H6 H3 \ / C1 - C2 - H5 / \ H9 - C7 H4 | \ Cl10 H8
The multiplicity is 2.

## Atomic Charges and Dipole Moment

C1 charge= 0.031
C2 charge=-0.401
H3 charge= 0.119
H4 charge= 0.160
H5 charge= 0.149
H6 charge= 0.126
C7 charge=-0.395
H8 charge= 0.220
H9 charge= 0.196
CL10 charge=-0.207
with a dipole moment of 2.87736 Debye

## Bond Lengths:

between C1 and C2: distance=1.491 ang___ between C1 and H6: distance=1.098 ang___
between C1 and C7: distance=1.447 ang___ between C2 and H3: distance=1.104 ang___
between C2 and H4: distance=1.112 ang___ between C2 and H5: distance=1.105 ang___
between C7 and H8: distance=1.099 ang___ between C7 and H9: distance=1.097 ang___
between C7 and CL10: distance=1.983 ang___

## Bond Angles:

for H3-C2-C1: angle=111.7 deg___ for H4-C2-C1: angle=110.4 deg___
for H5-C2-C1: angle=112.1 deg___ for H6-C1-C2: angle=118.4 deg___
for C7-C1-C2: angle=122.5 deg___ for H8-C7-C1: angle=115.3 deg___
for H9-C7-C1: angle=115.4 deg___ for CL10-C7-C1: angle=109.2 deg___

## Bond Orders (Mulliken):

between C1 and C2: order=0.819___ between C1 and H6: order=0.908___
between C1 and C7: order=0.992___ between C2 and H3: order=0.977___
between C2 and H4: order=0.958___ between C2 and H5: order=1.005___
between C7 and H8: order=0.979___ between C7 and H9: order=0.950___
between C7 and CL10: order=0.755___

## 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. Please note that your structure can't be well described by a single Lewis structure, because of extensive delocalization.

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-C2 with 0.9967 electrons
__has 51.31% C 1 character in a sp1.87 hybrid
__has 48.69% C 2 character in a sp2.42 hybrid

2. A bonding orbital for C1-H6 with 0.9916 electrons
__has 60.96% C 1 character in a sp2.44 hybrid
__has 39.04% H 6 character in a s orbital

3. A bonding orbital for C1-C7 with 0.9971 electrons
__has 50.27% C 1 character in a sp1.85 hybrid
__has 49.73% C 7 character in a sp1.93 hybrid

4. A bonding orbital for C2-H3 with 0.9962 electrons
__has 59.19% C 2 character in a s0.94 p3 hybrid
__has 40.81% H 3 character in a s orbital

5. A bonding orbital for C2-H4 with 0.9974 electrons
__has 58.21% C 2 character in a s0.88 p3 hybrid
__has 41.79% H 4 character in a s orbital

6. A bonding orbital for C2-H5 with 0.9962 electrons
__has 59.11% C 2 character in a s0.95 p3 hybrid
__has 40.89% H 5 character in a s orbital

7. A bonding orbital for C7-H8 with 0.9937 electrons
__has 59.80% C 7 character in a sp2.74 hybrid
__has 40.20% H 8 character in a s orbital

8. A bonding orbital for C7-H9 with 0.9936 electrons
__has 60.06% C 7 character in a sp2.72 hybrid
__has 39.94% H 9 character in a s orbital

9. A bonding orbital for C7-Cl10 with 0.9966 electrons
__has 28.69% C 7 character in a s0.44 p3 hybrid
__has 71.31% Cl10 character in a s0.53 p3 hybrid

18. A lone pair orbital for C1 with 0.8881 electrons

19. A lone pair orbital for Cl10 with 0.9993 electrons

20. A lone pair orbital for Cl10 with 0.9960 electrons

21. A lone pair orbital for Cl10 with 0.9959 electrons

-With core pairs on: C 1 C 2 C 7 Cl10 Cl10 Cl10 Cl10 Cl10 -

#### Up Electrons

1. A bonding orbital for C1-C2 with 0.9968 electrons
__has 46.76% C 1 character in a sp1.85 hybrid
__has 53.24% C 2 character in a sp2.31 hybrid

2. A bonding orbital for C1-H6 with 0.9924 electrons
__has 55.93% C 1 character in a sp2.37 hybrid
__has 44.07% H 6 character in a s orbital

3. A bonding orbital for C1-C7 with 0.9974 electrons
__has 45.98% C 1 character in a sp1.83 hybrid
__has 54.02% C 7 character in a sp1.91 hybrid

4. A bonding orbital for C2-H3 with 0.9919 electrons
__has 60.67% C 2 character in a s0.92 p3 hybrid
__has 39.33% H 3 character in a s orbital

5. A bonding orbital for C2-H4 with 0.9814 electrons
__has 62.49% C 2 character in a s0.89 p3 hybrid
__has 37.51% H 4 character in a s orbital

6. A bonding orbital for C2-H5 with 0.9942 electrons
__has 60.12% C 2 character in a s0.93 p3 hybrid
__has 39.88% H 5 character in a s orbital

7. A bonding orbital for C7-H8 with 0.9940 electrons
__has 61.06% C 7 character in a sp2.89 hybrid
__has 38.94% H 8 character in a s orbital

8. A bonding orbital for C7-H9 with 0.9936 electrons
__has 61.24% C 7 character in a sp2.87 hybrid
__has 38.76% H 9 character in a s orbital

9. A bonding orbital for C7-Cl10 with 0.9795 electrons
__has 47.19% C 7 character in a s0.50 p3 hybrid
__has 52.81% Cl10 character in a s0.29 p3 hybrid

19. A lone pair orbital for Cl10 with 0.9994 electrons

20. A lone pair orbital for Cl10 with 0.9960 electrons
__made from a p-pi orbital ( 99.99% p)

21. A lone pair orbital for Cl10 with 0.9912 electrons
__made from a s0.20 p3 hybrid

-With core pairs on: C 1 C 2 C 7 Cl10 Cl10 Cl10 Cl10 Cl10 -

#### 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, 5, for C2-H4 with the lone pair acceptor orbital, 18, for C1 is 32.5 kJ/mol.

The interaction of bonding donor orbital, 9, for C7-Cl10 with the lone pair acceptor orbital, 18, for C1 is 35.1 kJ/mol.

The interaction of lone pair donor orbital, 18, for C1 with the antibonding acceptor orbital, 139, for C7-Cl10 is 75.5 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.

25 ----- 1.883

24 ----- 1.586
23 ----- 1.561

22 ----- -0.951

21 -^--- -5.129

20 -^-v- -6.841

19 -^-v- -6.993

18 -^-v- -9.178

17 -^-v- -9.561

16 -^-v- -9.661

15 -^-v- -10.70

14 -^-v- -11.05

13 -^-v- -12.09

12 -^-v- -14.34

11 -^-v- -17.11

10 -^-v- -19.15

9 -^-v- -20.71

8 -^-v- -189.3
7 -^-v- -189.4

6 -^-v- -189.7

5 -^-v- -247.8

4 -^-v- -266.6

3 -^-v- -267.5

2 -^-v- -267.9

1 -^-v- -2729.

## 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 = -578.1572806860 Hartrees