CH2O->O, formaldehyde oxide

H3
\
C1 = O2
/ \
H4O5
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= 0.056
O2 charge= 0.019
H3 charge= 0.116
H4 charge= 0.134
O5 charge=-0.327
with a dipole moment of 4.01145 Debye

Bond Lengths:

between C1 and O2: distance=1.286 ang___ between C1 and H3: distance=1.094 ang___
between C1 and H4: distance=1.097 ang___ between C1 and O5: distance=2.281 ang___
between O2 and O5: distance=1.359 ang___

Bond Angles:

for H3-C1-O2: angle=114.4 deg___ for H4-C1-O2: angle=119.1 deg___
for O5-O2-C1: angle=119.1 deg___

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Bond Orders (Mulliken):

between C1 and O2: order=1.575___ between C1 and H3: order=0.943___
between C1 and H4: order=0.945___ between C1 and O5: order=0.194___
between O2 and O5: order=0.587___

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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-O2 with 1.9978 electrons
__has 32.16% C 1 character in a sp2.28 hybrid
__has 67.84% O 2 character in a sp1.80 hybrid

2. A bonding orbital for C1-O2 with 1.9979 electrons
__has 27.76% C 1 character in a p-pi orbital ( 99.46% p 0.54% d)
__has 72.24% O 2 character in a p-pi orbital ( 99.87% p 0.13% d)

3. A bonding orbital for C1-H3 with 1.9892 electrons
__has 58.75% C 1 character in a sp1.91 hybrid
__has 41.25% H 3 character in a s orbital

4. A bonding orbital for C1-H4 with 1.9947 electrons
__has 59.71% C 1 character in a sp1.80 hybrid
__has 40.29% H 4 character in a s orbital

5. A bonding orbital for O2-O5 with 1.9907 electrons
__has 67.97% O 2 character in a sp2.91 hybrid
__has 32.03% O 5 character in a s0.27 p3 hybrid

9. A lone pair orbital for O2 with 1.9776 electrons
__made from a sp1.55 hybrid

10. A lone pair orbital for O5 with 1.9955 electrons
__made from a sp0.35 hybrid

11. A lone pair orbital for O5 with 1.9827 electrons
__made from a s0.68 p3 hybrid

12. A lone pair orbital for O5 with 1.8779 electrons
__made from a p-pi orbital ( 99.97% p)

81. A antibonding orbital for C1-O2 with 0.1188 electrons
__has 72.24% C 1 character in a p-pi orbital ( 99.46% p 0.54% d)
__has 27.76% O 2 character in a p-pi orbital ( 99.87% p 0.13% d)

-With core pairs on: C 1 O 2 O 5 -

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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-H3 with the antibonding acceptor orbital, 84, for O2-O5 is 22.8 kJ/mol.

The interaction of lone pair donor orbital, 9, for O2 with the antibonding acceptor orbital, 83, for C1-H4 is 24.9 kJ/mol.

The interaction of the second lone pair donor orbital, 11, for O5 with the antibonding acceptor orbital, 80, for C1-O2 is 35.6 kJ/mol.

The interaction of the third lone pair donor orbital, 12, for O5 with the second antibonding acceptor orbital, 81, for C1-O2 is 159. kJ/mol.

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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.

16 ----- 1.778

15 ----- 1.543


14 ----- -0.003


13 ----- -3.954


12 -^-v- -5.808

11 -^-v- -6.456


10 -^-v- -10.16


9 -^-v- -12.55

8 -^-v- -13.32

7 -^-v- -13.60


6 -^-v- -16.36


5 -^-v- -22.71


4 -^-v- -30.27


3 -^-v- -269.3


2 -^-v- -506.9


1 -^-v- -511.1

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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 = -189.6716652231 Hartrees

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