N(OH)2O-

 H6 O4 H3 | | | O5 - N1 - O2
The ion charge is -1.

Atomic Charges and Dipole Moment

N1 charge= 0.156
O2 charge=-0.729
H3 charge= 0.354
O4 charge=-0.398
O5 charge=-0.736
H6 charge= 0.353
with a dipole moment of 2.30940 Debye

Bond Lengths:

between N1 and O2: distance=1.770 ang___ between N1 and O4: distance=1.233 ang___
between N1 and O5: distance=1.782 ang___ between O2 and H3: distance=0.981 ang___
between O2 and O5: distance=2.728 ang___ between O5 and H6: distance=0.981 ang___

Bond Angles:

for H3-O2-N1: angle=94.39 deg___ for O4-N1-O2: angle=106.9 deg___
for O5-N1-O2: angle=100.3 deg___ for H6-O5-N1: angle=94.11 deg___

Bond Orders (Mulliken):

between N1 and O2: order=0.542___ between N1 and O4: order=1.343___
between N1 and O5: order=0.536___ between O2 and H3: order=0.909___
between O2 and O5: order=-0.086___ between O5 and H6: order=0.911___

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 N1-O2 with 1.9892 electrons
__has 31.51% N 1 character in a s0.16 p3 hybrid
__has 68.49% O 2 character in a s0.33 p3 hybrid

2. A bonding orbital for N1-O4 with 1.9923 electrons
__has 43.88% N 1 character in a sp2.65 hybrid
__has 56.12% O 4 character in a sp2.73 hybrid

3. A bonding orbital for N1-O5 with 1.9892 electrons
__has 31.02% N 1 character in a s0.15 p3 hybrid
__has 68.98% O 5 character in a s0.32 p3 hybrid

4. A bonding orbital for O2-H3 with 1.9974 electrons
__has 70.93% O 2 character in a s0.84 p3 hybrid
__has 29.07% H 3 character in a s orbital

5. A bonding orbital for O5-H6 with 1.9975 electrons
__has 70.86% O 5 character in a s0.84 p3 hybrid
__has 29.14% H 6 character in a s orbital

10. A lone pair orbital for N1 with 1.9924 electrons

11. A lone pair orbital for O2 with 1.9966 electrons

12. A lone pair orbital for O2 with 1.9844 electrons
__made from a s0.09 p3 hybrid

13. A lone pair orbital for O4 with 1.9900 electrons

14. A lone pair orbital for O4 with 1.7618 electrons
__made from a s0.06 p3 hybrid

15. A lone pair orbital for O4 with 1.7382 electrons

16. A lone pair orbital for O5 with 1.9967 electrons

17. A lone pair orbital for O5 with 1.9852 electrons
__made from a s0.09 p3 hybrid

104. A antibonding orbital for N1-O2 with 0.2535 electrons
__has 68.49% N 1 character in a s0.16 p3 hybrid
__has 31.51% O 2 character in a s0.33 p3 hybrid

106. A antibonding orbital for N1-O5 with 0.2618 electrons
__has 68.98% N 1 character in a s0.15 p3 hybrid
__has 31.02% O 5 character in a s0.32 p3 hybrid

-With core pairs on: N 1 O 2 O 4 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 the second lone pair donor orbital, 12, for O2 with the antibonding acceptor orbital, 106, for N1-O5 is 23.8 kJ/mol.

The interaction of the second lone pair donor orbital, 14, for O4 with the antibonding acceptor orbital, 104, for N1-O2 is 300. kJ/mol.

The interaction of the second lone pair donor orbital, 14, for O4 with the antibonding acceptor orbital, 106, for N1-O5 is 149. kJ/mol.

The interaction of the third lone pair donor orbital, 15, for O4 with the antibonding acceptor orbital, 104, for N1-O2 is 191. kJ/mol.

The interaction of the third lone pair donor orbital, 15, for O4 with the antibonding acceptor orbital, 106, for N1-O5 is 366. kJ/mol.

The interaction of the second lone pair donor orbital, 17, for O5 with the antibonding acceptor orbital, 104, for N1-O2 is 22.3 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.

21 ----- 7.464

20 ----- 6.455

19 ----- 4.305

18 ----- 3.725

17 -^-v- 0.251

16 -^-v- -0.158

15 -^-v- -1.014
14 -^-v- -1.085

13 -^-v- -3.363

12 -^-v- -4.299

11 -^-v- -5.427

10 -^-v- -5.816

9 -^-v- -6.056

8 -^-v- -10.13

7 -^-v- -17.26

6 -^-v- -17.47

5 -^-v- -22.99

4 -^-v- -375.5

3 -^-v- -500.0
2 -^-v- -500.1

1 -^-v- -501.8

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 = -281.6676891721 Hartrees