Table 2: Numbering convention used for the molecular orbitals.
Number Orbital Number Orbital

1 $1s_{\rm N}$ 8 $\ensuremath {\sigma _{{\rm NH}}^*}$

2 $1s_{\rm C}$ 9 $\ensuremath {\sigma _{{\rm CH}}^*}$

3 $\ensuremath{\sigma_{{\rm CN}}}$ 10 $\ensuremath{\sigma_{\rm Ryd}}$

4 $\ensuremath{\pi_{{\rm CN}}} (x)$ 11 $\ensuremath{\sigma_{\rm Ryd}}$

5 $\ensuremath{\pi_{{\rm CN}}} (y)$ 12 $\ensuremath{\pi_{{\rm CN}}^*} (x)$

6 $\ensuremath{\sigma_{{\rm CH}}}$ 13 $\ensuremath{\pi_{{\rm CN}}^*} (y)$

7 $\ensuremath{\sigma_{{\rm NH}}}$

**Table 2:** Numbering convention used for the molecular orbitals.
Number	Orbital	Number	Orbital
1	$1s_{\rm N}$	8	$\ensuremath {\sigma _{{\rm NH}}^*}$
2	$1s_{\rm C}$	9	$\ensuremath {\sigma _{{\rm CH}}^*}$
3	$\ensuremath{\sigma_{{\rm CN}}}$	10	$\ensuremath{\sigma_{\rm Ryd}}$
4	$\ensuremath{\pi_{{\rm CN}}} (x)$	11	$\ensuremath{\sigma_{\rm Ryd}}$
5	$\ensuremath{\pi_{{\rm CN}}} (y)$	12	$\ensuremath{\pi_{{\rm CN}}^*} (x)$
6	$\ensuremath{\sigma_{{\rm CH}}}$	13	$\ensuremath{\pi_{{\rm CN}}^*} (y)$
7	$\ensuremath{\sigma_{{\rm NH}}}$

Source LaTeX | All tables | In the text

	1 Introduction
	2 Potential curves
	3 Dynamics calculations
	4 Concluding remarks
	References