Formoylperoxide

 O3 || C1 O2 / \ / \ H4 O6 H5
Tell me about the atomic charges, dipole moment, bond lengths, angles, bond orders,
molecular orbital energies, or total energy.
Tell me about the best Lewis structure.

Atomic Charges and Dipole Moment

C1 charge= 0.578
O2 charge=-0.318
O3 charge=-0.441
H4 charge= 0.040
H5 charge= 0.402
O6 charge=-0.261
with a dipole moment of 3.01408 Debye

Bond Lengths:

between C1 and O2: distance=2.358 ang___ between C1 and O3: distance=1.207 ang___
between C1 and H4: distance=1.116 ang___ between C1 and O6: distance=1.375 ang___
between O2 and H5: distance=0.983 ang___ between O2 and O6: distance=1.485 ang___
between O3 and O6: distance=2.328 ang___ between H4 and O6: distance=1.970 ang___

Bond Angles:

for O3-C1-O2: angle=92.61 deg___ for H4-C1-O2: angle=140.0 deg___
for H5-O2-C1: angle=121.5 deg___ for O6-O2-C1: angle=32.97 deg___

Bond Orders (Mulliken):

between C1 and O2: order=0.054___ between C1 and O3: order=1.969___
between C1 and H4: order=0.981___ between C1 and O6: order=0.934___
between O2 and H5: order=0.862___ between O2 and O6: order=0.821___
between O3 and O6: order=-0.117___ between H4 and O6: order=-0.076___

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. Please note that your structure can't be well described by a single Lewis structure, because of extensive delocalization.

Hybridization in the Best Lewis Structure

1. A bonding orbital for C1-O3 with 1.9981 electrons
__has 28.70% C 1 character in a s0.07 p3 hybrid
__has 71.30% O 3 character in a s0.07 p3 hybrid

2. A bonding orbital for C1-O3 with 1.9978 electrons
__has 35.24% C 1 character in a sp1.81 hybrid
__has 64.76% O 3 character in a sp1.72 hybrid

3. A bonding orbital for C1-H4 with 1.9760 electrons
__has 57.22% C 1 character in a sp1.93 hybrid
__has 42.78% H 4 character in a s orbital

4. A bonding orbital for C1-O6 with 1.9932 electrons
__has 31.36% C 1 character in a sp2.48 hybrid
__has 68.64% O 6 character in a sp2.25 hybrid

5. A bonding orbital for O2-H5 with 1.9945 electrons
__has 73.85% O 2 character in a s0.82 p3 hybrid
__has 26.15% H 5 character in a s orbital

6. A bonding orbital for O2-O6 with 1.9923 electrons
__has 45.74% O 2 character in a s0.32 p3 hybrid
__has 54.26% O 6 character in a s0.44 p3 hybrid

11. A lone pair orbital for O2 with 1.9988 electrons

12. A lone pair orbital for O2 with 1.9934 electrons
__made from a s0.08 p3 hybrid

13. A lone pair orbital for O3 with 1.9826 electrons

14. A lone pair orbital for O3 with 1.8619 electrons

15. A lone pair orbital for O6 with 1.9850 electrons

16. A lone pair orbital for O6 with 1.8822 electrons
__made from a p-pi orbital ( 99.95% p)

103. A antibonding orbital for C1-O3 with 0.1083 electrons
__has 71.30% C 1 character in a s0.07 p3 hybrid
__has 28.70% O 3 character in a s0.07 p3 hybrid

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

The interaction of bonding donor orbital, 3, for C1-H4 with the antibonding acceptor orbital, 108, for O2-O6 is 32.5 kJ/mol.

The interaction of the second lone pair donor orbital, 14, for O3 with the antibonding acceptor orbital, 105, for C1-H4 is 116. kJ/mol.

The interaction of the second lone pair donor orbital, 14, for O3 with the antibonding acceptor orbital, 106, for C1-O6 is 194. kJ/mol.

The interaction of lone pair donor orbital, 15, for O6 with the second antibonding acceptor orbital, 104, for C1-O3 is 29.8 kJ/mol.

The interaction of the second lone pair donor orbital, 16, for O6 with the antibonding acceptor orbital, 103, for C1-O3 is 196. 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.

20 ----- 1.921

19 ----- 0.581

18 ----- -1.901

17 ----- -2.825

16 -^-v- -7.211

15 -^-v- -7.357

14 -^-v- -8.944

13 -^-v- -10.07

12 -^-v- -11.17

11 -^-v- -12.00

10 -^-v- -13.04

9 -^-v- -13.51

8 -^-v- -16.21

7 -^-v- -23.91

6 -^-v- -26.59

5 -^-v- -29.20

4 -^-v- -270.2

3 -^-v- -506.9

2 -^-v- -508.8

1 -^-v- -509.8

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 = -265.0011399175 Hartrees