CH2FCH2Cl, fluorochloroethane

H3CL8H7
\ | /
H5 - C1 - C2
/ \
F4H6
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= 0.269
C2 charge=-0.331
H3 charge= 0.049
F4 charge=-0.277
H5 charge= 0.050
H6 charge= 0.191
H7 charge= 0.190
CL8 charge=-0.142
with a dipole moment of 0.06869 Debye

Bond Lengths:

between C1 and C2: distance=1.526 ang___ between C1 and H3: distance=1.105 ang___
between C1 and F4: distance=1.420 ang___ between C1 and H5: distance=1.105 ang___
between C2 and H6: distance=1.101 ang___ between C2 and H7: distance=1.101 ang___
between C2 and CL8: distance=1.825 ang___

Bond Angles:

for H3-C1-C2: angle=111.4 deg___ for F4-C1-C2: angle=107.8 deg___
for H5-C1-C2: angle=111.4 deg___ for H6-C2-C1: angle=111.4 deg___
for H7-C2-C1: angle=111.4 deg___ for CL8-C2-C1: angle=108.7 deg___

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Bond Orders (Mulliken):

between C1 and C2: order=0.908___ between C1 and H3: order=0.985___
between C1 and F4: order=0.759___ between C1 and H5: order=0.985___
between C2 and H6: order=0.944___ between C2 and H7: order=0.944___
between C2 and CL8: order=0.856___

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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 1.9953 electrons
__has 48.73% C 1 character in a sp2.37 hybrid
__has 51.27% C 2 character in a sp2.46 hybrid

2. A bonding orbital for C1-H3 with 1.9914 electrons
__has 58.43% C 1 character in a sp2.91 hybrid
__has 41.57% H 3 character in a s orbital

3. A bonding orbital for C1-F4 with 1.9953 electrons
__has 27.32% C 1 character in a s0.74 p3 hybrid
__has 72.68% F 4 character in a sp2.88 hybrid

4. A bonding orbital for C1-H5 with 1.9913 electrons
__has 58.43% C 1 character in a sp2.91 hybrid
__has 41.57% H 5 character in a s orbital

5. A bonding orbital for C2-H6 with 1.9916 electrons
__has 60.68% C 2 character in a sp2.85 hybrid
__has 39.32% H 6 character in a s orbital

6. A bonding orbital for C2-H7 with 1.9916 electrons
__has 60.68% C 2 character in a sp2.85 hybrid
__has 39.32% H 7 character in a s orbital

7. A bonding orbital for C2-Cl8 with 1.9900 electrons
__has 42.97% C 2 character in a s0.72 p3 hybrid
__has 57.03% Cl 8 character in a s0.52 p3 hybrid

16. A lone pair orbital for F4 with 1.9953 electrons
__made from a sp0.35 hybrid

17. A lone pair orbital for F4 with 1.9811 electrons
__made from a p-pi orbital ( 99.98% p)

18. A lone pair orbital for F4 with 1.9780 electrons
__made from a p3 hybrid

19. A lone pair orbital for Cl8 with 1.9982 electrons
__made from a sp0.17 hybrid

20. A lone pair orbital for Cl8 with 1.9836 electrons
__made from a p-pi orbital ( 99.98% p)

21. A lone pair orbital for Cl8 with 1.9796 electrons
__made from a p3 hybrid

-With core pairs on: C 1 C 2 F 4 Cl 8 Cl 8 Cl 8 Cl 8 Cl 8 -

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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 the second lone pair donor orbital, 17, for F4 with the antibonding acceptor orbital, 122, for C1-H3 is 24.5 kJ/mol.

The interaction of the second lone pair donor orbital, 17, for F4 with the antibonding acceptor orbital, 124, for C1-H5 is 24.5 kJ/mol.

The interaction of the third lone pair donor orbital, 18, for F4 with the antibonding acceptor orbital, 121, for C1-C2 is 27.6 kJ/mol.

The interaction of the third lone pair donor orbital, 21, for Cl8 with the antibonding acceptor orbital, 121, for C1-C2 is 20.2 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.

25 ----- 1.852

24 ----- 1.663

23 ----- 0.776


22 ----- -1.277


21 -^-v- -7.476
20 -^-v- -7.556

19 -^-v- -8.361

18 -^-v- -8.831


17 -^-v- -10.49

16 -^-v- -10.63


15 -^-v- -11.69

14 -^-v- -12.65

13 -^-v- -12.77


12 -^-v- -15.71


11 -^-v- -18.48


10 -^-v- -21.66


9 -^-v- -29.65


8 -^-v- -190.2 7 -^-v- -190.3

6 -^-v- -190.7


5 -^-v- -248.7


4 -^-v- -268.3

3 -^-v- -268.8


2 -^-v- -655.6


1 -^-v- -2729.

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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 = -638.7672308425 Hartrees

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