1-dehydro-1-fluoroethylene anion, CH2=CF-

C1 = C2
/ \
The ion charge is -1.

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= 0.044
C2 charge=-0.778
H3 charge=-0.038
H4 charge=-0.033
F5 charge=-0.193
with a dipole moment of 2.16391 Debye

Bond Lengths:

between C1 and C2: distance=1.367 ang___ between C1 and H3: distance=1.101 ang___
between C1 and H4: distance=1.107 ang___ between C2 and H4: distance=2.206 ang___
between C2 and F5: distance=1.515 ang___

Bond Angles:

for H3-C1-C2: angle=117.3 deg___ for H4-C1-C2: angle=125.7 deg___
for F5-C2-C1: angle=106.5 deg___

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Bond Orders (Mulliken):

between C1 and C2: order=1.601___ between C1 and H3: order=0.971___
between C1 and H4: order=0.937___ between C2 and H4: order=0.056___
between C2 and F5: order=0.378___

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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.

Hybridization in the Best Lewis Structure

1. A bonding orbital for C1-C2 with 1.9981 electrons
__has 66.81% C 1 character in a p-pi orbital ( 99.90% p 0.10% d)
__has 33.19% C 2 character in a p-pi orbital ( 99.71% p 0.29% d)

2. A bonding orbital for C1-C2 with 1.9938 electrons
__has 55.02% C 1 character in a sp1.41 hybrid
__has 44.98% C 2 character in a sp1.61 hybrid

3. A bonding orbital for C1-H3 with 1.9845 electrons
__has 57.53% C 1 character in a sp2.54 hybrid
__has 42.47% H 3 character in a s orbital

4. A bonding orbital for C1-H4 with 1.9900 electrons
__has 58.09% C 1 character in a sp2.25 hybrid
__has 41.91% H 4 character in a s orbital

5. A bonding orbital for C2-F5 with 1.9912 electrons
__has 19.28% C 2 character in a s0.42 p3 hybrid
__has 80.72% F 5 character in a sp2.77 hybrid

9. A lone pair orbital for C2 with 1.9648 electrons
__made from a sp0.93 hybrid

10. A lone pair orbital for F5 with 1.9947 electrons
__made from a sp0.48 hybrid

11. A lone pair orbital for F5 with 1.9923 electrons
__made from a s0.20 p3 hybrid

12. A lone pair orbital for F5 with 1.9713 electrons
__made from a p-pi orbital ( 99.99% p)

-With core pairs on: C 1 C 2 F 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 C2-F5 is 23.0 kJ/mol.

The interaction of lone pair donor orbital, 9, for C2 with the antibonding acceptor orbital, 83, for C1-H4 is 51.6 kJ/mol.

The interaction of the third lone pair donor orbital, 12, for F5 with the antibonding acceptor orbital, 80, for C1-C2 is 58.6 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 ----- 8.636

15 ----- 7.157
14 ----- 6.980

13 ----- 5.511

12 -^-v- 1.606

11 -^-v- 0.220

10 -^-v- -2.347

9 -^-v- -3.244

8 -^-v- -4.086

7 -^-v- -4.894

6 -^-v- -7.112

5 -^-v- -11.63

4 -^-v- -21.79

3 -^-v- -259.7

2 -^-v- -260.7

1 -^-v- -648.3

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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 = -177.2541948371 Hartrees

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