H9 \ H3 H10 - C6 - H11 \ / H5 - C1 - C2 - C7 - H13 / | | \ H4 O8 H14 H12
The multiplicity is 2.

## Atomic Charges and Dipole Moment

C1 charge=-0.655
C2 charge= 0.888
H3 charge= 0.149
H4 charge= 0.174
H5 charge= 0.152
C6 charge=-0.588
C7 charge=-0.653
O8 charge=-0.458
H9 charge= 0.158
H10 charge= 0.178
H11 charge= 0.178
H12 charge= 0.148
H13 charge= 0.151
H14 charge= 0.174
with a dipole moment of 2.56613 Debye

## Bond Lengths:

between C1 and C2: distance=1.552 ang___ between C1 and H3: distance=1.105 ang___
between C1 and H4: distance=1.104 ang___ between C1 and H5: distance=1.103 ang___
between C1 and C6: distance=2.562 ang___ between C1 and C7: distance=2.575 ang___
between C1 and O8: distance=2.428 ang___ between C2 and H3: distance=2.209 ang___
between C2 and C6: distance=1.593 ang___ between C2 and C7: distance=1.552 ang___
between C2 and O8: distance=1.372 ang___ between C2 and H9: distance=2.183 ang___
between C2 and H12: distance=2.209 ang___ between C6 and C7: distance=2.563 ang___
between C6 and O8: distance=2.302 ang___ between C6 and H9: distance=1.104 ang___
between C6 and H10: distance=1.101 ang___ between C6 and H11: distance=1.101 ang___
between C7 and O8: distance=2.427 ang___ between C7 and H12: distance=1.105 ang___
between C7 and H13: distance=1.103 ang___ between C7 and H14: distance=1.104 ang___

## Bond Angles:

for H3-C1-C2: angle=111.3 deg___ for H4-C1-C2: angle=109.1 deg___
for H5-C1-C2: angle=110.3 deg___ for C6-C2-C1: angle=109.1 deg___
for C7-C2-C1: angle=112.1 deg___ for O8-C2-C1: angle=112.1 deg___
for H9-C6-C2: angle=106.6 deg___ for H10-C6-C2: angle=110.0 deg___
for H11-C6-C2: angle=110.0 deg___ for H12-C7-C2: angle=111.4 deg___
for H13-C7-C2: angle=110.3 deg___ for H14-C7-C2: angle=109.1 deg___

## Bond Orders (Mulliken):

between C1 and C2: order=1.023___ between C1 and H3: order=0.995___
between C1 and H4: order=0.953___ between C1 and H5: order=0.956___
between C1 and C6: order=-0.101___ between C1 and C7: order=-0.147___
between C1 and O8: order=-0.099___ between C2 and H3: order=-0.067___
between C2 and C6: order=0.955___ between C2 and C7: order=1.024___
between C2 and O8: order=0.904___ between C2 and H9: order=-0.090___
between C2 and H12: order=-0.067___ between C6 and C7: order=-0.101___
between C6 and O8: order=-0.100___ between C6 and H9: order=1.002___
between C6 and H10: order=0.953___ between C6 and H11: order=0.954___
between C7 and O8: order=-0.099___ between C7 and H12: order=0.995___
between C7 and H13: order=0.956___ between C7 and H14: order=0.953___

## 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 0.9959 electrons
__has 49.37% C 1 character in a sp2.68 hybrid
__has 50.63% C 2 character in a sp2.63 hybrid

2. A bonding orbital for C1-H3 with 0.9954 electrons
__has 59.30% C 1 character in a s0.97 p3 hybrid
__has 40.70% H 3 character in a s orbital

3. A bonding orbital for C1-H4 with 0.9958 electrons
__has 59.44% C 1 character in a s0.94 p3 hybrid
__has 40.56% H 4 character in a s orbital

4. A bonding orbital for C1-H5 with 0.9962 electrons
__has 59.77% C 1 character in a s0.98 p3 hybrid
__has 40.23% H 5 character in a s orbital

5. A bonding orbital for C2-C6 with 0.9948 electrons
__has 49.05% C 2 character in a s0.89 p3 hybrid
__has 50.95% C 6 character in a sp2.88 hybrid

6. A bonding orbital for C2-C7 with 0.9959 electrons
__has 50.63% C 2 character in a sp2.64 hybrid
__has 49.37% C 7 character in a sp2.69 hybrid

7. A bonding orbital for C2-O8 with 0.9977 electrons
__has 33.79% C 2 character in a s0.85 p3 hybrid
__has 66.21% O 8 character in a sp2.34 hybrid

8. A bonding orbital for C6-H9 with 0.9966 electrons
__has 58.95% C 6 character in a s0.92 p3 hybrid
__has 41.05% H 9 character in a s orbital

9. A bonding orbital for C6-H10 with 0.9969 electrons
__has 59.98% C 6 character in a sp2.93 hybrid
__has 40.02% H10 character in a s orbital

10. A bonding orbital for C6-H11 with 0.9969 electrons
__has 59.98% C 6 character in a sp2.93 hybrid
__has 40.02% H11 character in a s orbital

11. A bonding orbital for C7-H12 with 0.9954 electrons
__has 59.30% C 7 character in a s0.97 p3 hybrid
__has 40.70% H12 character in a s orbital

12. A bonding orbital for C7-H13 with 0.9962 electrons
__has 59.77% C 7 character in a s0.98 p3 hybrid
__has 40.23% H13 character in a s orbital

13. A bonding orbital for C7-H14 with 0.9958 electrons
__has 59.44% C 7 character in a s0.94 p3 hybrid
__has 40.56% H14 character in a s orbital

19. A lone pair orbital for O8 with 0.9947 electrons

20. A lone pair orbital for O8 with 0.9851 electrons

21. A lone pair orbital for O8 with 0.9786 electrons
__made from a p-pi orbital ( 99.96% p)

-With core pairs on: C 1 C 2 C 6 C 7 O 8 -

#### Up Electrons

1. A bonding orbital for C1-C2 with 0.9920 electrons
__has 48.20% C 1 character in a sp2.72 hybrid
__has 51.80% C 2 character in a sp2.65 hybrid

2. A bonding orbital for C1-H3 with 0.9955 electrons
__has 59.17% C 1 character in a s0.97 p3 hybrid
__has 40.83% H 3 character in a s orbital

3. A bonding orbital for C1-H4 with 0.9962 electrons
__has 59.33% C 1 character in a s0.95 p3 hybrid
__has 40.67% H 4 character in a s orbital

4. A bonding orbital for C1-H5 with 0.9964 electrons
__has 59.64% C 1 character in a s0.98 p3 hybrid
__has 40.36% H 5 character in a s orbital

5. A bonding orbital for C2-C6 with 0.9663 electrons
__has 54.56% C 2 character in a s0.88 p3 hybrid
__has 45.44% C 6 character in a s0.96 p3 hybrid

6. A bonding orbital for C2-C7 with 0.9919 electrons
__has 51.80% C 2 character in a sp2.65 hybrid
__has 48.20% C 7 character in a sp2.73 hybrid

7. A bonding orbital for C2-O8 with 0.9973 electrons
__has 38.30% C 2 character in a s0.88 p3 hybrid
__has 61.70% O 8 character in a sp2.16 hybrid

8. A bonding orbital for C6-H9 with 0.9930 electrons
__has 59.75% C 6 character in a s0.99 p3 hybrid
__has 40.25% H 9 character in a s orbital

9. A bonding orbital for C6-H10 with 0.9971 electrons
__has 59.50% C 6 character in a sp2.93 hybrid
__has 40.50% H10 character in a s orbital

10. A bonding orbital for C6-H11 with 0.9971 electrons
__has 59.50% C 6 character in a sp2.93 hybrid
__has 40.50% H11 character in a s orbital

11. A bonding orbital for C7-H12 with 0.9955 electrons
__has 59.17% C 7 character in a s0.97 p3 hybrid
__has 40.83% H12 character in a s orbital

12. A bonding orbital for C7-H13 with 0.9964 electrons
__has 59.64% C 7 character in a s0.98 p3 hybrid
__has 40.36% H13 character in a s orbital

13. A bonding orbital for C7-H14 with 0.9962 electrons
__has 59.33% C 7 character in a s0.95 p3 hybrid
__has 40.67% H14 character in a s orbital

19. A lone pair orbital for O8 with 0.9938 electrons

20. A lone pair orbital for O8 with 0.9742 electrons
__made from a p-pi orbital ( 99.97% p)

-With core pairs on: C 1 C 2 C 6 C 7 O 8 -

#### 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, 5, for C2-C6 with the third lone pair acceptor orbital, 21, for O8 is 49.5 kJ/mol.

The interaction of the second lone pair donor orbital, 20, for O8 with the antibonding acceptor orbital, 162, for C1-C2 is 26.9 kJ/mol.

The interaction of the second lone pair donor orbital, 20, for O8 with the antibonding acceptor orbital, 167, for C2-C7 is 26.8 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.

25 ----- 2.101
24 ----- 2.018

23 ----- 1.793

22 ----- 0.968

21 -^--- -6.194

20 -^-v- -6.904

19 -^-v- -8.741

18 -^-v- -8.917

17 -^-v- -9.098

16 -^-v- -9.231

15 -^-v- -9.865

14 -^-v- -10.10

13 -^-v- -11.32
12 -^-v- -11.33

11 -^-v- -11.46

10 -^-v- -13.28

9 -^-v- -17.05

8 -^-v- -17.27

7 -^-v- -19.19

6 -^-v- -25.11

5 -^-v- -266.2 4 -^-v- -266.2

3 -^-v- -266.8

2 -^-v- -268.3

1 -^-v- -507.0

## 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 = -233.0788024510 Hartrees