NCN2-

N3 - C1 - N2
The ion charge is -2.

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= 0.780
N2 charge=-1.390
N3 charge=-1.389
with a dipole moment of 0.00170 Debye

Bond Lengths:

between C1 and N2: distance=1.266 ang___ between C1 and N3: distance=1.266 ang___
between N2 and N3: distance=2.533 ang___

Bond Angles:

for N3-C1-N2: angle=179.9 deg___

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Bond Orders (Mulliken):

between C1 and N2: order=-1.650___ between C1 and N3: order=0.556___
between N2 and N3: order=-2.001___

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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 1.8293 electrons
__has 47.56% C 1 character in a sp1.74 d0.15 hybrid
__has 52.44% N 2 character in a sp0.47 d1.28 hybrid

5. A lone pair orbital for C1 with 1.9623 electrons
__made from a sp0.42 hybrid

6. A lone pair orbital for C1 with 1.8055 electrons
__made from a p3 d0.42 hybrid

7. A lone pair orbital for C1 with 1.8055 electrons
__made from a p3 d0.42 hybrid

8. A lone pair orbital for N2 with 1.9999 electrons
__made from a p-pi orbital ( 99.90% p 0.10% d)

9. A lone pair orbital for N2 with 1.9999 electrons
__made from a p-pi orbital ( 99.90% p 0.10% d)

10. A lone pair orbital for N2 with 1.9994 electrons
__made from a sp0.82 hybrid

11. A lone pair orbital for N2 with 1.9858 electrons
__made from a sp1.21 hybrid

12. A lone pair orbital for N3 with 0.1792 electrons
__made from a sp1.68 hybrid

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

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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, 72, for C1-N2 is 24.5 kJ/mol.

The interaction of bonding donor orbital, 1, for C1-N2 with the lone pair acceptor orbital, 12, for N3 is 946. kJ/mol.

The interaction of bonding donor orbital, 1, for C1-N2 with the second lone pair acceptor orbital, 13, for N3 is 24.2 kJ/mol.

The interaction of lone pair donor orbital, 5, for C1 with the lone pair acceptor orbital, 12, for N3 is 36.6 kJ/mol.

The interaction of lone pair donor orbital, 5, for C1 with the second lone pair acceptor orbital, 13, for N3 is 104. kJ/mol.

The interaction of the second lone pair donor orbital, 6, for C1 with the third lone pair acceptor orbital, 14, for N3 is 33.3 kJ/mol.

The interaction of the third lone pair donor orbital, 7, for C1 with the 4th lone pair acceptor orbital, 15, for N3 is 33.3 kJ/mol.

The interaction of the third lone pair donor orbital, 10, for N2 with the lone pair acceptor orbital, 12, for N3 is 4.01 kJ/mol.

The interaction of 4th lone pair donor orbital, 11, for N2 with the lone pair acceptor orbital, 12, for N3 is 3.76 kJ/mol.

The interaction of lone pair donor orbital, 12, for N3 with the second lone pair acceptor orbital, 13, for N3 is 34.0 kJ/mol.

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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.

15 ----- 14.92
14 ----- 14.59
13 ----- 14.35 12 ----- 14.35

11 -^-v- 8.201 10 -^-v- 8.200

9 -^-v- 4.999

8 -^-v- 4.396 7 -^-v- 4.395

6 -^-v- 3.924


5 -^-v- -6.281


4 -^-v- -8.243


3 -^-v- -254.2


2 -^-v- -362.8 1 -^-v- -362.8

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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 = -147.4523963866 Hartrees

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