cis-difluoroethylene, CHF=CHF

H3H6
\ /
C1 = C2
/ \
F4F5
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=-0.053
C2 charge=-0.057
H3 charge= 0.154
F4 charge=-0.099
F5 charge=-0.098
H6 charge= 0.154
with a dipole moment of 2.53617 Debye

Bond Lengths:

between C1 and C2: distance=1.338 ang___ between C1 and H3: distance=1.094 ang___
between C1 and F4: distance=1.359 ang___ between C1 and F5: distance=2.366 ang___
between C2 and F4: distance=2.365 ang___ between C2 and F5: distance=1.359 ang___
between C2 and H6: distance=1.094 ang___

Bond Angles:

for H3-C1-C2: angle=123.0 deg___ for F4-C1-C2: angle=122.5 deg___
for F5-C2-C1: angle=122.6 deg___ for H6-C2-C1: angle=122.9 deg___

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Bond Orders (Mulliken):

between C1 and C2: order=1.883___ between C1 and H3: order=0.987___
between C1 and F4: order=0.920___ between C1 and F5: order=-0.099___
between C2 and F4: order=-0.099___ between C2 and F5: order=0.920___
between C2 and H6: order=0.987___

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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 1.9966 electrons
__has 50.00% C 1 character in a sp1.41 hybrid
__has 50.00% C 2 character in a sp1.41 hybrid

2. A bonding orbital for C1-C2 with 1.9936 electrons
__has 50.00% C 1 character in a p-pi orbital ( 99.79% p 0.21% d)
__has 50.00% C 2 character in a p-pi orbital ( 99.79% p 0.21% d)

3. A bonding orbital for C1-H3 with 1.9842 electrons
__has 59.15% C 1 character in a sp1.96 hybrid
__has 40.85% H 3 character in a s orbital

4. A bonding orbital for C1-F4 with 1.9968 electrons
__has 28.18% C 1 character in a sp2.97 hybrid
__has 71.82% F 4 character in a sp2.57 hybrid

5. A bonding orbital for C2-F5 with 1.9968 electrons
__has 28.18% C 2 character in a sp2.97 hybrid
__has 71.82% F 5 character in a sp2.57 hybrid

6. A bonding orbital for C2-H6 with 1.9842 electrons
__has 59.14% C 2 character in a sp1.96 hybrid
__has 40.86% H 6 character in a s orbital

11. A lone pair orbital for F4 with 1.9933 electrons
__made from a sp0.39 hybrid

12. A lone pair orbital for F4 with 1.9751 electrons
__made from a p3 hybrid

13. A lone pair orbital for F4 with 1.9530 electrons
__made from a p-pi orbital ( 99.98% p)

14. A lone pair orbital for F5 with 1.9933 electrons
__made from a sp0.39 hybrid

15. A lone pair orbital for F5 with 1.9751 electrons
__made from a p3 hybrid

16. A lone pair orbital for F5 with 1.9530 electrons
__made from a p-pi orbital ( 99.98% p)

-With core pairs on: C 1 C 2 F 4 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, 107, for C2-F5 is 28.5 kJ/mol.

The interaction of bonding donor orbital, 6, for C2-H6 with the antibonding acceptor orbital, 106, for C1-F4 is 28.5 kJ/mol.

The interaction of the second lone pair donor orbital, 12, for F4 with the antibonding acceptor orbital, 103, for C1-C2 is 35.7 kJ/mol.

The interaction of the second lone pair donor orbital, 12, for F4 with the antibonding acceptor orbital, 105, for C1-H3 is 36.3 kJ/mol.

The interaction of the third lone pair donor orbital, 13, for F4 with the second antibonding acceptor orbital, 104, for C1-C2 is 100. kJ/mol.

The interaction of the second lone pair donor orbital, 15, for F5 with the antibonding acceptor orbital, 103, for C1-C2 is 35.8 kJ/mol.

The interaction of the second lone pair donor orbital, 15, for F5 with the antibonding acceptor orbital, 108, for C2-H6 is 36.3 kJ/mol.

The interaction of the third lone pair donor orbital, 16, for F5 with the second antibonding acceptor orbital, 104, for C1-C2 is 100. 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.

20 ----- 2.058
19 ----- 2.003


18 ----- -0.198

17 ----- -1.170


16 -^-v- -6.590


15 -^-v- -9.124

14 -^-v- -9.796


13 -^-v- -10.94

12 -^-v- -11.77

11 -^-v- -12.06


10 -^-v- -13.51

9 -^-v- -13.89


8 -^-v- -15.51


7 -^-v- -19.39


6 -^-v- -30.51

5 -^-v- -30.83


4 -^-v- -268.9
3 -^-v- -268.9


2 -^-v- -656.4 1 -^-v- -656.4

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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 = -277.1646671083 Hartrees

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