(HO)2NH->O, Dihydroxylamine oxide

H7O3 - H4
| /
O1 - N2
| \
H6O5
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=-0.497
N2 charge= 0.153
O3 charge=-0.498
H4 charge= 0.429
O5 charge=-0.397
H6 charge= 0.383
H7 charge= 0.427
with a dipole moment of 0.35410 Debye

Bond Lengths:

between O1 and N2: distance=1.533 ang___ between O1 and O3: distance=2.429 ang___
between O1 and H7: distance=0.985 ang___ between N2 and O3: distance=1.532 ang___
between N2 and O5: distance=1.250 ang___ between N2 and H6: distance=1.043 ang___
between O3 and H4: distance=0.985 ang___

Bond Angles:

for O3-N2-O1: angle=104.8 deg___ for H4-O3-N2: angle=99.02 deg___
for O5-N2-O1: angle=114.8 deg___ for H6-N2-O1: angle=100.3 deg___
for H7-O1-N2: angle=99.09 deg___

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Bond Orders (Mulliken):

between O1 and N2: order=0.864___ between O1 and O3: order=-0.084___
between O1 and H7: order=0.837___ between N2 and O3: order=0.865___
between N2 and O5: order=1.180___ between N2 and H6: order=0.869___
between O3 and H4: order=0.837___

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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-N2 with 1.9898 electrons
__has 51.68% O 1 character in a s0.40 p3 hybrid
__has 48.32% N 2 character in a s0.73 p3 hybrid

2. A bonding orbital for O1-H7 with 1.9944 electrons
__has 74.49% O 1 character in a s0.90 p3 hybrid
__has 25.51% H 7 character in a s orbital

3. A bonding orbital for N2-O3 with 1.9898 electrons
__has 48.33% N 2 character in a s0.73 p3 hybrid
__has 51.67% O 3 character in a s0.41 p3 hybrid

4. A bonding orbital for N2-O5 with 1.9948 electrons
__has 52.73% N 2 character in a sp1.88 hybrid
__has 47.27% O 5 character in a s0.78 p3 hybrid

5. A bonding orbital for N2-H6 with 1.9886 electrons
__has 71.10% N 2 character in a sp2.77 hybrid
__has 28.90% H 6 character in a s orbital

6. A bonding orbital for O3-H4 with 1.9944 electrons
__has 74.49% O 3 character in a s0.90 p3 hybrid
__has 25.51% H 4 character in a s orbital

11. A lone pair orbital for O1 with 1.9929 electrons
__made from a sp0.56 hybrid

12. A lone pair orbital for O1 with 1.9785 electrons
__made from a p3 hybrid

13. A lone pair orbital for O3 with 1.9929 electrons
__made from a sp0.56 hybrid

14. A lone pair orbital for O3 with 1.9783 electrons
__made from a p3 hybrid

15. A lone pair orbital for O5 with 1.9877 electrons
__made from a sp0.27 hybrid

16. A lone pair orbital for O5 with 1.8617 electrons
__made from a p3 hybrid

17. A lone pair orbital for O5 with 1.8157 electrons
__made from a p-pi orbital ( 99.90% p 0.10% d)

109. A antibonding orbital for O1-N2 with 0.1557 electrons
__has 48.32% O 1 character in a s0.40 p3 hybrid
__has 51.68% N 2 character in a s0.73 p3 hybrid

111. A antibonding orbital for N2-O3 with 0.1548 electrons
__has 51.67% N 2 character in a s0.73 p3 hybrid
__has 48.33% O 3 character in a s0.41 p3 hybrid

-With core pairs on: O 1 N 2 O 3 O 5 -

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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, 12, for O1 with the antibonding acceptor orbital, 111, for N2-O3 is 31.6 kJ/mol.

The interaction of the second lone pair donor orbital, 14, for O3 with the antibonding acceptor orbital, 109, for O1-N2 is 31.9 kJ/mol.

The interaction of the second lone pair donor orbital, 16, for O5 with the antibonding acceptor orbital, 109, for O1-N2 is 71.8 kJ/mol.

The interaction of the second lone pair donor orbital, 16, for O5 with the antibonding acceptor orbital, 111, for N2-O3 is 74.4 kJ/mol.

The interaction of the second lone pair donor orbital, 16, for O5 with the antibonding acceptor orbital, 113, for N2-H6 is 93.3 kJ/mol.

The interaction of the third lone pair donor orbital, 17, for O5 with the antibonding acceptor orbital, 109, for O1-N2 is 175. kJ/mol.

The interaction of the third lone pair donor orbital, 17, for O5 with the antibonding acceptor orbital, 111, for N2-O3 is 171. 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.

21 ----- 1.172

20 ----- 0.399


19 ----- -0.972

18 ----- -1.708


17 -^-v- -7.236
16 -^-v- -7.317

15 -^-v- -7.763

14 -^-v- -8.353


13 -^-v- -10.64

12 -^-v- -11.29


11 -^-v- -13.26

10 -^-v- -14.15

9 -^-v- -14.65


8 -^-v- -19.64


7 -^-v- -25.39

6 -^-v- -25.56


5 -^-v- -30.20


4 -^-v- -384.2


3 -^-v- -507.3

2 -^-v- -507.8 1 -^-v- -507.8

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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 = -282.2086986483 Hartrees

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