## cis-dichloroethylene, ClHC=CHCl

 H3 H6 \ / C1 = C2 / \ CL4 CL5
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=-0.166
C2 charge=-0.162
H3 charge= 0.189
CL4 charge=-0.023
CL5 charge=-0.025
H6 charge= 0.188
with a dipole moment of 1.89638 Debye

## Bond Lengths:

between C1 and C2: distance=1.340 ang___ between C1 and H3: distance=1.094 ang___
between C1 and CL4: distance=1.742 ang___ between C2 and CL5: distance=1.743 ang___
between C2 and H6: distance=1.094 ang___

## Bond Angles:

for H3-C1-C2: angle=120.8 deg___ for CL4-C1-C2: angle=125.0 deg___
for CL5-C2-C1: angle=124.9 deg___ for H6-C2-C1: angle=121.0 deg___

## Bond Orders (Mulliken):

between C1 and C2: order=1.899___ between C1 and H3: order=0.916___
between C1 and CL4: order=0.864___ between C2 and CL5: order=0.865___
between C2 and H6: order=0.916___

## 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 1.9967 electrons
__has 50.00% C 1 character in a sp1.38 hybrid
__has 50.00% C 2 character in a sp1.38 hybrid

2. A bonding orbital for C1-C2 with 1.9932 electrons
__has 50.00% C 1 character in a p-pi orbital ( 99.86% p 0.14% d)
__has 50.00% C 2 character in a p-pi orbital ( 99.86% p 0.14% d)

3. A bonding orbital for C1-H3 with 1.9791 electrons
__has 61.42% C 1 character in a sp2.11 hybrid
__has 38.58% H 3 character in a s orbital

4. A bonding orbital for C1-Cl4 with 1.9919 electrons
__has 45.79% C 1 character in a sp2.81 hybrid
__has 54.21% Cl 4 character in a s0.62 p3 hybrid

5. A bonding orbital for C2-Cl5 with 1.9919 electrons
__has 45.75% C 2 character in a sp2.82 hybrid
__has 54.25% Cl 5 character in a s0.62 p3 hybrid

6. A bonding orbital for C2-H6 with 1.9792 electrons
__has 61.43% C 2 character in a sp2.11 hybrid
__has 38.57% H 6 character in a s orbital

19. A lone pair orbital for Cl4 with 1.9950 electrons
__made from a sp0.20 hybrid

20. A lone pair orbital for Cl4 with 1.9743 electrons
__made from a p3 hybrid

21. A lone pair orbital for Cl4 with 1.9427 electrons
__made from a p-pi orbital ( 99.97% p)

22. A lone pair orbital for Cl5 with 1.9951 electrons
__made from a sp0.20 hybrid

23. A lone pair orbital for Cl5 with 1.9744 electrons
__made from a p3 hybrid

24. A lone pair orbital for Cl5 with 1.9428 electrons
__made from a p-pi orbital ( 99.97% p)

118. A antibonding orbital for C1-C2 with 0.1101 electrons
__has 50.00% C 1 character in a p-pi orbital ( 99.86% p 0.14% d)
__has 50.00% C 2 character in a p-pi orbital ( 99.86% p 0.14% d)

-With core pairs on: C 1 C 2 Cl 4 Cl 4 Cl 4 Cl 4 Cl 4 Cl 5 Cl 5 Cl 5 Cl 5 Cl 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, 121, for C2-Cl5 is 38.6 kJ/mol.

The interaction of bonding donor orbital, 6, for C2-H6 with the antibonding acceptor orbital, 120, for C1-Cl4 is 38.4 kJ/mol.

The interaction of the second lone pair donor orbital, 20, for Cl4 with the antibonding acceptor orbital, 117, for C1-C2 is 28.7 kJ/mol.

The interaction of the second lone pair donor orbital, 20, for Cl4 with the antibonding acceptor orbital, 119, for C1-H3 is 28.2 kJ/mol.

The interaction of the third lone pair donor orbital, 21, for Cl4 with the second antibonding acceptor orbital, 118, for C1-C2 is 91.7 kJ/mol.

The interaction of the second lone pair donor orbital, 23, for Cl5 with the antibonding acceptor orbital, 117, for C1-C2 is 28.7 kJ/mol.

The interaction of the second lone pair donor orbital, 23, for Cl5 with the antibonding acceptor orbital, 122, for C2-H6 is 28.0 kJ/mol.

The interaction of the third lone pair donor orbital, 24, for Cl5 with the second antibonding acceptor orbital, 118, for C1-C2 is 91.4 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.

28 ----- 1.809

27 ----- 0.210

26 ----- -1.124

25 ----- -1.750

24 -^-v- -6.448

23 -^-v- -7.735

22 -^-v- -8.001

21 -^-v- -8.553

20 -^-v- -9.829

19 -^-v- -10.27

18 -^-v- -11.81

17 -^-v- -12.76

16 -^-v- -14.38

15 -^-v- -18.41

14 -^-v- -21.50

13 -^-v- -22.54

12 -^-v- -190.6 11 -^-v- -190.6
10 -^-v- -190.7 9 -^-v- -190.7

8 -^-v- -191.0 7 -^-v- -191.1

6 -^-v- -249.1 5 -^-v- -249.1

4 -^-v- -268.4
3 -^-v- -268.4

2 -^-v- -2730. 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 = -997.8988580470 Hartrees