Hi,
I wonder if someone can help me get a synthesis description for Ni(NH3)6(NO3)2 in inorganic chemistry and where I can find other synthesis descriptions online or books.
I can't understand your problem. What about your literature survey ? I will help you, If you tell me clearly. Email id : [email protected]
It is not possible to synthesize Ni(NH3)6(NO3)2 . The highest number of coordination of Ni(II) is 6. If it is possible to synthesize Ni(NH3)4(NO3)2. See the article Y. R. Laskar et al. New J. Chem, 2001, 25, 764.
Herman Jimenez is right, but the synthesis may still be possible, and easy. I mean clathrates, that is non-stoichiometric inclusion compounds, where additional molecules are loosely encaged in the crystal's structure of the complex. I have long experience with similar, nickel-based ammine complexes (gamma-methylpyridine ones), and I know for fact that nickel-ammonia complexes form clathrates, too. The synthesis of those ammine complexes is simple: mix the nickel-salt solution with the ammine, and a thick blue sedimentation is produced. Ammonia should be added in some excess over the number of 4, but a large excess of ammonia may dissolve the solid back, so not too much. Decant, rinse with water and dry on filter paper. I can expand on clathrates.
If what you are looking for is [Ni(NH3)6](NO3)2 then you can probably adapt this procedure, substituting nickel nitrate for the nickel chloride starting material.
http://alpha.chem.umb.edu/chemistry/ch118/documents/HexamminenickelChlorideSynthesis.pdf
An addition to my previous comment: Since the original question was about the [Ni(NH3)6](NO3)2 then I did not say, what may be of interest, that the compounds of that kind that are best for clathrating, are Ni(SCN)2 -(gamma-methylpypidine)4 complex, Pyridines smell really badly, but they are not as harmful as they smell. Even for us, educated chemists, it is difficult to resist the misleading connection between appearances and facts.
Hello,
you can make [Ni(NH3)6](NO3)2 with nickel nitrate and ammonia. Have you done a scifinder search (if you don't use scifinder, I highly recommend you learn how to use it for your research, its a great tool)? There are over 100 references covering that compound.
\The crystal structure has also been solved. You can use the CSD to find the structure and then use that to find papers on the compound.
One paper that covers its synthesis is Green Chem, 2002, v4, p71. If you look at the footnote, you will see they bubbled NH3 through a methanolic solution of Ni(NO3)2 to obtain crystals of the compound.
-Kyle Grice
Nickel chemistry is dominated by four coordinate nickel. Pushing the NO3- to the outer sphere, the LIKELY compound is Ni(NH3)4(NO3)2
I don't think so, Scott. Hexamminenickel chloride is easy to make (my first-year undergraduates do it every year), as is tris(ethylenediamine)nickel chloride.
I stand corrected (as evidenced by attached absract). The hydrogen bonding in the lattice is definitely fair game. It does sound like the complex is more loosely bound axially than equatorially though, so that lets me save at least a little face.
- Badges
- Science topic
- Similar topics
- Chemistry
- Sulfites
- Inorganic Chemistry
- Inorganic Chemicals