## CNN+

 C3 - N1 = N2
The ion charge is 1. The multiplicity is 2.

## Atomic Charges and Dipole Moment

N1 charge= 0.630
N2 charge= 0.144
C3 charge= 0.224
with a dipole moment of 0.57679 Debye

## Bond Lengths:

between N1 and N2: distance=1.156 ang___ between N1 and C3: distance=1.366 ang___
between N2 and C3: distance=2.522 ang___

## Bond Angles:

for C3-N1-N2: angle=179.9 deg___

## Bond Orders (Mulliken):

between N1 and N2: order=1.809___ between N1 and C3: order=0.875___
between N2 and C3: order=-0.092___

## 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.

The Lewis structure is built for the up and down electrons, separately. Note that the up and down structures can be very different.

### Hybridization in the Best Lewis Structure

#### Down Electrons

1. A bonding orbital for N1-N2 with 0.9996 electrons
__has 54.91% N 1 character in a sp1.13 hybrid
__has 45.09% N 2 character in a sp2.54 hybrid

2. A bonding orbital for N1-N2 with 0.9996 electrons
__has 26.84% N 1 character in a p-pi orbital ( 99.59% p 0.41% d)
__has 73.16% N 2 character in a p-pi orbital ( 99.67% p 0.33% d)

3. A bonding orbital for N1-N2 with 0.9860 electrons
__has 52.80% N 1 character in a p-pi orbital ( 99.81% p 0.19% d)
__has 47.20% N 2 character in a p-pi orbital ( 99.43% p 0.57% d)

4. A bonding orbital for N1-C3 with 0.9988 electrons
__has 74.23% N 1 character in a sp0.88 hybrid
__has 25.77% C 3 character in a s0.44 p3 hybrid

8. A lone pair orbital for N2 with 0.9930 electrons
__made from a sp0.38 hybrid

9. A lone pair orbital for C3 with 0.9915 electrons
__made from a sp0.14 hybrid

10. A lone pair orbital for C3 with 0.7373 electrons
__made from a p-pi orbital ( 99.56% p 0.44% d)

70. A antibonding orbital for N1-N2 with 0.2545 electrons
__has 73.16% N 1 character in a p-pi orbital ( 99.59% p 0.41% d)
__has 26.84% N 2 character in a p-pi orbital ( 99.67% p 0.33% d)

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

#### Up Electrons

1. A bonding orbital for N1-N2 with 0.9995 electrons
__has 59.92% N 1 character in a sp1.14 hybrid
__has 40.08% N 2 character in a sp2.22 hybrid

2. A bonding orbital for N1-N2 with 0.9788 electrons
__has 84.07% N 1 character in a p-pi orbital ( 99.96% p)
__has 15.93% N 2 character in a p-pi orbital ( 99.21% p 0.79% d)

3. A bonding orbital for N1-N2 with 0.9719 electrons
__has 82.30% N 1 character in a p-pi orbital ( 99.97% p)
__has 17.70% N 2 character in a p-pi orbital ( 99.27% p 0.73% d)

4. A bonding orbital for N1-C3 with 0.9988 electrons
__has 78.60% N 1 character in a sp0.87 hybrid
__has 21.40% C 3 character in a s0.53 p3 hybrid

8. A lone pair orbital for N2 with 0.9922 electrons
__made from a sp0.44 hybrid

9. A lone pair orbital for C3 with 0.9920 electrons
__made from a sp0.17 hybrid

-With core pairs on: N 1 N 2 C 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 the second bonding donor orbital, 2, for N1-N2 with the third lone pair acceptor orbital, 11, for C3 is 52.4 kJ/mol.

The interaction of the third bonding donor orbital, 3, for N1-N2 with the second lone pair acceptor orbital, 10, for C3 is 64.9 kJ/mol.

The interaction of lone pair donor orbital, 8, for N2 with the antibonding acceptor orbital, 72, for N1-C3 is 22.2 kJ/mol.

The interaction of lone pair donor orbital, 9, for C3 with the antibonding acceptor orbital, 69, for N1-N2 is 31.0 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. Only the spin up electron orbital energies are given.

14 ----- -5.961

13 ----- -10.60 12 ----- -10.61

11 ----- -15.60
10 -^--- -15.67

9 -^-v- -17.84

8 -^-v- -20.82

7 -^-v- -21.66
6 -^-v- -21.75

5 -^-v- -30.97

4 -^-v- -37.86

3 -^-v- -280.5

2 -^-v- -390.6

1 -^-v- -390.9

## 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 = -147.0775535358 Hartrees

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