## CH2=OH+, Methyl oxonium ion

 H3 \ C1 = O2 / \ H4 H5
The ion charge is 1.

## Atomic Charges and Dipole Moment

C1 charge= 0.349
O2 charge=-0.228
H3 charge= 0.209
H4 charge= 0.168
H5 charge= 0.501
with a dipole moment of 2.26814 Debye

## Bond Lengths:

between C1 and O2: distance=1.264 ang___ between C1 and H3: distance=1.103 ang___
between C1 and H4: distance=1.105 ang___ between O2 and H5: distance=0.998 ang___

## Bond Angles:

for H3-C1-O2: angle=115.4 deg___ for H4-C1-O2: angle=121.7 deg___
for H5-O2-C1: angle=116.0 deg___

## Bond Orders (Mulliken):

between C1 and O2: order=1.505___ between C1 and H3: order=0.924___
between C1 and H4: order=0.916___ between O2 and H5: order=0.780___

## 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-O2 with 1.9996 electrons
__has 17.35% C 1 character in a p-pi orbital ( 99.08% p 0.92% d)
__has 82.65% O 2 character in a p-pi orbital ( 99.87% p 0.13% d)

2. A bonding orbital for C1-O2 with 1.9987 electrons
__has 31.75% C 1 character in a sp2.18 hybrid
__has 68.25% O 2 character in a sp1.71 hybrid

3. A bonding orbital for C1-H3 with 1.9905 electrons
__has 61.51% C 1 character in a sp1.89 hybrid
__has 38.49% H 3 character in a s orbital

4. A bonding orbital for C1-H4 with 1.9937 electrons
__has 60.77% C 1 character in a sp1.87 hybrid
__has 39.23% H 4 character in a s orbital

5. A bonding orbital for O2-H5 with 1.9878 electrons
__has 78.55% O 2 character in a s0.90 p3 hybrid
__has 21.45% H 5 character in a s orbital

8. A lone pair orbital for O2 with 1.9791 electrons

-With core pairs on: C 1 O 2 -

#### 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 lone pair donor orbital, 8, for O2 with the antibonding acceptor orbital, 65, for C1-H4 is 25.2 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.

12 ----- -3.582

11 ----- -4.544

10 ----- -6.659

9 ----- -11.69

8 -^-v- -16.80

7 -^-v- -19.20

6 -^-v- -20.34

5 -^-v- -22.22

4 -^-v- -25.66

3 -^-v- -36.52

2 -^-v- -277.9

1 -^-v- -517.4

## 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 = -114.8261324144 Hartrees