O=CHF

H3
\
C1 = O2
/
F4
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= 0.550
O2 charge=-0.384
H3 charge= 0.056
F4 charge=-0.222
with a dipole moment of 2.17383 Debye

Bond Lengths:

between C1 and O2: distance=1.194 ang___ between C1 and H3: distance=1.107 ang___
between C1 and F4: distance=1.378 ang___ between O2 and F4: distance=2.256 ang___

Bond Angles:

for H3-C1-O2: angle=128.7 deg___ for F4-C1-O2: angle=122.4 deg___

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Bond Orders (Mulliken):

between C1 and O2: order=2.041___ between C1 and H3: order=0.981___
between C1 and F4: order=0.887___ between O2 and F4: order=-0.076___

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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 1.9989 electrons
__has 34.71% C 1 character in a sp1.63 hybrid
__has 65.29% O 2 character in a sp1.50 hybrid

2. A bonding orbital for C1-O2 with 1.9990 electrons
__has 29.60% C 1 character in a p-pi orbital ( 99.36% p 0.64% d)
__has 70.40% O 2 character in a p-pi orbital ( 99.77% p 0.23% d)

3. A bonding orbital for C1-H3 with 1.9867 electrons
__has 57.48% C 1 character in a sp1.71 hybrid
__has 42.52% H 3 character in a s orbital

4. A bonding orbital for C1-F4 with 1.9959 electrons
__has 26.71% C 1 character in a sp2.82 hybrid
__has 73.29% F 4 character in a s0.98 p3 hybrid

8. A lone pair orbital for O2 with 1.9833 electrons
__made from a sp0.65 hybrid

9. A lone pair orbital for O2 with 1.8509 electrons
__made from a p3 hybrid

10. A lone pair orbital for F4 with 1.9935 electrons
__made from a sp0.34 hybrid

11. A lone pair orbital for F4 with 1.9777 electrons
__made from a p3 hybrid

12. A lone pair orbital for F4 with 1.9323 electrons
__made from a p-pi orbital ( 99.97% p)

78. A antibonding orbital for C1-F4 with 0.1092 electrons
__has 73.29% C 1 character in a sp2.82 hybrid
__has 26.71% F 4 character in a s0.98 p3 hybrid

-With core pairs on: C 1 O 2 F 4 -

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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, 78, for C1-F4 is 27.5 kJ/mol.

The interaction of the second lone pair donor orbital, 9, for O2 with the antibonding acceptor orbital, 77, for C1-H3 is 106. kJ/mol.

The interaction of the second lone pair donor orbital, 9, for O2 with the antibonding acceptor orbital, 78, for C1-F4 is 237. kJ/mol.

The interaction of the second lone pair donor orbital, 11, for F4 with the antibonding acceptor orbital, 75, for C1-O2 is 43.6 kJ/mol.

The interaction of the second lone pair donor orbital, 11, for F4 with the antibonding acceptor orbital, 77, for C1-H3 is 23.7 kJ/mol.

The interaction of the third lone pair donor orbital, 12, for F4 with the second antibonding acceptor orbital, 76, for C1-O2 is 137. 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 ----- 3.748

15 ----- 2.405

14 ----- 1.089


13 ----- -2.741


12 -^-v- -8.108


11 -^-v- -9.907

10 -^-v- -10.11


9 -^-v- -12.33

8 -^-v- -12.49


7 -^-v- -14.09


6 -^-v- -16.49


5 -^-v- -27.36


4 -^-v- -31.17


3 -^-v- -271.2


2 -^-v- -507.8


1 -^-v- -656.8

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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 = -213.8586995909 Hartrees

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