CO3OH-, hydroperoxocarbonate anion

O6
//
O5 = C4H3
\ |
O1 - O2
The ion charge is -1.

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

O1 charge=-0.323
O2 charge=-0.497
H3 charge= 0.379
C4 charge= 0.848
O5 charge=-0.690
O6 charge=-0.717
with a dipole moment of 5.41591 Debye

Bond Lengths:

between O1 and O2: distance=1.510 ang___ between O1 and C4: distance=1.448 ang___
between O1 and O5: distance=2.236 ang___ between O1 and O6: distance=2.294 ang___
between O2 and H3: distance=1.025 ang___ between O2 and C4: distance=2.399 ang___
between O2 and O6: distance=2.473 ang___ between H3 and O6: distance=1.637 ang___
between C4 and O5: distance=1.247 ang___ between C4 and O6: distance=1.273 ang___
between O5 and O6: distance=2.314 ang___

Bond Angles:

for H3-O2-O1: angle=92.94 deg___ for C4-O1-O2: angle=108.4 deg___
for O5-C4-O1: angle=111.9 deg___ for O6-C4-O1: angle=114.7 deg___

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Bond Orders (Mulliken):

between O1 and O2: order=0.753___ between O1 and C4: order=0.946___
between O1 and O5: order=-0.133___ between O1 and O6: order=-0.102___
between O2 and H3: order=0.761___ between O2 and C4: order=0.088___
between O2 and O6: order=-0.063___ between H3 and O6: order=0.118___
between C4 and O5: order=1.774___ between C4 and O6: order=1.535___
between O5 and O6: order=-0.146___

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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 O1-O2 with 1.9904 electrons
__has 51.90% O 1 character in a s0.40 p3 hybrid
__has 48.10% O 2 character in a s0.31 p3 hybrid

2. A bonding orbital for O1-C4 with 1.9897 electrons
__has 69.46% O 1 character in a sp2.90 hybrid
__has 30.54% C 4 character in a sp2.99 hybrid

3. A bonding orbital for O2-H3 with 1.9960 electrons
__has 77.41% O 2 character in a s0.98 p3 hybrid
__has 22.59% H 3 character in a s orbital

4. A bonding orbital for C4-O5 with 1.9981 electrons
__has 19.56% C 4 character in a p-pi orbital ( 99.19% p 0.81% d)
__has 80.44% O 5 character in a p-pi orbital ( 99.86% p 0.14% d)

5. A bonding orbital for C4-O5 with 1.9944 electrons
__has 36.44% C 4 character in a sp1.60 hybrid
__has 63.56% O 5 character in a sp1.85 hybrid

6. A bonding orbital for C4-O6 with 1.9962 electrons
__has 35.90% C 4 character in a sp1.71 hybrid
__has 64.10% O 6 character in a sp2.00 hybrid

12. A lone pair orbital for O1 with 1.9865 electrons
__made from a sp0.59 hybrid

13. A lone pair orbital for O1 with 1.9279 electrons
__made from a p-pi orbital ( 99.96% p)

14. A lone pair orbital for O2 with 1.9963 electrons
__made from a p-pi orbital ( 99.97% p)

15. A lone pair orbital for O2 with 1.9945 electrons
__made from a sp0.51 hybrid

16. A lone pair orbital for O5 with 1.9764 electrons
__made from a sp0.53 hybrid

17. A lone pair orbital for O5 with 1.8776 electrons
__made from a p3 hybrid

18. A lone pair orbital for O6 with 1.9714 electrons
__made from a sp0.55 hybrid

19. A lone pair orbital for O6 with 1.8586 electrons
__made from a s0.07 p3 hybrid

20. A lone pair orbital for O6 with 1.7389 electrons
__made from a p-pi orbital ( 99.89% p 0.11% d)

122. A antibonding orbital for O1-C4 with 0.1375 electrons
__has 30.54% O 1 character in a sp2.90 hybrid
__has 69.46% C 4 character in a sp2.99 hybrid

124. A antibonding orbital for C4-O5 with 0.3181 electrons
__has 80.44% C 4 character in a p-pi orbital ( 99.19% p 0.81% d)
__has 19.56% O 5 character in a p-pi orbital ( 99.86% p 0.14% d)

-With core pairs on: O 1 O 2 C 4 O 5 O 6 -

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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 lone pair donor orbital, 12, for O1 with the antibonding acceptor orbital, 126, for C4-O6 is 21.1 kJ/mol.

The interaction of the second lone pair donor orbital, 13, for O1 with the antibonding acceptor orbital, 124, for C4-O5 is 141. kJ/mol.

The interaction of lone pair donor orbital, 16, for O5 with the antibonding acceptor orbital, 126, for C4-O6 is 31.6 kJ/mol.

The interaction of the second lone pair donor orbital, 17, for O5 with the antibonding acceptor orbital, 122, for O1-C4 is 172. kJ/mol.

The interaction of the second lone pair donor orbital, 17, for O5 with the antibonding acceptor orbital, 126, for C4-O6 is 99.7 kJ/mol.

The interaction of the second lone pair donor orbital, 19, for O6 with the antibonding acceptor orbital, 122, for O1-C4 is 135. kJ/mol.

The interaction of the second lone pair donor orbital, 19, for O6 with the antibonding acceptor orbital, 123, for O2-H3 is 129. kJ/mol.

The interaction of the second lone pair donor orbital, 19, for O6 with the second antibonding acceptor orbital, 125, for C4-O5 is 93.0 kJ/mol.

The interaction of the third lone pair donor orbital, 20, for O6 with the antibonding acceptor orbital, 124, for C4-O5 is 547. kJ/mol.

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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.

24 ----- 8.738

23 ----- 7.074

22 ----- 5.378

21 ----- 3.170


20 -^-v- -0.775

19 -^-v- -1.140

18 -^-v- -1.779

17 -^-v- -2.104


16 -^-v- -3.581

15 -^-v- -4.151

14 -^-v- -4.982


13 -^-v- -6.024

12 -^-v- -6.214

11 -^-v- -6.930


10 -^-v- -9.138


9 -^-v- -16.68


8 -^-v- -19.16


7 -^-v- -20.48


6 -^-v- -22.82


5 -^-v- -264.9


4 -^-v- -500.5

3 -^-v- -500.8


2 -^-v- -502.4

1 -^-v- -503.1

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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 = -339.7639557006 Hartrees

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