## H2COO triplet state

 H3 | C1 - O2 / \ H4 O5
The multiplicity is 3.

## Atomic Charges and Dipole Moment

C1 charge=-0.309
O2 charge= 0.042
H3 charge= 0.218
H4 charge= 0.217
O5 charge=-0.167
with a dipole moment of 2.33437 Debye

## Bond Lengths:

between C1 and O2: distance=1.383 ang___ between C1 and H3: distance=1.094 ang___
between C1 and H4: distance=1.094 ang___ between O2 and O5: distance=1.405 ang___

## Bond Angles:

for H3-C1-O2: angle=116.6 deg___ for H4-C1-O2: angle=116.6 deg___
for O5-O2-C1: angle=106.7 deg___

## Bond Orders (Mulliken):

between C1 and O2: order=0.875___ between C1 and H3: order=0.954___
between C1 and H4: order=0.954___ between O2 and O5: order=0.770___

## 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. The Lewis structure is built for the up and down electrons, separately. Note that the up and down structures can be very different.

### Hybridization in the Best Lewis Structure

#### Down Electrons

1. A bonding orbital for C1-O2 with 0.9971 electrons
__has 32.60% C 1 character in a sp2.75 hybrid
__has 67.40% O 2 character in a sp2.39 hybrid

2. A bonding orbital for C1-H3 with 0.9965 electrons
__has 59.92% C 1 character in a sp1.82 hybrid
__has 40.08% H 3 character in a s orbital

3. A bonding orbital for C1-H4 with 0.9965 electrons
__has 59.93% C 1 character in a sp1.82 hybrid
__has 40.07% H 4 character in a s orbital

4. A bonding orbital for O2-O5 with 0.9980 electrons
__has 41.75% O 2 character in a s0.31 p3 hybrid
__has 58.25% O 5 character in a s0.43 p3 hybrid

8. A lone pair orbital for C1 with 0.9628 electrons
__made from a s0.09 p3 hybrid

9. A lone pair orbital for O2 with 0.9971 electrons

10. A lone pair orbital for O2 with 0.9862 electrons
__made from a p-pi orbital ( 99.97% p)

11. A lone pair orbital for O5 with 0.9993 electrons

12. A lone pair orbital for O5 with 0.9987 electrons
__made from a p-pi orbital ( 99.98% p)

13. A lone pair orbital for O5 with 0.9968 electrons

-With core pairs on: C 1 O 2 O 5 -

#### Up Electrons

1. A bonding orbital for C1-O2 with 0.9984 electrons
__has 28.92% C 1 character in a sp2.58 hybrid
__has 71.08% O 2 character in a sp2.14 hybrid

2. A bonding orbital for C1-H3 with 0.9975 electrons
__has 54.48% C 1 character in a sp1.77 hybrid
__has 45.52% H 3 character in a s orbital

3. A bonding orbital for C1-H4 with 0.9975 electrons
__has 54.49% C 1 character in a sp1.77 hybrid
__has 45.51% H 4 character in a s orbital

4. A bonding orbital for O2-O5 with 0.9857 electrons
__has 64.92% O 2 character in a s0.61 p3 hybrid
__has 35.08% O 5 character in a s0.32 p3 hybrid

9. A lone pair orbital for O2 with 0.9877 electrons

10. A lone pair orbital for O2 with 0.9177 electrons
__made from a p-pi orbital ( 99.94% p 0.06% d)

11. A lone pair orbital for O5 with 0.9982 electrons

12. A lone pair orbital for O5 with 0.9900 electrons
__made from a s0.15 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 bonding donor orbital, 4, for O2-O5 with the lone pair acceptor orbital, 8, for C1 is 27.5 kJ/mol.

The interaction of lone pair donor orbital, 9, for O2 with the lone pair acceptor orbital, 8, for C1 is 20.5 kJ/mol.

The interaction of the second lone pair donor orbital, 10, for O2 with the third lone pair acceptor orbital, 13, for O5 is 142. 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. Only the spin up electron orbital energies are given.

17 ----- 2.872

16 ----- 1.818

15 ----- 1.271

14 ----- -0.928

13 -^--- -6.041

12 -^--- -7.107

11 -^-v- -7.365

10 -^-v- -10.32

9 -^-v- -12.24

8 -^-v- -13.23

7 -^-v- -13.39

6 -^-v- -16.76

5 -^-v- -22.59

4 -^-v- -29.65

3 -^-v- -268.9

2 -^-v- -508.9

1 -^-v- -510.3

## 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 = -189.6235007344 Hartrees