H2O2+ dication singlet*

H3
\
O1
\
H2
The ion charge is 2.

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= 0.489
H2 charge= 0.755
H3 charge= 0.754
with a dipole moment of 3.46893 Debye

Bond Lengths:

between O1 and H2: distance=1.258 ang___ between O1 and H3: distance=1.257 ang___

Bond Angles:

for H3-O1-H2: angle=179.9 deg___

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Bond Orders (Mulliken):

between O1 and H2: order=0.370___ between O1 and H3: order=0.371___

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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-H3 with 1.8811 electrons
__has 92.91% O 1 character in a p3 hybrid
__has 7.09% H 3 character in a s orbital

3. A lone pair orbital for O1 with 1.9995 electrons
__made from a p-pi orbital (100.00% p)

4. A lone pair orbital for O1 with 1.9189 electrons
__made from a s orbital

6. A lone pair orbital for H2 with 0.1649 electrons
__made from a s orbital

-With core pairs on: O 1 -

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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 the second lone pair donor orbital, 4, for O1 with the antibonding acceptor orbital, 36, for O1-H3 is 141. kJ/mol.

The interaction of bonding donor orbital, 1, for O1-H3 with the lone pair acceptor orbital, 6, for H2 is 343. kJ/mol.

The interaction of the second lone pair donor orbital, 4, for O1 with the lone pair acceptor orbital, 6, for H2 is 182. kJ/mol.

The interaction of lone pair donor orbital, 6, for H2 with the antibonding acceptor orbital, 36, for O1-H3 is 94.5 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.

8 ----- -8.197


7 ----- -17.80


6 ----- -21.35


5 ----- -32.72


4 -^-v- -30.73


3 -^-v- -35.39


2 -^-v- -47.46


1 -^-v- -535.4

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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 = -74.9519824697 Hartrees

* See H2O2+ triplet for the more stable triplet state.

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