HOOH2+

 H3 | O1 - O2 | | H4 H5
The ion charge is 1.

Atomic Charges and Dipole Moment

O1 charge=-0.336
O2 charge=-0.262
H3 charge= 0.544
H4 charge= 0.544
H5 charge= 0.509
with a dipole moment of 2.29836 Debye

Bond Lengths:

between O1 and O2: distance=1.486 ang___ between O1 and H3: distance=1.001 ang___
between O1 and H4: distance=1.001 ang___ between O2 and H5: distance=0.997 ang___

Bond Angles:

for H3-O1-O2: angle=104.0 deg___ for H4-O1-O2: angle=104.0 deg___
for H5-O2-O1: angle=99.80 deg___

Bond Orders (Mulliken):

between O1 and O2: order=0.823___ between O1 and H3: order=0.769___
between O1 and H4: order=0.769___ between O2 and H5: order=0.811___

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 O1-O2 with 1.9973 electrons
__has 64.14% O 1 character in a s0.60 p3 hybrid
__has 35.86% O 2 character in a s0.22 p3 hybrid

2. A bonding orbital for O1-H3 with 1.9978 electrons
__has 79.54% O 1 character in a sp2.89 hybrid
__has 20.46% H 3 character in a s orbital

3. A bonding orbital for O1-H4 with 1.9978 electrons
__has 79.54% O 1 character in a sp2.89 hybrid
__has 20.46% H 4 character in a s orbital

4. A bonding orbital for O2-H5 with 1.9952 electrons
__has 76.64% O 2 character in a s0.87 p3 hybrid
__has 23.36% H 5 character in a s orbital

7. A lone pair orbital for O1 with 1.9977 electrons

8. A lone pair orbital for O2 with 1.9990 electrons

9. A lone pair orbital for O2 with 1.9942 electrons
__made from a p-pi orbital ( 99.95% p)

-With core pairs on: O 1 O 2 -

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.

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.

13 ----- -5.063

12 ----- -5.588

11 ----- -7.422

10 ----- -11.08

9 -^-v- -15.41

8 -^-v- -17.10

7 -^-v- -20.56

6 -^-v- -22.40

5 -^-v- -24.09

4 -^-v- -31.85

3 -^-v- -37.82

2 -^-v- -516.5

1 -^-v- -519.0

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 = -151.8856958869 Hartrees