## CN2, N=C=N singlet

 N3 = C1 = N2
Tell me about the atomic charges, dipole moment, bond lengths, angles, bond orders,
molecular orbital energies, or total energy.
Tell me about the best Lewis structure.

## Atomic Charges and Dipole Moment

C1 charge= 0.660
N2 charge=-0.330
N3 charge=-0.330
with a dipole moment of 0.00138 Debye

## Bond Lengths:

between C1 and N2: distance=1.242 ang___ between C1 and N3: distance=1.242 ang___
between N2 and N3: distance=2.483 ang___

## Bond Angles:

for N3-C1-N2: angle=179.8 deg___

## Bond Orders (Mulliken):

between C1 and N2: order=1.758___ between C1 and N3: order=1.758___
between N2 and N3: order=0.224___

## Best Lewis Structure

The Lewis structure that is closest to your structure is determined. The hybridization of the atoms in this idealized Lewis structure is given in the table below. Please note that your structure can't be well described by a single Lewis structure, because of extensive delocalization.

### Hybridization in the Best Lewis Structure

1. A bonding orbital for C1-N2 with 1.9976 electrons
__has 45.90% C 1 character in a sp1.00 hybrid
__has 54.10% N 2 character in a sp1.83 hybrid

2. A bonding orbital for C1-N3 with 1.9976 electrons
__has 45.90% C 1 character in a sp1.00 hybrid
__has 54.10% N 3 character in a sp1.82 hybrid

3. A bonding orbital for C1-N3 with 1.5899 electrons
__has 74.21% C 1 character in a p-pi orbital (100.00% p)
__has 25.79% N 3 character in a p-pi orbital ( 99.57% p 0.43% d)

7. A lone pair orbital for C1 with 0.7685 electrons
__made from a p-pi orbital (100.00% p)

8. A lone pair orbital for N2 with 1.9734 electrons

9. A lone pair orbital for N2 with 1.6099 electrons
__made from a p-pi orbital ( 99.75% p 0.25% d)

10. A lone pair orbital for N2 with 0.4100 electrons
__made from a p-pi orbital ( 99.58% p 0.42% d)

11. A lone pair orbital for N3 with 1.9734 electrons

12. A lone pair orbital for N3 with 1.6099 electrons
__made from a p-pi orbital ( 99.75% p 0.25% d)

-With core pairs on: C 1 N 2 N 3 -

#### Donor Acceptor Interactions in the Best Lewis Structure

The localized orbitals in your best Lewis structure can interact strongly. A filled bonding or lone pair orbital can act as a donor and an empty or filled bonding, antibonding, or lone pair orbital can act as an acceptor. These interactions can strengthen and weaken bonds. For example, a lone pair donor->antibonding acceptor orbital interaction will weaken the bond associated with the antibonding orbital. Conversly, an interaction with a bonding pair as the acceptor will strengthen the bond. Strong electron delocalization in your best Lewis structure will also show up as donor-acceptor interactions.
Interactions greater than 20 kJ/mol for bonding and lone pair orbitals are listed below.

The interaction of bonding donor orbital, 1, for C1-N2 with the antibonding acceptor orbital, 71, for C1-N3 is 26.8 kJ/mol.

The interaction of bonding donor orbital, 2, for C1-N3 with the antibonding acceptor orbital, 70, for C1-N2 is 26.8 kJ/mol.

The interaction of the second bonding donor orbital, 3, for C1-N3 with the third lone pair acceptor orbital, 10, for N2 is 927. kJ/mol.

The interaction of the second bonding donor orbital, 3, for C1-N3 with the second antibonding acceptor orbital, 72, for C1-N3 is 41.7 kJ/mol.

The interaction of lone pair donor orbital, 8, for N2 with the antibonding acceptor orbital, 71, for C1-N3 is 95.3 kJ/mol.

The interaction of the second lone pair donor orbital, 9, for N2 with the lone pair acceptor orbital, 7, for C1 is 1340 kJ/mol.

The interaction of the third lone pair donor orbital, 10, for N2 with the second antibonding acceptor orbital, 72, for C1-N3 is 112. kJ/mol.

The interaction of lone pair donor orbital, 11, for N3 with the antibonding acceptor orbital, 70, for C1-N2 is 95.3 kJ/mol.

The interaction of the second lone pair donor orbital, 12, for N3 with the lone pair acceptor orbital, 7, for C1 is 1340 kJ/mol.

## Molecular Orbital Energies

The orbital energies are given in eV, where 1 eV=96.49 kJ/mol. Orbitals with very low energy are core 1s orbitals. More antibonding orbitals than you might expect are sometimes listed, because d orbitals are always included for heavy atoms and p orbitals are included for H atoms. Up spins are shown with a ^ and down spins are shown as v.

14 ----- 1.880

13 ----- -0.127

12 ----- -0.706

11 ----- -8.016

10 -^-v- -7.206

9 -^-v- -10.37

8 -^-v- -11.07

7 -^-v- -11.37

6 -^-v- -11.72

5 -^-v- -23.07

4 -^-v- -24.83

3 -^-v- -269.7

2 -^-v- -380.3 1 -^-v- -380.3

## Total Electronic Energy

The total electronic energy is a very large number, so by convention the units are given in atomic units, that is Hartrees (H). One Hartree is 2625.5 kJ/mol. The energy reference is for totally dissociated atoms. In other words, the reference state is a gas consisting of nuclei and electrons all at infinite distance from each other. The electronic energy includes all electric interactions and the kinetic energy of the electrons. This energy does not include translation, rotation, or vibration of the the molecule.

Total electronic energy = -147.4911336146 Hartrees

The triplet state is lower in energy