H3 | N1 - O2 | | H4 H5
Tell me about atomic charges, the dipole moment, bond lengths, angles, bond orders,
or molecular orbital energies.
Tell me about the best Lewis structure.

## Atomic Charges and Dipole Moment

N1 charge=-0.783
O2 charge=-0.466
H3 charge= 0.403
H4 charge= 0.402
H5 charge= 0.444
with a dipole moment of 0.67553 Debye

## Bond Lengths:

between N1 and O2: distance=1.474 ang___ between N1 and H3: distance=1.029 ang___
between N1 and H4: distance=1.029 ang___ between O2 and H5: distance=0.976 ang___

## Bond Angles:

for H3-N1-O2: angle=103.3 deg___ for H4-N1-O2: angle=103.3 deg___
for H5-O2-N1: angle=101.4 deg___

## Bond Orders (Mulliken):

between N1 and O2: order=0.831___ between N1 and H3: order=0.928___
between N1 and H4: order=0.928___ between O2 and H5: order=0.863___

## 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 N1-O2 with 1.9961 electrons
__has 42.01% N 1 character in a s0.62 p3 hybrid
__has 57.99% O 2 character in a s0.63 p3 hybrid

2. A bonding orbital for N1-H3 with 1.9955 electrons
__has 66.93% N 1 character in a s0.98 p3 hybrid
__has 33.07% H 3 character in a s orbital

3. A bonding orbital for N1-H4 with 1.9955 electrons
__has 66.94% N 1 character in a s0.98 p3 hybrid
__has 33.06% H 4 character in a s orbital

4. A bonding orbital for O2-H5 with 1.9959 electrons
__has 73.50% O 2 character in a s0.83 p3 hybrid
__has 26.50% H 5 character in a s orbital

7. A lone pair orbital for N1 with 1.9958 electrons
__made from a sp1.96 hybrid

8. A lone pair orbital for O2 with 1.9982 electrons
__made from a sp0.63 hybrid

9. A lone pair orbital for O2 with 1.9865 electrons
__made from a p-pi orbital ( 99.96% p)

-With core pairs on: N 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 ----- 3.294

12 ----- 2.493

11 ----- 1.062

10 ----- 0.186

9 -^-v- -6.094

8 -^-v- -6.763

7 -^-v- -10.52

6 -^-v- -12.29 5 -^-v- -12.31

4 -^-v- -19.87

3 -^-v- -26.01

2 -^-v- -378.3

1 -^-v- -507.1