CH2=C=O, Ketene

 H3 \ C1 = C2 = O5 / 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=-1.134
C2 charge= 0.719
H3 charge= 0.383
H4 charge= 0.383
O5 charge=-0.351
with a dipole moment of 1.62944 Debye

Bond Lengths:

between C1 and C2: distance=1.318 ang___ between C1 and H3: distance=1.092 ang___
between C1 and H4: distance=1.092 ang___ between C2 and O5: distance=1.180 ang___

Bond Angles:

for H3-C1-C2: angle=119.9 deg___ for H4-C1-C2: angle=120.0 deg___
for O5-C2-C1: angle=179.9 deg___

Bond Orders (Mulliken):

between C1 and C2: order=1.854___ between C1 and H3: order=0.941___
between C1 and H4: order=0.941___ between C2 and O5: order=1.841___

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.

Hybridization in the Best Lewis Structure

1. A bonding orbital for C1-C2 with 1.9957 electrons
__has 48.77% C 1 character in a sp1.90 hybrid
__has 51.23% C 2 character in a sp0.70 hybrid

2. A bonding orbital for C1-C2 with 1.9931 electrons
__has 64.24% C 1 character in a p-pi orbital ( 99.80% p 0.20% d)
__has 35.76% C 2 character in a p-pi orbital ( 99.71% p 0.29% d)

3. A bonding orbital for C1-H3 with 1.9620 electrons
__has 62.14% C 1 character in a sp2.05 hybrid
__has 37.86% H 3 character in a s orbital

4. A bonding orbital for C1-H4 with 1.9621 electrons
__has 62.15% C 1 character in a sp2.04 hybrid
__has 37.85% H 4 character in a s orbital

5. A bonding orbital for C2-O5 with 1.9985 electrons
__has 34.88% C 2 character in a sp1.40 hybrid
__has 65.12% O 5 character in a sp1.41 hybrid

6. A bonding orbital for C2-O5 with 1.9930 electrons
__has 26.16% C 2 character in a p-pi orbital ( 99.44% p 0.56% d)
__has 73.84% O 5 character in a p-pi orbital ( 99.76% p 0.24% d)

10. A lone pair orbital for O5 with 1.9754 electrons

11. A lone pair orbital for O5 with 1.7677 electrons
__made from a p-pi orbital ( 99.83% p 0.17% d)

80. A antibonding orbital for C1-C2 with 0.2216 electrons
__has 35.76% C 1 character in a p-pi orbital ( 99.80% p 0.20% d)
__has 64.24% C 2 character in a p-pi orbital ( 99.71% p 0.29% d)

-With core pairs on: C 1 C 2 O 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, 83, for C2-O5 is 30.7 kJ/mol.

The interaction of bonding donor orbital, 3, for C1-H3 with the second antibonding acceptor orbital, 84, for C2-O5 is 51.9 kJ/mol.

The interaction of bonding donor orbital, 4, for C1-H4 with the antibonding acceptor orbital, 83, for C2-O5 is 30.7 kJ/mol.

The interaction of bonding donor orbital, 4, for C1-H4 with the second antibonding acceptor orbital, 84, for C2-O5 is 51.5 kJ/mol.

The interaction of lone pair donor orbital, 10, for O5 with the antibonding acceptor orbital, 79, for C1-C2 is 52.3 kJ/mol.

The interaction of the second lone pair donor orbital, 11, for O5 with the second antibonding acceptor orbital, 80, for C1-C2 is 526. 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.

15 ----- 2.440

14 ----- 1.731

13 ----- 0.060

12 ----- -2.496

11 -^-v- -6.107

10 -^-v- -10.11

9 -^-v- -11.06

8 -^-v- -12.05

7 -^-v- -12.16

6 -^-v- -13.27

5 -^-v- -19.25

4 -^-v- -27.85

3 -^-v- -266.7

2 -^-v- -269.7

1 -^-v- -508.3

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 = -152.6599479912 Hartrees