H5 H6 H11 \ | / O1 C4 - C7 - H12 \\ / \ C2 - C3 - H9 H10 \ H8
The multiplicity is 2.

Atomic Charges and Dipole Moment

O1 charge=-0.210
C2 charge=-0.130
C3 charge= 0.418
C4 charge= 0.323
H5 charge=-0.047
H6 charge=-0.047
C7 charge=-0.613
H8 charge=-0.062
H9 charge=-0.061
H10 charge= 0.135
H11 charge= 0.159
H12 charge= 0.135
with a dipole moment of 2.94434 Debye

Bond Lengths:

between O1 and C2: distance=1.202 ang___ between O1 and C3: distance=2.449 ang___
between O1 and C4: distance=2.965 ang___ between C2 and C3: distance=1.514 ang___
between C3 and C4: distance=1.544 ang___ between C3 and H5: distance=2.173 ang___
between C3 and H6: distance=2.172 ang___ between C3 and C7: distance=2.550 ang___
between C3 and H8: distance=1.109 ang___ between C3 and H9: distance=1.109 ang___
between C4 and H5: distance=1.106 ang___ between C4 and H6: distance=1.106 ang___
between C4 and C7: distance=1.540 ang___ between C4 and H11: distance=2.195 ang___
between C7 and H10: distance=1.106 ang___ between C7 and H11: distance=1.104 ang___
between C7 and H12: distance=1.105 ang___

Bond Angles:

for C3-C2-O1: angle=128.4 deg___ for C4-C3-C2: angle=115.7 deg___
for H5-C4-C3: angle=109.0 deg___ for H6-C4-C3: angle=109.0 deg___
for C7-C4-C3: angle=111.5 deg___ for H8-C3-C2: angle=106.1 deg___
for H9-C3-C2: angle=106.0 deg___ for H10-C7-C4: angle=111.4 deg___
for H11-C7-C4: angle=111.1 deg___ for H12-C7-C4: angle=111.4 deg___

Bond Orders (Mulliken):

between O1 and C2: order=2.020___ between O1 and C3: order=-0.096___
between O1 and C4: order=0.063___ between C2 and C3: order=0.742___
between C3 and C4: order=0.643___ between C3 and H5: order=-0.058___
between C3 and H6: order=-0.057___ between C3 and C7: order=-0.057___
between C3 and H8: order=0.981___ between C3 and H9: order=0.980___
between C4 and H5: order=1.002___ between C4 and H6: order=1.001___
between C4 and C7: order=0.774___ between C4 and H11: order=-0.055___
between C7 and H10: order=0.985___ between C7 and H11: order=1.007___
between C7 and H12: order=0.984___

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 O1-C2 with 0.9987 electrons
__has 67.89% O 1 character in a sp1.44 hybrid
__has 32.11% C 2 character in a sp2.13 hybrid

2. A bonding orbital for O1-C2 with 0.9969 electrons
__has 72.24% O 1 character in a p-pi orbital ( 99.80% p 0.20% d)
__has 27.76% C 2 character in a p-pi orbital ( 99.36% p 0.64% d)

3. A bonding orbital for C2-C3 with 0.9953 electrons
__has 43.72% C 2 character in a sp2.22 hybrid
__has 56.28% C 3 character in a sp2.78 hybrid

4. A bonding orbital for C3-C4 with 0.9966 electrons
__has 50.95% C 3 character in a sp2.48 hybrid
__has 49.05% C 4 character in a sp2.73 hybrid

5. A bonding orbital for C3-H8 with 0.9869 electrons
__has 60.86% C 3 character in a s0.87 p3 hybrid
__has 39.14% H 8 character in a s orbital

6. A bonding orbital for C3-H9 with 0.9868 electrons
__has 60.86% C 3 character in a s0.87 p3 hybrid
__has 39.14% H 9 character in a s orbital

7. A bonding orbital for C4-H5 with 0.9922 electrons
__has 59.58% C 4 character in a s0.87 p3 hybrid
__has 40.42% H 5 character in a s orbital

8. A bonding orbital for C4-H6 with 0.9922 electrons
__has 59.59% C 4 character in a s0.87 p3 hybrid
__has 40.41% H 6 character in a s orbital

9. A bonding orbital for C4-C7 with 0.9966 electrons
__has 50.78% C 4 character in a sp2.52 hybrid
__has 49.22% C 7 character in a sp2.43 hybrid

10. A bonding orbital for C7-H10 with 0.9963 electrons
__has 59.04% C 7 character in a s0.93 p3 hybrid
__has 40.96% H10 character in a s orbital

11. A bonding orbital for C7-H11 with 0.9961 electrons
__has 59.42% C 7 character in a s0.93 p3 hybrid
__has 40.58% H11 character in a s orbital

12. A bonding orbital for C7-H12 with 0.9963 electrons
__has 59.04% C 7 character in a s0.93 p3 hybrid
__has 40.96% H12 character in a s orbital

18. A lone pair orbital for O1 with 0.9929 electrons

19. A lone pair orbital for O1 with 0.9736 electrons
__made from a s0.06 p3 hybrid

20. A lone pair orbital for C2 with 0.9815 electrons

-With core pairs on: O 1 C 2 C 3 C 4 C 7 -

Up Electrons

1. A bonding orbital for O1-C2 with 0.9987 electrons
__has 66.76% O 1 character in a sp1.48 hybrid
__has 33.24% C 2 character in a sp1.38 hybrid

2. A bonding orbital for O1-C2 with 0.9975 electrons
__has 78.26% O 1 character in a p-pi orbital ( 99.81% p 0.19% d)
__has 21.74% C 2 character in a p-pi orbital ( 99.03% p 0.97% d)

3. A bonding orbital for O1-C2 with 0.9969 electrons
__has 78.55% O 1 character in a s0.08 p3 hybrid
__has 21.45% C 2 character in a s0.08 p3 hybrid

4. A bonding orbital for C2-C3 with 0.9972 electrons
__has 50.28% C 2 character in a sp0.78 hybrid
__has 49.72% C 3 character in a s0.87 p3 hybrid

5. A bonding orbital for C3-C4 with 0.9895 electrons
__has 52.89% C 3 character in a sp2.04 hybrid
__has 47.11% C 4 character in a sp2.79 hybrid

6. A bonding orbital for C3-H8 with 0.9873 electrons
__has 60.20% C 3 character in a s0.86 p3 hybrid
__has 39.80% H 8 character in a s orbital

7. A bonding orbital for C3-H9 with 0.9872 electrons
__has 60.20% C 3 character in a s0.86 p3 hybrid
__has 39.80% H 9 character in a s orbital

8. A bonding orbital for C4-H5 with 0.9922 electrons
__has 59.36% C 4 character in a s0.86 p3 hybrid
__has 40.64% H 5 character in a s orbital

9. A bonding orbital for C4-H6 with 0.9922 electrons
__has 59.37% C 4 character in a s0.86 p3 hybrid
__has 40.63% H 6 character in a s orbital

10. A bonding orbital for C4-C7 with 0.9947 electrons
__has 50.92% C 4 character in a sp2.44 hybrid
__has 49.08% C 7 character in a sp2.44 hybrid

11. A bonding orbital for C7-H10 with 0.9962 electrons
__has 59.02% C 7 character in a s0.92 p3 hybrid
__has 40.98% H10 character in a s orbital

12. A bonding orbital for C7-H11 with 0.9949 electrons
__has 59.70% C 7 character in a s0.94 p3 hybrid
__has 40.30% H11 character in a s orbital

13. A bonding orbital for C7-H12 with 0.9962 electrons
__has 59.03% C 7 character in a s0.92 p3 hybrid
__has 40.97% H12 character in a s orbital

19. A lone pair orbital for O1 with 0.9912 electrons

-With core pairs on: O 1 C 2 C 3 C 4 C 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.

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.

24 ----- 1.798

23 ----- 1.415

22 ----- 1.185

21 ----- -2.093

20 -^--- -4.227

19 -^-v- -8.307

18 -^-v- -8.659

17 -^-v- -9.269

16 -^-v- -9.459

15 -^-v- -9.595

14 -^-v- -10.55

13 -^-v- -10.97

12 -^-v- -11.61

11 -^-v- -12.04

10 -^-v- -13.23

9 -^-v- -15.11

8 -^-v- -17.84

7 -^-v- -20.03

6 -^-v- -26.95

5 -^-v- -266.3

4 -^-v- -266.7

3 -^-v- -267.2

2 -^-v- -268.8

1 -^-v- -507.6

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 = -231.8851390590 Hartrees