F3 \ C1 - F2 / F4
The multiplicity is 2.

## Atomic Charges and Dipole Moment

C1 charge= 0.390
F2 charge=-0.130
F3 charge=-0.129
F4 charge=-0.129
with a dipole moment of 0.00615 Debye

## Bond Lengths:

between C1 and F2: distance=1.334 ang___ between C1 and F3: distance=1.334 ang___
between C1 and F4: distance=1.334 ang___

## Bond Angles:

for F3-C1-F2: angle=119.9 deg___ for F4-C1-F2: angle=120.0 deg___

## Bond Orders (Mulliken):

between C1 and F2: order=1.055___ between C1 and F3: order=1.055___
between C1 and F4: order=1.055___

## 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. The Lewis structure is built for the up and down electrons, separately. Note that the up and down structures can be very different.

### Hybridization in the Best Lewis Structure

#### Down Electrons

1. A bonding orbital for C1-F2 with 0.9958 electrons
__has 31.37% C 1 character in a sp1.99 hybrid
__has 68.63% F 2 character in a s0.76 p3 hybrid

2. A bonding orbital for C1-F3 with 0.9958 electrons
__has 31.37% C 1 character in a sp1.99 hybrid
__has 68.63% F 3 character in a s0.76 p3 hybrid

3. A bonding orbital for C1-F4 with 0.9958 electrons
__has 31.37% C 1 character in a sp1.99 hybrid
__has 68.63% F 4 character in a s0.76 p3 hybrid

8. A lone pair orbital for C1 with 0.9974 electrons
__made from a p-pi orbital (100.00% p)

9. A lone pair orbital for F2 with 0.9988 electrons
__made from a p-pi orbital ( 99.98% p)

10. A lone pair orbital for F2 with 0.9944 electrons
__made from a sp0.25 hybrid

11. A lone pair orbital for F2 with 0.9787 electrons
__made from a p-pi orbital ( 99.97% p)

12. A lone pair orbital for F3 with 0.9988 electrons
__made from a p-pi orbital ( 99.98% p)

13. A lone pair orbital for F3 with 0.9944 electrons
__made from a sp0.25 hybrid

14. A lone pair orbital for F3 with 0.9787 electrons
__made from a p-pi orbital ( 99.97% p)

15. A lone pair orbital for F4 with 0.9988 electrons
__made from a p-pi orbital ( 99.98% p)

16. A lone pair orbital for F4 with 0.9943 electrons
__made from a sp0.25 hybrid

17. A lone pair orbital for F4 with 0.9787 electrons
__made from a p-pi orbital ( 99.97% p)

-With core pairs on: C 1 F 2 F 3 F 4 -

#### Up Electrons

1. A bonding orbital for C1-F2 with 0.9985 electrons
__has 26.36% C 1 character in a sp1.99 hybrid
__has 73.64% F 2 character in a sp2.92 hybrid

2. A bonding orbital for C1-F3 with 0.9985 electrons
__has 26.36% C 1 character in a sp1.99 hybrid
__has 73.64% F 3 character in a sp2.92 hybrid

3. A bonding orbital for C1-F4 with 0.9985 electrons
__has 26.36% C 1 character in a sp1.99 hybrid
__has 73.64% F 4 character in a sp2.92 hybrid

8. A lone pair orbital for C1 with 0.1201 electrons
__made from a p-pi orbital (100.00% p)

9. A lone pair orbital for F2 with 0.9955 electrons
__made from a sp0.34 hybrid

10. A lone pair orbital for F2 with 0.9791 electrons
__made from a p-pi orbital ( 99.96% p)

11. A lone pair orbital for F2 with 0.9589 electrons
__made from a p-pi orbital ( 99.96% p)

12. A lone pair orbital for F3 with 0.9955 electrons
__made from a sp0.34 hybrid

13. A lone pair orbital for F3 with 0.9790 electrons
__made from a p-pi orbital ( 99.96% p)

14. A lone pair orbital for F3 with 0.9589 electrons
__made from a p-pi orbital ( 99.96% p)

15. A lone pair orbital for F4 with 0.9955 electrons
__made from a sp0.34 hybrid

16. A lone pair orbital for F4 with 0.9790 electrons
__made from a p-pi orbital ( 99.96% p)

17. A lone pair orbital for F4 with 0.9589 electrons
__made from a p-pi orbital ( 99.96% p)

-With core pairs on: C 1 F 2 F 3 F 4 -

#### 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 the second lone pair donor orbital, 10, for F2 with the antibonding acceptor orbital, 95, for C1-F3 is 30.3 kJ/mol.

The interaction of the second lone pair donor orbital, 10, for F2 with the antibonding acceptor orbital, 96, for C1-F4 is 30.3 kJ/mol.

The interaction of the third lone pair donor orbital, 11, for F2 with the lone pair acceptor orbital, 8, for C1 is 105. kJ/mol.

The interaction of the second lone pair donor orbital, 13, for F3 with the antibonding acceptor orbital, 94, for C1-F2 is 30.3 kJ/mol.

The interaction of the second lone pair donor orbital, 13, for F3 with the antibonding acceptor orbital, 96, for C1-F4 is 30.3 kJ/mol.

The interaction of the third lone pair donor orbital, 14, for F3 with the lone pair acceptor orbital, 8, for C1 is 105. kJ/mol.

The interaction of the second lone pair donor orbital, 16, for F4 with the antibonding acceptor orbital, 94, for C1-F2 is 30.3 kJ/mol.

The interaction of the second lone pair donor orbital, 16, for F4 with the antibonding acceptor orbital, 95, for C1-F3 is 30.3 kJ/mol.

The interaction of the third lone pair donor orbital, 17, for F4 with the lone pair acceptor orbital, 8, for C1 is 105. 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. Only the spin up electron orbital energies are given.

21 ----- 3.733

20 ----- 3.021 19 ----- 3.017

18 ----- -1.387

17 -^--- -3.995

16 -^-v- -10.79

15 -^-v- -11.59 14 -^-v- -11.59

13 -^-v- -11.92 12 -^-v- -11.92

11 -^-v- -14.12

10 -^-v- -15.51 9 -^-v- -15.52

8 -^-v- -17.71

7 -^-v- -31.55 6 -^-v- -31.55

5 -^-v- -33.22

4 -^-v- -272.5

3 -^-v- -657.7 2 -^-v- -657.7 1 -^-v- -657.7

## 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 = -337.6670502303 Hartrees