H8 H9 \ / O7 - C6 H3 | \ / H11 C1 - C2 - H5 / \ H10 H4
The multiplicity is 2.

## Atomic Charges and Dipole Moment

C1 charge=-0.000
C2 charge=-0.522
H3 charge= 0.151
H4 charge= 0.154
H5 charge= 0.148
C6 charge= 0.066
O7 charge=-0.652
H8 charge= 0.419
H9 charge= 0.074
H10 charge= 0.104
H11 charge= 0.056
with a dipole moment of 2.04888 Debye

## Bond Lengths:

between C1 and C2: distance=1.493 ang___ between C1 and H3: distance=2.167 ang___
between C1 and C6: distance=1.487 ang___ between C1 and O7: distance=2.397 ang___
between C1 and H9: distance=2.144 ang___ between C1 and H10: distance=1.096 ang___
between C2 and H3: distance=1.108 ang___ between C2 and H4: distance=1.104 ang___
between C2 and H5: distance=1.115 ang___ between C6 and O7: distance=1.448 ang___
between C6 and H9: distance=1.116 ang___ between C6 and H11: distance=1.122 ang___
between O7 and H8: distance=0.975 ang___

## Bond Angles:

for H3-C2-C1: angle=112.0 deg___ for H4-C2-C1: angle=111.7 deg___
for H5-C2-C1: angle=112.3 deg___ for C6-C1-C2: angle=121.1 deg___
for O7-C6-C1: angle=109.4 deg___ for H8-O7-C6: angle=108.3 deg___
for H9-C6-C1: angle=110.0 deg___ for H10-C1-C2: angle=120.5 deg___
for H11-C6-O7: angle=109.8 deg___

## Bond Orders (Mulliken):

between C1 and C2: order=0.745___ between C1 and H3: order=-0.061___
between C1 and C6: order=0.843___ between C1 and O7: order=-0.051___
between C1 and H9: order=-0.068___ between C1 and H10: order=0.914___
between C2 and H3: order=1.004___ between C2 and H4: order=0.994___
between C2 and H5: order=0.969___ between C6 and O7: order=0.817___
between C6 and H9: order=1.023___ between C6 and H11: order=0.972___
between O7 and H8: order=0.858___

## 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-C2 with 0.9966 electrons
__has 50.73% C 1 character in a sp1.84 hybrid
__has 49.27% C 2 character in a sp2.39 hybrid

2. A bonding orbital for C1-C6 with 0.9960 electrons
__has 49.85% C 1 character in a sp2.03 hybrid
__has 50.15% C 6 character in a sp2.31 hybrid

3. A bonding orbital for C1-H10 with 0.9921 electrons
__has 61.12% C 1 character in a sp2.30 hybrid
__has 38.88% H10 character in a s orbital

4. A bonding orbital for C2-H3 with 0.9964 electrons
__has 58.56% C 2 character in a s0.94 p3 hybrid
__has 41.44% H 3 character in a s orbital

5. A bonding orbital for C2-H4 with 0.9964 electrons
__has 59.28% C 2 character in a s0.95 p3 hybrid
__has 40.72% H 4 character in a s orbital

6. A bonding orbital for C2-H5 with 0.9984 electrons
__has 57.09% C 2 character in a s0.89 p3 hybrid
__has 42.91% H 5 character in a s orbital

7. A bonding orbital for C6-O7 with 0.9978 electrons
__has 33.59% C 6 character in a s0.91 p3 hybrid
__has 66.41% O 7 character in a sp2.54 hybrid

8. A bonding orbital for C6-H9 with 0.9957 electrons
__has 56.61% C 6 character in a s0.95 p3 hybrid
__has 43.39% H 9 character in a s orbital

9. A bonding orbital for C6-H11 with 0.9970 electrons
__has 55.29% C 6 character in a s0.89 p3 hybrid
__has 44.71% H11 character in a s orbital

10. A bonding orbital for O7-H8 with 0.9953 electrons
__has 73.15% O 7 character in a s0.79 p3 hybrid
__has 26.85% H 8 character in a s orbital

15. A lone pair orbital for C1 with 0.9466 electrons
__made from a s0.05 p3 hybrid

16. A lone pair orbital for O7 with 0.9940 electrons
__made from a sp0.96 hybrid

17. A lone pair orbital for O7 with 0.9850 electrons
__made from a p3 hybrid

-With core pairs on: C 1 C 2 C 6 O 7 -

#### Up Electrons

1. A bonding orbital for C1-C2 with 0.9969 electrons
__has 45.71% C 1 character in a sp1.82 hybrid
__has 54.29% C 2 character in a sp2.27 hybrid

2. A bonding orbital for C1-C6 with 0.9961 electrons
__has 45.04% C 1 character in a sp1.99 hybrid
__has 54.96% C 6 character in a sp2.20 hybrid

3. A bonding orbital for C1-H10 with 0.9932 electrons
__has 55.65% C 1 character in a sp2.23 hybrid
__has 44.35% H10 character in a s orbital

4. A bonding orbital for C2-H3 with 0.9932 electrons
__has 60.26% C 2 character in a s0.91 p3 hybrid
__has 39.74% H 3 character in a s orbital

5. A bonding orbital for C2-H4 with 0.9939 electrons
__has 60.50% C 2 character in a s0.92 p3 hybrid
__has 39.50% H 4 character in a s orbital

6. A bonding orbital for C2-H5 with 0.9847 electrons
__has 61.78% C 2 character in a s0.89 p3 hybrid
__has 38.22% H 5 character in a s orbital

7. A bonding orbital for C6-O7 with 0.9977 electrons
__has 34.31% C 6 character in a s0.88 p3 hybrid
__has 65.69% O 7 character in a sp2.59 hybrid

8. A bonding orbital for C6-H9 with 0.9909 electrons
__has 58.66% C 6 character in a s0.91 p3 hybrid
__has 41.34% H 9 character in a s orbital

9. A bonding orbital for C6-H11 with 0.9848 electrons
__has 59.58% C 6 character in a s0.89 p3 hybrid
__has 40.42% H11 character in a s orbital

10. A bonding orbital for O7-H8 with 0.9958 electrons
__has 73.10% O 7 character in a s0.79 p3 hybrid
__has 26.90% H 8 character in a s orbital

16. A lone pair orbital for O7 with 0.9945 electrons
__made from a sp0.95 hybrid

17. A lone pair orbital for O7 with 0.9861 electrons
__made from a p3 hybrid

-With core pairs on: C 1 C 2 C 6 O 7 -

#### 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, 6, for C2-H5 with the lone pair acceptor orbital, 15, for C1 is 27.9 kJ/mol.

The interaction of bonding donor orbital, 9, for C6-H11 with the lone pair acceptor orbital, 15, for C1 is 27.5 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.

21 ----- 2.376
20 ----- 2.167

19 ----- 1.571

18 ----- 0.567

17 -^--- -4.094

16 -^-v- -6.344

15 -^-v- -8.026

14 -^-v- -8.865

13 -^-v- -9.471

12 -^-v- -9.812

11 -^-v- -10.69

10 -^-v- -11.30

9 -^-v- -12.69

8 -^-v- -13.93

7 -^-v- -16.80

6 -^-v- -19.20

5 -^-v- -25.09

4 -^-v- -266.2

3 -^-v- -266.5

2 -^-v- -267.6

1 -^-v- -506.3

## 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 = -193.7536727675 Hartrees