## CNPO

 C3 \\ N1 O2 \ // P4
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= 0.224
O2 charge=-0.331
C3 charge=-0.299
P4 charge= 0.406
with a dipole moment of 2.39102 Debye

## Bond Lengths:

between N1 and O2: distance=2.650 ang___ between N1 and C3: distance=1.200 ang___
between N1 and P4: distance=1.772 ang___ between O2 and P4: distance=1.501 ang___

## Bond Angles:

for C3-N1-O2: angle=159.7 deg___ for P4-O2-N1: angle=39.52 deg___

## Bond Orders (Mulliken):

between N1 and O2: order=-0.050___ between N1 and C3: order=1.984___
between N1 and P4: order=0.613___ between O2 and P4: order=1.820___

## 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-C3 with 1.9983 electrons
__has 67.52% N 1 character in a sp0.85 hybrid
__has 32.48% C 3 character in a sp2.12 hybrid

2. A bonding orbital for N1-C3 with 1.9861 electrons
__has 76.92% N 1 character in a p3 hybrid
__has 23.08% C 3 character in a p3 hybrid

3. A bonding orbital for N1-C3 with 1.9539 electrons
__has 79.15% N 1 character in a p3 hybrid
__has 20.85% C 3 character in a p3 hybrid

4. A bonding orbital for N1-P4 with 1.9333 electrons
__has 84.12% N 1 character in a sp1.22 hybrid
__has 15.88% P 4 character in a s0.55 p3 d0.96 hybrid

5. A bonding orbital for O2-P4 with 1.9444 electrons
__has 87.71% O 2 character in a s0.86 p3 hybrid
__has 12.29% P 4 character in a s0.63 p3 d1.19 hybrid

6. A bonding orbital for O2-P4 with 1.9950 electrons
__has 78.24% O 2 character in a p3 hybrid
__has 21.76% P 4 character in a p3 d0.12 hybrid

7. A bonding orbital for O2-P4 with 1.9099 electrons
__has 89.11% O 2 character in a s0.36 p3 hybrid
__has 10.89% P 4 character in a s0.86 p3 d2.30 hybrid

16. A lone pair orbital for O2 with 1.9923 electrons

17. A lone pair orbital for C3 with 1.9818 electrons

18. A lone pair orbital for P4 with 1.9806 electrons

-With core pairs on: N 1 O 2 C 3 P 4 P 4 P 4 P 4 P 4 -

#### 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 third bonding donor orbital, 3, for N1-C3 with the second antibonding acceptor orbital, 102, for O2-P4 is 49.4 kJ/mol.

The interaction of bonding donor orbital, 4, for N1-P4 with the antibonding acceptor orbital, 101, for O2-P4 is 47.9 kJ/mol.

The interaction of bonding donor orbital, 4, for N1-P4 with the third antibonding acceptor orbital, 103, for O2-P4 is 208. kJ/mol.

The interaction of bonding donor orbital, 5, for O2-P4 with the antibonding acceptor orbital, 100, for N1-P4 is 24.8 kJ/mol.

The interaction of bonding donor orbital, 5, for O2-P4 with the third antibonding acceptor orbital, 103, for O2-P4 is 227. kJ/mol.

The interaction of the third bonding donor orbital, 7, for O2-P4 with the antibonding acceptor orbital, 100, for N1-P4 is 112. kJ/mol.

The interaction of the third bonding donor orbital, 7, for O2-P4 with the antibonding acceptor orbital, 101, for O2-P4 is 194. kJ/mol.

The interaction of lone pair donor orbital, 17, for C3 with the antibonding acceptor orbital, 100, for N1-P4 is 29.5 kJ/mol.

The interaction of lone pair donor orbital, 18, for P4 with the antibonding acceptor orbital, 97, for N1-C3 is 35.8 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.

22 ----- -0.344

21 ----- -1.517

20 ----- -2.444

19 ----- -5.098

18 -^-v- -7.659

17 -^-v- -8.557

16 -^-v- -9.315

15 -^-v- -9.696

14 -^-v- -10.81

13 -^-v- -10.95

12 -^-v- -12.41

11 -^-v- -17.39

10 -^-v- -23.98

9 -^-v- -25.95

8 -^-v- -126.1

7 -^-v- -126.4
6 -^-v- -126.5

5 -^-v- -173.9

4 -^-v- -268.7

3 -^-v- -379.0

2 -^-v- -507.8

1 -^-v- -2071.

## 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 = -509.4846224869 Hartrees