Co No3 2 Compound Name
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| Other names Cobaltous nitrate | |
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| ECHA InfoCard | 100.030.353 |
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| UN number | 1477 |
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| Chemical formula | Co(NO3)2(H2O)6 |
| Molar mass | 291.03 one thousand/mol (hexahydrate) 182.943 g/mol (anhydrous) |
| Appearance | pale red powder (anhydrous) red crystalline (hexahydrate) |
| Scent | odorless |
| Density | i.87 g/cmthree (hexahydrate) two.49 g/cm3 (anhydrous) |
| Melting point | 100 °C (212 °F; 373 K) decomposes (anhydrous) 55 °C (hexahydrate) |
| Boiling point | 100 to 105 °C (212 to 221 °F; 373 to 378 K) decomposes (anhydrous)[ citation needed ] 74 °C, decomposes (hexahydrate) |
| Solubility in h2o | anhydrous:[i] 84.03 g/100 mL (0 °C) 334.9 g/100 mL (90 °C) soluble (anhydrous) |
| Solubility | soluble in alcohol, acetone, ethanol, ammonia (hexahydrate), methanol 2.one g/100 mL |
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| Coordination geometry | monoclinic (hexahydrate) |
| Hazards | |
| GHS labelling: | |
| Pictograms |   |
| Signal word | Danger |
| Run a risk statements | H317, H334, H341, H350, H360, H410 |
| Precautionary statements | P201, P202, P261, P272, P273, P280, P281, P285, P302+P352, P304+P341, P308+P313, P321, P333+P313, P342+P311, P363, P391, P405, P501 |
| NFPA 704 (burn diamond) | 2 0 0 OX |
| Lethal dose or concentration (LD, LC): | |
| LDfifty (median dose) | 434 mg/kg; rat, oral (anhydrous) 691 mg/kg; rat, oral (hexahydrate) |
| Safety data sheet (SDS) | Cobalt (Two) Nitrate MSDS |
| Related compounds | |
| Other anions | Cobalt(II) sulfate Cobalt(Two) chloride Cobalt oxalate |
| Other cations | Fe(Three) nitrate Nickel(II) nitrate |
| Except where otherwise noted, information are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Infobox references | |
Cobalt nitrate is the inorganic compound with the formula Co(NO3)ii .xH2O. It is cobalt(Two)'s salt. The most mutual form is the hexahydrate Co(NOiii)2·6H2O, which is a red-brown deliquescent common salt that is soluble in water and other polar solvents.[2]
Composition and structures [edit]
Besides as the anhydrous compound Co(NO3)2, several hydrates of cobalt(II) nitrate be. These hydrates have the chemical formula Co(NOthree)2·nHtwoO, where n = 0, 2, 4, 6.
Anhydrous cobalt(2) nitrate adopts a three-dimensional polymeric network structure, with each cobalt(II) atom approximately octahedrally coordinated past half-dozen oxygen atoms, each from a different nitrate ion. Each nitrate ion coordinates to three cobalts.[3] The dihydrate is a 2-dimensional polymer, with nitrate bridges between Co(II) centres and hydrogen bonding property the layers together.[iv] The tetrahydrate consists of discrete, octahedral [(H2O)4Co(NO3)ii] molecules. The hexahydrate is improve described as hexaaquacobalt(II) nitrate, [Co(OH2)6][NO3]2, as it consists of discrete [Co(OHii)6]ii+ and [NO3]− ions.[5] Above 55 °C, the hexahydrate converts to the trihydrate and at higher temperatures to the monohydrate.[two]
Uses and reactions [edit]
Information technology is usually reduced to metal high purity cobalt.[2] It tin be absorbed on to various catalyst supports for use in Fischer–Tropsch catalysis.[half-dozen] It is used in the preparation of dyes and inks.[7]
Cobalt(II) nitrate is a common starting fabric for the preparation of coordination complexes such as cobaloximes,[eight] carbonatotetraamminecobalt(3),[ix] and others.[10]
Product [edit]
The hexahydrate is prepared treating metallic cobalt or 1 of its oxides, hydroxides, or carbonate with nitric acrid:
- Co + 4 HNO3 + 4 H2O → Co(HtwoO)6(NO3)2 + ii NO2
- CoO + two HNOthree + 5 H2O → Co(HiiO)half-dozen(NO3)two
- CoCO3 + 2 HNO3 + 5 H2O → Co(H2O)6(NO3)2 + CO2
References [edit]
- ^ Perrys' Chem Eng Handbook, 7th Ed
- ^ a b c John Dallas Donaldson, Detmar Beyersmann, "Cobalt and Cobalt Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2005. doi:10.1002/14356007.a07_281.pub2
- ^ Tikhomirov, G. A.; Znamenkov, G. O.; Morozov, I. V.; Kemnitz, E.; Troyanov, S. I. (2002). "Anhydrous Nitrates and Nitrosonium Nitratometallates of Manganese and Cobalt, M(NO3)2, NO[Mn(NO3)three], and (NO)2[Co(NO3)4]: Synthesis and Crystal Construction". Z. anorg. allg. Chem. 628 (i): 269–273. doi:10.1002/1521-3749(200201)628:ane<269::Assistance-ZAAC269>3.0.CO;2-P.
- ^ Ribár, B.; Milinski, N.; Herak, R.; Krstanovič, I.; Djurič, S. (1976). "The Crystal Structure of Cobalt Nitrate Dihydrate, Co(NO3)2·2H2O". Zeitschrift für Kristallographie. 144 (1–6): 133–138. Bibcode:1976ZK....144..133R. doi:10.1524/zkri.1976.144.1-half dozen.133.
- ^ Prelesnik, P. V.; Gabela, F.; Ribar, B.; Krstanovic, I. (1973). "Hexaaquacobalt(Ii) nitrate". Cryst. Struct. Commun. ii (4): 581–583.
- ^ Ernst B, Libs S, Chaumette P, Kiennemann A. Appl. Catal. A 186 (ane-2): 145-168 1999
- ^ Lewis, Richard J., Sr. (2002). Hawley'due south Condensed Chemic Lexicon (14th Edition). John Wiley & Sons. http://www.knovel.com/knovel2/Toc.jsp?BookID=704&VerticalID=0
- ^ Schrauzer, Thousand. N. (1968). Bis(Dimethylglyoximato)Cobalt Complexes: ("Cobaloximes"). Inorganic Syntheses. pp. 61–70. doi:10.1002/9780470132425.ch12. ISBN9780470132425.
- ^ Schlessinger, Thousand. (1960). "Carbonatotetramminecobalt(III) Nitrate". Inorganic Syntheses. 6: 173–175. doi:x.1002/9780470132371.ch55. ISBN9780470132371.
- ^ Hargens, Robert D.; Min, Woonza; Henney, Robert C. (1973). "Bis(ethylenediamine)sulfito Complexes of Cobalt(III)". Inorganic Syntheses. Inorganic Syntheses. pp. 77–81. doi:10.1002/9780470132456.ch15. ISBN9780470132456.
Co No3 2 Compound Name,
Source: https://en.wikipedia.org/wiki/Cobalt(II)_nitrate
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