For the synthesis of trinitramide
, I've already suggested atomic nitrogen in NO2http://www.chemicalforums.com/index.php?topic=72951.msg338230#msg338230
whose most probable result is nitrogen, oxygen and their mundane compounds, plus oxidized tantalum. Worth a try?
Here is a different attempt, with NX3 in NO2
reacts easily with X2
, bonds are stronger in NX3
, in kJ/mol according towww.nist.gov/data/nsrds/NSRDS-NBS31.pdf
: 243 F-NF2
so light shall break X-NX2
to let the fragments react with NO2
. Advantageously, the compounds can be cold and diluted.
One unknown is the fragile O2
bond. A software estimate is 110kJ/mol, less than mean 168kJ/mol for I-N in NI3
. This favours a big halogen in NX3
, alas, and the wavelength should excite the trihalide rather than the nitramide if this is possible, and pass through XNO2
The only NX3
spectra I havehttp://satellite.mpic.de/spectral_atlas
are for NF3
(absorbs too little) and NCl3
, which absorbs better than NO2
at 254nm (8*10-19
should be more sensitive to this wavelength.
So the procedure would be: cool and evacuate the reactor, fill it with NO2
and a carrier gas, switch the lamp, sublimate NX3
, separate the lab debris by sedimentation, analyze.
Marc Schaefer, aka Enthalpy