vinylchloride, CH2=CHCl

 H3 H6 \ / C1 = C2 / \ CL4 H5
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=-0.122
C2 charge=-0.382
H3 charge= 0.187
CL4 charge=-0.075
H5 charge= 0.208
H6 charge= 0.184
with a dipole moment of 1.49447 Debye

Bond Lengths:

between C1 and C2: distance=1.336 ang___ between C1 and H3: distance=1.095 ang___
between C1 and CL4: distance=1.762 ang___ between C2 and CL4: distance=2.732 ang___
between C2 and H5: distance=1.094 ang___ between C2 and H6: distance=1.095 ang___

Bond Angles:

for H3-C1-C2: angle=124.7 deg___ for CL4-C1-C2: angle=123.1 deg___
for H5-C2-C1: angle=122.5 deg___ for H6-C2-C1: angle=119.2 deg___

Bond Orders (Mulliken):

between C1 and C2: order=1.938___ between C1 and H3: order=0.907___
between C1 and CL4: order=0.838___ between C2 and CL4: order=0.059___
between C2 and H5: order=0.965___ between C2 and H6: order=0.963___

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 50.81% C 1 character in a sp1.30 hybrid
__has 49.19% C 2 character in a sp1.53 hybrid

2. A bonding orbital for C1-C2 with 1.9963 electrons
__has 51.38% C 1 character in a p-pi orbital ( 99.87% p 0.13% d)
__has 48.62% C 2 character in a p-pi orbital ( 99.83% p 0.17% d)

3. A bonding orbital for C1-H3 with 1.9848 electrons
__has 60.82% C 1 character in a sp2.12 hybrid
__has 39.18% H 3 character in a s orbital

4. A bonding orbital for C1-Cl4 with 1.9916 electrons
__has 44.07% C 1 character in a s0.99 p3 hybrid
__has 55.93% Cl 4 character in a s0.63 p3 hybrid

5. A bonding orbital for C2-H5 with 1.9866 electrons
__has 60.24% C 2 character in a sp2.24 hybrid
__has 39.76% H 5 character in a s orbital

6. A bonding orbital for C2-H6 with 1.9782 electrons
__has 59.89% C 2 character in a sp2.33 hybrid
__has 40.11% H 6 character in a s orbital

14. A lone pair orbital for Cl4 with 1.9945 electrons

15. A lone pair orbital for Cl4 with 1.9774 electrons

16. A lone pair orbital for Cl4 with 1.9504 electrons
__made from a p-pi orbital ( 99.97% p)

-With core pairs on: C 1 C 2 Cl 4 Cl 4 Cl 4 Cl 4 Cl 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 bonding donor orbital, 3, for C1-H3 with the antibonding acceptor orbital, 96, for C2-H5 is 20.5 kJ/mol.

The interaction of bonding donor orbital, 5, for C2-H5 with the antibonding acceptor orbital, 94, for C1-H3 is 24.5 kJ/mol.

The interaction of bonding donor orbital, 6, for C2-H6 with the antibonding acceptor orbital, 95, for C1-Cl4 is 43.3 kJ/mol.

The interaction of the second lone pair donor orbital, 15, for Cl4 with the antibonding acceptor orbital, 92, for C1-C2 is 26.1 kJ/mol.

The interaction of the second lone pair donor orbital, 15, for Cl4 with the antibonding acceptor orbital, 94, for C1-H3 is 25.7 kJ/mol.

The interaction of the third lone pair donor orbital, 16, for Cl4 with the second antibonding acceptor orbital, 93, for C1-C2 is 79.9 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.

20 ----- 2.256

19 ----- 1.847

18 ----- -0.349

17 ----- -1.584

16 -^-v- -6.585

15 -^-v- -7.610

14 -^-v- -9.047

13 -^-v- -9.444

12 -^-v- -11.19

11 -^-v- -12.08

10 -^-v- -14.37

9 -^-v- -18.54

8 -^-v- -21.72

7 -^-v- -190.3
6 -^-v- -190.3

5 -^-v- -190.7

4 -^-v- -248.7

3 -^-v- -266.7

2 -^-v- -268.2

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 = -538.2567283497 Hartrees