## NH2CN, Cyanamide

 H3 \ N1 - C2 E N5 / 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=-0.822
C2 charge= 0.569
H3 charge= 0.397
H4 charge= 0.397
N5 charge=-0.542
with a dipole moment of 4.79495 Debye

## Bond Lengths:

between N1 and C2: distance=1.346 ang___ between N1 and H3: distance=1.020 ang___
between N1 and H4: distance=1.020 ang___ between C2 and N5: distance=1.175 ang___

## Bond Angles:

for H3-N1-C2: angle=116.4 deg___ for H4-N1-C2: angle=116.4 deg___
for N5-C2-N1: angle=177.6 deg___

## Bond Orders (Mulliken):

between N1 and C2: order=0.963___ between N1 and H3: order=0.907___
between N1 and H4: order=0.907___ between C2 and N5: order=2.737___

## 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-C2 with 1.9968 electrons
__has 59.29% N 1 character in a sp1.92 hybrid
__has 40.71% C 2 character in a sp1.10 hybrid

2. A bonding orbital for N1-H3 with 1.9803 electrons
__has 70.68% N 1 character in a sp2.49 hybrid
__has 29.32% H 3 character in a s orbital

3. A bonding orbital for N1-H4 with 1.9803 electrons
__has 70.68% N 1 character in a sp2.49 hybrid
__has 29.32% H 4 character in a s orbital

4. A bonding orbital for C2-N5 with 1.9967 electrons
__has 44.00% C 2 character in a sp0.97 hybrid
__has 56.00% N 5 character in a sp1.37 hybrid

5. A bonding orbital for C2-N5 with 1.9946 electrons
__has 38.88% C 2 character in a s0.05 p3 hybrid
__has 61.12% N 5 character in a p3 hybrid

6. A bonding orbital for C2-N5 with 1.9851 electrons
__has 47.29% C 2 character in a p-pi orbital ( 99.81% p 0.19% d)
__has 52.71% N 5 character in a p-pi orbital ( 99.59% p 0.41% d)

10. A lone pair orbital for N1 with 1.8772 electrons
__made from a s0.28 p3 hybrid

11. A lone pair orbital for N5 with 1.9674 electrons

83. A antibonding orbital for C2-N5 with 0.1154 electrons
__has 61.12% C 2 character in a s0.05 p3 hybrid
__has 38.88% N 5 character in a p3 hybrid

-With core pairs on: N 1 C 2 N 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 bonding donor orbital, 1, for N1-C2 with the antibonding acceptor orbital, 82, for C2-N5 is 23.7 kJ/mol.

The interaction of bonding donor orbital, 2, for N1-H3 with the antibonding acceptor orbital, 82, for C2-N5 is 26.0 kJ/mol.

The interaction of bonding donor orbital, 2, for N1-H3 with the third antibonding acceptor orbital, 84, for C2-N5 is 27.6 kJ/mol.

The interaction of bonding donor orbital, 3, for N1-H4 with the antibonding acceptor orbital, 82, for C2-N5 is 26.1 kJ/mol.

The interaction of bonding donor orbital, 3, for N1-H4 with the third antibonding acceptor orbital, 84, for C2-N5 is 27.5 kJ/mol.

The interaction of bonding donor orbital, 4, for C2-N5 with the antibonding acceptor orbital, 79, for N1-C2 is 26.0 kJ/mol.

The interaction of lone pair donor orbital, 10, for N1 with the antibonding acceptor orbital, 82, for C2-N5 is 21.2 kJ/mol.

The interaction of lone pair donor orbital, 10, for N1 with the second antibonding acceptor orbital, 83, for C2-N5 is 197. kJ/mol.

The interaction of lone pair donor orbital, 11, for N5 with the antibonding acceptor orbital, 79, for N1-C2 is 87.8 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.

15 ----- 2.236

14 ----- 0.719

13 ----- -0.013

12 ----- -0.631

11 -^-v- -6.735

10 -^-v- -8.304

9 -^-v- -8.455

8 -^-v- -9.971

7 -^-v- -14.18

6 -^-v- -15.25

5 -^-v- -21.87

4 -^-v- -24.12

3 -^-v- -268.1

2 -^-v- -377.1

1 -^-v- -379.1

## 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 = -148.8414115717 Hartrees