## CH2NH->O, Methanimine oxide

 H3 O6 \ / C1 = N2 / \ H4 H5
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=-0.538
N2 charge= 0.317
H3 charge= 0.266
H4 charge= 0.206
H5 charge= 0.208
O6 charge=-0.460
with a dipole moment of 3.55300 Debye

## Bond Lengths:

between C1 and N2: distance=1.319 ang___ between C1 and H3: distance=1.091 ang___
between C1 and H4: distance=1.091 ang___ between C1 and O6: distance=2.338 ang___
between N2 and H5: distance=1.044 ang___ between N2 and O6: distance=1.276 ang___

## Bond Angles:

for H3-C1-N2: angle=118.4 deg___ for H4-C1-N2: angle=117.7 deg___
for H5-N2-C1: angle=115.8 deg___ for O6-N2-C1: angle=128.5 deg___

## Bond Orders (Mulliken):

between C1 and N2: order=1.580___ between C1 and H3: order=0.974___
between C1 and H4: order=0.973___ between C1 and O6: order=0.226___
between N2 and H5: order=0.839___ between N2 and O6: order=0.936___

## 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 1.9979 electrons
__has 36.58% C 1 character in a sp2.08 hybrid
__has 63.42% N 2 character in a sp1.42 hybrid

2. A bonding orbital for C1-N2 with 1.9947 electrons
__has 42.37% C 1 character in a p-pi orbital ( 99.79% p 0.21% d)
__has 57.63% N 2 character in a p-pi orbital ( 99.88% p 0.12% d)

3. A bonding orbital for C1-H3 with 1.9902 electrons
__has 60.39% C 1 character in a sp1.90 hybrid
__has 39.61% H 3 character in a s orbital

4. A bonding orbital for C1-H4 with 1.9876 electrons
__has 59.21% C 1 character in a sp1.99 hybrid
__has 40.79% H 4 character in a s orbital

5. A bonding orbital for N2-H5 with 1.9869 electrons
__has 70.00% N 2 character in a sp2.87 hybrid
__has 30.00% H 5 character in a s orbital

6. A bonding orbital for N2-O6 with 1.9966 electrons
__has 53.32% N 2 character in a sp2.00 hybrid
__has 46.68% O 6 character in a s0.76 p3 hybrid

10. A lone pair orbital for O6 with 1.9883 electrons

11. A lone pair orbital for O6 with 1.9375 electrons

12. A lone pair orbital for O6 with 1.7300 electrons
__made from a p-pi orbital ( 99.92% p 0.08% d)

86. A antibonding orbital for C1-N2 with 0.2627 electrons
__has 57.63% C 1 character in a p-pi orbital ( 99.79% p 0.21% d)
__has 42.37% N 2 character in a p-pi orbital ( 99.88% p 0.12% d)

-With core pairs on: C 1 N 2 O 6 -

#### 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, 4, for C1-H4 with the antibonding acceptor orbital, 90, for N2-O6 is 32.9 kJ/mol.

The interaction of lone pair donor orbital, 10, for O6 with the antibonding acceptor orbital, 85, for C1-N2 is 22.8 kJ/mol.

The interaction of the second lone pair donor orbital, 11, for O6 with the antibonding acceptor orbital, 85, for C1-N2 is 51.6 kJ/mol.

The interaction of the second lone pair donor orbital, 11, for O6 with the antibonding acceptor orbital, 89, for N2-H5 is 80.5 kJ/mol.

The interaction of the third lone pair donor orbital, 12, for O6 with the second antibonding acceptor orbital, 86, for C1-N2 is 444. 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.

16 ----- 2.598

15 ----- 2.070

14 ----- 0.360

13 ----- -2.296

12 -^-v- -5.922

11 -^-v- -6.036

10 -^-v- -10.38

9 -^-v- -11.26

8 -^-v- -11.96

7 -^-v- -13.59

6 -^-v- -16.41

5 -^-v- -21.41

4 -^-v- -27.78

3 -^-v- -267.6

2 -^-v- -381.2

1 -^-v- -506.2

## 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 = -169.8763061433 Hartrees