H3 \ H5 - C1 - O2 / \ H4 O6
The multiplicity is 2.

## Atomic Charges and Dipole Moment

C1 charge=-0.075
O2 charge=-0.039
H3 charge= 0.098
H4 charge= 0.116
H5 charge= 0.116
O6 charge=-0.216
with a dipole moment of 3.13198 Debye

## Bond Lengths:

between C1 and O2: distance=1.466 ang___ between C1 and H3: distance=1.101 ang___
between C1 and H4: distance=1.102 ang___ between C1 and H5: distance=1.102 ang___
between O2 and O6: distance=1.345 ang___

## Bond Angles:

for H3-C1-O2: angle=105.5 deg___ for H4-C1-O2: angle=108.7 deg___
for H5-C1-O2: angle=108.8 deg___ for O6-O2-C1: angle=110.9 deg___

## Bond Orders (Mulliken):

between C1 and O2: order=0.726___ between C1 and H3: order=0.972___
between C1 and H4: order=0.974___ between C1 and H5: order=0.974___
between O2 and O6: order=0.930___

## 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. 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 C1-O2 with 0.9972 electrons
__has 31.04% C 1 character in a s0.78 p3 hybrid
__has 68.96% O 2 character in a sp2.57 hybrid

2. A bonding orbital for C1-H3 with 0.9950 electrons
__has 59.04% C 1 character in a sp2.77 hybrid
__has 40.96% H 3 character in a s orbital

3. A bonding orbital for C1-H4 with 0.9985 electrons
__has 58.50% C 1 character in a sp2.76 hybrid
__has 41.50% H 4 character in a s orbital

4. A bonding orbital for C1-H5 with 0.9985 electrons
__has 58.52% C 1 character in a sp2.75 hybrid
__has 41.48% H 5 character in a s orbital

5. A bonding orbital for O2-O6 with 0.9974 electrons
__has 50.98% O 2 character in a s0.54 p3 hybrid
__has 49.02% O 6 character in a s0.43 p3 hybrid

9. A lone pair orbital for O2 with 0.9962 electrons

10. A lone pair orbital for O2 with 0.9889 electrons
__made from a p-pi orbital ( 99.97% p)

11. A lone pair orbital for O6 with 0.9989 electrons

12. A lone pair orbital for O6 with 0.9982 electrons
__made from a p-pi orbital ( 99.98% p)

13. A lone pair orbital for O6 with 0.9935 electrons
__made from a s0.52 p3 hybrid

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

#### Up Electrons

1. A bonding orbital for C1-O2 with 0.9975 electrons
__has 32.12% C 1 character in a s0.79 p3 hybrid
__has 67.88% O 2 character in a sp2.57 hybrid

2. A bonding orbital for C1-H3 with 0.9959 electrons
__has 58.90% C 1 character in a sp2.80 hybrid
__has 41.10% H 3 character in a s orbital

3. A bonding orbital for C1-H4 with 0.9979 electrons
__has 58.83% C 1 character in a sp2.76 hybrid
__has 41.17% H 4 character in a s orbital

4. A bonding orbital for C1-H5 with 0.9979 electrons
__has 58.85% C 1 character in a sp2.75 hybrid
__has 41.15% H 5 character in a s orbital

5. A bonding orbital for O2-O6 with 0.9974 electrons
__has 56.57% O 2 character in a s0.66 p3 hybrid
__has 43.43% O 6 character in a s0.50 p3 hybrid

6. A bonding orbital for O2-O6 with 0.9917 electrons
__has 88.72% O 2 character in a p-pi orbital ( 99.93% p 0.07% d)
__has 11.28% O 6 character in a p-pi orbital ( 99.59% p 0.41% d)

10. A lone pair orbital for O2 with 0.9957 electrons

11. A lone pair orbital for O6 with 0.9981 electrons

12. A lone pair orbital for O6 with 0.9922 electrons
__made from a s0.41 p3 hybrid

-With core pairs on: C 1 O 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.

## 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.

17 ----- 3.138

16 ----- 1.857

15 ----- 1.149

14 ----- -0.130

13 -^--- -6.350

12 -^-v- -6.459

11 -^-v- -9.933
10 -^-v- -10.00

9 -^-v- -12.32

8 -^-v- -12.60

7 -^-v- -12.96

6 -^-v- -16.97

5 -^-v- -21.75

4 -^-v- -29.61

3 -^-v- -268.2

2 -^-v- -508.2

1 -^-v- -510.0

## 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 = -190.2989586787 Hartrees