## CH3NO, Nitrosomethane

 H3 \ H5 - C1 - N2 / \\ H4 O6
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= 0.422
N2 charge=-0.205
H3 charge=-0.019
H4 charge=-0.023
H5 charge=-0.044
O6 charge=-0.130
with a dipole moment of 2.76810 Debye

## Bond Lengths:

between C1 and N2: distance=1.491 ang___ between C1 and H3: distance=1.106 ang___
between C1 and H4: distance=1.106 ang___ between C1 and H5: distance=1.104 ang___
between N2 and O6: distance=1.227 ang___

## Bond Angles:

for H3-C1-N2: angle=106.2 deg___ for H4-C1-N2: angle=106.5 deg___
for H5-C1-N2: angle=112.5 deg___ for O6-N2-C1: angle=113.6 deg___

## Bond Orders (Mulliken):

between C1 and N2: order=0.841___ between C1 and H3: order=0.953___
between C1 and H4: order=0.955___ between C1 and H5: order=0.975___
between N2 and O6: order=1.655___

## 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.

### Hybridization in the Best Lewis Structure

1. A bonding orbital for C1-N2 with 1.9942 electrons
__has 41.71% C 1 character in a s0.96 p3 hybrid
__has 58.29% N 2 character in a sp2.67 hybrid

2. A bonding orbital for C1-H3 with 1.9797 electrons
__has 59.83% C 1 character in a s0.96 p3 hybrid
__has 40.17% H 3 character in a s orbital

3. A bonding orbital for C1-H4 with 1.9808 electrons
__has 59.82% C 1 character in a s0.97 p3 hybrid
__has 40.18% H 4 character in a s orbital

4. A bonding orbital for C1-H5 with 1.9967 electrons
__has 60.05% C 1 character in a sp2.68 hybrid
__has 39.95% H 5 character in a s orbital

5. A bonding orbital for N2-O6 with 1.9962 electrons
__has 44.15% N 2 character in a sp2.63 hybrid
__has 55.85% O 6 character in a sp2.62 hybrid

6. A bonding orbital for N2-O6 with 1.9913 electrons
__has 37.97% N 2 character in a p-pi orbital ( 99.51% p 0.49% d)
__has 62.03% O 6 character in a p-pi orbital ( 99.79% p 0.21% d)

10. A lone pair orbital for N2 with 1.9826 electrons

11. A lone pair orbital for O6 with 1.9923 electrons

12. A lone pair orbital for O6 with 1.9646 electrons
__made from a s0.16 p3 hybrid

-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, 2, for C1-H3 with the second antibonding acceptor orbital, 90, for N2-O6 is 26.1 kJ/mol.

The interaction of bonding donor orbital, 3, for C1-H4 with the second antibonding acceptor orbital, 90, for N2-O6 is 24.2 kJ/mol.

The interaction of the second lone pair donor orbital, 12, for O6 with the antibonding acceptor orbital, 85, for C1-N2 is 73.4 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 ----- 3.049

15 ----- 2.006

14 ----- 1.454

13 ----- -3.985

12 -^-v- -5.199

11 -^-v- -9.326

10 -^-v- -9.938

9 -^-v- -11.75

8 -^-v- -12.12
7 -^-v- -12.16

6 -^-v- -15.19

5 -^-v- -19.80

4 -^-v- -28.93

3 -^-v- -267.3

2 -^-v- -380.5

1 -^-v- -508.1

## 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 = -169.8636658968 Hartrees