H8 H3 \ / C1 = C2 // \ H7 - C5 H4 \ Cl6
The multiplicity is 2.

Atomic Charges and Dipole Moment

C1 charge= 0.019
C2 charge=-0.431
H3 charge= 0.175
H4 charge= 0.196
C5 charge=-0.246
CL6 charge=-0.026
H7 charge= 0.187
H8 charge= 0.124
with a dipole moment of 1.25684 Debye

Bond Lengths:

between C1 and C2: distance=1.387 ang___ between C1 and H4: distance=2.168 ang___
between C1 and C5: distance=1.395 ang___ between C1 and H8: distance=1.100 ang___
between C2 and H3: distance=1.093 ang___ between C2 and H4: distance=1.095 ang___
between C2 and C5: distance=2.497 ang___ between C5 and CL6: distance=1.745 ang___
between C5 and H7: distance=1.093 ang___

Bond Angles:

for H3-C2-C1: angle=120.5 deg___ for H4-C2-C1: angle=121.3 deg___
for C5-C1-C2: angle=127.7 deg___ for CL6-C5-C1: angle=122.9 deg___
for H7-C5-C1: angle=123.7 deg___ for H8-C1-C2: angle=118.4 deg___

Bond Orders (Mulliken):

between C1 and C2: order=1.242___ between C1 and H4: order=-0.065___
between C1 and C5: order=1.253___ between C1 and H8: order=0.908___
between C2 and H3: order=0.981___ between C2 and H4: order=0.975___
between C2 and C5: order=0.163___ between C5 and CL6: order=0.790___
between C5 and H7: order=0.926___

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 0.9961 electrons
__has 49.97% C 1 character in a sp1.65 hybrid
__has 50.03% C 2 character in a sp1.58 hybrid

2. A bonding orbital for C1-C5 with 0.9963 electrons
__has 47.98% C 1 character in a sp1.85 hybrid
__has 52.02% C 5 character in a sp1.37 hybrid

3. A bonding orbital for C1-H8 with 0.9857 electrons
__has 58.39% C 1 character in a sp2.63 hybrid
__has 41.61% H 8 character in a s orbital

4. A bonding orbital for C2-H3 with 0.9943 electrons
__has 60.91% C 2 character in a sp2.25 hybrid
__has 39.09% H 3 character in a s orbital

5. A bonding orbital for C2-H4 with 0.9942 electrons
__has 61.25% C 2 character in a sp2.23 hybrid
__has 38.75% H 4 character in a s orbital

6. A bonding orbital for C5-Cl6 with 0.9955 electrons
__has 45.93% C 5 character in a sp2.97 hybrid
__has 54.07% Cl 6 character in a s0.59 p3 hybrid

7. A bonding orbital for C5-H7 with 0.9933 electrons
__has 62.49% C 5 character in a sp2.04 hybrid
__has 37.51% H 7 character in a s orbital

16. A lone pair orbital for C1 with 0.2887 electrons
__made from a p-pi orbital ( 99.94% p 0.06% d)

17. A lone pair orbital for C2 with 0.8432 electrons
__made from a p-pi orbital ( 99.97% p)

18. A lone pair orbital for C5 with 0.8674 electrons
__made from a p-pi orbital ( 99.99% p)

19. A lone pair orbital for Cl6 with 0.9974 electrons

20. A lone pair orbital for Cl6 with 0.9932 electrons
__made from a p-pi orbital (100.00% p)

21. A lone pair orbital for Cl6 with 0.9880 electrons

-With core pairs on: C 1 C 2 C 5 Cl 6 Cl 6 Cl 6 Cl 6 Cl 6 -

Up Electrons

1. A bonding orbital for C1-C2 with 0.9957 electrons
__has 54.79% C 1 character in a sp1.63 hybrid
__has 45.21% C 2 character in a sp1.64 hybrid

2. A bonding orbital for C1-C2 with 0.8677 electrons
__has 84.85% C 1 character in a p-pi orbital ( 99.98% p)
__has 15.15% C 2 character in a p-pi orbital ( 99.78% p 0.22% d)

3. A bonding orbital for C1-C5 with 0.9961 electrons
__has 53.23% C 1 character in a sp1.80 hybrid
__has 46.77% C 5 character in a sp1.44 hybrid

4. A bonding orbital for C1-H8 with 0.9854 electrons
__has 61.40% C 1 character in a sp2.76 hybrid
__has 38.60% H 8 character in a s orbital

5. A bonding orbital for C2-H3 with 0.9951 electrons
__has 56.64% C 2 character in a sp2.22 hybrid
__has 43.36% H 3 character in a s orbital

6. A bonding orbital for C2-H4 with 0.9947 electrons
__has 57.12% C 2 character in a sp2.19 hybrid
__has 42.88% H 4 character in a s orbital

7. A bonding orbital for C5-Cl6 with 0.9964 electrons
__has 41.17% C 5 character in a sp2.84 hybrid
__has 58.83% Cl 6 character in a s0.69 p3 hybrid

8. A bonding orbital for C5-H7 with 0.9943 electrons
__has 57.82% C 5 character in a sp2.02 hybrid
__has 42.18% H 7 character in a s orbital

17. A lone pair orbital for C5 with 0.1789 electrons
__made from a p-pi orbital ( 99.87% p 0.13% d)

18. A lone pair orbital for Cl6 with 0.9976 electrons

19. A lone pair orbital for Cl6 with 0.9870 electrons

20. A lone pair orbital for Cl6 with 0.9518 electrons
__made from a p-pi orbital ( 99.92% p 0.08% d)

-With core pairs on: C 1 C 2 C 5 Cl 6 Cl 6 Cl 6 Cl 6 Cl 6 -

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 bonding donor orbital, 2, for C1-C2 with the lone pair acceptor orbital, 17, for C5 is 263. kJ/mol.

The interaction of the third lone pair donor orbital, 20, for Cl6 with the lone pair acceptor orbital, 17, for C5 is 88.6 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.

24 ----- 2.123

23 ----- 1.742

22 ----- -0.330

21 ----- -0.544

20 -^--- -4.802

19 -^-v- -7.528

18 -^-v- -7.749

17 -^-v- -9.127

16 -^-v- -9.444

15 -^-v- -10.15

14 -^-v- -11.34

13 -^-v- -12.47

12 -^-v- -13.68

11 -^-v- -16.71

10 -^-v- -19.41

9 -^-v- -22.00

8 -^-v- -190.5
7 -^-v- -190.6

6 -^-v- -190.9

5 -^-v- -249.0

4 -^-v- -266.7

3 -^-v- -266.9

2 -^-v- -268.3

1 -^-v- -2730.

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 = -576.9416853441 Hartrees