## H2O...CH2C=O, Water formaldehyde complex

 H3 / H4 - C1 O5 - H6 \ | O2 H7
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= 0.380
O2 charge=-0.393
H3 charge= 0.033
H4 charge= 0.028
O5 charge=-0.788
H6 charge= 0.384
H7 charge= 0.355
with a dipole moment of 2.60585 Debye

## Bond Lengths:

between C1 and O2: distance=1.226 ang___ between C1 and H3: distance=1.117 ang___
between C1 and H4: distance=1.118 ang___ between O5 and H6: distance=0.972 ang___
between O5 and H7: distance=0.986 ang___

## Bond Angles:

for H3-C1-O2: angle=121.2 deg___ for H4-C1-O2: angle=120.8 deg___
for O5-O2-C1: angle=98.13 deg___ for H6-O2-C1: angle=107.0 deg___
for H7-O2-C1: angle=105.6 deg___

## Bond Orders (Mulliken):

between C1 and O2: order=1.838___ between C1 and H3: order=0.943___
between C1 and H4: order=0.938___ between O5 and H6: order=0.889___
between O5 and H7: order=0.841___

## 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.

### Hybridization in the Best Lewis Structure

1. A bonding orbital for C1-O2 with 1.9999 electrons
__has 30.16% C 1 character in a p3 hybrid
__has 69.84% O 2 character in a p3 hybrid

2. A bonding orbital for C1-O2 with 1.9989 electrons
__has 34.43% C 1 character in a sp1.89 hybrid
__has 65.57% O 2 character in a sp1.52 hybrid

3. A bonding orbital for C1-H3 with 1.9934 electrons
__has 57.54% C 1 character in a sp1.99 hybrid
__has 42.46% H 3 character in a s orbital

4. A bonding orbital for C1-H4 with 1.9934 electrons
__has 56.79% C 1 character in a sp2.04 hybrid
__has 43.21% H 4 character in a s orbital

5. A bonding orbital for O5-H6 with 1.9993 electrons
__has 72.99% O 5 character in a s0.89 p3 hybrid
__has 27.01% H 6 character in a s orbital

6. A bonding orbital for O5-H7 with 1.9992 electrons
__has 75.28% O 5 character in a sp2.92 hybrid
__has 24.72% H 7 character in a s orbital

10. A lone pair orbital for O2 with 1.9848 electrons

11. A lone pair orbital for O2 with 1.9088 electrons

12. A lone pair orbital for O5 with 1.9986 electrons

13. A lone pair orbital for O5 with 1.9979 electrons
__made from a s0.07 p3 hybrid

-With core pairs on: C 1 O 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 the second lone pair donor orbital, 11, for O2 with the antibonding acceptor orbital, 93, for C1-H3 is 99.9 kJ/mol.

The interaction of the second lone pair donor orbital, 11, for O2 with the antibonding acceptor orbital, 94, for C1-H4 is 105. kJ/mol.

The interaction of lone pair donor orbital, 10, for O2 with the antibonding acceptor orbital, 96, for O5-H7 is 6.65 kJ/mol.

The interaction of the second lone pair donor orbital, 11, for O2 with the antibonding acceptor orbital, 96, for O5-H7 is 25.6 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.

17 ----- 2.505

16 ----- 1.575

15 ----- 1.142

14 ----- -3.424

13 -^-v- -6.619

12 -^-v- -6.857

11 -^-v- -8.580

10 -^-v- -10.68

9 -^-v- -11.50

8 -^-v- -12.21

7 -^-v- -13.01

6 -^-v- -16.01

5 -^-v- -24.24

4 -^-v- -26.96

3 -^-v- -269.5

2 -^-v- -505.7

1 -^-v- -507.6

## 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 = -191.0143556723 Hartrees