chlorovinylidene, ClCH=C

 H3 \ C1 = C2 / CL4
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=-0.017
C2 charge=-0.198
H3 charge= 0.208
CL4 charge= 0.007
with a dipole moment of 2.07773 Debye

Bond Lengths:

between C1 and C2: distance=1.322 ang___ between C1 and H3: distance=1.104 ang___
between C1 and CL4: distance=1.752 ang___ between C2 and CL4: distance=2.697 ang___

Bond Angles:

for H3-C1-C2: angle=119.7 deg___ for CL4-C1-C2: angle=121.9 deg___

Bond Orders (Mulliken):

between C1 and C2: order=1.879___ between C1 and H3: order=0.877___
between C1 and CL4: order=0.869___ between C2 and CL4: order=0.078___

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 1.9969 electrons
__has 58.57% C 1 character in a sp1.36 hybrid
__has 41.43% C 2 character in a sp2.09 hybrid

2. A bonding orbital for C1-C2 with 1.9969 electrons
__has 59.09% C 1 character in a p3 hybrid
__has 40.91% C 2 character in a p3 hybrid

3. A bonding orbital for C1-H3 with 1.9737 electrons
__has 63.26% C 1 character in a sp2.15 hybrid
__has 36.74% H 3 character in a s orbital

4. A bonding orbital for C1-Cl4 with 1.9844 electrons
__has 47.65% C 1 character in a sp2.78 hybrid
__has 52.35% Cl 4 character in a s0.54 p3 hybrid

12. A lone pair orbital for C2 with 1.9815 electrons

14. A lone pair orbital for Cl4 with 1.9949 electrons

15. A lone pair orbital for Cl4 with 1.9713 electrons
__made from a s0.05 p3 hybrid

16. A lone pair orbital for Cl4 with 1.9596 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 second lone pair acceptor orbital, 13, for C2 is 54.8 kJ/mol.

The interaction of bonding donor orbital, 4, for C1-Cl4 with the second lone pair acceptor orbital, 13, for C2 is 22.8 kJ/mol.

The interaction of the second lone pair donor orbital, 15, for Cl4 with the antibonding acceptor orbital, 82, for C1-C2 is 24.3 kJ/mol.

The interaction of the second lone pair donor orbital, 15, for Cl4 with the antibonding acceptor orbital, 84, for C1-H3 is 26.5 kJ/mol.

The interaction of the third lone pair donor orbital, 16, for Cl4 with the second antibonding acceptor orbital, 83, for C1-C2 is 67.1 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.

19 ----- 2.300

18 ----- -0.453

17 ----- -1.462

16 ----- -5.241

15 -^-v- -7.104

14 -^-v- -7.356

13 -^-v- -8.657

12 -^-v- -9.778

11 -^-v- -12.33

10 -^-v- -13.96

9 -^-v- -19.04

8 -^-v- -22.66

7 -^-v- -191.3 6 -^-v- -191.3

5 -^-v- -191.8

4 -^-v- -249.8

3 -^-v- -268.4

2 -^-v- -268.8

1 -^-v- -2731.

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 = -536.9093200563 Hartrees