ASPECTS OF THE CH5N2 POTENTIAL-ENERGY SURFACE - IONS CH3NHNH+, CH3NNH2+ AND CH2NHNH2+ AND RADICALS CH2NHNH2. STUDIED BY THEORY AND EXPERIMENT

The CH5N2+ system has been investigated by ab initio MO calculations at the SDCI/6-31G**//6-31G** level of theory and by mass spectrometric experiments. The calculations confirm earlier experimental observations that the diazapropylium ions CH3-NH = NH+,1+,CH3-N = NH2+,2+ and CH2-NH-NH2+, 3+ and the hydrazonium ion CH2 = N-NH3+, 4+, are stable species. Theory predicts 1+ and 2+ to be higher in energy than 3+, by 7-8 kcal mol-1, causing a serious discrepancy with existing experimental values, which indicate that 1+ and 2+ are considerably more stable than 3+. The theoretical values are insensitive to inclusion of electron correlation in the geometry determinations. From a critical evaluation of existing energetic data for N2H3+, CH5N2+ and CH7N+ ions, and collision experiments on deuterium labelled species, it is concluded that theory is correct and that several reported appearance energy (AE) measurements on hydrazines are probably in error owing to interferences from traces of amines. From AE measurements not affected by these interferences, DELTAHf(3+) is proposed to be 204 +/-5 kcal mol-1 from which theory leads us to recommend DELTAH(f) values of 211 +/- 5 kcal mol for 1+ and 2+. Ab initio calculated proton affinities for HN = NH, CH3-N = NH and CH3-N = N-CH3 lead to proposed enthalpies for 1+ and 2+ which are consistent with these values. Theory further predicts the ring-closed form of 3+ to be a remarkably stable species (1 6.7 kcal mol-1 above 3+) but the hydrogen bridged entity CH2 = N.H.NH2+ previously proposed to be responsible for the facile interconversion between 3+ and 4+, is not a minimum on the potential energy surface. In fact, large energy barriers (42-63 kcal mol-1) prohibit interconversion among ions 1+, 2+, 3+ and 4+, via 1,2-H shifts. Metastable CH5N2+ions dissociate to HC = N + NH4+ and to HCNH+ + NH3 and in agreement with experiment, the reacting configuration for HC = N formation is the ion 4+. Formation of HC = N from 4+ is exothermic but the reverse barrier is large (84 kcal mol-1) thus accounting for the persistence of 4+ in the gas phase and in neutral solvents. The small kinetic energy release (KER) accompanying this reaction is rationalized in terms of ion/dipole attraction in the dissociating [HC = N ... NH4]+ complex.