kazaa81 - 15-7-2005 at 12:57
Hallo to all,
for producing metallic nitrides, the process is something like:
- get a metal salt and reduce to the Me oxide
-put the MeOxide in conc. NH3 (aq).
Now, to what metals can this process applied? And how reduce the metal salt (ex. AlCl3, Al2(SO4)3....) to the Me oxide?
Thanks for info.!
Help needed.....
kazaa81 - 27-7-2005 at 12:57
Any ideas?
Madandcrazy - 4-8-2005 at 07:08
Me Oxide ?
You mean the way back than usual when
the oxigen ion is bounded to a salt ion 
to get a -OH group ?
(murexide)
Besides the Me Oxide is oxidized to mononitromethane.
(CH3NO2)
Me oxide
kazaa81 - 6-8-2005 at 07:42
As Me oxide i would mean oxide of a metal, example Al2O3 (to get Al nitride), CuO (to get Cu nitride) etc...
Please post anything which helps to get metal nitrides.
Thanks at all for help!
12AX7 - 6-8-2005 at 08:36
Reactive metals such as Al, Mg etc. are best burned with N2, IIRC. I would suppose you could start with oxides and ammonia, as Al2O3 + 2NH3 = 2AlN +
3H2O, as well. I doubt either works at a particularly low temperature. These can't be prepared from water sol'n since they hydrolyze.
Transition metal nitrides tend to be made by reduction in an ammonia solution, such as the silver mirroring process, when it goes wrong and produces
fulminating silver.
Tim
.
kazaa81 - 6-8-2005 at 10:10
By mixing an AlCl3 solution with a NH3 solution I get a gel....is it Al(OH)3?
Calcification (or dryness) of it would produce Al2O3?
What metal nitrides decompose with water? Would NH3 in benzine resolve the problem of nitrides decompositoon with water?
Please post anything which help!
Thanks at all for help!
12AX7 - 6-8-2005 at 13:04
Probably alumina hydrate, presuming your solution was NH4OH. That would leave NH4Cl solution. just ions, no action on the ammonia.
I somehow doubt benzene would work very well, are the reactants even particularly soluble in it?
Look at MSDS's or a chemical data book to see what nitrides are reactive.
Tim
kazaa81 - 7-8-2005 at 08:39
Unfortunately, I can't get other solvents now.....what about moving to others nitrides? Please post anything, links, documents and
firstly.....ideas!
Thanks at all for help!
Some nitrides infos....
kazaa81 - 8-10-2005 at 06:46
Aluminum Nitride
Formula: AlN
CAS # 24304-00-5
Density: 3,26
Solubility: decomposition in H2O
M.P 2200°C
B.P 2517°C
Some reactions it does:
AlN + 3 NaOH ---> NH3 + Na2AlO3
2 AlN + H2SO4 + 6 H2O ---> 2 Al(OH)3 + (NH4)2SO4
Making AlN from aqueous NH3 is not possible, because AlN decomposes in water....so I will try to make a solution of NH3 in petroleum ether.
Al2O3 + 2 NH3 ---> 2 AlN + 3 H2O
2 AlN + 3 H2O ---> 2 NH3 + Al2O3
Because of these 2 opposed reactions, I think which Al2O3 + NH3 would make an equilibrium:
Al2O3 + 2 NH3 <---> 2 AlN + 3 H2O
or am I wrong?
Al2O3 would be suitable to produce Al4C3 (aluminum carbide), an interesting compound which gives CH4 (methane) with water?
If anyone have informations or ideas about producing metal nitride (excluded burning metals in N2 atmosphere), please post!
praseodym - 8-10-2005 at 07:57
The only reaction of gaseous nitrogen at room temperature to form a nitride is with lithium, forming lithium nitride.
I was just wondering if it would be possible to form nitrides using hydrazoic acid.
kazaa81 - 8-10-2005 at 08:09
I was not thinking to make nitrides by burning metals or reacting them with N2 (which is stable), but to put a metal oxide in conc. NH3 (ammonia)
solution.
With hydrazoic acid (it can be made from hydrazine and H2O2 or HNO2, but I've never tried) you will get only azides, not nitrides (also...Pb
azide by reaction of Pb salts with hydrazoic acid is risky because of the formations of large crystals).
Post any idea and/or informations!