## B=NHF

 B3 \ N1 - F2 / H4
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

N1 charge= 0.325
F2 charge=-0.149
B3 charge=-0.321
H4 charge= 0.145
with a dipole moment of 2.57927 Debye

## Bond Lengths:

between N1 and F2: distance=1.428 ang___ between N1 and B3: distance=1.421 ang___
between N1 and H4: distance=1.030 ang___

## Bond Angles:

for B3-N1-F2: angle=125.9 deg___ for H4-N1-F2: angle=109.3 deg___

## Bond Orders (Mulliken):

between N1 and F2: order=0.784___ between N1 and B3: order=0.664___
between N1 and H4: order=0.859___

## 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-F2 with 1.9962 electrons
__has 38.15% N 1 character in a s0.77 p3 hybrid
__has 61.85% F 2 character in a s0.50 p3 hybrid

2. A bonding orbital for N1-B3 with 1.9917 electrons
__has 84.88% N 1 character in a sp1.01 hybrid
__has 15.12% B 3 character in a s0.60 p3 hybrid

3. A bonding orbital for N1-B3 with 1.9964 electrons
__has 91.64% N 1 character in a p3 hybrid
__has 8.36% B 3 character in a p3 hybrid

4. A bonding orbital for N1-H4 with 1.9879 electrons
__has 70.64% N 1 character in a sp2.38 hybrid
__has 29.36% H 4 character in a s orbital

8. A lone pair orbital for F2 with 1.9967 electrons

9. A lone pair orbital for F2 with 1.9935 electrons
__made from a p-pi orbital ( 99.99% p)

10. A lone pair orbital for F2 with 1.9908 electrons
__made from a s0.05 p3 hybrid

11. A lone pair orbital for B3 with 1.9847 electrons

-With core pairs on: N 1 F 2 B 3 -

#### 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 bonding donor orbital, 4, for N1-H4 with the second lone pair acceptor orbital, 12, for B3 is 24.5 kJ/mol.

The interaction of bonding donor orbital, 4, for N1-H4 with the antibonding acceptor orbital, 75, for N1-F2 is 22.9 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.

15 ----- 0.480

14 ----- -0.903

13 ----- -1.627

12 ----- -4.563

11 -^-v- -5.979

10 -^-v- -7.852

9 -^-v- -10.36

8 -^-v- -11.88

7 -^-v- -14.77

6 -^-v- -15.03

5 -^-v- -22.04

4 -^-v- -31.25

3 -^-v- -177.3

2 -^-v- -380.6

1 -^-v- -657.4

## 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 = -179.9440699767 Hartrees