO3)3 |
Co(NO3)2 Co(NO3)3 |
Ni(NO3)2 | CuNO3 Cu(NO3)2 |
Zn(NO3)2 | Ga(NO3)3 | Ge | As | Se | BrNO3 | Kr |
| RbNO3 | Sr(NO3)2 | Y(NO3)3 | Zr(NO3)4 | Nb | Mo | Tc | Ru(NO3)3 | Rh(NO3)3 | Pd(NO3)2 Pd(NO3)4 |
AgNO3 Ag(NO3)2 |
Cd(NO3)2 | In(NO3)3 | Sn(NO3)4 | Sb(NO3)3 | Te | INO3 | Xe(NO3)2 |
| CsNO3 | Ba(NO3)2 | Hf(NO3)4 | Ta | W | Re | Os | Ir | Pt(NO3)2 Pt(NO3)4 |
Au(NO3)3 | Hg2(NO3)2 Hg(NO3)2 |
TlNO3 Tl(NO3)3 |
Pb(NO3)2 | Bi(NO3)3 BiO(NO3) |
Po(NO3)4 | At | Rn | |
| FrNO3 | Ra(NO3)2 | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | |
| ↓ | |||||||||||||||||
| La(NO3)3 | Ce(NO3)3 Ce(NO3)4 |
Pr(NO3)3 | Nd(NO3)3 | Pm(NO3)3 | Sm(NO3)3 | Eu(NO3)3 | Gd(NO3)3 | Tb(NO3)3 | Dy(NO3)3 | Ho(NO3)3 | Er(NO3)3 | Tm(NO3)3 | Yb(NO3)3 | Lu(NO3)3 | |||
| Ac(NO3)3 | Th(NO3)4 | PaO2(NO3)3 | UO2(NO3)2 | Np(NO3)4 | Pu(NO3)4 | Am(NO3)3 | Cm(NO3)3 | Bk(NO3)3 | Cf | Es | Fm | Md | No | Lr | |||