## CH2=CHF, fluoroethylene

 H3 H6 \ / C1 = C2 / \ H4 F5
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=-0.599
C2 charge= 0.163
H3 charge= 0.220
H4 charge= 0.265
F5 charge=-0.174
H6 charge= 0.125
with a dipole moment of 1.55758 Debye

## Bond Lengths:

between C1 and C2: distance=1.332 ang___ between C1 and H3: distance=1.093 ang___
between C1 and H4: distance=1.094 ang___ between C1 and F5: distance=2.361 ang___
between C2 and F5: distance=1.370 ang___ between C2 and H6: distance=1.095 ang___

## Bond Angles:

for H3-C1-C2: angle=119.2 deg___ for H4-C1-C2: angle=121.6 deg___
for F5-C2-C1: angle=121.8 deg___ for H6-C2-C1: angle=126.7 deg___

## Bond Orders (Mulliken):

between C1 and C2: order=1.947___ between C1 and H3: order=0.966___
between C1 and H4: order=0.980___ between C1 and F5: order=-0.056___
between C2 and F5: order=0.815___ between C2 and H6: order=0.977___

## 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 1.9972 electrons
__has 49.71% C 1 character in a sp1.63 hybrid
__has 50.29% C 2 character in a sp1.25 hybrid

2. A bonding orbital for C1-C2 with 1.9971 electrons
__has 52.71% C 1 character in a p-pi orbital ( 99.83% p 0.17% d)
__has 47.29% C 2 character in a p-pi orbital ( 99.82% p 0.18% d)

3. A bonding orbital for C1-H3 with 1.9816 electrons
__has 59.98% C 1 character in a sp2.26 hybrid
__has 40.02% H 3 character in a s orbital

4. A bonding orbital for C1-H4 with 1.9860 electrons
__has 60.37% C 1 character in a sp2.16 hybrid
__has 39.63% H 4 character in a s orbital

5. A bonding orbital for C2-F5 with 1.9967 electrons
__has 27.12% C 2 character in a s0.93 p3 hybrid
__has 72.88% F 5 character in a sp2.50 hybrid

6. A bonding orbital for C2-H6 with 1.9855 electrons
__has 58.70% C 2 character in a sp2.09 hybrid
__has 41.30% H 6 character in a s orbital

10. A lone pair orbital for F5 with 1.9925 electrons

11. A lone pair orbital for F5 with 1.9785 electrons

12. A lone pair orbital for F5 with 1.9529 electrons
__made from a p-pi orbital ( 99.98% p)

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

#### 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, 89, for C2-F5 is 38.4 kJ/mol.

The interaction of bonding donor orbital, 4, for C1-H4 with the antibonding acceptor orbital, 90, for C2-H6 is 23.9 kJ/mol.

The interaction of the second lone pair donor orbital, 11, for F5 with the antibonding acceptor orbital, 85, for C1-C2 is 29.6 kJ/mol.

The interaction of the second lone pair donor orbital, 11, for F5 with the antibonding acceptor orbital, 90, for C2-H6 is 33.9 kJ/mol.

The interaction of the third lone pair donor orbital, 12, for F5 with the second antibonding acceptor orbital, 86, for C1-C2 is 99.9 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.

16 ----- 2.457

15 ----- 1.934

14 ----- 1.307

13 ----- -1.223

12 -^-v- -6.722

11 -^-v- -8.959

10 -^-v- -10.02

9 -^-v- -11.06

8 -^-v- -11.88

7 -^-v- -13.05

6 -^-v- -14.99

5 -^-v- -19.04

4 -^-v- -30.25

3 -^-v- -266.5

2 -^-v- -268.7

1 -^-v- -656.0

## 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 = -177.8932442008 Hartrees