## CH2Si, CH2=Si

 H3 \ C1 = SI2 / H4
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=-0.493
SI2 charge= 0.247
H3 charge= 0.123
H4 charge= 0.123
with a dipole moment of 0.07834 Debye

## Bond Lengths:

between C1 and SI2: distance=1.727 ang___ between C1 and H3: distance=1.102 ang___
between C1 and H4: distance=1.102 ang___

## Bond Angles:

for H3-C1-SI2: angle=123.6 deg___ for H4-C1-SI2: angle=123.5 deg___

## Bond Orders (Mulliken):

between C1 and SI2: order=1.745___ between C1 and H3: order=0.927___
between C1 and H4: order=0.927___

## 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-Si2 with 1.9999 electrons
__has 67.35% C 1 character in a p-pi orbital ( 99.87% p 0.13% d)
__has 32.65% Si 2 character in a p-pi orbital ( 98.73% p 1.27% d)

2. A bonding orbital for C1-Si2 with 1.9992 electrons
__has 76.88% C 1 character in a sp1.40 hybrid
__has 23.12% Si 2 character in a s0.81 p3 hybrid

3. A bonding orbital for C1-H3 with 1.9894 electrons
__has 61.57% C 1 character in a sp2.41 hybrid
__has 38.43% H 3 character in a s orbital

4. A bonding orbital for C1-H4 with 1.9894 electrons
__has 61.57% C 1 character in a sp2.41 hybrid
__has 38.43% H 4 character in a s orbital

11. A lone pair orbital for Si2 with 1.9932 electrons

-With core pairs on: C 1 Si 2 Si 2 Si 2 Si 2 Si 2 -

#### 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.

## 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.

15 ----- 2.898

14 ----- 0.602

13 ----- -1.951

12 ----- -3.652

11 -^-v- -5.668

10 -^-v- -6.615

9 -^-v- -10.06

8 -^-v- -11.16

7 -^-v- -16.33

6 -^-v- -94.48

5 -^-v- -94.72

4 -^-v- -95.06

3 -^-v- -137.1

2 -^-v- -265.9

1 -^-v- -1772.

## 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 = -328.7512545824 Hartrees